Compilation of Data to Estimate Groundwater Migration Potential for Constituents in Active Liquid Discharges at the Hanford Site

1. L. Ames R. J. Serne

March 1991

Prepared for the U.S. Department of Energy under Contract DE-AC06-76RLO 1 830

Pacific Northwest Laboratory Operated for the U.S. Department of Energy by Battelle Memorial Institute

DISCLAIMER

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COMPILATION OF DATA TO ESTIMATE GROUNDWATER MIGRATION POTENTIAL FOR CONSTITUENTS I N ACTIVE LIQUID DISCHARGES AT THE HANFORD SITE

L. L. Ames R. J. Serne

March 1991

Prepared f o r t h e U.S. Department o f Energy under Con t rac t DE-AC06-76RLO 1830

P a c i f i c Northwest Labora to ry R ich land , Washington 99352

EXECUTIVE SUMMARY

A preliminary characterization of the constituents present in the 33

liquid waste streams at the U.S. Department of Energy's Hanford Site has been

completed by Westinghouse Hanford Company. In addition, Westinghouse Hanford

has summarized the soil characteristics based on drill logs collected at each

site that receives these liquid wastes. Literature searches were conducted

and available Hanford-specific data were tabulated and reviewed. General

literature on organic chemicals present in the liquid waste streams was also

reviewed. Specifically, values for water solubi 1 ity, soi 1 adsorption,

sediment organic carbon adsorption properties, octanol-water partition

coefficients (KOw) , Henry' s Law constants (a measure of vol at i 1 i ty) , and biodegradation half-lives were gleaned from the literature to allow estimates

of migration potential. Using all of this information, Pacific Northwest

Laboratory has developed a best estimate of the transport characteristics

(water sol ubi 1 i ty and soi 1 adsorption properties) for those radionucl ides and

inorganic and organic chemicals identified in the various waste streams.

We assume that the potential for transport is qualified through the four

geochemical parameters: solubility, distribution coefficient, persistence

(radiogenic or biochemical half-1 ife) , and volati 1 ity. Summary tables of

these parameters are presented for more than 50 inorganic and radioactive

species and more than 50 organic compounds identified in the liquid waste

streams. Brief descriptions of the chemical characteristics of Hanford

sediments, solubility, and adsorption processes, and of how geochemical

parameters are used to estimate migration in groundwater-sediment environments

are also presented. Groundwater monitoring data are tabulated for wells

neighboring the facilities that receive the liquid wastes.

The radioactive and organic constituents measured in groundwaters can be used to infer actual migration potentials for comparison with the literature

assessments. In general the comparison is good. Compounds that appear to be

mobile include methylene chloride, chloroform, bis(2-ethylhexyl) phthalate,

acetone, methyl ethyl ketone, tetrachloroethylene, lZ91 , 6 0 ~ o , 1 0 6 ~ ~ , 9 9 ~ c , 3 ~ , 137~s, and 90~r. Bis(2-ethylhexyl) phthalate, 137~s, and 9 0 ~ r are not expected (based on their adsorption properties) to be mobile, but a1 1 of the

other species identified are expected to be mobile. The report recommends

data collection activity to gather important data on the solubility,

adsorption, and degradation properties of the potentially mobile species

identified.

ACKNOWLEDGMENTS

The s tudy was funded by t h e Environmental Technology Group o f

Westinghouse Hanford Company. The au thors w ish t o thank J. W. Cammann and

J. C. Sonnichsen o f t h e Environmental Technology Group f o r t h e i r suppor t .

We w ish t o thank S. R. Peterson, ICF Northwest Company, f o r p r o v i d i n g

access t o t h e S o i l T ranspor t Fate computer ized database, and N. G. Ca r t e r ,

P a c i f i c Northwest Labora to ry , f o r pe r f o rm ing computer searches and a l e r t i n g us

t o t h e ex i s t ence o f t h e Syracuse Un i ve rs i t y - suppo r t ed databases on chemical

f a t e and b i o l o g i c a l degrada t ion . We wish t o acknowledge t h e he lp o f

W. J. M a r t i n and L. J. C r i s c e n t i i n access ing these computer databases.

F i n a l l y we w ish t o thank J. A. Schramke f o r p r e p a r i n g t h e o rgan ic

s t r u c t u r e s shown i n t h e document us i ng t h e so f twa re package Chembase and

E. A. Fa i rwea ther f o r t y p i n g t h e manuscr ip t and c o l l a t i n g t h e sec t i ons i n t o a

cohes ive document.

CONTENTS

EXECUTIVE SUMMARY . . . . . . . . . . . . . . . . . . . . . . . . . . ACKNOWLEDGMENTS . . . . . . . . . . . . . . . . . . . . . . . . . . . 1.0 INTRODUCTION . . . . . . . . . . . . . . . . . . . . . . . . . . 2.0 DESCRIPTION OF WASTE STREAMS . . . . . . . . . . . . . . . . . .

2.1 CONSTITUENTS . . . . . . . . . . . . . . . . . . . . . . . 2.1.1 I n o r g a n i c s . . . . . . . . . . . . . . . . . . . . . 2.1 .2 O r g a n i c s . . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . 2.1 .3 R a d i o n u c l i d e s

2 . 2 ESTIMATES OF WASTE STREAM VOLUME . . . . . . . . . . . . . 3 . 0 CHARACTERISTICS OF HANFORD SEDIMENTS . . . . . . . . . . . . . . 4.0 SEDIMENT INTERACTIONS . . . . . . . . . . . . . . . . . . . . .

. . . . . . . . . . . . . 4 . 1 CONSTANT D I S T R I B U T I O N COEFF IC IENT

4 . 2 INTRODUCTION TO EST IMAT ING ADSORPTION CONSTANTS . . . . . . 4.3 D I S T R I B U T I O N COEFF IC IENTS FOR INORGANICS AND

. . . . . . . . . . . . . . . . . . . . . . . RADIONUCLIDES

4 . 4 S O L U B I L I T Y OF INORGANIC AND RADIONUCLIDE CONSTITUTENTS . . 4 .5 CHEMICAL/RADIOLOGICAL H A L F - L I V E S . . . . . . . . . . . . . 4 . 6 D I S T R I B U T I O N COEFF IC IENTS FOR ORGANICS . . . . . . . . . .

. . . . . . . . . . . . . . . . . . . . . . . . . . 5.0 FUTURE WORK

6.0 REFERENCES . . . . . . . . . . . . . . . . . . . . . . . . . . . APPENDIX A . ENVIRONMENTAL FATE OF ORGANIC ANALYTES REPORTED I N THE

3 3 W A S T E S T R E A M S . . . . . . . . . . . . . . . . . . . . . . . . APPENDIX B . EXAMPLES OF HANFORD SEDIMENT COLUMN LEAKAGE OF ORGANIC . . . . . . . . . . . . . . . . . . COMPOUNDS AND RADIONUCLIDES

iii

FIGURES

1 Classification of Waste Streams Based on Five Key Parameters of Acidity. Radioactivity. Organic Content. Dissolved Solids . . . . . . . . . . . . . . . . Content. and Waste Stream Volume

. . . . . . . 2 Rd Estimates for Beryllium. Calcium. and Magnesium

. . . . . . . . . . . . . 3 Rd Estimates for Strontium and Barium

4 Rd Estimates for Lithium. Potassium. Sodium. and . . . . . . . . . . . . . . . . . . . . . . . . . . . . Ammonium

. . . . . . . . . . 5 Rd Estimates for Cobalt. Iron. and Manganese

6 Rd Estimates for Lead. Zinc. Cadmium. Copper. Nickel . Silver. andMercury . . . . . . . . . . . . . . . . . . . . . .

7 Rd Estimates for Antimony. Molybdenum. and Sulfide . . . . . . . . . . . . . 8 Rd Estimates for Zirconium. Niobium. and Tin

9 R Estimates for Chromi um(V1) . Tritium. Technetium. ~bloride. Fluoride. Iodine. Sulfate. Nitrate. Xenon . Krypton. . . . . . . . . . . . . . . . . . . . . . . . . . . . . and Argon

. . . . . . . . . . . . . . . . . . . . . 10 Rd Estimates for Cesium

11 Rd Estimates for Chromium(II1) . Rare Earths. Americium. . . . . . . . . . . . . . . . . . . . . . . . . . . . and Curium

. . . . . . . . . . . . . . . . . . . 12 Rd Estimates for Plutonium

. . . . . . . . . . . . . 13 Rd Estimates f o r Neptunium and Uranium

. . . . . . . . 14 Rd Estimates for Aluminum. Silicon. and Titanium

. . . . . . . . . . . . . 15 Rd Estimates for Phosphate and Vanadium

. . . . . . . . . . . . . . . . . . . 16 Rd Estimates for Ruthenium

viii

TABLES

1 The 33 L i q u i d E f f l u e n t Streams and t h e F a c i l i t i e s Rece iv ing t h e Streams . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 1.2

2 I no rgan i c Ana l y te Repor t ing Frequency f o r t h e Waste Stream Analyses . . . . . . . . . . . . . . . . . . . . . . . . . 2.2

3 Waste Stream Ino rgan i c Ana l y te Content and Mean F i e l d pH Based on Reported Data . . . . . . . . . . . . . . . . . . . . . . . . 2.4

4 Discharge Rate o f P r i n c i p a l I no rgan i c Analy tes . . . . . . . . . 2.5

5 A n a l y t i c a l Frequency f o r t h e Organic Analy tes . . . . . . . . . . 2.6

6 C l a s s i f i c a t i o n s o f Some Hazardous Chemicals Found i n t h e 33 Wastest reams . . . . . . . . . . . . . . . . . . . . . . . . . . 2.8

7 Waste Streams Con ta in i ng t h e Larges t Contents o f Organic . . . . . . . . . . . . . . . . . . . . . . . . . . . . Ana ly tes 2.9

8 D a i l y Discharge Amounts o f Organic Analy tes Based on Analyses and E f f l u e n t Volumes o f t h e 33 Waste Streams . . . . . . . . . . 2.10

9 Organic Analy tes Reported i n Three 200 West Area Wel lwater Samples . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 2.11

10 Frequency o f Radionuc l ides i n t h e 33 Waste Streams . . . . . . . 2.12

11 Waste Streams w i t h t h e Bu lk o f t h e To ta l R a d i o a c t i v i t y i n t h e 33 Waste Streams . . . . . . . . . . . . . . . . . . . . . 2.13

12 Waste Stream Volume Est imates . . . . . . . . . . . . . . . . . . 2.14

13 . Recent Sediment Data That I n c l u d e Organic Carbon Values . . . . 3.2

14 Waste Stream I d e n t i f i c a t i o n . . . . . . . . . . . . . . . . . . . 4.7

15 Q u a l i t a t i v e Est imate o f M ine ra l S o l u b i l i t y of Hanford Sediment i n Pore Water . . . . . . . . . . . . . . . . . . . . . 4.28

16 H a l f - L i f e f o r Rad ionuc l ides I d e n t i f i e d i n A c t i v e Wastest reams . . . . . . . . . . . . . . . . . . . . . . . . . . 4.30

17 Radionuc l ides w i t h H a l f - L i v e s Long Enough f o r Environmental Concern . . . . . . . . . . . . . . . . . . . . . . 4.31

18 Phys ica l and Chemical Processes Used t o Assess t h e D i s t r i b u t i o n and Fa te o f Organic Compounds . . . . . . . . . . . . . . . . . 4.33

19 Physicochemical Parameters Used in Evaluation of Transport Properties of Organic Compounds . . . . . . . . . . . . . . . . . 4.34

20 Envi ronmental Processes Affecting the Organic Compounds Identified in the 33 Waste Streams . . . . . . . . . . . . . . . 4.35

21 Regression Equations Useful for Estimation of Partition Coefficients . . . . . . . . . . . . . . . . . . . . . . . . . . 4.39

22 Available Physicochemical Data for the Organic Compounds Listed inTable5 . . . . . . . . . . . . . . . . . . . . . . . . . . . 4.42

23 Qualitative Ranking of Geochemical Attributes of the Organic Compounds Listed in Table 5 . . . . . . . . . . . . . . . . . . 4.44

1.0 INTRODUCTION

Operating facilities at the Hanford Site in Washington State have historical ly discharged large quantities of 1 iquid effluent, the bulk of which did not routinely contain radioactive materials, into the sediments. Because

the radionuclide contents of the waste streams were generally low, this technique of disposal was chosen after consideration of the sediment column's cation exchange capacity characteristics, unsaturated sediment column depth, and groundwater migration rates.

The U .S. Department of Energy, Rich1 and Operations Office (DOE-RL) established a policy in 1984 to eliminate discharges of contaminated liquid to the sediment column and to meet all applicable federal and state environmental

regulations. A plan and schedule were prepared in response to a request by Congress for discontinuation of the disposal of contaminated solutions into the sediment column.

At the request of the Washington State Department of Ecology (Ecology) and the U.S. Environmental Protection Agency (EPA), DOE-RL has initiated a

study by its contractors, Westinghouse Hanford Company and Pacific Northwest Laboratory (PNL) , (a) of the characteristics of 1 iquid discharges at the Hanford Site. This report addresses in some detail the 33 waste streams

identified in the Waste Stream Characterization Report (Westinghouse Hanford 1989) to provide a best estimate of the waste stream constitutents' potential for migration. In this report, the potential for transport is assumed to be quantified by three geochemical parameters: water sol ubi 1 i ty, adsorption distribution coefficient, and persistence (radiogenic or biochemical half-1 ife) . The 33 waste streams and their respective disposal units are

listed in Table 1. Seven of the waste streams go to the same facility (216-B-3 pond system), and three go to double-shell tanks for interim storage.

(a) PNL is operated for DOE by Battel le Memorial Institute.

TABLE 1. The 33 L i q u i d E f f l u e n t Streams and t h e F a c i l i t i e s Receiving t h e Streams (Westi nghouse Hanford 1989)

Ef f l uent Stream

8 Plant process condensate WRM PI ant ammon i a scrubber condensate 241-AY, 2 4 1 4 steam condensate N Reactor e f f l uen t PURE Plant process condensate U03 Plant process condensate Plutonium Finishing Plant wastewater WRM Plant chemical sewer 8 Plant c h e ~ i c a l sewer 222-S Laboratory wastewater 2101-M Laboratory wastewater 209-E Laboratory wastewater T Plant wastewater 300 Area process wastewater 183-D F i l t e r backf lush wastewater 8 Plant steam condensate WRM Plant steam condensate S Plant wastewater 242-A Evaporator steam condensate 242-A Evaporator process condensate 2724-W Laundry wastewater 163-N Den i nera l i zed wastewater UO Plant wastewater 8 %lant cooling water WRM Plant cooling water T Plant laboratory wastewater 241-A Tank Farm cooling water 242-A Evaporator cool ing water 242-S Evaporator steam condensate 244-AR Vau I t cool ing water 284-E Powerplant cool ing water 284-W Powerp l ant cool i ng water 400 Area secondary cool i ng water(g)

Receiving (Disposa I) Fac i l i ty (a)

Double-she1 I tanks(b) Double-she1 I tanks(c) Double-she1 I tanks(d) 1325-N c r i b 216-A-45 c r i b 216-U-17 c r i b 216-2-20 c r i b 216-A-29 d i tch1216-8-3 pond 216-8-63 trench 216-S-26 c r ' b 2101-tA ponde) 216-C-7 c r i b 216-T-4-2 d i t ch 300 Area pr c ss trenches(e) 100-0 pondsTel 216-8-55 c r i b 216-A-381216-A-37 c r ibs 216-S-10 d i tchlpond 216-8-3 pond sy 216-A-37-1 c r i b 216-W-LWC c r i b 1324-NINA pond(e) 216-Y-14 d i t ch 216-8-3 pond system(e) 216-8-3 pond system(e) 216-T-1 d i t ch 216-8-3 pond system(e) 216-8-3 pond 216-U-14 d i t ch 216-8-3 pond system(e) 216-8-3 pond 200-W Powerhouse pond 400 Area pond

(a) Disposition as of September 1989. (b) Discharged t o 216-8-62 c r i b unt i l January 1986. Currently discharged t o double-she1 l

tanks; w i l l be rerouted t o 216-8-62. (c) Discharged t o 216-A-36-8 c r i b u n i t September 1987. Currently discharged t o

double-she l l tanks. (d) Discharged t o 216-A-8 c r i b u n t i l 1983. Currently discharged t o double-shell tanks.

Resumption of discharge t o 216-A-8 i s pending review by Westinghouse Hanford and approva I by DOE-RL.

(e) Resource Conservation and Recovery Act o f 1976 (RCRA) disposal un i t . (f) Current discharge has been suspended; studies are under way t o ident i fy a fu ture

disposal s i t e . (g) 400 Area secondary cool ing water i s not related t o Fast Flux Test Faci l i t y reactor

heat remova I .

2.0 DESCRIPTION OF WASTE STREAMS

The waste streams contain dissolved inorganics, organics, and

radionuclides, as well as suspended solids. Because the chemical composition

of the waste streams (e.g., the pH and types and amounts of dissolved salts) influences the solubility and adsorption properties of radionuclides and

regulated chemicals, a discussion of the overall chemical nature of the waste

streams is provided here. Each of these constituents will be discussed for

the 33 streams for which data are available. The waste stream samples used

for chemical analyses were collected over short time intervals and therefore

may not be representative of overall chemical compositions for the life of the

waste stream. The same can be said for the stream volumes given in this

report, because the waste stream volumes were taken over a short time interval

and the streams often fluctuate widely in volume.

2.1 CONSTITUENTS

2.1.1 Inorganics

A total of 33 inorganic constituents make up the bulk of the inorganic

materi a1 s (not including radionucl ides) that have been measured in the waste

streams. These are listed in Table 2 in terms of analytical reporting

frequency, N. Uranium, which is classifiable as either a radionuclide or a

heavy metal, was the most frequently reported analyte, followed by sodium,

calcium, and potassium. Magnesium and zinc are also commonly reported in

these chemical analyses.

Average inorganic chemical analyses have been published for each waste

stream (Westinghouse Hanford 1989) . The averaged analyses were used to

determine total waste stream inorganic content, by converting the average

cation concentration to molarities and summing them. This treatment assumes

that anions are present to maintain an electrostatic balance, but it is not a

material-balancing procedure. Using the inorganic cation analysis averages

presented by Westinghouse Hanford (1989) often conceals the considerable range

in the individual analyses making up the average. For example, the analytical

sodium content of B Plant chemical sewage varies from 4 to 6,000 mg/L for

TABLE 2. I no rgan i c Ana ly te Repor t ing Frequency (N) f o r t h e Waste Stream Analyses (West i nghouse Hanford 1989)

Analy te N Analy te - N

Uran i urn 3 14 Mercury 9 7

Sodi urn 3 10 S i l i c o n 74

Cal c i urn 307 Lead 6 1

Potass i urn 300 N icke l 43

Z inc 285 Cadmi urn 39

Magnesi urn 281 Chrorni urn 3 8

S u l f a t e 277 Vanadi urn 33

B a r i urn 265 Phosphate 24

Ch lo r i de 250 S u l f i d e 16

I r o n 227 Bery l 1 i urn 5

F l u o r i d e 178 S i 1 ver 4

Manganese 171 L i t h i u m 2

Copper 155 Arsenic 1

N i t r a t e 146 Antimony 1

St ron t ium 136 T i n 1

Aluminum 128 T i taniurn 1

Ammonium 124

individual analyses. I t i s doubtful that the sampling period was long enough

or the number of individual analyses large enough to obtain a representative sample average.

Of more interest t o determining environmental f a t e i s the total waste

stream content of inorganics, as shown in Table 3. For comparison, the

analyte contents of Hanford groundwater and Columbia River waters range from

7 x lom3 to 1 x 1 0 ' ~ M . Most of the waste streams are more d i lu te than these

natural waters. The wastewaters from power plants were among the highest in

total dissolved inorganics. Only three of the waste streams show average

f i e ld pH values less than pH 6.0, and even these three have pH values a t or

above 5.2. The overall inorganic analyte discharge rates (kglmo) are given in

Table 4. The amounts of Ca, Mg, SO4, HC03, K, and N H 4 discharged each month

exceed or approach 5,000 k g , and NO3 exceeds f ive times that amount. There are several known inorganic carcinogens and/or toxic substances in th i s 1 i s t ,

including beryllium, cadmium, lead, s i lve r , and mercury. The allowable l imits

for these constituents have been given by Ecology (1987). If these toxic metals were homogeneously distributed in the water discharged each month,

concentrations would be below the maximum permissible l imits and in the range

0.01 to 3 pg/L, depending on the metal. The chemical analyses do not,

however, indicate how these metals are distributed or the i r forms in the

wastes.

2.1.2 Organics

There are 51 organic constituents that were identified a t least twice in

analyses of the 33 waste streams. These are l i s ted with the i r frequencies in

Table 5. These 51 organic constituents are classif ied by structure group in Appendix A . Along with the s t ructure, the data pertaining to soil sorption, so lubi l i ty , and vo la t i l i t y are given for most of the organic constituents. Chloroform was the most prevalent organic analyte, even though i t i s not used in any of the chemical processes a t the Hanford Si te (Jungfleisch 1988). The

ch 1 ori nat i on of natural waters has been shown to commonly produce chloroform

as well as other halogenated hydrocarbons (Dowty e t a l . 1975; Rook 1977;

Larson and Rockwell 1979; Norwood e t a l . 1980). Chloroform and the phthalates

TABLE 3. Waste Stream Inorgan ic Analyte Content and Mean F i e l d pH Based on Reported Data (Westinghouse Hanford 1989)

Waste Stream

N Reactor e f f l u e n t 163-N Demineral izer wastewater 183-D F i l t e r backf lush wastewater PUREX P lant chemical sewer PUREX P lant process condensate PUREX P l ant ammonia scrubber condensate PUREX P lan t stream condensate PUREX P lan t cool i n g water B P lan t chemical sewer B P lan t process condensate B P lan t steam condensate B P l ant cool i ng water Plutonium F i n i s h i n g P lan t wastewater S P lan t wastewater T P lan t headend wastewater T P lan t wastewater U03 P lan t process condensate UO / U P lan ts wastewater 2 4 ? - ~ Tank Farm coo l i ng water 241-AY, 241-AZ Tank Farms steam condensate 242-A Evaporator process condensate 242-A Evaporator steam condensate 242-A Evaporator c o o l i n g water 242-S Evaporator steam condensate 244-AR Vau l t c o o l i n g water 209-E Laboratory r e f l e c t o r water 222-S Laboratory wastewater 2101-M Laboratory wastewater 2724-W Laundry wastewater 284-E Powerplant wastewater 284-W Powerplant wastewater 300 Area process wastewater 400 Area secondary c o o l i n g water

Tota l Inorganics , - M

Mean F i e l d pH

7.8 6.1 6.3 6.2 6.6 9.3 6.1 6.7 7.4 8.2 6.3 6.8 6.4 6.6 6.8 6.3 5.8 6.6 6.4 5.2

10.4 6.1 6.2 5.7 6.8 7.3 6.3 6.2 9.1 8.3 8.2 6.0 8.0

TABLE 4. Discharge Rate of Principal Inorganic Analytes (Jungf 1 ei sch 1988)

Inorganic Analyte

Aluminum sulfate Ammoni um nitrate Ammoni um bicarbonate Ammonium hydroxide Barium sulfate Beryllium sulfate Cadmium sulfate Calcium nitrate Calcium bicarbonate Calcium sulfate Sodium chromate Copper sulfate Ferrous sulfate Lead sulfate Magnesium nitrate Magnesium bicarbonate Manganese sulfate Mercury sulfate Nickel sulfate Potassium sulfate Si 1 ver sulfate Sodium bicarbonate Strontium chloride Uranyl nitrate Vanadyl sulfate Zinc sulfate Sodium chloride Sodi um cyanide Sodi um f 1 uori de Sodi um nitrate Sodium phosphate monobasic Sodium phosphate dibasic Sodium bisulfide Sodium sulfate

Discharge Rate, kg/mo

10,866 281.2

5,896.8 4.128

140.6 95.26

0.313 185,976

15,422 19,051

1.225 331.13

2,948.4 21.773

TABLE 5. A n a l y t i c a l Frequency (N) f o r t he Organic Analytes (West i nghouse Hanford 1989)

Organic Analyte N

Ch 1 o r o f orm 153 Acetone 9 7 Bu ty l a1 coho1 44 T r i b u t y l phosphate 3 9 Methyl e t h y l ketone 3 5 T r i decane 3 1 2-butoxyethanol 30 Tetradecane 3 0 Tetrahydrofuran 2 6 Butoxyglycol 2 1 Methyl -n -bu ty l ketone 19 Bu ty ra l dehyde 17 B is (2 -e thy l hexy l ) ph tha la te 16 Benzyl a1 coho1 13 2-propanol 12 MIBK (hexone) 11 Dodecane 9 Methylene c h l o r i d e 9 Methyl n-propyl ketone 8 Buty l n i t r a t e 7 Methyl n i t r a t e 6 Pentadecane 6 Phenol 6 N-methoxymethanami ne 5 E t h o x y t r i e t h y l ene g l y c o l 4 Benzoic a c i d 3

Organic Analyte

3 ,5-d imethy lpyr id ine Ethy l a1 cohol Heptadecane Hexadecane Hexadecanoic a c i d Methyl formate Acetophenone Benzal dehyde Butoxyd ig lyco l Buty l benzyl ph tha l a t e Decane D i -n-buty l ph tha l a t e Dichlorof luoromethane Dimethoxymethane Dimethylni trosoarnine D i -n -oc ty l ph tha l a t e Methoxydiglycol Me thoxy t r i g l yco l 2-methylnonane 2-methyl-5-propylnonane Morphol i ne Pe larg ic a c i d Phenanthrene Tetrachloroethy lene Undecane

are of concern because they are carcinogens (Ecology 1987). Table 6 1 ists those compounds designated as acutely and moderately toxic by Ecology that were identified in the 33 active waste streams.

The waste streams containing the highest concentrations of organic analytes are listed in Table 7. The PUREX Process Condensate stream contains the highest concentration of organics.

Discharge rates for several organic constituents within the 33 waste streams are shown in Table 8. Tributyl phosphate and aliphatic hydrocarbons were present in the largest quantities, and tetrachloroethylene and chloroform were also high in ranking.

In addition to the organic analyte content of the 33 waste streams that is listed in Table 5, there is a considerable volume of data on organic compounds found in groundwaters taken from wells associated with the waste stream disposal sites. For example, Table 9 gives the analytical data on three 200 West Area wellwater samples. A large amount of wellwater sample analytical data were reported by Westinghouse Hanford (1989) as being associated with the ground disposal of the 33 waste streams. These data show

that little degradation or sediment sorption is occurring for many of the

organic constituents of the waste. Many of the organics in effluent streams were used to extract uranium and plutonium from spent fuel. The origins,

uses, and degradation sequences of the uranium and plutonium extractants, the

solvents, and their degradation products are discussed in detail by Burr (1958), Lane (1960, 1963), Dennis and West (1961), Blake et al. (1963), Huggard and Warner (1963), Gaumann et al. (1972), and Nowak (1971).

Several characteristics of the organic compounds found in the waste streams relating to migration are given in detail, with references, in Appendix A.

TABLE 6. C l a s s i f i c a t i o n s o f Some Hazardous Chemicals Found i n t h e 33 Waste Streams (Ecology 1987; Jungf l e i s c h 1988)

Pe rs i s ten t Substance

Chl oroform Methylene c h l o r i d e Pentachlorophenol

P o s i t i v e Carcinogen

Bery l 1 i um su l f a t e Cadmi um s u l f a t e Lead s u l f a t e B is (2-e thy l hexyl ) ph tha l a t e Chloroform

I g n i t a b l e Substance

Sodium b i s u l f i d e Acetone Benzyl a1 cohol 2-butoxyethanol Buty l a lcohol Dodecane Isopropy l a1 cohol (2-propanol ) Phenol Py r id ine Tetradecane Tetrahydrofuran

React ive Substance

Sodium cyanide Sodium b i s u l f i d e

Toxic Contaminant

Ba r i urn Cadmi urn Chromi um Lead Mercury S i l v e r

TABLE 7. Waste Streams Conta in ing t h e Largest Contents o f Organic Analy tes (Westi nghouse Hanford 1989)

To ta l Organic Waste Stream Contents, ppb

PUREX P l a n t process condensate

242-A Evaporator process condensate

2724-W Laundry wastewater

U03 P l an t process condensate

2101-M Labora to ry wastewater

U03/U P lan t s wastewater

B P l a n t process condensate

Pluton ium F i n i s h i n g P l a n t wastewater

B P l a n t chemical sewer

241-AY, 241-AZ Tank Farms steam condensate

2.1.3 Radionuc l ides

The r a d i o a c t i v i t y w i t h i n t h e 33 waste streams i s wide-ranging, as seen

i n Table 10. The rad ionuc l i d e occurrence frequency (N) i s shown f o r t h e

samples c o l l ec ted . The f i s s i o n and a c t i v a t i o n p roduc ts 9 0 ~ r , 1 3 7 ~ s , and 2 3 9 ~ u

a r e t h e most p r e v a l e n t , as migh t be expected. Most o f t h e r a d i o a c t i v i t y i s

concen t ra ted i n f o u r waste streams, as shown i n Table 11. Although t h e N

Reactor e f f l u e n t (105-N c o o l i n g water and f u e l bas in wate r ) con ta ined more

than h a l f o f t h e t o t a l r a d i o a c t i v i t y i n t h e 33 waste streams, t h i s waste

stream no l onge r e x i s t s i n t h e same volume because t h e N Reactor i s n o t i n

ope ra t i on , b u t r a t h e r i n a co ld-s tandby s t a t u s ( M i l 1 i k i n 1989).

2.2 WASTE STREAM VOLUME ESTIMATES

A b e s t es t ima te o f t h e volumes o f t h e 33 waste streams i s g iven i n

Table 12. The d isposa l s i t e s f o r 163-N deminera l i zed wastewater, t h e PUREX

steam condensate, and t h e T P l a n t headend wastewater a re l i s t e d by

Westinghouse Hanford (1989) as be ing c u r r e n t l y i n a c t i v e . Therefore, t h e

va lues i n Table 12 f o r these streams a re no l onge r v a l i d .

TABLE 8. D a i l y Discharge o f Organic Analytes Based on Analyses and E f f l u e n t Volumes o f t h e 33 Waste Streams (Westinghouse Hanford 1989)

Dai l y Discharge Organic Analy te Amount, g

T r i b u t y l phosphate 13,977.750

T r i decane 8,676.711

Tetradecane 7,683.627

Dodecane 2,794.086

Pentadecane

Tet rach lo roe thy lene

Chloroform 273.045

B i s (2 -e thy l hexy l ) ph tha l a t e 159.174

Undecane

2-butoxyethanol

Bu ty l a1 cohol

Acetone

Hexadecane

Methyl n i t r i t e

Dimethoxymethane

Heptadecane

Octadecane

Decane

Methyl formate

Phenol

N-methoxymethanamine

D i -n -bu ty l ph tha l a t e

Benzyl a1 cohol

Methylene c h l o r i d e

D i -n -oc ty l ph tha l a t e

Benzoic a c i d

Methyl e t h y l ketone 11.126

Bu ty l benzyl ph tha l a t e 9.895

2-methyl-5-propylnonane 9.615

Pel a r g i c a c i d 4.688

TABLE 9. Organic Analytes Reported in Three 200 West Area We1 lwater Samples

Concentration, ppb We1 1 We1 1 We1 1

Organic Analyte

Vol at i 1 e Compounds

Carbon tetrachloride Chloroform Dichloromethane

Trichloroethylene

Cyclohexane Methyl cycl ohexane

To1 uene 2-butoxyethanol 2-ethyl-1-hexanol

Solvent Extractable Compounds

Tri -n-butylphosphate (TBP) 3

Di-n-octyladipate - - Bis (2-ethyl hexyl) phthalate 2

Di-n-octylphthalate - - Phthal ates, mixed - -

Chelating Agents

Ethy lened iam ine te t raace t i c

acid (EDTA) ~ 0 . 1

TABLE 10. Frequency (N) o f Radionucl i des i n t h e 33 Waste Streams (Westinghouse Hanford 1989)

Radionucl i d e N

Gross p 1 3 7 ~ s

2 3 9 ~ ~

9 0 ~ r

H

Gross a

60co

5 4 ~ n

144ce

To ta l U

9 5 ~ b

O3 RU

238pu

5 9 ~ e

9 5 ~ r

1 4 O ~ a

141ce 1311

134cs

241pu

3 2 ~

5 8 ~ o

9 9 ~ o

8 9 ~ r

1 4 0 ~ a

l o 6 ~ u

147pm

5 1 ~ r

241~m 132

TABLE 11. Waste Streams w i t h t h e Bu lk o f t h e T o t a l R a d i o a c t i v i t y i n t h e 33 Waste Streams

T o t a l A c t i v i t y , P e r c e n t o f Waste Stream C i / y r T o t a l A c t i v i t y

N Reactor e f f l u e n t (1976 - 1988) 2,400 54.00

PUREX P l a n t process condensate 1,500 35.00

242-A Evaporator c o o l i n g wate r 280 6.30

242-A Evaporator process condensate 150 3.50

T o t a l 4,330 98.80

TABLE 12. Waste Stream Volume Estimates (from Stordeur and Flyckt 1988)

Eff luent Stream

PUREX P lant cool ing water 242-A Evaporator cool ing water B Plant cool ing water 300 Area process wastewater 241-A Tank Farm cooling water PUREX P lant chemic 1 sewer N Reactor e f f 1 uentfc) 163-N Demineral i z e r wastewater(^) PUREX P lant steam condensate B Plant chemical sewer U03/U P lan t s wastewater Plutonium Fin ish ing Plant wastewater S Plant wastewater 284-E Powerhouse cool ing water 244-AR Vault cool ing water 284-W Powerhouse cooling water T P lant wastewater 2724-W Laundry wastewater PUREX P lant process condensate 400 Area secondary cool ing water 242-A Evaporator steam condensate 222-S Laboratory wastewater PUREX P lant ammonia scrubber condensate 242-A Evaporator process condensate 242-S Evaporator steam condensate B P lant steam condensate B Plant process condensate 2101-M Laboratory wastewater UO P lant process condensate A Y ~ A Z Tank Farm steam condensate 209-E Laboratory r e f l e c t o r water T Plant 1 abora tory ( o r headend) wastewater 183-D F i l t e r backflush wastewater

V O I ume, (a ) mi l l i ons of

L/yr

7,800 .OO 5,300.00 2,800.00 1 , 9 0 0 . 0 0 ( ~ )

880.00 840.00 760.00 600.00 590.00 350 .OO 340.00 200.00 200.00 180 . o o ( ~ ) 120 .oo 110.00(b) 7 2 . 0 0 ( ~ ) 61 .OO 51 .OO 4 9 . 0 0 ( ~ ) 45.00 34.00 28.00 25 .OO 14.00

Percent of

Total Flow

33.39 22.69 11.99 8.13 3.73 3.60 3.25 2.57 2.53 1.50 1.46 0.86 0.86 0.77 0.51 0.47 0.31 0.27 0.22 0.21 0.20 0.15 0.12 0.11 0.06 0.02 0.02 0.02 0.00 0.00

Total

(a ) 1987 flow da ta (except as noted) . (b) Estimated. (c ) These have decreased a s a r e s u l t of t h e placement of N Reactor

i n t o cold-standby s t a t u s . (d) 1986 flow d a t a used. (e ) 1985 flow da ta used. ( f ) NA = Not a v a i l a b l e , minor con t r ibu t ion t o t o t a l .

3.0 CHARACTERISTICS OF HANFORD SEDIMENTS

Cation exchange capacity (CEC) i s one of the more important soi 1

character is t ics associated with determining the f a t e of constituents when

liquid waste i s disposed into sediments. The C E C values for Hanford Si te

sediments were given by McHenry (1957), Routson e t a l . (1981), and Delegard

and Barney (1983) for the 200 Areas (process areas) and vicinity and by Bensen

e t a1 . (1963) for the 100 Areas (reactors) . These CEC values are not

necessarily comparable because the resul ts are a function of how the CEC i s

measured, including the cation used t o saturate the exchange s i t e s and the one

used t o replace the adsorbed cation. More recent CEC par t ic le s ize and carbon

data for 200 Area (separations areas) and 100 Area (reactors) sediments are

given in Table 13. The typical 200 Area sediment i s high in sand content,

with an average C E C of 4.3 meq/100 g and an average organic carbon (OC)

content of s l ight ly less than 0.10 w t % . The 100 Area sediments also have very

low values for OC content. Total carbon, in the case of the 100 Area

sediments, was determined by microcombustion and infrared analysis. Particle

s ize analysis for the 200 Area so i l s was conducted using the technique of Gee

and Bauder (1986), and total carbon was determined by dry combustion with the

coulometric method of Huffman (1977). Inorganic carbon was determined by the

same coulometric method a f t e r the samples had been digested for 10 min in 3 - N

HC1 a t 8 0 ' ~ t o release a l l inorganic carbon. Both the total and the inorganic

carbon procedures were cal i brated with reagent-grade CaC03. Organic carbon

was obtained as the difference, i f any, between the total carbon and the

inorganic carbon.

The organic carbon content of the soil/sediment i s important because

neutral hydrophobic organic compounds (compounds having a water sol ubi 1 i ty of

less than a few parts per mil 1 ion) have been shown to adsorb preferentially

onto the organic carbon fraction of the soil (Lambert e t a1 . 1965; Briggs

1973). Lambert e t a l . suggested that the role of organic matter in the

sediment was similar t o that of an organic solvent in solvent extraction and

that the parti t ioning of a neutral organic compound between sediment organic

matter and water should correlate well with i t s parti t ioning between water and

an immiscible solvent. Briggs (1973) developed a regression equation re1 ating

TABLE 13. Recent Sediment Data That Include Organic Carbon Values

Well Number Depth, ft

Cation Exchange Capacity, meq/100 g

5.1 4.2 4.4 1.6 2.6 3.6 2.5 4.7 2.0 4.2 2.2 3.5 2.4 2.9 2.9 6.0 2.3 2.2 3.6 3.2 6.9 2.9 4.1 1.5 1.8 3.2 6.2 6.2 9.0 5.3 8.5 4.0 6.1 4.9 5.3 5.9 3.3 5.3 8.1 6.2

Wt%

TC(~) I C ( ~ ) OC(C) Sand ---- 0.10 0.04 0.06 61.59 0.39 0.18 0.21 93.82 0.16 0.16 0.00 90.63 0.04 0.04 0.00 85.66 0.02 0.01 0.01 91.17 0.13 0.11 0.02 70.37 0.15 0.10 0.05 -- 0.22 0.11 0.11 63.63 0.14 0.18 0.00 88.36 0.09 0.03 0.06 66.45 0.11 0.07 0.04 74.68 0.26 0.14 0.12 93.79 0.78 0.13 0.65 93.46 0.13 0.08 0.05 68.87 0.03 0.04 0.00 74.29 0.48 0.73 0.00 -- 0.13 0.13 0.00 88.28 0.04 0.01 0.03 -- 0.15 0.15 0.00 78.92 0.02 0.01 0.01 87.24 0.32 0.20 0.12 -- 0.27 0.19 0.08 -- 0.28 0.26 0.02 -- 0.42 0.04 0.38 -- 0.07 0.04 0.03 -- 0.03 0.01 0.02 73.67 0.01 0.00 0.01 78.38 0.05 0.03 0.02 -- 0.24 0.14 0.10 -- 0.17 0.17 0.00 74.30 2.75 2.58 0.18 -- 0.02 0.10 0.01 -- 1.07 0.16 0.91 -- 0.13 0.10 0.03 -- 0.17 0.18 0.00 -- 0.67 0.16 0.51 -- 0.25 0.28 0.00 -- 0.48 0.44 0.04 -- 0.02 0.00 0.02 -- 0.09 0.05 0.04 73.43

Silt

(a) TC = total carbon, TC = IC + OC. (b) IC = inorganic carbon. (c) OC = organic carbon.

soillsediment sorption of phenyl urea herbicides to their octanol-water

parti tion coefficient, KO/,. Karickhoff et a1 . (1979) then used this concept to determine sorption isotherms for 10 hydrophobic organic compounds on

natural sediments.

The adsorption data for all of the organic compounds fit well, over a

broad range of water phase concentrations, to linear isotherms where X = KpC.

The variable X is the concentration of sorbate (ppb) on the sediment re1 ative

to the sediment's dry weight, C is the equilibrium solution sorbate concentration (ppb) , and Kp is the parti tion coefficient (uni tless) . When

adsorption depends on only organic carbon, KO, = Kp/foc. The foc is the fractional mass of organic carbon in the sediment, and KO, is a normalized

parti tion coefficient. When the log KO/, (octanol -water parti tion coefficient) is plotted versus the log KO, or log S (water solubility

expressed as a mole fraction), relationships such as log KO, = 1.00 log KO/,

- 0.21 and log Koc = -0.54 log S + 0.44 were obtained. The covariation of KO, and KO/, were linear, but KO, varies nonlinearly with S.

These relationships would be very useful as they make it possible for the

hydrophobic organic compound distribution coefficients to be easi ly computed

from available data, except for one circumstance. As can be seen from

Table 12, Hanford sediments are relatively low in organic carbon content,

averaging slightly less than 0.1 wt%. Hanford sediments often contain no

organic carbon at a1 1. According to Means et a1 . (1982), the re1 iabi 1 i ty of predictive equations is impaired for substrates with very low carbon contents,

such as the Hanford sediments. Means et al. found that correlations between

KO, and Kp were erratic for sediments that contain less than 1.0 wt% organic carbon content, as do Hanford sediments. Hence, application of generic

hydrophobic organics-water-sediment relationships to Hanford sediments cannot

be justified, except as a means of roughly estimating Hanford sediment

reactions with organic analytes.

Hydrophi 1 i c compounds, by definition, prefer an aqueous environment and minimal sediment sorption can be expected. Some organic compounds can

dissociate, such as the benzoic or hexadecanoic acids reported in Table 5.

These ionized compounds are theoretically able to adsorb on the sediment as an

exchangeable cation or anion under the appropriate conditions. However,

benzoic acid is not known to sorb on sediments (see Appendix A) and little is

known about the sorption properties of the other dissociating compounds shown

in Table 5.

4.0 SEDIMENT INTERACTIONS

Transport of solutes (including contaminants) in the subsurface is controlled by advection, hydrodynamic dispersion, molecular diffusion, and geochemical interaction. Advection and hydrodynamic dispersion refer to movement of solute at a rate dependent on the various water pathways and velocities. Molecular diffusion refers to the gradual mixing of molecules of two or more substances as a result of random motion and/or a chemical concentration gradient. Diffusion flux spreads solute via the concentration gradient (i .e., according to Fick's law). Diffusion is a dominant transport mechanism when advection is insignificant but is usually negligible when water

is being advected in response to various forces. Variability in the advection process gives rise to hydrodynamic dispersion. Hydrodynamic dispersion is a result of variability in travel paths, that is, velocities, taken by the advected sol ute. Geochemical interactions cover a1 1 reactions that are driven by chemical and biochemical forces.

Once the liquid wastes contact the vadose zone sediments, they can chemically interact with the soils and sediments. The major geochemical processes affecting transport include dissolution/precipitation, adsorption/desorption, filtration of colloids and small suspended particles,

diffusion into micropores within mineral grains, and vol ati 1 ization and eventual escape to the atmosphere. Di ssol utionlprecipi tation and

adsorption/desorption are considered the most important for the inorganic

wastes present in the 33 active waste streams at the Hanford Site. However,

when assessing the organics in the waste streams, volatilization should also be considered. Furthermore, for the disposal of low-level radioactive waste

(LLW) at the Hanford Site, precipitation is likely to be significant only for cases where pH and/or redox changes occur when waste streams contact the sediments. In most active liquid discharge situations at the Hanford Site, we

speculate that adsorption processes are the key to inorganic contaminant migration. The knowledge base for the environmental fate of organics

identified in the wastes is meager, and we cannot offer an opinion on what specific process dominates their fate.

Adsorption reactions have been acknowledged to be the most important

contaminant retardat ion process in far-f i el d transport analyses conducted for hazardous waste-disposal options. Adsorption processes are known to increase the travel times for some contaminants by lo3 to lo6 times relative to the

groundwater. Such long travel times allow nuclides to decay to lower

concentrations and less hazardous nucl ides before they reach the accessible environment (i .e., the biosphere). Furthermore, some adsorption processes are

effectively irreversible and permanently prevent contaminants from reaching

the groundwater, thus preventing their release to the biosphere.

4.1 CONSTANT DISTRIBUTION COEFFICIENT

To predict the effects of retardation using mathematical codes, adsorption processes must be described in quantitative terms. An empirical parameter, the distribution coefficient (often called Rd or Kd), is readily measured by laboratory experimentation and a1 lows such a quantitative estimate of migration and retardation. Knowledge of the Rd and of either media bulk density and porosity (for porous flow) or media fracture surface area, aperture width, and matrix diffusion attributes (for fracture flow) a1 lows calculation of the retardation factor, R or Rf. The retardation factor is defined as R = -%- , where Vw is the velocity of water through a control volume and Vn is the velocity of the contaminant.

For one-dimensional advection-dispersion flow with chemical reaction, the transport equation can be written as

where Ci = concentration of a particular radioactive species i in solution

(mass11 ength3)

Dx = dispersion coefficient of species i (length2/time)

V, = pore velocity of groundwater (1 engthltime) Ri = retardation factor for species i.

(For simplicity, radioactive decay has been left out.)

The retardation factor is a function of all of the contaminant retardation mechanisms: 1) chemical precipitation/dissolution of bulk sol id phases, 2) chemical substitution of one element for another in a solid phase, 3) exchange of a stable isotope of an element with a radioactive isotope in solution, 4) physical filtration of colloids, 5) cation and anion exchange, and 6) adsorption (Muller et a1 . 1983), plus for organic compounds, 7) microbial and other degradation. Typical ly, a1 1 these mechanisms are melded into a single empirical distribution coefficient that implicitly assumes that the reactions go to equilibrium and are reversible and that the chemical environment along a solute flow path does not vary over either space or time. The limitations associated with these assumptions are well known to investigators, but the current paucity of Hanford Site-specific geochemical data precludes a more rigorous conceptual model at this time. Even though

geochemical processes may be irreversible or at least directionally dependent

(e.g . , adsorption and de-sorption may be represented by different model parameters), the assumption of reversibi 1 i ty and use of single-val ued model parameters are standard with the justification that the approach builds conservatism into the analysis.

In the constant Rd model, the distribution of the contaminant of interest between the solid adsorbent and solution is assumed to be a constant value. There is no explicit accommodation of dependence on characteristics of the sediments, groundwater, or contaminant concentration. Typically, an Rd value for a given contaminant is determined in the laboratory using sediment from the study area and actual or simulated groundwater to which a radionuclide tracer is added. Then

amount of radionuclide adsorbed on solid per gram Rd =

amount of radionuclide in solution per milliliter ( 2

The mass or activity of the tracer must be sufficient to facilitate good

counting statistics. The solids and liquids are often equilibrated by

contacting the solid with several aliquots of the liquid before adding the

radiotracer, to attempt to approach the condition expected in the field.

Several standardized laboratory techniques are commonly used to determine this

ratio (Serne and Relyea 1983; ASTM 1984).

Most of the laboratory experiments performed to measure distribution

coefficients do not systematical ly investigate the effect of various important

parameters and do not attempt to identify the processes causing the adsorption

that is observed. Because it is an empirical measurement, the Rd value does

not necessarily denote an equilibrium value or require some of the other

assumptions inherent in the use of the more rigorous term Kd. The term Rd

will be used to refer to the observed distribution ratio for the nuclide

between the solid and solution. The term Kd will be reserved for true

equilibrium reactions that show reversibility and that do not yield a

distribution ratio that is dependent on the tracer concentration in solution.

It is customary with the constant Rd model to measure the total

concentration or radioactivity of the tracer and thus to treat the tracer as

being one species. This assumption is not an inherent requirement, but it is

generally applied for convenience. If the tracer is known to distribute among

several species and the distribution can be measured or predicted, separate Rd

values can and should be calculated for each species.

This conceptual model , which depends on experimental determination of the distribution coefficient Rd, is quite simple, but it is also limited in that

it does not address sensitivity to changing conditions. If the groundwater

properties (e.g., pH, dissolved solids content) change, a new value for Rd must be obtained.

The constant Rd model is mathematically very simple and readily

incorporated into transport models and codes via the retardation factor term.

That is, for porous flow

where R = the retardation factor pb = porous media bulk density (mass/length3) + E = effective porosity at saturation of media Rd = distribution coefficient

P = particle density (mass/length3).

For the constant Rd model, the retardation factor (R) is a constant for each layer of geologic media (each layer is assumed to have a constant bulk density and saturated effective porosity) . Therefore, this transport equation does not require knowledge of any other parameters, such as pH or surface area, and it is easily solved to determine the solution concentration as a function of time and for any given point. However, the use of the constant Rd conceptualization in the retardation factor has caused criticism because few natural groundwater pathways are spatially or geochemically homogeneous enough for the retardation factor of a species to remain constant.

4.2 INTRODUCTION TO ESTIMATING ADSORPTION CONSTANTS

The purpose of this subsection is to document any available Hanford Site-

specific data that provide actual Rd values for identified contaminants. Because the database is small and the constant Rd adsorption model is simp1 istic, we do not discuss the adsorption potential of each contaminant from each waste stream separately.

As mentioned above, the adsorption tendencies of contaminants are influenced by characteristics of the waste stream, sediments, and contaminants. Vadose zone sediments at the Hanford Site do not show large ranges for such characteristics as organic carbon content, CEC, soil paste pH, and so on. Thus we do not gain much understanding of contaminant adsorption by attempting detai led differentiation (i .e., categorization) of Hanford sediments. On the other hand, the effects of solution characteristics (e.g.,

pH, Eh, dissolved sol ids, dissolved organic content) on inorganic contaminant adsorption are better understood and the ranges of solution characteristics of

Hanford waste streams can be quite large. Therefore, all available waste

stream data have been categorized into generic types based on five independent parameters (Figure 1) .

FIGURE 1. Classification of Waste Streams Based on Five Key Parameters o f Acidity, Radioactivity, Organic Content, Dissolved Sol ids Content, and Waste Stream Volume. The definitions for the parameters are given in parentheses under each heading. The waste stream identifications (~.1, etc.) are listed in Table 14.

7- z? L 0. -

* - > x + CT CI

" U - .- U r n

x 0 0 -I+

? ul V I a - > I- - E U =I

I

2 I

LOW VOLUME

HIGH DISSOLVED

> I-- -

5: 2

= I- z z I+-

0 u

7

rC1 PC,

L Z z w 0-'4- A + 0

U

U S v V

A - rC1 C,

> 0 I -*

I- w > ' t z p O U .\o U d

A V

(>2.0% of total)

LOW DISSOLVED SOLIDS

HIGH ORGANICS

A.21

A.17

HIGH VOLUME (>2.0%

HIGH DISSOLYED SOLIDS

HIGH ORGANICS

A.29

A.5

LOW ORGANICS

A.2

of total)

LOW DISSOLV D 5 SOLIDS

HIGH ORGANICS

(>2,000 ppb;

A. 6

LOW ORGANICS

A.3, A.4, A.7 A.8, A.lO,A.ll A.12, A.13, A.15, A.18, A.26, A.27, A.28, A.33

A. 1

A.20

SOLIDS

HIGH ORGANICS

(>lo- M)

LOW ORGANICS

(<2,000 ppb)

A.9, A.30, A.31

(40- M)

LOW ORGANICS

A.14, A.16, A.19, A.22, A.25, A.32

A.23

A. 24

TABLE 14. Waste Stream I d e n t i f i c a t i o n

Des igna t ion

A. 1 A. 2 A.3 A.4 A.5 A.6 A.7 A.8 A. 9 A. 10 A . l l A. 12 A. 13 A. 14 A. 15 A. 16 A. 17 A. 18 A. 19 A.20 A.21 A.22 A.23 A. 24 A. 25 A.26 A. 27 A. 28 A.29 A. 30 A. 3 1 A.32 A.33

Waste Stream

N Reactor e f f l u e n t 163-N Deminera l i ze r wastewater 183-D F i l t e r back f l ush wastewater PUREX P l a n t chemical sewer PUREX P l a n t process condensate PUREX P l a n t ammonia scrubber condensate PUREX P l a n t steam condensate PUREX P l a n t c o o l i n g wa te r B P l a n t chemical sewer B P l a n t process condensate B P l a n t steam condensate B P l a n t c o o l i n g wa te r P lu ton ium F i n i s h i n g P l a n t wastewater S P l a n t wastewater T P l a n t headend wastewater T P l a n t wastewater U03 P l a n t process condensate UO /U P l a n t s wastewater 24?-A Tank Farm coo l i ng wate r 241-AY, 241-AZ Tank Farms steam condensate 242-A Evaporator process condensate 242-A Evaporator steam condensate 242-A Evaporator c o o l i n g wa te r 242-S Evaporator steam condensate 244-AR V a u l t c o o l i n g wa te r 209-E Labora to ry r e f l e c t o r wa te r 222-S Labora to ry wastewater 2101-M Labora to ry wastewater 2724-W Laundry wastewater 284-E Powerplant wastewater 284-W Powerplant wastewater 300 Area process wastewater 400 Area secondary c o o l i n g wa te r

A volume quanti ty of more than 2% of t he t o t a l waste stream flow was a r b i t r a r i l y chosen as t he high-volume category. This choice put nine of the 33 waste streams i n to t he high-volume category. These nine streams contained

92% of the t o t a l waste stream volumes (Table 12). I t should be kept in mind, however, t h a t these volume data a re from 1988 and may not be accurate f o r

present waste stream flows.

The dissolved sol ids content of low2 - M was chosen t o define t he high

category because natural groundwater a t Hanford contains dissolved so l i d s

ranging from 1 X low3 t o 7 X - M. Migration of many cat ions through

sediments in pore waters would tend t o be accelerated by contact with high-

ionic-strength solut ions . Hence, streams showing dissolved so l i d s contents

higher than - M would tend t o accelera te ion migration.

The pH parameter was used t o define a neutral- to-basic category (pH >6.0)

and an ac id ic (pH <6.0) category, with ac id i ty being known t o adversely a f fec t

the sorption of many cat ionic radionucl ides (McHenry 1954, 1957, 1958) , such

as 9 0 ~ r and 1 3 7 ~ s , as well as the transuranics. Therefore, ac id ic streams, of

which there a re only th ree , would be higher-priori ty candidates f o r treatment

o r cessation than the 30 neutral -to-a1 kal ine streams.

Four of the waste streams included 98.8% of the rad ioac t iv i ty being

subjected t o ground disposal . One of the four high-activity streams, N

Reactor e f f luen t (A. I ) , i s no longer produced. The high-activi t y category

was defined t o include any streams having more than 1% of the t o t a l waste

stream rad ioac t iv i ty . I t i s assumed tha t the higher radionuclide

concentrations tend t o enhance radionuclide migration.

The organic contents of the waste streams a re generally low, ranging from

about 100 t o 241,000 ppb. There are only four streams with organic contents

above 2,000 ppb (Table 7 ) , and only 10 of the 33 streams have measurable

organic contents a t a l l . Therefore, the dividing l i ne between categories was

placed a t an organic content of 2,000 ppb. Waste streams having organic

contents above 2,000 ppb are considered t o be high in organics, although the

presence of these organics may or may not be detrimental t o radionuclide

sorption on sediments. Very l i t t l e work has been done t o date on t he e f f e c t s

of organics on radionuclide sorption on Hanford s o i l s .

Table 14 lists the 33 waste streams and their designations (A.l to A.33). Figure 1 shows each waste stream as a member of one of the 32 categories based

on the data obtained from Westinghouse Hanford (1989). In general, migration potential and resultant hazard from a waste stream increase with increasing

volume, dissolved solids, organics, radionuclide activity, and acidity.

Conversely, waste streams with low values for volume, dissolved solids,

activity, and organics and a high value for pH are not likely to promote

migration of contaminants.

Most of the active waste streams identified in Table 14 are in the

categories that do not promote migration. Waste streams A.3, A.4, A.7, A.8,

A.10 to A.13, A.15, A.18, A.26 to A.28, and A.33 have low values for all five

parameters (note that low acidity = high pH). Waste streams A.14, A.16, A.19,

A.22, A.25, and A.32 are low in all parameters but discharge volume. These

"low-value" waste streams represent chemical sewerage, steam and process

condensates, cooling waters, and miscellaneous laboratory wastewaters.

Three waste streams have three high values and two low values for the

five parameters. These three streams may warrant closer scrutiny than all of

the others because of their higher potential for contaminant migration. The

three waste streams are the PUREX ammonia scrubber condensate, which has high

volume, high dissolved solids content, and high organic content; U03 Plant

process condensate, which has high dissolved solids, high organics, and acid

pH; and 242-A evaporator steam condensate, which has high dissolved solids, high organics, and high radionuclide content.

4.3 DISTRIBUTION COEFFICIENTS FOR INORGANICS AND RADIONUCLIDES

Figures 2 through 16 provide estimates of distribution coefficient (Rd)

values for selected inorganic and radionuclide constitutents found in the

33 active waste streams. Rd values are presented for each of eight waste

types based on the waste streams' pH, total dissolved sol ids content, and

organic content (see Figure 1 to determine which waste streams belong in each

category).

The Rd figures provide estimates for each waste stream category for a

typical Hanford sediment. To obtain accurate Rd values requires testing of

FIGURE 2. Rd Est imates (mL/g) f o r Bery l 1 ium, Calcium, and Magnesium. The numbers i n parentheses a r e conse rva t i ve Rd ranges above them. See F igu re 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

ACID

H I G H DISSOLVED SOLIDS LOW DISSOLVED SOLIDS

H I G H ORGANICS

3-15 (5

0.1-5 (1.5)

H I G H ORGANICS

15-70 (15)

3-15 (7.5)

LOW ORGANICS

7-70 (7.5)

0.5-15 (3.5)

LOW ORGANICS

15-200 (20)

7-15 (10)

FIGURE 3. Rd Estimates (mL/g) f o r S t ron t ium and Barium. The numbers i n parentheses are conserva t ive Rd averages est imated f rom t h e Rd ranges above them. See F igure 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

A C I D

H I G H DISSOLVED SOLIDS LOW DISSOLVED SOLIDS

H I G H ORGANICS

5-20 (7)

Rhodes (1956) Routson e t . a1 (1981)

0.1-5 (2)

Knol l (1969)

H I G H ORGANICS

20-100 (20

5-15 (10)

LOW ORGANICS

10-100 (10)

Routson e t . a1 (1981)

0.5-20 (5

Hawkins and Shor t (1965)

LOW ORGANICS

20-200 (25)

Rhodes (1956) McHenry (1958)

Routson e t . a1 (1981)

50-20 (5

Rhodes (1957a)

FIGURE 4. Rd Est imates (mL/g) f o r L i t h i um, Potassium, Sodium, and Ammonium. The numbers i n parentheses a r e conse rva t i ve Rd ranges above them. See F igu re 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

ACID

H I G H DISSOLVED SOLIDS

H I G H ORGANICS

0-30 (1)

0-10 (0 )

LOW DISSOLVED SOLIDS

LOW ORGANICS

0-30 (2)

0-10 (0)

H I G H ORGANICS

1-30 (2)

0-10 (0)

LOW ORGANICS

1-30 (4 )

Buel t e t a1 . (1988)

0-10 (1

FIGURE 5. Rd Estimates (mL/g) f o r Cobalt , I r o n , and Manganese. The numbers i n parentheses are conservat ive Rd ranges above them. See F igure 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

A C I D

H I G H DISSOLVED SOLIDS

H I G H ORGANICS

0.1-10 (3

Haney (1967) Barney (1978)

0

Haney (1957) Rhodes and Nelson

(1957)

LOW DISSOLVED SOLIDS

LOW ORGANICS

5-20 (10)

Routson e t a1 . (1981)

0.2-20 (5)

H I G H ORGANICS

0.1-10 (3

W i ld ing and Rhodes (1963)

0

LOW ORGANICS

10-3000 (50)

Routson e t a1 . (1981)

0.2-20 (5)

FIGURE 6. Rd Est imates (mL/g) f o r Lead, Z inc, Cadmium, Copper, N i c k e l , S i l v e r , and Mercury. The numbers i n parentheses a re conse rva t i ve Rd ranges above them. See F i g u r e 1 f o r parameter d e f i n i t i o n s .

-

NEUTRAL TO BASIC

ACID

H I G H DISSOLVED SOLIDS

H I G H ORGANICS

0-100 (10)

0-10 (2)

LOW DISSOLVED SOLIDS

LOW ORGANICS

0-200 (30)

5-50 (6)

H I G H ORGANICS

0-200 (10)

0-40 (2)

LOW ORGANICS

100-200 (30)

10-100 (10)

FIGURE 7. Rd Estimates (mL/g) f o r Antimony, Molybdenum, and S u l f i d e . The numbers i n parentheses are conservat ive Rd ranges above them. See F igure 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

A C I D

H I G H DISSOLVED SOLIDS

H I G H ORGANICS

0-2 (0)

0-5 (0)

LOW DISSOLVED SOLIDS

LOW ORGANICS

0-5 (0)

Haney (1967) Ames and Rai (1978)

2-20 (2)

H I G H ORGANICS

0-2 (0)

0-5 (0)

LOW ORGANICS

0-40 (0)

2-40 (2)

FIGURE 8. Rd Est imates (mL/g) f o r Zirconium, Niobium, and Tin. The numbers i n parentheses are conserva t ive Rd ranges above them. See Figure 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

ACID

H I G H DISSOLVED SOLIDS LOW DISSOLVED SOLIDS

H I G H ORGANICS

0-30 (10)

Prout (1959)

0-10 (5)

Prout (1959)

H I G H ORGANICS

2-20 (10)

2-20 (5

LOW ORGANICS

20-500 (20)

10-500 (10)

LOW ORGANICS

10- 1,000 (40)

Rhodes (1957a)

10-1,000 (20)

Rhodes (1957a)

H I G H DISSOLVED SOLIDS LOW DISSOLVED SOLIDS

H I G H ORGANICS LOW ORGANICS H I G H ORGANICS LOW ORGANICS

0 0 0 0

NEUTRAL TO BASIC

Brown and Haney Haney (1964) (1964) W i ldung e t a1 . (1975)

Brown (1967) Routson e t a l . (1976)

A C I D

FIGURE 9. Rd Estimates (mL/g) f o r Chromium(VI), T r i t i um, Technetium, Ch lor ide , F luo r i de , Iod ine , Sul f a te , N i t r a t e , Xenon, Krypton, and Argon. The numbers i n parentheses are conserva t ive Rd ranges above them. See F igu re 1 f o r parameter d e f i n i t i o n s .

FIGURE 10. R Est imates (mL/g) f o r Cesium. The numbers i n parentheses a r e conse rva t i ve Rd ranges a I! ove them. See F igure 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

A C I D

H I G H DISSOLVED SOLIDS

H I G H ORGANICS

3 -300 (10)

Barney (1978)

5-50 (5

K n o l l (1969)

LOW DISSOLVED SOLIDS

LOW ORGANICS

3 -300 (10)

Rhodes and Nelson (1957)

Hajek and Ames (1968) Routson e t a l . (1981)

5-50 (5 )

McHenry (1954) Rhodes and Nelson

(1957)

H I G H ORGANICS

50-3,000 (50)

Barney (1978)

10-100 (30)

LOW ORGANICS

50-3,000 (50)

Rhodes and Nelson (1957)

Hajek and Ames (1968) Routson e t a l . (1981)

10-100 (30)

McHenry (1954) Rhodes and Nelson

(1957)

FIGURE 11. Rd Estimates (mL/g) f o r Chromium(II I) , Rare Earths (Ce, La, Eu, Pm), Americium, and Curium. The numbers i n parentheses are conservat ive Rd ranges above them. See F igure 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

A C I D

H I G H DISSOLVED SOLIDS LOW DISSOLVED SOLIDS

P

H I G H ORGANICS

0-10 (2)

0-2 (0)

Knol l (1969)

H IGH ORGANICS

0-20 (5)

0-10 (2)

LOW ORGANICS

10-200 (100)

Benson (1960) Hajek (1966)

10-40 (20)

Rhodes (1957a) Hajek and Kno l l

(1966)

LOW ORGANICS

100-500 (200

Benson (1960) Routson e t a l . (1976)

Sheppard e t a l . (1976)

50-200 (100)

Rhodes (1957a) Routson e t a l . (1976)

FIGURE 12. R Estimates (mL/g) f o r Plutonium. The numbers i n parentheses a re conservat ive Rd ranges a f ove them. See Figure 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

ACID

H I G H DISSOLVED SOLIDS LOW DISSOLVED SOLIDS

H I G H ORGANICS

0.2-20 (10)

0.1-1 .o (0.5)

Benson (1960) Kno l l (1969)

H I G H ORGANICS

0.2-20 (10)

0.1-10 (2)

LOW ORGANICS

20-200 (50

Rhodes (1957b)

1-20 (5)

Hajek and Knol l (1966)

LOW ORGANICS

100-2,000 (25)

Rhodes (1957b) Emery and Garland

(1974) Emery e t a l . (1974)

20-200 (20)

Rhodes (1957b)

FIGURE 13. Rd Estimates (mL/g) f o r Neptunium and Uranium. The numbers i n parentheses are conservat ive Rd ranges above them. See F igure 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

A C I D

H I G H DISSOLVED SOLIDS LOW DISSOLVED SOLIDS

H I G H ORGANICS

0.2-20 (1)

0.1-1 .o (0.5)

H I G H ORGANICS

0.2-20 (1)

0.1-10 (0 5)

LOW ORGANICS

0.2-200 (0.5)

Routson e t a l . (1976)

2-20 (10)

LOW ORGANICS

2-2,000 (2

Benson (1961) Routson e t a l . (1976) Sheppard e t a l . (1976)

20-200 (20)

FIGURE 14. Rd Estimates (mL/g) f o r Aluminum, S i l i c o n , and Titanium. The numbers i n parentheses are conserva t ive Rd ranges above them. See F igure 1 f o r parameter d e f i n i t i o n s .

NEUTRAL TO BASIC

A C I D

H I G H DISSOLVED SOLIDS LOW DISSOLVED SOLIDS

H I G H ORGANICS

1-1,000 (10)

3-1,000 (3)

H I G H ORGANICS

10-1,000 (20

10-1,000 (20)

LOW ORGANICS

5-2,000 (20)

5-2,000 (5)

LOW ORGANICS

10-2,000 (20

10-2,000 (20)

(a) Presence o f h igh n i t r a t e s and/or n i t r i t e s 1 owers ru then i um adsorpt ion tendencies; o the r s a l t s a re n o t important.

NEUTRAL TO BASIC

A C I D

FIGURE 16. R Est imates (mL/g) f o r Ruthenium. The numbers i n parentheses are conservat ive Rd ranges a g ove them. See Figure 1 f o r parameter d e f i n i t i o n s .

HIGH DISSOLVED SOLIDS (a) LOW DISSOLVED SOLIDS

H I G H ORGANICS

0-30 (0)

Raymond (1964, 1965)

0-10 (2)

H I G H ORGANICS

2-20 (5)

Wi ld ing and Rhodes (1963)

2-1,000 (20)

LOW ORGANICS

0 - 500 (2)

Ames and Rai (1978) Barney (1978)

1-500 (50)

LOW ORGANICS

10-1,000 (20)

Rhodes (1957a)

10- 1,000 (40

Rhodes (1957a)

site-specific sediments and the specific waste stream of interest. However, the Rd values in the figures provide a conservative estimate that can be used for scoping performance assessment calculations and an estimate of the range

in values. If data on a Hanford sediment and liquid waste similar to one of

the 33 active discharges are available, the specific reference is cited.

Where no citations are given, we re1 ied on experience and general knowledge of contaminant-sediment interactions to develop the estimates (e.g., Coughtrey et

al. 1983-1984; Ames and Rai 1978; Serne and Wood 1990).

4.4 SOLUBILITY OF INORGANIC AND RADIONUCLIDE CONSTITUENTS

Solubi 1 ity (dissol ution-precipitation) reactions are often important in controlling the fate of inorganic contaminants that have been disposed of to

sediments. Certain constituents are very insoluble with the slightly alkaline

pH and alkaline earth-rich pore waters present in Hanford sediments.

Generally oxide, hydroxide, carbonate, and phosphate minerals of certain

metallic elements can be expected to control solution concentrations at low

values. Some common solubility controls include A1 and Si oxides; Pb and Ca

carbonates or phosphates; Ti, Cr, Mn, Fe, Zr, lanthanum, and actinide oxides

and hydroxides; and Ba sulfate. Krupka (in Evans et al. 1988b) has discussed

solubility calculations for Hanford groundwaters and suggested that many of

the elements 1 isted above could be control led by these minerals under existing conditions in the upper unconfined aquifer. Rai and Serne (1978), Lindsay

(1979), Stumm and Morgan (1981), Drever (1982), and Nordstrom and Munoz

(1985) have a1 1 presented generic discussions of solubi 1 ity controls in soils and sediments and presented methods to aid researchers in performing such

calculations for site-specific conditions. It should be pointed out that a

solubility limit is not a constant value in a chemically dynamic system. That

is, the solubility limit (e.g., on Pu, Sr, Cd, or Pb) is determined by the

product of the thermodynamic activities of species that constitute the solid.

If the system chemistry changes, then the individual species activities wi 1 1

likely change. For example, if the controlling solid for plutonium is the

hydrous oxide Pu(OH) 4, the sol ubi 1 i ty product is [PU] [OH] = Ksp, where

brackets indicate activities. The value of Ksp is fixed, but the values of

[Pu] and [OH] can vary. In fact, if the pH decreases 1 unit (meaning that

[OH] decreases by lo), then for KSp to remain constant, [Pu] must increase by

lo4, with all else held constant. A true solubility model must consider the

total system and does not reduce to a fixed value for the concentration of a

constituent under all conditions. Numerous constant-concentration (i.e.,

empirical sol ubi 1 ity) models are used in performance assessment activities; such models assume a controlling solid and fix the chemistry of all

constituents to derive a fixed value for the concentration of specific

contaminants. However, the value obtained is only valid for the specific

conditions assumed.

Solubility-controlled release models assume that a known solid is

present, or rapidly forms, and controls the solution concentration of the

constituents being released. Solubility models are thermodynamic equilibrium

models and do not consider kinetics (i .e., the time required for the sol id to

dissolve or completely precipitate). When identification of the probable controlling solid is difficult or when kinetic constraints are suspected,

empirical solubility experiments are often performed to gather data that can

be used to generate an empirical solubility release model (a model with

mathematical similarity to solubility but no identified thermodynamically

acceptable control 1 ing sol id) . Currently, two commonly used performance assessment codes, TRANSS and the

Mu1 t imedi a Envi ronmental Pol 1 utant Assessment System (MEPAS) , can accommodate only the constant solubility release model. The geochemical code MINTEQ

(Felrny et a1 . 1984; Peterson et a1 . 1987) is the current detailed solubi 1 i ty model and code used at PNL. Less detailed, constant-concentration-limit

models have been generated from empirical studies (Delegard and Gallagher

1983; Delegard et a1 . 1984). The active waste streams identified by Westinghouse Hanford (1989)

generally have near-neutral to slightly alkaline pH and low to moderate total

dissolved solids contents. On contact between the waste stream and the

Hanford sediments, we do not expect any dramatic changes in pH or redox state,

two variables that can cause significant dissolution/precipitation reactions.

Thus, it is not likely that most contaminants within the liquid waste streams,

aside from very insoluble constituents (e.g., Al, Fe, Mn, Am, Pu, PO4), will

be controlled by solubility processes.

Another way of looking at the waste streams' fate is that the

measurements of the chemical composition available reflect precipitation

reactions that have already occurred within the process facilities. That is, highly insoluble constituents are not found in the liquid effluents discharged

to Hanford sediments because they have already been removed before reaching

the disposal crib. The active waste effluents contain soluble constituents

that, in general, will remain soluble in the sediment pore waters.

Qualitative solubility rankings for important inorganic contaminants in

Hanford waste streams are provided by Serne and Wood (1990, Appendix A). For

convenience, a similar table for the major inorganic and radionuclide

constituents identified in active waste streams is provided here (Table 15).

At present, we recommend that preliminary performance assessments assume

that solubility effects are incorporated into the Rd value used to calculate

retardation factors. Therefore, no additional computing provisions other than

the Rd values presented in Figures 2 through 16 must be made to predict the

fate of contaminants.

The organic carbon content of most active waste streams does not appear

to be significant and probably would not influence the fate of the identified

hazardous inorganics and radionuclides. Only five waste streams contain more

than 2 ppm organics (see Figure 1). The organic content of only streams A.5

and A.21 have concentrations of known complexers (e.g., tributylphosphate)

that reach the parts per million range. Thus, if more detailed and mechanistic modeling of contaminant migration were required, the available

thermodynamic data, codes (i.e., MINTEQ), and waste stream analyses could be

used to determine plausible solubility controls for most inorganic and radionuclide constituents in at least 31 of the 33 waste streams. MINTEQ

currently contains thermodynamic data for the following components of interest

to active disposal of liquid waste: Li, B, C, NOi, NOj, NH;, F, Na, Mg, Al,

Si, poi-, s2-, SO$-, C1, K , Ca, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, As, Se, Br, Rb, Sr, Mo, Ag, Cd, Sb, I, Sc, Ba, Hg, TI, Pb, Ra, U, Am, and ~ ~ ( 1 1 1 ) ~ Pu(1V) , Pu(V) , and Pu(V1). Currently absent from the MINTEQ database are

TABLE 15. Qualitative Estimate of Mineral Solubility of Hanford Sediment in Pore Water

High Organic Carbon

Solut ion Const i tuent ()2,000 ppb)

3~ vs (a) L i VS Be Unknown

C I Ar K Ca T i v Cr (VI) Cr ( I I1 ) Mn Fe Co Cu Zn As K r Sr Z r Nb MO Tc Ru Ag Cd Sn Sb

Cs Ba

Lanthanides Hg Pb U NP Pu Am

VS MS VS MS LS MS VS LS MS MS MS MS MS VS MS MS MS MS VS VS

Unknown MS Ms MS VS MS Ms VS LS MS

Unknown Ms MS Ms MS MS

Low Organic Carbon

Solut ion ((2,080 ppb)

VS VS

Unknown VS VS MS VS MS LS MS LS MS 6 VS MS VS MS LS Ms VS LS LS LS MS Ms MS VS Ms MS LS

VS Ur~known

LS Ms LS VS Ms US VS LS LS

Unknown LS Ms MS LS LS

L im i t i ng So l i d

-- - - - -

-- CaF2

-- Carbonates Oxides Ox ides Ca phosphates

i:E:c!?! i des --

Carbonates, phosphates Oxides

-- Mi xed Fe(OH)3 Ox ides, hydroxides Oxides, hydroxides Hydroxides Hydroxides, carbonates Hydroxides, carbonates

- - Carbonates Hydroxides, ox ides Hydroxides, oxides

-- - - --

Chlorides Carbonates Hydroxides, oxides

- - - - - - - -

Su l fa te Hyd row ides, phosphates

- - Carbonate-hydrox ide n i x Phosphate, oxide, a lka l ine ear th uranate Hydroxides Hydrox ides Hydroxides, phosphates

(a) VS = Very soluble; common cont ro l l ing so l ids i n Hanford sedinents/waste stream environments (pH between 6.6 and 10.5) would a l low nore than 1,000 ng/L i n so lu t ion .

(b) MS = Moderately soluble; conmon cont ro l l i n g so l ids i n Hanford sedinents/waste stream environments (pH between 6.5 and 18.6) would a l low no more than 26 ng/L i n so lu t i on .

(c) LS = Low so lub i l i t y ; conmon cont ro l l ing so l i ds i n Hanford sedinents/waste stream environments (pH between 6.5 and 10.6) would a l low less than 1 mg/L i n so lu t i on .

thermodynamic data for Be, Ti, Zr, Nb, Sn, Tc, Ru, lanthanides, Np, and Cm. Detailed solubility calculations for these neglected components would require an effort to collect data from the literature, critically review the information, and enter the reviewed data into the appropriate data files. Depending on complexity and data quantity, the cost of performing such activities would be between $20,000 and $30,000 for each element.

4.5 CHEMICAL/RADIOLOGICAL HALF-LIVES

Inorganic contaminants found in the active waste streams do not degrade biotical ly or convert into other constituents and can therefore be considered to remain present forever. Certain nutrients (N- and P-contai ning compounds) , such as NH;, NO?, NOi, and poi-, can be transformed by microbiological reactions, but we will not consider such reactions here. Microbiological

activity is not currently considered to be significant in Hanford vadose zone sediments. Nitrate plumes from past and current disposal practices are extensive in the Hanford Site's upper unconfined aquifer (see, for example, Evans et al. 1988a, 1988b, 1989). From this fact we infer that biological

degradation of nitrate is not significant and that it is probably not significant for other inorganic nutrients.

All of the radionuclides identified in the 33 active waste streams decay to other elements with a characteristic half-life, as presented in Table 16.

For probable scenarios of concern (e.g., liquid disposal to the vadose sediments, percolation to the water table, and subsequent transport in the

upper unconfined aquifer to a future domestic drinking water well or the Columbia River), nonreacting nuclides with half-lives longer than 100 years can be considered stable. That is, how long it takes for water to reach the well or river after disposal to the vadose zone sediments is likely to vary between tens of days to many tens of years (e.g., DOE 1987; USGS 1987; Buelt et al. 1988). Mobile contaminants that do not significantly interact with the sediments would reach the well or river in about the same lengths of time as

the water. Conversely, contaminants that do interact significantly with the

sediments will travel at reduced rates, as quantified by the retardation

TABLE 16. H a l f - L i f e f o r Radionucl ides I d e n t i f i e d i n A c t i v e Waste Streams

H a l f - L i f e , y r I so tope

lZ5sb 1291

1311

132

133 I

1351

135xe

134cs

1 3 7 ~ s

138cs

1 4 O ~ a

1400,

141ce

144ce

147pm

153sm

1 5 4 ~ u

1 5 5 ~ u 234u

2 3 5 ~

2 3 6 ~

238u

2 3 9 ~ p

2 3 8 ~ ~

2 3 9 ~ ~

241 PU

2 4 4 ~ ~

Hal f - L i f e , y r

factor [see Equation (3)]. In such cases, even radionucl ides with ha1 f-1 ives as long as thousands of years may in fact decay before reaching the well or river. Performance assessment codes will explicitly consider the decay during

transportation of nuclides if one supplies the retardation factor,

radionucl ide half-1 ife, and water travel time.

Table 16 lists all of the radionuclides identified in the 33 active waste

streams. The list is extensive but only a small portion of the radionuclides

have half-lives longer than 3 months, an arbitrarily chosen cut-off time for

environmental concern for typical Hanford active discharges. Table 17 lists

those radionuclides from Table 15 that have half-lives longer than 3 months.

The uranium isotopes, lZ91, and 9 9 ~ c have ha1 f-1 i ves 1 onger than 100,000 years

and for most scenarios germane to active liquid discharges at the Hanford

Site, these isotopes will not decay significantly prior to reaching the

accessible environment.

TABLE 17. Radionuclides with Half-Lives Long Enough for Environmental Concern

Half-Life. vr Isotope

60co

lZ5sb

147~m

134~s

155~u

lo6~u

5 4 ~ n

144ce

6 2 ~ n 1 lornAg

113sn

Half-Life, yr

5.3

2.7

2.6

2.0

1.8

1 .o 0.8

0.8

0.7

0.7

0.3

4.6 DISTRIBUTION COEFFICIENTS FOR ORGANICS

The processes affecting migration rates of both organic and inorganic

compounds are listed in Table 18. The transformation processes in Table 18

can be graded relative to the properties of a compound, and field data for

environmental factors yield a good indication of the compound ' s persistence in the sediment/water column. Volatilization is an important exchange process

that occurs between a compound being dissolved in solution that is vaporized

in the atmosphere. Organic compounds with high vapor pressures and low water sol ubi 1 i ties are most susceptible to vol ati 1 ization (for example, a1 iphatic

hydrocarbons, monocycl ic aromatics, and some nitrogen-substi tuted compounds).

The magnitude of the Henry's law constant is used as an indicator of compound

volatility because it accounts for compound water solubility and vapor

pressure. However, quantitative measurement of compound volatility also must

take into account wind velocity, water turbulence, and temperature.

Photolysis is another transformation process that depends on both compound

properties and environmental conditions. The degree of photolysis is

dependent on the amount of light (energy) a chemical can absorb and the efficiency with which it uses that energy, as well as sunlight intensity,

cloud cover, time of day, season, latitude, ozone layer thickness, and water

turbidity.

The migration behavior of organic compounds in the environment is

primarily a result of the interaction between the physical and chemical properties of the compound and the sorbent. The effect of these properties in

the water and sediment column may be subject to changes in such variables as

pH, Eh, dissolved organics and inorganics, temperature, and water

hydrodynamics. The transformation processes shown in Table 18 are quantified

using the parameters shown in Table 19. From knowledge of the values for each

parameter, one can rank the importance of the various processes, as shown in

Table 20. For some groups, such as halogenated aliphatic hydrocarbons, a

single process dominates transformation and fate in most environments. The

fates of many organic compounds are more complex and depend on competing

processes that vary in importance depending on compound properties and

TABLE 18. Phys ica l and Chemical Processes Used t o Assess t h e D i s t r i b u t i o n and Fate o f Organic Compounds (Witkowski e t a l . 1987)

Process D e f i n i t i o n and Contro l l i n g Var iables

V o l a t i l i z a t i o n Evaporative loss o f a chemical

Depends on vapor pressure and water so lub i l i t y o f t he chenical and on envi ronnental var iab les such as wind, water turbulence, and temperature.

Poten t ia l l y important f o r compounds w i t h h igh vapor pressures, low so lub i l i t i e s , and high a c t i v i t y c o e f f i c i e n t s .

Sorpt ion

Photo lys is

Ceneral term encompassing surface a t t r a c t i o n (adsorption) and p a r t i t i o n (solubi l i za t ion) .

Depends on the hydrophi l i c and l ipophi l i c p roper t ies o f t he chemical and the composition o f the sorbent .

I n d i c a t i v e parameters are so lub i l i t y , octanol-water p a r t i t i o n c o e f f i c i e n t , and sorbent organic carbon content .

Nonmetabol i c degradation r equ i r i ng l i g h t energy: chemical undergoes e i t h e r a d i r e c t t rans format ion reac t ion from the absorbed energy o r an i n d i r e c t change from a reac t ion (e.g., ox ida t ion) w i t h an exc i ted chemical species o r f r e e r ad i ca l .

Depends on the c h e ~ i c a l ' s absorpt ion spectrum c o e f f i c i e n t i n the u l t r a v i o l e t t o v i s i b l e range, as wel l as the sun l i gh t i n t e n s i t y d i s t r i b u t i o n f o r a g iven t ime o f day, season, l a t i t ude , depth i n water, and ozone th ickness. Also depends on the chemical 's reac t ion quantun y i e l d .

Chemical ox ida t ion Breaking down o f the chemical bonds i n organic conpounds through a chemical reac t ion w i th photochemical l y der ived oxidants (s ing le oxygen o r f r e e radica I s ) .

Depends on the number and types o f possib le r eac t i ve s i t e s and on the presence o f oxidants.

Rate constants e i t h e r measured d i r e c t l y o r estimated from s t r uc tu re -ac t i v i t y r e l a t i ons

Hydrolys is Reaction o f a chemical w i t h water, hydrogen, o r hydroxide ion, commonly r esu l t i ng i n the in t roduc t ion o f a hydroxy l group i n exchange f o r the renoval o f another func t iona l group.

Depends on t he presence and number o f hydrolyzable func t iona l groups a t neut ra l pH p lus the c a t a l y t i c e f f e c t o f the add i t i on o f acids and bases a t other pHs.

Bioaccumu l a t ion Uptake and re ten t i on o f chemicals i n the water column by aquat ic organisms through intake f r o n water o r d i e t .

Depends on the nature o f the chemical (i .e . , if l ipophi l i c ) and the organism's f a t content and metabolic and depurat ion ra tes .

Biotransformat ion Enzyme-cata lyzed t ransformat ion o f chen ica I s as a source o f energy, carbon, and nu t r i en t s . and biodegradat ion

Depends on t he r e f r ac to r y and t o x i c nature o f the chenical and on the,presence o f an acc l iaated n i c r ob i a l populat ion and a host o f env i ronmenta l f ac to r s , ~ n c l u d i n g pH, temperature, d issolved oxygen, avai lab le nu t r i en t s , and conetabol i t e s .

TABLE 19. Physicochemical Parameters Used in Eva1 uation of Transport Propert ies of Orqan i c Compounds

Character is t ics

Water solubi l i t y

Vapor pressure

Henry I s law constant

Reaerat ion ra te r a t i o

Daf i n i t i o n s

I nd i ca t i ve o f chemical I s hydrophobic/hydrophi l i c nature, t he l im i t i ng load i n water, and i t s potent ia l behavior i n so lu t ion . Uni ts: mass per volume.

The p a r t i a l pressure o f vapor t h a t i s i n equi l ibrium wi th a substance i n i t s impure s ta te a t a speci f ied temperature. Re la t ive o r qua1 i t a t i v e easure o f t he v o l a t i l i t y 1 o f the chenical i n i t s pure s ta te . Uni ts: mass/length*time (e.g., pascal, atm).

Relat ive equi l ibrium concentration o f a compound i n a i r and water a t standard temperature and pressure. Rat io o f the vapor pressure d iv ided by the ch n i c a l ' s B water solubi l i t y ; i nd i ca t i ve o f the compound's v o l a t i l i t y . Un i ts : atmom /no1 .

Rat io o f the f i rs t -order ra te constant f o r loss o f a chemical from aqueous, so lu t i on d iv ided by the ra te constant f o r oxygen uptake by the sane so lu t ion . Un i t less . Estimate o f the v o l a t i l i t y o f compounds wi th Henry's law constants )3,500 t o r r per no la r f o r which the v o l a t i l i z a t i o n ra te constant i s l im i t ed by d i f f u s i o n through the l iquid-phase boundary layer.

P a r t i t i o n c o e f f i c i e n t Equi l ib r ium d i s t r i b u t i o n o f a compound solubi l ized between two immiscible solvents. (K) Uni t less (see so i l /sed inent p a r t i t i o n c o e f f i c i e n t below).

Octanol-water p a r t i t i o n Equi l i brium d i s t r i b u t i o n o f a compound between water and n-octanol . Ind i ca t i ve coe f f i c i en t (K ) 01'1 cha rac te r i s t i c o f the bioconcentration po ten t i a l o f compounds. Un i t less.

Soi l lsediment p a r t i t i o n Equi l i brium d i s t r i b u t i o n o f a compound between water and a sediment/soi l substrate. coe f f i c i en t (Kp) Mass o f chemical per mass o f sediment div ided by the dissolved mass o f chemical i n

so lu t i on per mass o f so lu t ion . Un i t less .

Soi l /sedinent organic Soi l lsediment p a r t i t i o n c o e f f i c i e n t d iv ided by the so i l/sediment percent organic carbon p a r t i t i o n carbon content. This normalizes t he p a r t i t i o n c o e f f i c i e n t t o a soi l /sediment constant (Koc) substrate t h a t i s 100% organic carbon, permi t t ing comparison o f p a r t i t i o n

coe f f i c i en t s between substrates o f d i f f e r i n g carbon content. U n i t less.

Absorption spectrum quant i ty o f l i g h t absorbed by the chemical a t a p a r t i c u l a r wavelength i n the coe f f i c i en t u l t r a v i o l e t - v i s i b l e range o f the electromagnetic spectrum.

Reaction quantum y i e l d Ef f ic iency o f l i g h t u t i l i z a t i o n by a chemical. Rat io o f the number o f moles o f the chemical transformed t o the quant i ty ( f lux) o f l igh t adsorbed. Un i t less.

Photolysis ra te constant F i rs t -order ra te constant f o r d i r e c t photolysis. Un i ts : rec iproca l t i n e

Oxidation ra te constant Sum o f the ra te constants f o r each ind iv idua l type o f reac t ive s i t e i n the compound. Uni ts: reciprocal time.

Hydrolysis ra te constant F i rs t -order ra te constant a t pH o f 7 and the second-order ra te constants f o r acid- and base-promoted hydrolysis. Un i ts : reciprocal t i n e .

Bioconcentrat ion f ac to r Concentration o f a chemical i n t i s sue on a dry-weight basis d iv ided by the concentration i n water. Also the r a t i o o f the uptake t o depuration rates f o r a compound i n a given organism. U n i t less.

Biotransformat ion ra te Second-order ra te constant dependent on the chenica l concentrat ion and the microbial biomass. Un i ts : reciprocal t i n e .

TABLE 20. Environmental Processes A f f e c t i n g t h e Organic Compounds I d e n t i f i e d i n t h e 33 Waste Streams (Witkowski e t a1 . 1987)

Primary Mechanism

Secondary Mechanism Chem i ca l Group Comments

Halogenated a l ipha t i c hydrocarbons

V o l a t i l i z a t i o n Compounds w i t h more than f i v e ch l o r i ne atoms are so rp t i ve . Have a po ten t i a l f o r bioaccumu l a t ion.

Halogenated e thers Al i pha t i c

Hydrolys is V o l a t i l i z a t i o n and photo-ox idat ion i n atmosphere Bioaccumu l a t ion and biodegradation

Some pers istence due t o h igh s o l u b i l i t y . Also pers istence po ten t i a l due t o l i p o p h i l i c i t y .

Aromatic Sorpt ion

- Monocyc l i c aromatics V o l a t i l i z a t i o n Atmospher i c ox ida t ion /photo lys is

Vo la t i l i za t i on / so rp t i on are competing react ions w i t h env i ronmenta l cond i t ions determining which dominates Some pers istence from high s o l u b i l i t y .

Sorp t ion and b i oaccumu l a t i on

Slow biodegradation (espec i a l l y n i t rogen compounds)

Phenols Photo l y s i s

Biodegradation

(near a i r-water surface) No accumu l a t ion/pers istence except f o r n i tropheno Is, which sorb readi ly t o c lays (near water sediment i f

s u f f i c i e n t microbes)

Monocyc l i c aromatics and phenols w i t h f i v e o r more ch l o r i nes

Sorpt ion and bioaccumu l a t i o n

Chlor ine content dominates compound behavior .

Phtha l a te es te rs Sorp t ion Bioaccumulation, b iotransformat ion, and biodegradation

B i o l o g i c a l l y reac t ive i n meta- bo l i c processes. Because o f sorp t ion , t ranspor t depends on hydrogeo log ic cond i t ions .

Polynuclear aromatic hydrocarbons

Sorption, b i oaccumu l a t i on, and biodegradation

Photo lys is ( f o r com- pounds w i t h low r i n g numbers)

Bioaccumu l a t ion short - term because read i l y metabo l i zed. Sorpt ion increases and b io - degradation decreases w i t h increasing number o f benzene r i ngs .

Ni t rogen compounds A l i pha t i c Photo l y s i s

Sorpt ion

Mainly hydrospheric photo lys is due t o h igh s o l u b i l i t y bu t a lso atmospheric. Aromatic Biodegradation

prevailing environmental conditions. For example, monocyclic aromatics are susceptible to either volatilization followed by atmospheric photolysis or sorption followed by bioaccumulation. In this example, the transformation processes that control compound persistence vary with environmental factors, such as wind speed, temperature, and availability of particulates in the water column for sorption.

The presence of solvents other than water can alter an organic compound's water solubility. Hence, the presence of cosolutes must be considered when attempting to predict the transport of organic contaminants through the subsurface. In general, sediment contaminated with low-water-solubility organics tend to bind other organics to the organic carbon fraction of the sediment. However, if existing sorbed organics are contacted by other low- water-sol ubi 1 i ty (i .e., hydrophobic) organics (cosol vents) , the sorbed organics may be mobilized in the cosolvents.

Data on transformation of organic compounds (e.g., biological degradation) in water and sediments are available in many cases but are not very useful in predicting contaminant fate at the Hanford Site because of the numerous uncertainties derived from the influences of many environmental factors on transformation or degradation rates. These environmental factors include the presence, number, and species of organisms in the sediments, sediment pH, sediment type, moisture content, and temperature of the environment. Degradation rates or organic compound half-lives tend to be specific for a given environment and often cover a wide range of values for a single organic. Because the bulk of the half-lives given in the literature lack applicability to the Hanford Site, the values listed in Appendix A should not be given much credence because none were obtained in environments specific to the Hanford Site. Rather, the half-life information should be considered

as qualitative guidance.

The soillsediment partition coefficient, Kp, is defined as the ratio of

adsorbed organic chemical per unit weight of the sediment to the weight of the

aqueous solute per the same unit weight of solution. Kp is unitless. The

Koc, or partition constant, used to compare organic compound sorption of soils

or sediments with varying organic content is defined as

= Kp or (100) (Kp) Koc foc % foc

where foc is the fractional mass of organic carbon in the soil or sediment.

In fact, Rd values for organics are equivalent to (Koc*foc)lpb where foc =

fractional weight of natural ly occurring organic carbon in the sediment (0.001 for typical Hanford sediments) and pb is the sediment bulk density (1.5 i 0.3

g/cm3 for most Hanford sediments). Organic compounds that bind strongly to organic carbon have characteristically low water solubilities. Likewise, organic compounds with little tendency to sorb onto organic carbon have high

water solubilities. Organics that do sorb onto organic materials, if they are

present in an aquifer, are retarded in their movement in respect to the

groundwater.

If the KO, of a compound is known, the unitless retardation factor (R)

can be calculated using Equation (3). The Rd in Equation (3) is re1 ated to

Koc by the equation

For many compounds (Farmer 1976), a 1 inear relationship between the amount sorbed (Cs) and the concentration of the compound in the equi 1 ibrium

solution (Cw) has been demonstrated: CS = Kp*Cw, where Kp is the linear

partition coefficient. It is equivalent to a Freundlich constant (Rd) when

l/n equals unity: CS = Rd*Cw l/n.

The KO/, of an organic solute is the n-octanol/water partition

coefficient and defined as the equilibrium ratio of the solute concentration

in the water-saturated n-octanol phase to the solute concentration in the

n-octanol-saturated water phase. KO/, values are unitless. For ionizable

organic compounds (acids, amines, and phenols), KO/, values are a function of

pH. If a KO/, value is reported for an ionizable compound, the pH also should

be reported (see Means et a1 . 1982). For sorption based on organic carbon

(KO,), Karickhoff et a1 . (1979) reported a significant correlation between the

adsorption of several aromatic hydrocarbons and the partitioning of the

aromatic hydrocarbons between octanol and water (Kolw)

log KO, = 1.00 log KO/, -0.21 ( ~ 2 = 1.00) ( 7 )

where R* is the 1 east-squares 1 inear regression coefficient of determination. Linear least-squares fitting of the KO/, and KO, data from a series of

polycyclic aromatics and chlorinated hydrocarbons ranging in water solubility

from 1 ppb to 1,000 ppm gave the equation KO, = 0.63 KO/, (R2 = 0.96). Other

similar regression equations found in the literature and used to estimate KO,

values where none were available are listed in Table 21. Unfortunately, as

Means et al. (1982) point out, these relationships are applicable only to

hydrophobic, nonionizable organic compounds and to sediments containing more

than 1 wt% organic carbon content. As can be seen from the organic carbon

contents listed in Table 11, Hanford sediments are very low in organic carbon,

generally containing less than 0.10 wt%. Hence these KO/, and KO, relation-

ships are not applicable to Hanford conditions except as a tool for very

roughly estimating one when the other is known.

The Henry's law constant, sometimes referred to as the air-water

partition coefficient, is defined as the ratio of the partial pressure of a

compound in air to the concentration of the compound in water under

equilibrium conditions. If the vapor pressure and water solubility of a

compound are known, the Henry's law constant can be calculated at 1 atm

(760 mm Hg) as

where H = Henry's law constant (atm*m3/mol)

P = vapor pressure of the compound (mm Hg at 25'~)

S = water solubi 1 ity (g/L)

FW = formula weight of the compound (glmol).

TABLE 21. Regress ion Equat ions Use fu l f o r E s t i m a t i o n o f P a r t i t i o n C o e f f i c i e n t s (KO,; Wi tkowsk i e t a l . 1987)

Number o f U n i t s f o r Compound Regression equat i on (a ) Compounds R ~ ( ~ ) Sol ub i l i t y Groups References

log KO/, = -0.747 log S + 0.730 156 0.874 M o l e s p e r Low-molecular- H a n s c h e t a l . I i t e r weight o rgan ics (1968)

l og KO/, = -0.670 log S + 5.00

log KO, = -0.557 log S + 4.040

log KO, = -0.54 log S + 0.44

log KO, = -0.686 log S + 4.273

log KO, = -0.594 log S + 0 .197

33 0.970 Micromoles P e s t i c i d e s and Chiou e t a l pe r l i t e r p o l y c h l o r i n a t e d (1977)

bipheny I s

15 0.988 Micromoles P e s t i c i d e s and Chiou e t a l . per l i t e r hydrocarbons (1979)

10 0.940 Mole Ch lo r ina ted K a r i c k h o f f e t a l . f r a c t i o n hydrocarbons (1979)

22 0.933 Micrograms PAHs Means e t a l pe r I i t e r (1980b)

5 0.945 Mole PAHs K a r i c k h o f f f r a c t i o n (1981)

log KO, = -0.83 log S + 0 . 9 3 - 0 . 0 1 ( ~ ~ - 2 5 ) ( ~ ) 47 0 .93 Mole C h l o r i n a t e d K a r i c k h o f f f r a c t i o n hydrocarbons (1984)

l o g K o c = l . O O l o g K - 0 . 2 1 o/w

10 1.00 N A ( ~ ) Ch lo r ina ted K a r i c k h o f f e t a l . hydrocarbons (1979)

l og Koc = 1.00 log KO/, - 0.317 PAHs Means e t a l (1980b)

log Koc = 0.72 log KO/, - 0 .49 13 0 .95 NA S u b s t i t u t e d Schwarzenbach hydrocarbons and Westal l (1981)

log KO, = 0.9370 log KO/, - 0.006 9 0.95 NA Herb ic ides Brown and F lagg (1981)

log KO, = 0.989 log KO/, - 0.346 5 0.997 NA P AHs K a r i c k h o f f (1981)

log KO, = 1.029 log KO/, - 0.18 13 0 . 9 1 NA P e s t i c i d e s K a r i c k h o f f (1984)

(a) S = water s o l u b i l i t y o f t h e o rgan ic s o l u t e . Ko/w = oc tano l -wa te r p a r t i t i o n c o e f f i c i e n t . U n i t l ess .

Koc = measured p a r t i t i o n c o e f f i c i e n t / o r g a n i c carbon con ten t o f s o i l o r sediment sample. U n i t l e s s . Organic mat te r , depending on composi t ion, c o n t a i n s about 58% organ ic carbon (Hamaker and Thompson 1972) and consequent ly K = 1.72 Kom .

Kom = measured p a r t i e l o n c o e f f i c i e n t l o r g a n i c mat te r con ten t o f s o i I o r sediment sample. U n i t l e s s . (b) The l i near reg ress ion c o e f f i c i e n t o f de te rm ina t ion . (c) The l a s t term i n t h i s equa t ion compensates f o r m e l t i n g - p o i n t e f f e c t s t h a t occur i n t h e phase t r a n s i t i o n o f

o rgan ic compounds t h a t a re i n i t i a l l y s o l i d s . (d) NA = Not a p p l i c a b l e .

According to Lyman et al. (1982), if H is less then atm*m3/mol, the substance has low volatility. If H is greater than but less than 10-5 atm*m3/mol, the substance will volatilize slowly. Volatilization becomes an important transfer mechanism when H is between and atm*m3/mol. When H is larger than atm*m3/mol, volatilization becomes a principal transfer mechanism. Estimating the Henry's law constant for many compounds

assumes that the gas phase obeys the ideal gas law and that the aqueous solution acts as an ideal dilute solution. Neither of these assumptions always holds. In addition, the solubility and vapor pressure data used in Equation (8) are generally obtained from the pure substances. Many of the contaminants are not derived from pure substances, and vapor pressure and solubility data are often obtained without regard to standard states and temperatures. Therefore, many of the Henry's law constants given in Appendix A are actually only crude estimates.

The data presented in Appendix A on adsorption parameters, Henry's law constants, water solubilities, and degradation rates for the organic chemicals were mainly obtained from two computer databases. The two databases are the Soil Transport and Fate Database available from Utah State University's Department of Civi 1 and Envi ronmental Engineering (Sims et a1 . 1988) and Syracuse Research Corporation ' s Environmental Fate Data Base (EFDB) , as described by Howard et al. (1986).

Appendix A presents Freundlich adsorption constants for some organic substances. Like the half-life data, these are closely tied to the conditions under which they were obtained (e.g., soi 1 type, temperature, solution composition). These constants are 1 isted when avai 1 able, but the conditions under which they were obtained must be examined before their applicability to Hanford conditions can be judged.

Little, if any, data were available for several of the organic compounds

in Appendix A . In fact, for a few compounds, we could not even identify a

Chemical Abstracts Service Registry Number (CAS No.). The avai 1 able data

describing physical properties were included when no specific adsorption and

solubility data are presented for a given constituent. When no values are

present, the reader may assume that we were unable to find any information in the literature.

In Tables 22 and 23, we summarize the adsorption, water solubility, volati 1 ization (Henry's 1 aw constants), and degradation tendencies from Appendix A for those organic compounds identified in Table 5. When no data were found in the literature, we have estimated qualitatively whether the compound would exhibit high, medium, or low adsorption, water solubility, volatility, or degradation rates in Hanford sediments containing a solution representative of the 33 active waste streams. The qualitative rankings for all the organics identified in Table 5 are shown in Table 23. This table will a1 low scoping performance assessment activities to evaluate those compounds that have greater mobility.

Based on the organic data (especially KO, values) given in Appendix A, Rd

values were estimated for the most prevalent organic analytes, assuming a 0.1 wt% content of organic carbon for Hanford sediment and a bulk density of 1.5 g/cm3. The results are shown in Table 22. The Rd data are given only to show trends. As mentioned previously, Rd values computed from Koc values for soils containing less than 1.0 wt% organic carbon are speculative.

TABLE 22. Available Physicochemical Data for the Organic Compounds Listed in Table 5. An Rd was determined assuming an f of 0.1 wt% carbon. The relationship uti 1 ized for determination of an Rd value was ( K ~ ~ ) ? F , ~ ) I P ~ = Rd. For detai 1 s and references, see Appendix A.

Henry's La 9 D i s s o c i a t i o n Constant, atmom /mo 1 Es t imatefa) Constants,

0 rgan i c Compound Water Solubi l i t y a t 250C a t 250C Ko/w Rd, mL/g Acids and Bases

Tr i bu ty lphosphate

T r idecane Tetradecane

Dodecane

Pentadecane

Tetrach loroethy lene Chloroform

Bis(2-ethy l hexy I ) phtha l a t e

Undecane

2-butoxyethanol

Buty l a lcohol

P Acetone

Hexadecane P N Methy I nitrate(^)

~ i m e t h o x ~ n e t h a n e ( ~ )

Heptadecane

Octadecane

Decane

k t h y I fornate(e)

Phenol N-meth~x~methanam ine( f )

Di-n-buty l p h t h a l a t e

Benzy l a l coho l Methylene c h l o r i d e Di-n-octy lphtha l a t e

Benzoic a c i d

Methyl e t h y l ketone

Buty l benzy l phtha I a t e

45 g/L

74 g/L M i s c i b l e

8.82 t o 6.3 x 1 8 ~ ~ ag/L

TABLE 22. (con t I d )

Organic Compound

Pe la rg ic ac id

Tetrahydrofuran Butoxyg l yco l

Uethy I n-buty I ketone

Buty r a ldehyde

2-propano l

MIBK (hexone) Methy I n-propy I ketone

Buty l n i t r a t e

E thoxy t r ie thy lene g l y c o l 3,s-dimethy l p y r i d i n e

E thy l a lcohol P * Hexadecanoic a c i d P w Acetophenone

Benza Idehyde

Butoxydig lycol

Dich l o r o f l uoromethane

Dimethy ln i t rosamine Uethoxydig lycol

Methoxy t r ig l yco l

2-methy l nonane

Morpho I i ne Phenanthrene

Henry's Law Constant, atmon3/mo l

Water S o l u b i l i t y a t 25% a t 25%

M i s c i b l e

M i s c i b l e

17.5 g/L

71 g/L M i s c i b l e

19 g/L

43 g/L Low

High 9.5% ( W / W ) M i s c i b l e

I n s o l u b l e

6.13 g/L

3 g/L M i s c i b l e

Low

M i s c i b l e M i s c i b l e

M i s c i b l e

0.074 mg/L

M i s c i b l e 1.15 mg/L

N A 2.08 x

1.1 1.15 10-4

7.89 x 10-6 4.2 x lg- '

6.36 x 10-5

N A

Low Med i urn 1 . 2 10-5

N A

1.07 Med i un

Low

High 2.63 x 1 8 ~ ~ Low

Low

N A

1.44 x 2.28 x lo- '

2.88 6.76

23.99

7.586

1.122

15.48

8.129

High

Low N A

0.49

High

38-48 30.2

Low

N A

0.269 Low

Low

82,000

0.138 28,840

Low 67

15

9 .4

25

19

Low

Med i um

Low Med i urn

0.30

High

23-45 Med i um

Low

N A

12 Low

Low

High

Very low

230,000

D issoc ia t ion

Estimated Constants,

Rd , I L / ~ ( ~ ) Ac ids and Bases

Very low 0.045

u.u1 0.006

0.016 0.013

Very low

Low

Low Low

0.002

Medium 0.015-0.03 Low

Very low

Low

0 . 0 1 Very low

Very low

High

Very low 150

(a) Assumed foc = 0 . 1 wt% OC and pb = 1 . 5 g/cm3. (b) NA = Not a v a ~ l a b l e . (c) S l i g h t l y water so lub le ; explos ive vapor a t room temperature; dens i t y = 1.2075 ( a i r = 1); m e l t i n g p o i n t = 82.3%;

bo i l i n g p o i n t (explos ive) = 64.6%. (d) Moderately water so lub le , c o l o r l e s s gas; f lamaable; dens i t y = 1.617 ( a i r = 1); one volume o f water d i s s o l v e s 37

volumes o f gas; f l a s h p o i n t = -41%. (e) Co lo r less , flammable l i q u i d ; f l a s h po in t , c losed cup = -19%; dens i t y a t 15% = 0.987. ( f ) Compound no t found i n l i t e r a t u r e . (g) Compound no t found i n l i t e r a t u r e ; probably pe la rgon ic ac id, f o r which no environmental c h a c t e r i z a t i o n data a re avai l a b l e .

TABLE 23. Q u a l i t a t i v e Ranking o f Geochemical A t t r i b u t e s o f t h e Organic Compounds L i s t e d i n Table 5.

Organic Compound

Tr i buty l phosphate

Tr idecane

Tetradecane

Dodecane

Pentadecane

Tetrach l oroethy l ene

Chloroform

Bis(2 'ethy lhexy I ) phtha la te

Undecane 2-butoxyethano l

Buty l a l coho l Acetone

* Hexadecane Methyl n i t r a t e

P Dimethoxymethane

Heptadecane

Octadecane Decane

Methy I fo rnate Phenol

N-nethoxymethanam ine Di-n-buty l phtha l a te

Benzy I alcohol

Methy lene ch lo r i de

Di-n-octy lphtha l ate

Benzoic ac id

Methy lethy l ketone

Buty l benzy l ph tha la te

2-methy I-5-propy l nonane Pe larg ic ac id

Comment

Readi ly degrades, t 112 = 6 days i n r i v e r water Sorbed on sediment c lays and organic carbon

Sorbed on sediment c lays and organic carbon

Sorbed on sediment c lays and organic carbon

Sorbed on sediment c lays and organic carbon

L i t t l e sorpt ion

L i t t l e sorpt ion

Sorbed on sediment c lays and organic carbon

Sorbed on sediment c lays and organic carbon L i t t l e sorpt ion

L i t t l e sorpt ion

L i t t l e sorpt ion

Sorbed on sediment c lays and organic carbon No l i t e r a t u r e ava i lab le

No l i t e ra tu re avai lab le

Sorbed on sediment c lays and organic carbon

Sorbed on sediment c lays and organic carbon Sorbed on sediment c lays and organic carbon

No l i te ra ture avai lab le

Sorption a funct ion o f pH No conpound wi th t h i s s t r uc tu re i n l i t e ra tu re Sorbed on sediment c lays and organic carbon

L i t t l e sorpt ion

L i t t l e sorpt ion

Sorbed on sediment organic carbon

Sorption a funct ion o f pH

L i t t l e sorpt ion

Sorbed on sed iment organic carbon

No compound wi th t h i s s t r uc tu re i n l i t e r a t u r e

No l i t e ra tu re avai lab le

Qua l i t a t i ve Estimate o f SoIubi lity([tion - Med i um

Low

Low

Low

Low

Med i un

High

Med i um

Low High

High

High

Low Med i urn Med i un

Low

Low

Low

High

High -- ( 4

High High

High

High

High

High

Med i um

Low

High Low

Low

Low

High High

High

High

High High

High

Low

Med i um

High

High

High

High Low

Low

High High

Low

Low

Low High

Low

Low

High

High

Med i um Low

Low

Med i um Med i um

Med i um

High

Med i urn Low

Low

Med i um

Med i us Med i urn Med i um

High

Med i ua Low

Low

Med i urn Med i ua Med i um

Low

Med i um

Med i un Low High Med i um High Low Low Med i un

High Med i urn Low Med i urn Med i um Low High Med i um High Low Low Low

High Low Low High

Med i urn Low Medium High

TABLE 23. (cont'd)

Organic Compound Comment Solubi I i t y

qua l i t a t i ve estimate o f

Vo la t i l i t y Sorption Degradation

Tetrahydrof uran

Butoxyglycol Methy I n-buty I ketone

Butyra ldehyde

2-propano l MIBK (hexone) Methy I n-propy I ketone

Buty l n i t r a t e

Ethoxytriethylene glycol

3,5-dinethy lpyr id ine

Ethyl alcohol

Hexadecano i c acid

Acetophenone

Benza Idehyde Butoxydiglycol

Dich lo ro f luoromethane

Dinethy l nitrosam ine

Methoxydiglycol Methoxytr ig lycol

2-nethy l nonane

MorphoI ine

Phenanthrene

L i t t l e sorp t ion L i t t l e sorp t ion on organic carbon; some clay sorp t ion

L i t t l e sorpt ion

L i t t l e sorpt ion

L i t t l e sorpt ion

L i t t l e sorp t ion L i t t l e sorp t ion

L i t t l e sorpt ion

L i t t l e sorpt ion on organic carbon; some clay sorp t ion

L i t t l e sorption; odor o f pyr id ine and peppermint L i t t l e sorp t ion

Sorption a funct ion o f pH; o r d i n a r i l y a s o l i d

L i t t l e sorpt ion

L i t t l e sorpt ion L i t t l e sorpt ion on organic carbon; some clay sorp t ion

L i t t l e sorp t ion L i t t l e sorp t ion

L i t t l e sorpt ion on organic carbon; some clay sorp t ion L i t t l e sorpt ion on organic carbon; some clay sorp t ion

Good sorpt ion

L i t t l e sorp t ion

Good sorp t ion

High

High High

High

High

High

High

High

High

High High

Low

High

High High

High

High

High High

Low

High

Med i urn

High

Low Med i un

Med i ua

Med i urn Med i urn Med i urn Med i un

Low

Med i un Med i ua

Low

Med i urn Med i urn Low

Med i un

Low

Low Low

High

Low

Low

Low

Low Low

Low

Low

Low Low

Low

Low

Low Low

High

Low

Low Low

Low Low

Low Low

High

Low

High

Low

Med i urn Low

Med i un

Low

Med i un Med i un

Low

Med i un

Low High

Low

High

Med i um Med i ua

Med i urn Med i un

k d i urn Med i un

Med i um

Med i urn Med i un

(a) Sol ub i l i t y : High ) g/L; g/L 1 Med i um 1 mg/L; Low ( ng/L

(b) Vol a t i l i t y : High ) 5 x 10-' atm0m3/mo I; 5 x 10-' 1 Medium 1 1 x 10-4 atm0m3/mol ; Low ( 1 x 10-4atm0m3/mol

(c) Sorption: High Rd ) 50 mL/g; 50 mL/g ? Medium L 2 mL/g; Low ( 2 mL/g

(d) -- = No basis t o make an estimate.

5.0 FUTURE WORK

Regulations dealing with waste disposal require risk, health, and performance assessment analyses before licensing or remedial cleanup of disposal sites. These assessment analyses must predict the transport of

radionuclides/contaminants from the waste source to a receptor via pathways

that are considered credible. The groundwater pathway is generally most significant when 1 ong-term effects are considered. Geochemical reactions

between contaminants and the groundwater pathway and hydrologic characteristics largely control release and transport to the accessible

environment or receptor. Consequently, data that quantify these geochemical reactions are required to adequately complete a ri sklheal thlperformance assessment.

Sites at Hanford that contain contaminated soil include injection wells, covered French drains, cribs (covered drain fields) , trenches, and ponds. Currently, the contaminants within inactive disposal sites with contaminated soil exist as precipitated radionuclides and/or hazardous constituents that are bound in the soil column after discharged waste solutions have drained. The types of liquid wastes that were or are currently being disposed of at the Hanford Site range from very-low-ionic-strength cooling waters and condensates

to high-salt process wastes, with pH values ranging from less than 1 to more than 12. As mentioned in Section 2.0, the pH of the 33 active waste streams ranges between 5 and 10.5. Many of the alkaline waste streams disposed of in the past contained suspended particles of insoluble compounds. Some waste streams contained significant concentrations of organic solvents and compl exing agents. Geochemical conditions (ambient water chemistry, soi 1 exchange capacity, and soi 1 buffering capacities) in the soi 1 may vary widely as a function of discharge fluid chemistry and spatial proximity to the source of discharge.

Conceptual leaching models for contaminated soils have not been we1 1 established. It appears that two conceptual models, desorption and solubility, will be needed, depending on the contaminant of interest. To

characterize and predict release and transport of radionuclides and/or

hazardous constituents, solubility and sorption values specific to these various environments are needed. The quantity and quality of available

experimental and theoretical data vary with the environments. The best, most complete database is the one that corresponds to the moderately alkaline, low-

ionic-strength, organic-free groundwater contacting sandy soil, an environment that is in fact typical of much of the Hanford Site's vadose zone and unconfined aquifer. Although the amount of actual data in the database (radionuclide sorption and solubility measurements using Hanford soil and groundwater) is moderate, sufficient experimental work has been reported in the literature that a plausible range of sorption and solubility values can be estimated for many radionucl ides and inorganic contaminants. The database needed to quantify, with technical defensibi 1 i ty, specific sol ubi 1 ity or

sorption values for radionuclides and/or hazardous constituents is generally inadequate, and current transport modeling predictions should be considered as initial, rough estimates. The problem of inadequacy is compounded by the lack of specific data that quantify concentrations of radionuclides, hazardous constituents, and organic and inorganic complexants at existing contaminated soil sites.

To generate a useful database despite the lack of site-specific information, a list of potential conditions and important chemical constituents has been identified from records and past site-specific investigations (Serne and Wood 1990). It is recommended that a series of sorption and empirical solubility tests be run on the basis of the information available on inactive waste streams from Serne and Wood (1990) and the information on active waste streams from Westinghouse Hanford (1989) . Hanford Site soils should be used in these tests to provide ranges of sorption and solubility values for use in transport modeling. Because of the current lack

of information, emphasis must be placed on organic constituent interactions

with Hanford sediments. Actual data that describe the effects of partial saturation on radionuclide or contaminant transport in Hanford soils are very

sparse and more must be obtained. The primary tests to be completed include

1) batch sorption/desorption tests to develop distribution coefficients or empirical solubil ity values and to identify areas requiring further study, and

2) f low-through column tests to quantify retardation factors under the

combined influences of hydrologic flow and chemical/reactivity so that

sorption/desorption hysteresis and effects of unsaturated moisture contents, if any, can be determined. The parameters other than the chemical components

that should be varied in the test matrix include soil types, moisture content,

and flow characteristics (e.g., advection flow rates and diffusion fluxes as a function of moisture content).

The sorption/desorption of an organic group, such as the a1 kanes or

phthalates, should be experimentally examined as a function of several mixed

waste compositions. Emphasis should be placed on sorption/desorption systems

involving methylene chloride, chloroform, bis(2-ethythexyl) phthal ate,

acetone, methyl ethyl ketone, and tetrachloroethylene, which have been

recently identified as leaking through the soil column into groundwater

monitoring we1 1s adjacent to wastewater disposal sites (Appendix B) . Accompanying radionuclides that are also commonly detected as leaking through

the soil column into the groundwater with these organics include 3 ~ , 60~o,

90~r, 9 9 ~ c , 1 0 6 ~ ~ , 129~, and 137~s. In many Hanford waste streams, the Co, 1,

Ru, and Tc are usually anionic or partially anionic and can therefore be expected to sorb poorly on the soil column (i.e., to be mobile). Tritium is

present as water and would also be expected to be mobile. However, Cs and Sr

are normally present as cations and hence could be expected to sorb readily on

the soil column. The fact that 9 0 ~ r and 137~s are commonly found in

groundwaters adjacent to wastewater disposal sites suggests that there may be

unknown reactions between these radionuclides and the organics in mixed

wastes, such as complexing, that have resulted in the leakage of radionuclides

that are ordinarily adsorbed strongly. It is suggested that 8 5 ~ r and 134~s or 137~s , as gamma-emi tting isotopes, be added as tracers during selected experiments with the mixed-waste column studies proposed above. The two

radionuclides can be counted together to reduce the total number of

experiments required to understand the mixed-waste system.

Furthermore, some biodegradation studies (in batch reactors) of the

organics and of others in Table 5 that have low adsorption and high water

solubility potential should be performed under Hanford-specific conditions.

Initial studies should be performed on Hanford sediments and active waste

streams that have been acclimated to optimize growth of native microbes. Particular attention should be paid to the effects of moisture content on the rates of microbial degradation.

These initial batch equilibration and column tests would be used to furnish data for models to describe the process of contaminant sorption/ desorption/migration through actual Hanford sediments. This data collection

scheme emphasizes laboratory testing based on empiricism; in the tests the

expected environment is simulated, and geochemical and microbial reactions are measured through standard adsorption, solubility, and degradation tests. The data collection effort should rely on feedback from performance analyses (Serne and Wood 1990, pp. 1.4-1.6) to ascertain when adequate data have been collected. The data collection scheme proposed is estimated to take 3 person- years effort per year for a total duration of 4 years.

In the constant Rd model, the distribution of the contaminant of interest between the solid adsorbent and solution is assumed to be a constant value. There is no explicit accommodation of dependence on characteristics of the sediment, groundwater, or contaminant concentration. Possible retardation

mechanisms include 1) chemical precipitation of bulk sol id phases, 2) chemical substitution of one element for another in a solid phase, 3) exchange of a stable isotope of an element with a radioactive isotope in solution,

4) physical filtration of colloids, 5) cation and anion exchange, 6) chemisorption, and 7) physical adsorption. A1 1 these mechanisms are melded into the empirical distribution coefficient. The limitations associated with this approach are well known to investigators, but the paucity of Hanford Site-specific geochemical data precludes a more rigorous conceptual retardation model at this time. The constant Rd model is mathematically very simple and can be readily incorporated into transport models and codes.

A second practical conceptual model for adsorption is the parametric Rd model. Numerous statistical strategies have been used to develop empirical relationships that describe Rd as a function of other variables, such as the amount and types of minerals present in the sediment, amounts and types of dissolved species in the groundwater, pH, and Eh. Parametric Rd relationships

delineate apparent effects of key variables but do not conclusively identify

controlling processes. These statistical approaches have been demonstrated to yield accurate predictions for conditions within the range of conditions studied. When the parametric Rd retardation model is used, the performance assessment code must keep track of the current values of a1 1 of the independent variables that determine the value of Rd. Because of the added complexity of solving the transport equation, explicit use of the parametric Rd model has been rare. On the other hand, the parametric Rd approach can be used to objectively develop a suite of time- or space-dependent constant Rd values to be used in a given performance assessment analysis. This modified approach is recommended for near-future Hanford performance assessment activities. To pursue the parametric Rd approach, the same types of batch and column tests are required but more thorough characterization of the sediments

and solutions is necessary. The projected cost for the more detailed

characterization would be increased by a factor of 1.5 to 2.

As the data are collected, it would be beneficial to explore the efficacy of more detailed mechanistic studies to elucidate the controlling solubility, adsorption, microbiological, and physical (e.g., volati 1 ization) reactions that determine the fate of the contaminants. Knowledge of the controlling

reactions/processes is required to lend credibi 1 ity to the predictions made using performance, risk, or health assessment computer codes. The costs of performing such mechanistic tests cannot be determined at this time. Again, feedback from performance assessment activities (e.g., sensitivity studies, identification of key contaminants from consequence or health effects modeling) should be used to focus and prioritize the mechanistic tests to be

performed.

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A P P E N D I X A

ENVIRONMENTAL F A T E OF ORGANIC ANALYTES

REPORTED I N THE 33 WASTE STREAMS

APPENDIX A

ENVIRONMENTAL FATE OF ORGANIC ANALYTES

REPORTED IN THE 33 WASTE STREAMS

Classes of organic analytes found in the 33 waste streams a r e organized

by functional groups. Classes of organics in the 33 waste streams (see

Table 5 in main t ex t ) include a1 kanes, alcohols, organic acids, amines,

polyhydric alcohols o r glycols, e thers , phthalic acid- and carboxylic

acid-es ters , n i t r o compounds, caust ic aromatics, ketones, aldehydes, halides

and polynuclear aromatic hydrocarbons. The above s t ruc tures are i l l u s t r a t e d

in Table A.1. In addition t o the s t ruc tura l group involved, t h i s appendix

a lso l i s t s other physical and chemical propert ies of the iden t i f i ed analytes,

organized by c lass . Properties such as the Freundlich 1/N and re tardat ion

fac tor where avai 1 able , octanol -water par t i t ion coef f ic ien t s (KO/,) , and soi 1

organic carbon adsorption coef f ic ien t s (KO,), water sol ubi 1 i t y , and Henry's

law constant used t o predict v o l a t i l i t y are a lso provided (sources a re

iden t i f i ed in the reference l i s t a t the back of the appendix). Explanations

of these terms a re given in Section 4.6 of t h i s report . The Chemical

Abstracts Service Registry Number (CAS No.) i s given under each analyte when

available. Hazardous categories fo r many of the organic analytes given in

t h i s appendix are given by Jungfleisch (1988).

TABLE A. 1. C l a s s i f i c a t i o n o f Organic Analytes According t o Funct ional Groups

Exanp l e Analyte Class Funct ional Croup Formula N a ~ e

I I I I

Alkane L C - C - H3CCH2CH2CH3 n-butane I I

Alcohol

Ether

Ester

- C - M I

methanol

d imethy l ether

0 4

R -c \ CE'

methy lformate (carboxy l i c acid ester)

n-buty lph tha la te (phthal i c ac id ester)

Aldehyde

Ketone

propionaldehyde

H O H I I! I

H,C-C-C-C -H I I H H

acet ic ac id Carboxy l i c Acid

Am i ne

Hal ide

nethy l amine

methyl f l u o r i d e F, CI, Br o r I

2-n i tropropane N i t r o Compound

Polyhydric Alcohol Two o r more hydroxy l groups t h a t may be subst i tu ted

ethylene g l yco l I 1 H - C - C - H

I I H U

Polynuclear Aromatic Hydrocarbon

Benzene r i ngs w i th common or tho p o s i t ions

naphtha l ene

phenol Phenols Coal t a r de r i va t i ves based on benzene

Phosphate t r i buty l phosphate

A.2 ALKANES

Decane

H3C (CH2) 8CH3

CAS NO. 124-18-5

Synonyms: n-decane

Me1 t i n g Po in t : -30°C (Buckingham 1982, V2: 1459)

Boi 1 i ng Po in t : 174OC (Bucki ngham 1982, V2 : 1459)

Densi ty : 0.73 g/cm3 1 i q u i d a t environmental temperatures (Buckingham 1982, V2: 1459)

Vapor Pressure: 0.175 KPa (1.75 x atm) (MacKay and Shiu 1981)

Sol ub i 1 i t y : 0.0254 mg/L (MacKay e t a1 . 1981; MacKay and Shiu 1981) 0.052 mg/L (MacKay and Shiu 1981; Coates e t a l . 1985)

Henry 's Law Constant: 0.3 atm.m3/mol (Wakeh m e t a l . 1986) 3 5 t o 1.08 x 10' atmom /mol (M cKay and Shiu 1981) 3 recommended value 7 i 3 atmom /mol

K O 1.02 x l o 5 (Coates e t a1 . 1985) 1.66 x l o 6 (Hawker and Connell 1989)

Dodecane

H3C (CH2) 10CH3 CAS NO. 112-40-3

Freezing Po in t : -lZ°C (Buckingham 1982, V2:2 389-90) -9.6'C (MacKay and Shiu 1981)

Boi 1 i n g Po in t : 214.5'C (Buckingham 1982, V2:2 389-90) 216.3'C (MacKay and Shiu 1981)

Vapor Pressure: 1.57 x 1 0 - ~ k ~ a (1.57 x atm) (MacKay and Shiu 1981) a t 25'C

S o l u b i l i t y : 0.0034 mg/L (MacKay and Shiu 1981); 0.0037 mg/L (MacKay and Shiu 1981; Sut ton and Calder 1974) 0.0084 mg/L (MacKay and Shiu 1981; Coates e t a l . 1985)

Henry's Law Constant: 3.17 t o 7.86 atrn~rn3/mol (MacKay a d Shiu 1981) 9 recommended value 7.5 A 2.5 atrnern /mol

1. 6 x l o 6 (Coates e t a1 . 1985) 5 KO/w: 10 (Wakeham e t a l . 1983)

Degradation Rate: t 1 / 2 "5 days i n s o i l s l u r r y when dodecane conc 3.3 mg/L (Haines and Alexander 1974)

t 1 / 2 "10-15 days i n sedimentlseawater (Nazata and Kondo 1977)

T r i decane

H3C (CH2> 11CH3 CAS NO. 629-50-5

Freez ing Po in t : -5.5OC (Buckingham 1982, V5:5463)

Boi 1 i n g P o i n t : 234OC (Buckingham 1982, V5:5463)

Dens i ty : 0.7564 g/cm3; 1 i q u i d a t environmental temperatures (Buckingham 1982, V5:5162)

So lub i 1 i t y : 0.00104 mg/L (Coates e t a1 . 1985)

KO/,: 4.47 x l o 6 (Coates e t a l . 1985)

Tetradecane

CAS NO. 629-59-4

Me1 t i n g Po in t : 5.g°C (Buckingham 1982, V5:5162; MacKay and Shiu 1981)

B o i l i n g Po in t : 253.7OC (Buckingham 1982, V5:5162; MacKay and Sh iu 1981)

Dens i ty : 0.7628 g/cm3 1 i q u i d a t environmental temperatures (Buckingham 1982, V5:5162)

Vapor Pressure: 1.24 t o 1.27 x 10-A kPa; l i q u i d a t environmental temperatures (Buckingham 1982, V5:5162)

S o l u b i l i t y : 0.0022 mg/L (MacKay and Shiu 1981; Su t ton and Calder 1974) 0.0077 mg/L (MacKay and Shiu 1981; Su t ton and Calder 1974) 0.00028 mg/L (Coates e t a1 . 1985) 0.00033 mg/L (Coates e t a1 . 1985)

Henry 's Law Constant: 3.47 x 1 0 - I t o 1.1 x 10-0 atm*m3/mol (MacKay and Shiu 1981)

K O 1.58 x l o 7 (MacKay and Shiu 1981)

Pentadecane

H3C (CH2) 13CH3

CAS NO. 629-62-9

Me1 t i n g Po in t : 10°C (Buckingham 1982, V4:4513)

Boi 1 i n g Po in t : 270°C (Buckingham 1982, V4:4513)

Dens i ty : 0.7685 g/crn3; cou ld be 1 i q u i d o r s o l i d a t env i ronmenta l temperatures

Sol u b i 1 i t y : 0.000076 mg/L (Coates e t a1 . 1985)

K o l w : 5.25 x l o 7 (Coates e t a1 . 1985)

Hexadecane

CAS NO. 544-76-3

Synonym: n-hexadecane cetane

Me1 t i n g Po in t : 18.Z°C (Buckingham 1982, V3:2895; MacKay and Shiu 1981)

Boi 1 i n g Po in t : 287OC (Buckingham 1982, V3:2895; MacKay and Shiu 1981)

Densi ty : 0.7733; l i q u i d a t environmental temperatures (Buckingham 1982, V3:3895)

Vapor Pressure: 8.98 x t o 9.17 x kPa (MacKay and Shiu 1981) (8.98 x l o m 7 t o 9.17 x atm)

S o l u b i l i t y : 6.3 x l o m 3 mg/L (MacKay and Shiu 1981; Coates e t a l . 1985) 9.0 x 1~~~ mg/L (MacKay and Shiu 1981; Su t ton and Calder 1974) 2.1 10' mg/L (Coates e t a1 . 1985)

Henry 's Law Constant: 3.24 x t o 2.26 x 1 0 - I atm*mol (MacKay and Shiu 1981)

K O 47 t o 387 (Nathwani and P h i l 1 i p s 1977)

K O 1.78 x l o8 (Nathwani and P h i l 1 i p s 1977)

Adsorpt ion: 56% o f a 100-pg/L s o l u t i o n i n seawater adsorbed on to b e n t o n i t e c l a y (Meyer and Quinn 1973)

4% of a 100-pg/L s o l u t i o n i n seawater adsorbed on to mar ine sediments t h a t con ta ined 4% organ ic carbon (Meyer and Quinn 1973)

S i l t y Clay Sandy Loam S i l t Loam

pH 5.4 Org Content % 9.4 Sand % 6.7 S i l t % 47.9 Clay % 45.4

Spiked hexadecane 1-100 ppm i n t o A l b e r t a crude o i l , ba tch t e s t 1,000 g s o i l / L o f l i q u i d

Freundl i c h K 36.4 4.37 0.27 1 Freundl i c h l / n 0.68 1.21 1.10

'(0, 38.7 75.3 46.7

o n l y 60-80% o f adsorbed hexadecane desorbed o f f s o i l s i n t o wate r (Nathwani and P h i l l i p s 1977)

Heptadecane

H3C (CH2 ) 15CH3

CAS NO. 629-78-7

Me1 ting Point: 2Z°C (Buckingham 1982, V3:2852)

Boi 1 ing Point: 303OC (Buckingham 1982, V3:2852)

Density: 0.7780 c~/cm~; sol id at most environmental temperatures (Buckingham 1982, V3:2852)

Kolw: 3.16 x lo8 (Wakeham et a1 . 1983) 6.17 x lo8 (Coates et a l . 1985)

Sol ubi 1 i ty : 6 x mg/L (Coates et a1 . 1985)

2-methylnonane

(H3C) 2CH (CH2) 6CH3

CAS NO. 871-83-0

Synonym: i sodecane

Me1 t i n g Po in t : -74.7'C (Buckingham 1982, V4:3958)

Boi 1 i n g Po in t : 166 .8 '~ (Buckingham 1982, V4:3958)

Densi ty : 0.7281 g/cm3; 1 i q u i d a t environmental temperatures (Buckingham 1982, V4:3958)

Sol ub i 1 i t y : 0.074 mg/L ( ca l cu la ted , n o t measured) (Coates e t a1 . 1985)

KO/,: 8.2 x l o 4 ( ca l cu la ted , n o t measured) (Coates e t a1 . 1985)

Undecane

CAS NO. 1120-21-4

Freez ing Po in t : -25.6OC (Buckingham 1982, V5:5661)

Boi 1 i n g Po in t : 196OC (Buckingham 1982, V5:5661)

Dens i ty : 0.7402 g/cm3; 1 i q u i d a t environmental temperatures (Buckingham 1982, V5:5661)

Vapor Pressure: 5.22 x kPa (5.22 x atm) (MacKay and Sh iu 1981)

S o l u b i l i t y : 0.044 mg/L (MacKay and Sh iu 1981) 0.014 mg/L (Coates e t a l . 1985)

Henry1 s Law Constant: 1.85 atm*m3/mol recommended va lue 1.855 0.76 atm*m3/mol (MacKay and Shiu 1981)

KO/,: 3.80 x l o 5 (Coates e t a1 . 1985) 5.50 x l o 6 (Hawker and Connel l 1989)

Octadecane

H3C (CH2) 16CH3

CAS NO. 593-45-3

Melting Point: 28OC; a solid at temperatures below 82'~ (Buckingham 1982, V4:4351)

Boiling Point: 305 - 307OC (Buckingham 1982, V4:4351) Water Solubi 1 ity: 2 x to 6 x lom3 mg/L (Coates et a1 . 1985) Henry's Law Constant: very low (Sutton and Calder 1974)

K0lw: 2.09 x lo9 (Coates et a1 . 1985) KO,: 1.29 x lo9 (Computed using KO, = 1.00 log KO/, - 0.21)

CAS No. = unknown

Compound not found in the literature

A . 2 ALCOHOLS

C-OH

Ethyl A1 coho1

C2H50H

CAS NO. 64-17-5

Synonym: ethanol

I : 0.49 (Strenge and Peterson 1989) 0.49 (Hansch and Leo 1985)

Water Sol ubi 1 i t y : 280 g/L (Strenge and Peterson 1989) , misc ib l e (Riddick e t a l . 1986)

K O 0.30 (Strenge and Peterson 1989) 16 (Syracuse Research Corp. 1988)

Henry's Law Constant: 1.2 x l om5 atm.m3$mol (Strenge and Peterson 1989) 5.20 x lom6 atmom lmol (Snider and Dawson 1985)

Vapor Pressure: 59 mm Hg (Strenge and Peterson 1989)

Degradation Rate: t112 c1 day in r i v e r water (Apoteker and Thevenot 1983) degrades r ap id ly c 1 day in s i l t y c l a y loam (Griebel and Owens 1972)

Butyl A1 coho1

CAS N O . 71-36-3

Synonyms: n-butyl a lcohol 1-butanol

KOlw: 1.224 (Hansch and Leo 1985) 5.6 (S t renge and Peterson 1989) 0.88 (Verschueren 1983)

Core Sorp t ion : Freundl ich 1/N=1.16 a t 65OC, 500 t o 50,000 mg 1 - b u t a n o l l l ; Freundl ich l/N=l.ll a t 93OC, 500 t o 50,000 mg 1-butanol /L, a l l on a c leaned c o r e of Cot tage Grove sandstone (Donaldson e t a1 . 1975)

Montmoril l o n i t e Sorp t ion : s e e S tu l e t a1 . (1979)

Water S o l u b i l i t y : 74 g/L a t 25OC (ca l cu l a t ed ) (Merck Index 1976) 63.2 g/L a t 25OC (Tewari e t a1 . 1982) 79 g/L (Strenge and Peterson 1989)

Koc : 72 (ca l cul a t ed ) (Syracuse Research Corp. 1988) 4.7 (S t renge and Peterson 1989)

Henry's Law Constant: 8.81 x lom6 atm*9 m o l (But te ry e t a l . 1969) 4.8 x atmom /mol (Strenge and Peterson 1989)

Degradation Rate: t 1 / 2 -6 days in seawater when 3-10 mg/L butyl a lcohol -laden wastewater mixed (P r i ce e t a l . 1974)

t 1 / 2 -4 days in f reshwater when 3 mg/L added (Hammerton 1955)

t 1 / 2 = 52 days i n s o i l (Strenge and Peterson 1989)

2-Butoxyethanol

H3C (CH2) 30CH2CH20H

CAS NO. 111-76-2

Synonyms: e thy lene g l y c o l mono-n-butyl e t h e r b u t y l c e l l oso l ve

KO/,: 6.761 (Hansch and Leo 1985)

Henry 's Law Constant: 2.08 x atm*m3/mol (Syracuse Research Corp. recommended)

Water S o l u b i l i t y : m i s c i b l e (R idd ick e t a l . 1986); 4.5 g /L a t 2 5 ' ~ (Dorigan e t a1 . 1976)

Koc: 67 ( c a l c u l a ted) (Syracuse Research Corp. 1988)

2-Propanol

H3CCHOHCH3

CAS N O . 6763-0

Synonyms: isopropyl alcohol isopropanol secondary propyl alcohol

K O w : 1.122 (Hansch and Leo 1985)

Water S o l u b i l i t y : mi sc ib l e (Riddick e t a1 . 1986)

KO,: 25 (cal cul a ted) (Syracuse Research Corp. 1988)

Henry's Law Constant: 7.89 x atm*m3/mol (Snider and Dawson 1985)

Degradation Rate: i n seawater t h a t has i sopropanol (3-10 rng/L) -1 aden wastewater added, t 1 / 2 N 12 days (P r i ce e t a l . 1974)

Benzyl A1 coho1

CAS NO. 100-51-6

Synonyms: benzenemethanol phenylmethanol a-hydroxytoluene

KO/,: 12.30 (Hansch and Leo 1981)

Soi 1 Sorption: Eastern Austral i an Red-Brown Earth, 1.09% organic carbon, pH 8.0, 10 mg benzl alcohol/L in influent solution; Freundl ich adsorption of 0.17 mg/g (Briggs 1981)

Water Solubility: 40 g/L at 25OC (Ringk and Theimer 1978)

A.3 ETHERS

C-0-C

Dimethoxymethane

CAS NO. 109-87-5

Synonyms: formaldehyde dimethyl acetal methyl a1 f orma 1

Me1 ting Point: 105OC (Buckingham 1982, V2:2048)

Boi 1 ing Point: 4Z°C (Buckingham 1982, V2:2048)

Tet rahvdro fu ran

CAS NO. 109-99-9

Synonyms: d i e t h y l e n e ox ide te t ramethy lene ox ide 0x01 ane

K O 2.88 (Hansch and Leo 1979)

Water Sol u b i 1 i t y : m i s c i b l e (Dun1 op 1966)

Me1 t i ng P o i n t : -65OC (Grassel 1 i and R i t chey 1975, I I I : f386)

Boi 1 i n g Po in t : 67OC (Grassel 1 i and R i tchey 1975, I I I :f386)

Dens i ty : 0.889 a t 20°c ( G r a s s e l l i and R i tchey 1975, I I I : f 3 8 6 )

A . 4 ESTERS

0 /; l i

carboxylic acid esters F: -c,- '

phthalic acid es te rs

r - -,* - '.- [' ,' 'f' 4-: '

' I ---:--- H ---- I-y;; ' . -- - i . -

- - --. - .- I-

Methy l Formate

HCOOCH3

CAS NO. 107-31-3

Synonyms: f o r m i c a c i d methy l e s t e r

Freez ing P o i n t : -9g°C (Buckingham 1982, V4:3858)

B o i l i n g Po in t : 3 1 . 5 ' ~ (Buckingham 1982, V4:3858)

Very flammable; f l a s h p o i n t a t -lg°C (Buckingham 1982, V4:3858)

Densi ty : 0.974 a t 20°C (Grassel li and R i tchey 1975, I I I : f 2 9 7 )

Water Sol u b i 1 i t y : ve ry s o l u b l e (Grassel 1 i and R i t chey 1975, I I I : f297)

Di -n-Butyl Phthal a t e

'- C , .. t-1 CAS N O . 84-74-2 I' ,C -..Ft

" H' L i

Synonyoms: n-butyl p h t h a l a t e HI 'a.43

e l a01 DBP 1,2-benzenedicarboxyl i c ac id d i butyl e s t e r p h t h a l i c ac id d ibu ty l e s t e r

K O 52,490 (Hansch and Leo 1985) 40,000 (S t renge and Peterson 1989)

Soi l Sorp t ion : Natural seawater with 19 t o 3 ,930 pg d ibu ty l ph tha l a t e /L , "1% o rgan ic con ten t , 25OC (Sul l ivan e t a1 . 1982)

Materi a1 Freundlich Adsorpt ion, pg

Texas She l f Montmori l loni te 3 ,930 pg/L s o l u t i o n - 44 pg adsorp t ion 22 pg/L s o l u t i o n - 1.9 pg adso rp t ion

Kaol i n i t e

Ca-Montmorillonite

3 ,840 pg/L s o l u t i o n - 20 pg adso rp t ion 19 pg/L s o l u t i o n - 4 pg adso rp t ion

3,440 pg/L s o l u t i o n - 4 pg adso rp t ion 27 pg/L s o l u t i o n - 36 pg adso rp t ion

Water Solubi 1 i t y : 11.2 mg/L a t 2 5 ' ~ (Howard e t a1 . 1985) 400 mg/L a t 25OC (Verschueren 1983)

Koc : 1,800 (Russel 1 and McDuffie 1986) 170,000 (S t renge and Peterson 1989)

Henry's Law Constant: 1.81 x atrn*t~j~/rnol a t 23°C (At l a s e t a l . 1983) 2.8 x lo-' atm*m /mol (Strenge and Peterson 1989)

Degradation Rate: t112 <14 days in freshwater sediment (Johnson et a1 . 1984) t1/2 = 15.4 days soillactivated sludge (pH=7) after 14-day acclimation period (Sugatt et al. 1984)

t1/2 = 7 to 14 days in freshwater sediment (pond), mixed 9 parts water, 1 part sediment (Johnson and Lulves 1975; Johnson et al. 1984)

t112 = 1 to 3 days in freshwater at 0.5 mg/L concentration after 2- to 7- day acclimation period (Walker et al. 1984)

t1/2 = 2 to 4 days in freshwaterlsediment environment at 0.5 mg/L loading of phthalate (Walker et a1 . 1984) t112 = 60 to 70 days in sandy soil, pH = 6.2 in dissolved organic contents = 1.4% when original conc. 1,000 mg/L phthalate (Inman et al. 1984)

t112 = 30 to 50 days in silt loam saturated with water containing 1.96% disol ved organic carbon when original conc. 1,000 mg/L phthal ate (Inman et a1 . 1984)

Di -n-Octyl Phthal a t e

CAS N O . 117-84-0

Synonym: 1,2-benzenedicarboxyl i c ac id d i -n-octyl e s t e r

KO/,: 165,900 Hansch and Leo 1985) (not a recommended value) 4 7.4 x 10 (Strenge and Peterson 1989)

Water Sol ubi 1 i t y : 3 mg/L a t 25OC (Wol f e e t a1 . 1980) 0.34 mg/L (Strenge and Peterson 1989) 0.285 mg/L (Verschueren 1983)

Koc: 2,385 (S racuse Research Corp. 1988) ca l cu la t ed value 4 3.6 x 10 (Strenge and Peterson 1989)

Henry's Law Constant: 4.45 x atm*m3/mol a t 25OC, (Syracuse Resear h Corp. 1988) S 5.5 x 1g-6 atm*m /mol (Strenge and Peterson 1989) 1 x 10- atm*m3/mol (Petrasek e t a l . 1983)

Degradation Rate: t 1 / 2 = 5 days in freshwaterlsediment environment with i n i t i a l concentrat ion 5 mg/L (Sanborn e t a l . 1975)

CAS NO. 117-81-7 . .3-

Synonyms: di (2-ethyl hexy1)phthalate -

dioctyl phthal ate 1,2-benzenedicarboxyl ic acid bis (2-ethy 1 hexy1)ester octoi 1

Kolw: 128,800 40ECD 1981) 4.1 x 10 (Strenge and Peterson 1989)

Soil Sorption: Linear isotherm on kaolinite, montmorillonites, and sediments; more adsorption than dibutyl phthalate, less adsorption in distil led water than in seawater (Sull ivan et a1 . 1981, 1982)

Summary of phthalate sorption results in seawater at 25OC (Sull ivan et a1 . 1982).

Adsorbate

BE!p [ CIBEHP [14c] BEHP

Bf!P [ C] BEHP [14c] BEHP [14c] BEHP [14c] BEHP

D P [h] D B P D P [h] DBP

:y~c] DBP DBP

Adsorbent

montmorillonite montmori 1 1 oni te kaol i ni te calcite calcite calcium montmori 1 lonite sediment montmorillonite (distil led water) montmori 1 1 oni te montmorillonite kaol inite kaol inite calcite calcite calcium montmorillonite calcium montmorillonite sediment

Wt. Range of Adsorbent, mg

Initial Phthal ate conc., pg/ L K

BEHP = Bis(ethy1 hexy1)phthal ate DBP = Di-n-butyl phthalate K = partition coefficient = ng of phthalatelmg of adsorbent divided by the ng

of phthalatelml of seawater

For k a o l i n i t e , c a l c i t e , and Ca-montmorillonite, adsorp t ion = desorp t ion over 12 hours .

Water Sol ubi 1 i t y : 0.40 mg/L a t 25OC (Wolfe e t a1 . 1980) 0.34 mg/L a t 25OC (Howard e t a l . 1985) 0 .4 mg/L (S t renge and Peterson 1989)

K O 87,000 (S t renge and Peterson 1989)

Henry 's Law Constant: 1.47 x atm.9 3/mo1 a t 2 5 ' ~ (Syracuse Research Corp 4.4 x low7 atmom /mol (Strenge and Peterson 1989)

Degradation Rate: t 1 / 2 -5 days i n seawater near Japanese f a c t o r y (Hal tor i e t a l . 1975)

t 1 / 2 -14 days i n seawater away from p o l l u t i o n (Hal tor i e t a l . 1975)

t 1 / 2 -14 days i n r i v e r water i n Japan (Hal tor i e t a l . 1975)

t 1 / 2 = 15 t o >30 days i n f reshwater pond with 1 mg/L s t a r t i n g conc. (Johnson and Lulves 1975)

t 1 / 2 = <7 t o 30 days i n seawater when i n i t i a l conc. = 0.001 t o 0.1 mg/L (Perez e t a1 . 1985)

t 1 / 2 = 28 days in eu t roph ic l ake a t conc. t o 1 mg/L (Rubin e t a l . 1982; Subboa-Rao e t a l . 1982)

t 1 / 2 >> 14 days in f reshwater l sed iment a t 1-70 mg/L (Schwartz e t a l . 1979)

t 1 / 2 < 140 days i n sandy loam inocula ted wi th s ludge with 2-20 mg/L p h t h a l a t e (Fairbanks e t a1 . 1985)

t1/2- 15 garden s o i l a t 60% mois ture , pH 8 . 2 , 500 mg/L p h t h a l a t e (Shanker e t a1 . 1985)

Butyl Benzyl Phthal ate

K O 81,280 (Hansch and Leo 1985) 104.78 (Verschueren 1983)

Soil Sorpt ion: Three s o i l s with organic carbon contents of 0.70 t o 2.0%, i n f l u e n t concentrat ion between 0 and 1.0 mg/L. Freundlich adsorpt ion from 68 t o 350 mg butyl benzyl ph tha la t e (Gledhi 11 e t a1 . 1980)

Water Sol ubi 1 i t y : 2.69 mg/L a t 25OC (Howard e t a1 . 1985) 2.90 mg/L a t 2 5 ' ~ (Verschueren 1983)

K O 17,000 (Russel 1 and McDuffie 1986)

Henry1 s Law Constant: 1.26 x atm*m3/mol (Syracuse Research Corp. 1988) a t 25OC (ca lcu la t ed value)

Degradation Rate: t 1 / 2 <2 days in Mississippi River water when added a t 1 mg/L conc. (Saeger and Tucker 1976)

A . 5 ALDEHYDES

Buty ra l dehyde

CAS NO. 123-72-8

Synonym: butanal

Ko lw : 7.586 (Hansch and Leo 1985)

Water S o l u b i l i t y : 30 t o 71 g/L a t 25OC (Smith and Bonner 1951)

Koc: 9.4 (Syracuse Research Corp. 1988) c a l c u l a ted va l ue

Henry 's Law Constant: 1.15 x atm*m3/mol a t 2 5 ' ~ (Bu t te ry e t a1. 1969)

Degradat ion Rate: degrades f a s t i n sewage ( i n BIODEG summary database, no re fe rence g iven)

Benzal dehyde

CAS NO. 100-52-7

Synonym: benzoic aldehyde

K : 30.2 (Hansch and Leo 1981)

Water Sol ub i 1 i t y : 3 g/L a t 25OC (Sherman 1978) . Degradation Rate: degrades f a s t i n sewage ( i n BIODEG summary database,

no re fe rence g iven)

A . 6 KETONES

Acetone

(CH3) 2C=O

CAS NO. 67-64-1

Synonyms: P-ketopropane 2-propanone dimethyl ketone

K O 0.575 (Hansch and Leo 1985) 0.581 (Strenge and Peterson 1989)

So i l Sorpt ion: No so rp t ion on montmor i l lon i te , k a o l i n i t e , s t ream sed iments , l oca l s t ream a lgae , and loca l s t ream mold (Rathbun e t a l . 1982)

Water Solubi 1 i t y : m i sc ib l e (Riddick e t a1 . 1986) , 1 ,000 g/L (S t renge and Peterson 1989)

K O 18 (Syracuse Research Corp. 1988) ca l cul a t ed val ue 2.2 (Strenge and Peterson 1989)

Henry's Law Constant: 3.88 x lom5 atm*m3/mol (Snider and Dawson 1985) 2.10 x atm*m3/mol (Strenge and Peterson 1989)

Degradation Rate: i n seawater with 3-10 mg/L acetone added with wastewater t 1 / 2 -7 days ( P r i c e e t a l . 1974)

i n s o i l s t 1 / 2 = 4.8 days (Strenge and Peterson 1989)

Methyl E thy l Ketone (MEK)

CAS NO. 78-93-3

Synonyms: 2-butanone 2-oxobutane

KO,: 1.069 (Hansch and Leo 1985) 1.9 (Strenge and Peterson 1989)

Core Sorpt ion: Freundl i c h 1/N=1 .OO a t 60°C, 500 t o 5,000 mg methyl e t h y l ketone/L; F reund l i ch 1/N=0.99 a t 3g°C, 500 t o 5,000 mg methyl e t h y l ketone/L, a l l on a cleaned core o f Cottage Grove sandstone (Donaldson e t a1 . 1975)

Water S o l u b i l i t y : 223 g/L a t 2 5 ' ~ ( T a f t e t a l . 1985) 270 g/L (Strenge and Peterson 1989)

K O 5.2 (Syracuse Research Corp. 1988) ca l cu la ted value 4.5 (Strenge and Peterson 1989)

Henry 's Law Constant: 5.59 x atmoY 3/mo1 (Park e t a l . 1987) 2.7 x atmom /mol (Strenge and Peterson 1989)

Degradation Rate: t 1 / 2 -7.5 days i n seawater a t 3-10 mg/L MEK when wastewater 1 aden w i t h MEK added ( P r i c e e t a1 . 1974)

t 1 / 2 <1 day i n P o l i s h r i v e r water a t 10 mg/L load ing , w i t h 200 t o 400 ppm up t o 9 days ( D o j l i d o 1979)

t 1 / 2 = 16 days i n s o i 1 (Strenge and Peterson 1989)

Methyl n-Butyl Ketone

methyl butyl ketone C\H3

CAS N O . 591-78-6

Synonym: 2-hexanone

KO/,: 23.99 (Hansch and Leo 1981) 24 (S t renge and Peterson 1989)

Water S o l u b i l i t y : 17.5 g/L a t 2 0 ' ~ (Papa and Sherman 1981) 14 g/L (Strenge and Peterson 1989)

K O 15 (S t renge and Peterson 1989)

Henry's Law Constant: 1.1 x lom5 atmem3/mol (Strenge and Peterson 1989)

MIBK

CAS N O . 108-10-1

Synonyms: methyl isobutyl ketone hexanone 4-methy l -Z-pentanone

K O 15.48 (Syracuse Reasearch Corp. 1988) ca l cu la t ed value 5.3 (Strenge and Peterson 1989)

Water S o l u b i l i t y : 19 g/L (Strenge and Peterson 1989) 19.0 g/L (Verschueren 1983)

Koc: 19 (Syracuse Reasearch Corp. 1988) ca l cul a ted value 19 (Strenge and Peterson 1989)

Henry's Law Constant: 1.38 x atm*m3/mol a t 2 5 ' ~ (Syracuse Research Corp. 1988) cal u la ted value 4.2 x 10-6 atm*m3/mol a t 25OC (Strenge and Peterson 1989)

Degradation Rate: t 1 / 2 = 15 days i n seawater when present a t 3-10 mg/L concentrat ion added t o seawater a s wastewater ( P r i c e e t a1 . 1974)

Methyl n-Propyl Ketone

CAS N O . 107-87-9

Synonyms: 2-Pentanone e thyl acetone

K O 8.129 (Hansch and Leo 1985)

Water Sol ubi 1 i t y : 43 g/L a t 2 5 ' ~ (Yal kowsky e t a1 . 1987)

Henry's Law Constant: 6.36 x atm*m3/mol (Hine and Mookerjee 1975)

Degradation Rate: biodegrades f a s t in sewage a f t e r system accl imates t o presence of compound ( in BIODEG summary da tabase , no references given)

Acetophenone

CAS NO. 98-86-2

Synonyms: l-phenylehanone phenyl methyl ketone acetylbenzene

KOw: 38.01 (Hansch and Leo 1985) 48 (Strenge and Peterson 1989)

Selected chemical and physical

PH CEC Organic Soi I (1 : 1) neq/l00g) carbon, X -

1 7.79 23.72 2.07 2 7.44 19.00 2.28 3 7.83 33.01 0.72 4 8.32 3.72 0.15 5 8.34 12.40 0.11 6 4.45 18.86 0.48 7 7.79 11.30 0.95 8 7.76 15.43 0.66 9 5.50 8.50 1.30

10 7.80 8.33 1.88 11 7.55 8.53 1.67 12 6.70 31.15 2.38 13 7.75 20.86 1.48 14 6.35 3.72 1.21

properties of the sediments

Sand, X S i l t , X

3.0 41.8 33.6 35.4

0 .2 31.2 82.4 10.7

7 . 1 75.6 2.1 34.4

15.6 48.7 34.6 25.8

0.0 71.4 50.2 42.7 26.2 52.7 17.3 13.6

1.6 55.4 67.6 13.9

Clay, X

55.2 31.0 68.8

6.8 17.4 63.8 35.7 39.5 28.6 7 .1

21.2 69.1 42.9 18.8

and soils

( 1 Mod i f ied Freund l i c h p a r t i t i o n coe f f i cen t , l / n = l , Kp=0.04 + 0.32 (organic carbon percentage)

Influent contained 138 - 1,108 mg acetophenone/L, 2 5 ' ~ (Khan et a1 . 1979), sorption correlates with organic carbon content.

Rd = 0.14 Soil with 11.2% clay but no other characterization (Gerstl and Mi ngel gri n 1984)

Rd = 0.05 Soil with 6.9% clay but no other characterization (Gerstl and Mingelgrin 1984)

Rd = 0.37 Soil with 61.1% clay but no other characterization (Gerstl and Mingelgrin 1984)

Rd = 0.15 Soil with 23.8% clay but no other characterization (Gerstl and Mingelgrin 1984)

Rd = 0.30 Soil with 72.5% clay but no other characterization (Gerstl and Mingelgrin 1984)

Rd = 0.22 Soil with 10.6% clay but no other characterization (Gerstl and Mingelgrin 1984)

Water Solubility: 6.13 g/L at 25OC (Southworth and Kel ler 1986) 5.5 g/L (Strenge and Peterson 1989)

Koc: average of 14 soils, 45 (Khan et ad.81979) 23 (Strenge and Peterson 1989), 10 to

Henry's Law Constant: 1.07 x atmy 3/mo1 at 25OC (MacKay et a1 . 1982) 3.2 x atmom lmol (Strenge and Peterson 1989)

Degradation Rate: t1/2 = 4 days based on field observations (Dragun 1986)

t1/2 = 3.6 days based on field observations in soil in The Nether1 ands , redox condition not specified (Zoeteman et al. 1981)

t1/2 = el1 days (-4 days) in Ohio River; compound added in sewage overall concentration 20.5 mg/L, system pH 7.2 (Ludzack and Ett i nger 1963)

A.7 CARBOXYLIC AC IDS

Pel a r g i c Acid perhaps Westinghouse Hanford (1989) used t h i s t o mean p e l argonic ac id, which has t h e f o l l o w i n g da ta

H3C (CH2) 7COOH

CAS NO. 112-05-0

Synonym: nonanoic a c i d

Me1 t i n g Po in t : 15OC (Buckingham 1982, V4:4310)

Boi 1 i n g Point : 255OC (Buckingham 1982, V4:4310)

Water Solubi 1 i t y : i n s o l u b l e (Grassel 1 i and R i tchey 1975, I11 :n610)

Hexadecanoi c Ac id

H3C (CH2) 14COOH

CAS NO. 57-10-3

Synonym: p a l m i t i c a c i d

Me1 t i n g Po in t : 64OC (Buckingham 1982, V3:2895)

Boi 1 i n g Po in t : 3 9 0 " ~ (Buckingham 1982, V3:2895)

Water Sol ub i 1 i t y : i n s o l u b l e (Grassel 1 i and R i tchey 1975, I I I : h284)

Benzoic Acid

CAS N O . 65-85-0

KO/,: 74.13 (Chiou e t a1 . 1977) 74 (S t renge and Peterson 1989)

D i s soc i a t i on Constant: 4.205 (Sa r j ean t and Dernpsey 1979) ( s ee a l s o Mabey and Mi 11 1978)

S o i l Sorp t ion : No so rp t ion (Bai ley e t a l . 1968). 2 5 ' ~ ; Na-rnontmoril l o n i t e , CEC of 87 rneq/100 g , s o l u t i o n pH 6.8, 100 prnol benzoic acid/L; H-rnontrnori 1 l on i t e , CEC of 73 ,5 meq/lOOgf s o l u t i o n pH 3.35, 100 prnol benzoic acid/L

Water S o l u b i l i t y : 2.70 g/L a t 1 8 ' ~ (Chiou e t a l . 1977; MacKay e t a l . 1980) 3.4 g/L a t 2 5 ' ~ (S t renge and Peterson 1989)

Koc: 46 (S t renge and Peterson 1989)

Henry 's Law Constant: 0.287 x 1 atrn*rn3/rnol (U.S. EPA 1981) 1 .3 x 10-9-~trn*rn3/mol (S t renge and Peterson 1989)

A.8 AMINES

-NH2

Dimethylnitrosamine

(CH3) 2NNO

CAS NO. 62-75-9

Synonyms: n-nitrosodimethylamine 2,2'-(nitrosoimin0)-bisethanol 2,2'-nitrosiminodiethanol

K0lw: 0.269 (Hansch and Leo 1985)

Appearance % in Column

Organic pH Effluent

Soi 1 Col umn Transport: Wi 1 1 i amson si 1 t 1 oam 1.9 5.8 50 mL Lima loam 3.8 7.8 40 mL Deerfield sand 2.5 5.1 30 mL Scarboro sand 14.8 5.6 45 mL Influent: 5 mg dimethylnitrosamine/L, 25OC. Conclusion: Dimethylnitrosamine moves as rapidly in the soi 1 column as chloride (Dean-Raymond and Alexander 1976) . (" no adsorption) .

Water Solubi 1 ity: miscible (Cal lahan et a1 . 1979)

Koc: 12 (Syracuse Research Corp. 1988) calculated value

Henry's Law Constant: 2.63 x atm*m3/ mol at 20°C (Syracuse Research Corp. 1988) calculated value

Degradation Rate: t1/2 = 10 days in uncharacterized soil, pH 6.4 in laboratory batch study. Breaks down to methylamine and formaldehyde (Kaplan and Kaplan 1985)

17% percent degradation over a 10-30 day period in a sandy loam with 2.2% OC moistened to field capacity and pH 4.8, rate is fast initially, then levels off (Mallik et al. 1981)

no degradation in 2 days in a si 1 t loam (Tate and A1 exander 1976)

N-Methoxymethanamine

H3COCH2NH2

CAS No.

Compound not found in the literature.

CAS NO. 591-22-0

Synonym: 3,5-lutidine

Boi 1 ing Point: 171°C (Buckingham 1982, V2:2217)

Moderately soluble in water (Buckingham 1982, V2:2217)

Density: 0.942 at 20°C (Grasselli and Ritchey 1975, IV:p3725)

Morpholine

CAS NO. 110-91-8

Synonyms: tetrahydro-2H-1,4-oxazine diethylene imidoxide diethylene oximide

KO/,: 0.138 (Hansch and Leo 1985)

Water Solubi 1 ity: miscible (Nieneker 1971; Riddick et a1 . 1986) Henry's Law Constant: 1.41 x atm*m3/mol at 25OC (Syracuse Research Corp.

1988) cal cul ated val ue

Degradation Rate: t1/2 >>I4 days (only 2% degraded in 14 days) in river mud, pH=7.5 at morphol ine conc. of 10-100 mg/L (Calamari et al. 1980)

A.9 HALIDES

F, C1, Br, or I

Dichlorofluoromethane

C1 2CHF

CAS NO. 75-43-4

Synonyms: Freon 21 algofrene type 5 arcton 7 dichloromonofluoromethane genetron 21

Heavy, colorless gas

Boiling Point: 8.g°C

Me1 ting Point: -135OC

Vapor Pressure: 2 atm at 28.4OC

Vapor Density: 3.82 compared to 1.00 for air

Use: refrigerant (Sax and Lewis 1989)

Water Solubi 1 i ty: insoluble (Grassel 1 i and Ri tchey 1975, I11 :m326)

Tetrachloroethylene

CAS NO. 127-18-4

Synonyms: ethylene tetrachloride perch1 oroethyl ene

2,512 (Hansch and Leo 1979) KO'w: 400 (Munz and Roberts 1987)

Soil Sorption: Willamette silt loam; 3.3% sand, 69% silt, 26% clay, 1.6% organic carbon content; isotherms are linear, Freundlich 1/N is 1.0; calculated Koc was 210 (Chiou et al. 1977)

Materi a1 s Sorption Sediment Sorption: 1. Granular bentonite clay 10% in 10 min "

2. Dolomite limestone Sl ight 3. Ottawa sand None 4. Peat moss 40% in 10 min (Dilling et al. 1975) in 1 mg tetrachloroethylene/L influent, 25OC, closed system.

Lincoln fine sand, 92% sand, 0.087% organic carbon, CEC of 3.5 meq/100 g pH 6.4, 20°C; Freundlich adsorption was 0.2, KO, calculated at 200, retardation factor of 2.5 (Wilson et al. 1981).

Water Sol ubi 1 i ty: 200 mg/L at 25'~ (Coca and Diaz 1980) 150 mg/L (Strenge and Peterson 1989)

K O 238 at 25OC (Friesel et al. 1984) 360 (Strenge and Peterson 1989)

Henry's Law Constant: 1.84 x atmoY 3/mo1 at 25OC (Munz and Roberts 1987) 2.6 x atmom /mole (Strenge and Peterson 1989)

Degradation Rate: t1/2 = 300 days based on field observations in soi 1 /groundwater (Dragun 1986)

t1/2 = 13 days in lab when soil inoculated with microbial flora (Dragun 1986)

Chloroform

CAS N O . 67-66-3

Synonym: Trichloromethane

K 0 l w : 93.3 (Chiou e t a l . 1977) 93 (Strenge and Peterson 1989)

Freundlich 1/N: 0.77 t o 0.95 (Hutzler e t a1 . 1983) (sands, sandy loam, loamy sand and s i l t loam); no apprec iable so rp t ion on s o i l s of lower organic carbon content .

Soi 1 Sorpt ion: Retardat ion f a c t o r 4 . 5 (Wilson e t a1 . 1981) ; column movement per day in Lincoln f i n e sand was 41% in e f f l u e n t , 54% v o l a t i l i z e d , 5% degraded with 0.90 mg CHC13/L; 31% in e f f l u e n t , 61% v o l a t i l i z e d and 8% degraded with 0.25 mg CHC13/L i n f l u e n t ; Lincoln f i n e sand organic content was 0.087%, 92% sand, 5.9% s i l t and 2.1% c l a y , CEC was 3.5 meq/100 g.

Water Sol ubi 1 i t y : 7.95 g/L a t 25OC (Chiou e t a1 . 1977; MacKay e t a1 . 1980), 8.00 g/L a t 25OC (Wilson e t a1 . 1981) 10.62 g/L a t O°C (Deshon 1979) 8 .2 g/L (Strenge and Peterson 1989) 7.9 t o 8.2 g/L a t 20' (MacKay and Shiu 1981).

K O 80 (Wilson e t a l . 1981) 31 (Strenge and Peterson 1989)

Henry's Law Constant: 3.67 x lom3 atm* 3/mol (Gossett 1987) 2.9 x y/mol Strenge and Peterson 1989) 4 3.8 t 0.3 x a 3 atm*m lmol (MacKay and Shiu 1981)

Melting Point : -63.5OC (MacKay and Shiu 1981)

Boil ing Point : -61.7OC (MacKay and Shiu 1981)

Vapor Pressure: 2.0 t o 3.3 x lo1 kPa (0.2 t o 0.3 atm a t 20°C) (MacKay and Shiu 1981)

Methylene Chloride

CAS N O . 75-09-2

Synonyms: dichloromethane methyl ene dichl o r i d e Freon 30

KO/,: 17.38 (Hansch and Leo 1985) 20 (Strenge and Peterson 1989)

Materi a1 s Sorpt ion Sediment Sorpt ion: 1. Granular ben ton i t e c l ay 10% in 10 min

2. Dolomite limestone Sl i g h t 3. Ottawa sand None 4. Peat moss 40% in 10 min (Dil l i n g e t a l . 1975)

Water S o l u b i l i t y : 13.7 g/L a t 2 0 ' ~ (Horvath 1982) 20 g/L (Strenge and Peterson 1989) 16.7 g/L (Verschueren 1983)

K O 28 (Sabl j i c 1984) 8.8 (Strenge and Peterson 1989)

Henry's Law Constant: 2.19 x atm*y 3/mo1 (Gossett 1987) 2.0 x atm*m lmol (Strenge and Peterson 1989)

Degradation Rate: t 1 / 2 = 35 t o 50 days a t 5 mg/L present in Rhine River (Zoeteman e t a l . 1980)

t 1 / 2 = 3.3 days (Strenge and Peterson 1989)

Degrades r ap id ly under anaerobic s o i l cond i t ions (Cline and Vis te 1985)

A.10 N I T R O COMPOUNDS

Methyl n i t r a t e

CAS NO. 598-58-3

Synonym: n i t r i c a c i d methyl e s t e r

Boi 1 i n g Po in t : 65OC (Buckingham 1982, V4:3930)

Dens i ty a t 25OC: 1.20 (Buckingham 1982, V4:3930) Vapor explodes upon heat ing H igh l y i r r i t a n t

Me1 t i n g Po in t : -82.3OC (Grassel 1 i and R i tchey 1975, I11 :n534)

Water Solubi 1 i t y : s l i g h t l y so lub le (Grassel 1 i and R i tchey 1975, I11 :n534)

Butyl nitrate

H3C (CH2) 30N02

CAS NO. 928-45-0

Synonyms: nitric acid butyl ester n-butylnitrate

Boi 1 ing Point: 136OC (Buckingham 1982, V1:938)

Flammable 1 iquid; reacts explosively with Lewis acids (aluminum chloride, boron trifluoride, etc.) (Sax and Lewis 1989, VII:642)

Water Sol ubi 1 ity: insoluble (Grassel 1 i and Ri tchey 1975, I11 :n530)

A . l l POLYHYDRIC ALCOHOLS

Two or more hydroxyl groups (may be substitutions for hydrogens).

Methoxydiglycol

H3COCH2CH20CH2CH20H

CAS NO. 111-77-3

Synonyms : 2- (2-methoxyethoxy) ethanol diethylene glycol methyl ether diethylene glycol monomethyl ether

Water Solubi 1 i ty: 25OC miscible (Kirk-Othmer 1983, 21:382-383)

Boi 1 ing Point: 1 atm 194OC (Kirk-Othmer 1983, 21 :382-383)

Vapor Pressure at 25OC: 0.024 kPa (Ki rk-Othmer 1983, 21 :382-383)

Freezing Point: -76OC (Ki rk-Othmer 1983, 21 :382-383)

Specific Gravity at 20°C: 1.021 (Ki rk-Othmer 1983, 21 :382-383) (see also Dow Chemical Co. 1981)

Methoxy t r i g l yco l

HOCH2CH20CH2CH20HCH2CH20CH3

CAS NO. 112-35-6

Synonyms : 2- [2- (2-methoxyethoxy) ethoxy] ethanol t r i e t h y l e n e g l y c o l monomethyl e the r methoxy t r i e t h y l e n e g l y c o l

L i t t l e i n fo rma t ion loca ted

Boi 1 i n g Po in t : 2 4 9 ' ~ (Grassel l i and Ri tchey 1975, 111: e532)

Butoxygl ycol

OHCH2CH20 (CH2) 3CH3

CAS NO. 111-76-2

Synonym: ethylene glycol mono-n-butyl ether same as 2-butoxyethanol (see page A.18)

Water Sol ubi 1 i ty at 25OC: miscible (Ki rk-Othmer 1983, 21 :384-385)

Boiling Point at 1 atm: 170°C (Kirk-Othmer 1983, 21:384-385)

Vapor Pressure at 25OC: 0.11 kPa (Ki rk-Othmer 1983, 21:384-385)

Specific Gravity at 20°C: 0 .go075 (Ki rk-Othmer 1983, 21 :384-385)

Butoxydiglycol

OHCH2CH20CH2CH20 (CH2) 3CH3

CAS NO. 112-34-5

Synonyms: 2- (2-butoxyethoxy) ethanol diethylene glycol monobutyl ether diethylene glycol mono-n-butyl ether

Degradation Rate: In sewage, biodegrades fast once the system acclimates to presence of the compound in some instances (results inconsistent) (in BIODEG summary database; no references cited)

Water Sol ubi 1 i ty at 25OC: miscible (Kirk-Othmer 1983, 21:384-385)

Boiling Point at 1 atm: 231°C (Kirk-Othmer 1983, 21:384-385)

Vapor Pressure at 25'~: 0.003 kPa (Kirk-Othmer 1983, 21 :384-385)

Specific Gravity at 20°C: 0.9553 (Ki rk-Othmer 1983, 21 :384-385)

Freezing Point : -68OC (Ki rk-Othmer 1983, 21 :382-383)

Ethoxytriethylene glycol

C2H50CH2CH20CH2CH20CH2CH20H

CAS NO. 112-50-5

Synonyms : 2- [2- (2-ethoxyethoxy) ethoxy] ethanol triethyleneglycol monoethyl ether ethoxytriethylene glycol

Degradation Rate: t1/2 >20 days (only 22% degraded after 20 days) in seawater spiked with 3-10 mg/L glycol (Price et al. 1974)

Little information located

Boiling Point: 256OC (Grasselli and Ritchey 1975, IV: t1388)

A.12 POLYNUCLEAR AROMATIC HYDROCARBONS

Benzene Rings w i t h Common Ortho Pos i t i ons

Phenant hrene /='\

CAS N O . 85-01-8

Synonym: i sometr ic with anthracene

K O 28,840 (Hansch and Leo 1985) 29,000 (Strenge and Peterson 1989)

Freundl ich 1/N: 1.0 (Karickhoff e t a1 . 1979), DOE Run and Hickory Hil l coarse s i l t s 3.27% and 2.78% organic carbon content , r e spec t ive ly , 20- t o 50-pm p a r t i c l e s i z e range, 20 mg phenanthreneImL, 25OC

Water S o l u b i l i t y : 1.15 mg/L a t 2 5 ' ~ (Schwarz 1977) 1.3 mg/L (Strenge and Peterson 1989)

Koc : 230,000 (Karickhoff e t a l . 1979) 140,000 (Strenge and Peterson 1989)

Henry1 s Law Constant: 2.28 x atm*m3/mol (Syracuse Research Corp. 1988) c a l c u l a t e value 1.6 x 10- 1 l m o Strenge and Peterson 1989) 4 4.0 t 0.8 xa:!'! atmom /mol (MacKay and Shiu 1981)

Melting Point: 10I°C (MacKay and Shiu 1981)

Boiling Point : 33g°C (MacKay and Shiu 1981)

Sol id a t environmental condi t ions

Vapor Pressure: 2.67 x atm (MacKay and Shiu 1981)

Adsorption: no adsorpt ion on bentoni te c l ay from seawater (Meyer and Quinn 1973)

Rd = 50 f o r sandy loam, pH 7.9, C E C = 10.10 meq/100g, OC = 0.5% (Sims e t a l . 1988)

Rd = 160 f o r sandy loam, pH 4.8, C E C = 6.35 meq/100g, OC = 0.94% (Sims e t a l . 1988)

Degradation Rate: in sandy loam, pH 7.9, p a r t i a l l y sa tu ra t ed (80%), t 1 / 2 = 16 days a t 900 ppm loading in s o i l (Sims e t a l . 1988)

in sandy loam, pH 4.8, p a r t i a l l y sa tu ra t ed (80%), t 1 /2 = 35 days a t 900 ppm loading in s o i l (Sims e t a l . 1988)

A.13 PHENOLS

Phenol

CAS NO. 108-95-2

Synonyms: c a r b o l i c a c i d phenic a c i d phenyl i c a c i d phenyl hydrox ide hydroxybenzene oxybenzene

K0lw: 28.84 (Hansch and Leo 1985) 29 (Gaffney e t a l . 1987)

Soi 1 Sorpt ion: No adsorp t ion i n s i 1 t y c l a y (Greskovich 1974), adsorbed main ly by s o i l humus (Mozheiko and Solod 1969), no adsorp t ion on kaol i n i t e o r mon tmor i l l on i t e w i t h 1 t o 100 mg phenol/L i n t h e i n f l u e n t (Luh and Baker 1970)

Capt ina S i l t Loam Palouse S i 1 t Loam (Scot t e t a l . 1983)

Percent sand Percent s i l t Percent c l a y C EC pH Temperature % Organic carbon Freund l ich adsorp t ion Freundl i c h 1 / N KO, c a l c u l a ted

No phenol adsorp t ion on g o e t h i t e (Yost and Anderson 1984). Phenol s o r p t i o n can vary s i g n i f i c a n t l y w i t h pH and s o i l f rom ox ide content-KO o f 16 (Boyd 1982). No adsorp t ion on a q u i f e r m a t e r i a l s (Ehol i c h e t a1 . 1982)

K O 14 (S t renge and Peterson 1989).

Water So lub i l i t y : 82.8 g/L a t 2 5 ' ~ (Southworth and Kel l e r 1986) 93 g/L (Strenge and Peterson 1989)

Henry's Law Constant: 3.33 x atm*g3/mol a t 2 5 ' ~ (Gaffney e t a1 . 1987). 4.5 x atm*m 1.01 (Strenge and Peterson 1989)

K O 103*46 based on Connect icut Lake sediments with 4.2 t o 10.2% OC (Isaacson and Frink 1984)

based on var ious s o i l s (Dragun 1986)

Biodegradation Rate: t 1 / 2 = 1 t o 2.2 days i n s i l t loams with 1.1 t o 3.6% o rgan ic carbon, pH 5.4, and an extremely low concent ra t ion of phenol (Sims and Overcash 1983)

t 1 / 2 = 0.11 t o 0.15 days (Sco t t e t a1 . 1982, 1983)

t 1 / 2 = el day i n s o i l suspensions when p re sen t a t 25-50 mg/L (Alexander and Aleem 1961; Alexander and Lust i gman 1966)

t 1 / 2 = -100 days when p re sen t in l a n d f i l l l e a c h a t e a t concen t r a t i ons between 30-90 p a r t s p e r t r i 11 ion (ng/L) in so i 1 s i n Okl ahoma (Dee1 ey e t a1 . 1985)

t 1 / 2 = 2 t o 3 days when p re sen t i n s o i l a t 100 mg/L conc. from o i l r e f i n e r y s e t t l i n g pond (Meyer e t a l . 1984)

t 1 / 2 = -5 days i n seawater when p r e sen t a t 3-10 mg/L added a s wastewater ( P r i c e e t a l . 1974) ( s ee a1 s o Baker and Mayf i e l d 1980; Haider e t a1 . 1974)

Tributy l Phosphate

CAS N O . 126-73-8

9,800 (Strenge and Peterson 1989) (ca lcula ted) * 10,100 (Saeger e t a1 . 1979)

Water Sol ubi 1 i t y : 280 mg/L (Strenge and Peterson 1989; Saeger e t a1 . 1979)

K O 6,000 (Strenge and Peterson 1989) ca l cu la t ed

Henry's Law Constant: 0.019 atm*m3/mol (Strenge and Peterson 1989) ca l cu la t ed

Degradation Rate: t 1 / 2 -4 t o 7 days in Miss iss ippi River water when concent ra t ion 1 mg/L (Saeger e t a l . 1979)

t 1 / 2 >67 days (Strenge and Peterson 1989)

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APPENDIX B

EXAMPLES OF HANFORD SEDIMENT COLUMN LEAKAGE OF ORGANIC

COMPOUNDS AND RADIONUCLIDES

APPENDIX B

EXAMPLES OF SEDIMENT COLUMN LEAKAGE OF ORGANIC

COMPOUNDS AND RADIONUCLIDES AT THE HANFORD SITE

This appendix lists examples of probable sediment column leakage of

organic compounds and radionucl ides. Only positive values (greater than the analytical detection 1 imi t) for organics and radionucl ides in the groundwater were used as indicators of sediment column leakage because inorganics are present in the groundwater naturally and may even be leached from the soil

column by the wastewater. Inorganic analytical results for the groundwater

samples were not, therefore, used in the following examples.

The distribution of major contaminants on the Hanford Site (Figure B.l) is given in Figure B.2. A single waste stream has not been identified with each disposal faci 1 ity because many faci 1 i ties have received several wastes or been taken in and out of operation one or more times. Several facilities

have, however, been associated with a single wastewater. For example, the

216-W-LCW crib has always received laundry waste waters from the 2724-W and

2723-W buildings.

The various specific disposal facilities are associated with the major

unconfined aquifer contaminants as shown in Figure B.2. Available data are

best used as indicative of the type of radionuclides leaking through the

sediment column. Cesium-137 and strontium-90 leakage is generally low; groundwater contains low activities in the tenths of a picocurie per liter to

less than 5 pCi/L. Tritium, on the other hand, is often present in quantities

as high as millions of picocuries per liter. Cobalt-60, ruthenium-106, and antimony-125 are often present at levels of 10 to 800 pCi/L. These leakage

levels generally agree well with the sediment column distribution coefficients expected for these radionuclides, as discussed in Section 5. In this

appendix, monitoring we1 1 locations relative to each disposal unit are given first, fol lowed by tables of the wastewater components analytical ly identified

in the groundwater. Organic components were generally low in concentration,

but methylene chloride and TOX (total organic halogens) values can

occasionally be found into the 10,000-ppb range. The period during which

these samples were taken was March 1985 to March 1989.

Our presumption is that the detection of organics and radionuclides in

the monitoring wells is an indication that liquid disposal in the designated

facility (or a neighboring one) has lead to the migration of the designated

constituents to the upper unconfined aquifer.

ARID LAND ECOLOGY RESERVE

CITY OF RICHLAND

SADDLE MOUNTAIN NATIONAL WILDLIFE REFUGE

WASHINGTON STATE DEPARTMENT OF CAME RESERVE

FIGURE B-1. Hanford S i t e

CC1 = carbon tetrachloride TCE = 1 , 1 , 1-trichloroethane; tetrachloroethylene CHC13 = chloroform CN = cyanide

FIGURE 8-2. Distribution of Major Contaminants in the Unconfined Aquifer at the Hanford Site

\ 1324=N/NA PERCOLATION

SUFACE - 11-

FIGURE B.3. Monitoring We1 1 Locations at 1324-N/NA Pond

TABLE 0.1. Sediment Column Leakage of Waste Components Disposed to 1324-N/NA Pond (120-N-1)

Monitoring We1 1 Organics Identified in Groundwater

199-N-58 Methylene chloride, TOX 199-N-59 Chloroform, TOX

199-N-60 Chloroform, TOX

199-N-61 Chloroform, Bis (2-ethyl hexy1)phthal ate, TOH

Radionuclides Identified in Groundwater

199-N-58 None

199-N-59 None

199-N-60 None

199-N-61 None

1325-N C R I B

FIGURE B.4. Monitoring Well Locations around 1325-N Crib

TABLE B.2. Sediment Col umn Leakage of Waste Components Disposed to 1325-N Crib (120-N-2)

Monitoring We1 1 Organics Identified in Groundwater

Acetone, chloroform, TOX

Chloroform, TOX

Chloroform, TOX

Chloroform, TOX

Chloroform, bis (2-ethyl hexy1)phthal ate Acetone, chloroform

Methylene chloride, TOX

Acetone, methylene chloride, TOX

TOX

TOX

Radi onucl ides Identified in Groundwater

Cobalt-60, antimony-125, technetium-99, tritium

Antimony-125, cobalt-60, iodine-129, ruthenium-106,

strontium-90, tritium, technetium-99

Antimony-125, cobalt-60, ruthenium-106, strontium-90,

technetium-99, tritium

Cobalt-60, antimony-125, ruthenium-106, strontium-90,

technetium-99, tritium

Antimony-125, cobalt-60, iodine-129, ruthenium-106,

strontium-90, tritium

Antimony-125, cobalt-60, ruthenium-106, strontium-90, tritium

Cobalt-60, tritium Cobalt-60, tritium

Cobal t-60, technetium-99, tritium

Cobalt-60, ruthenium-106, tritium

WATW TABLE TO0 FLAT TO GBlWALIZE OROUID-WATER FLOW DIRECTION

FIGURE B.5. Mon i to r ing Well Locat ions a t 216-A-8 C r i b

TABLE B .3. Sediment Column Leakage o f Waste Components D i sposed t o 216-A-8 C r i b (216-A-8)

Mon i to r ing We1 1 Organics I d e n t i f i e d i n Groundwater

299-E25-6 None

299-E25-9 None

Radionucl ides I d e n t i f i e d i n Groundwater

299-E25-6 Ruthenium-106, t r i t i u m

299-E25-9 Ruthenium-106, t r i t i u m

( 200 EAST AREA + ,BOUNDARY

N 42.-

GROUNDWATER FLOW DIRECTION

299-E25.28 . . 299-E25-32

TANK FARM POND IN USE

POND NO LONGER IN USE

F I G U R E B.6. M o n i t o r i n g We1 1 L o c a t i o n s Around t h e 216-A-29 D i t c h

TABLE B.4. Sediment Column Leakage of Waste Components Disposed to 216-A-29 Ditch (216-A-29) /216-B-3 Pond

Monitoring We1 1 Organics Identified in Groundwater

299-E25-26 None

299-E25-28 TOX

299-E25-32 None

299-E25-34 TOX

299-E25-35 TOX

Radionucl ides Identified in Groundwater

Cobalt-60, cesium-137, ruthenium-106, tritium

Cesium-137, cobalt-60, ruthenium-106, technetium-99, tritium

Technetium-99, tritium

Tritium Tritium

WATER T M U T O 0 f U T TO OLNLR*LIlI OIIOUWD-WATER R O W OlRLCTlON --

FIGURE B.7. Monitoring Well Locations at 216-A-30 Crib

TABLE B.5. Sediment Column Leakage of Waste Components Disposed to 216-A-30 Crib (216-A-30)

Monitoring We1 1 Organics Identified in Groundwater

299-E16-2 None

299-E25-11 None

Radionuclides Identified in Groundwater

299-E16-2 Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

299-E25-11 Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

vS8, LOO

WATER TABLE TOO FLAT TO GENERALIZE GROUND-WATER FLOW DIRECTION

GROUND WATER MONITORING WELLS - 1

FIGURE B.8. Monitoring Well Locations at 2 1 6 - A - 3 6 B Crib

TABLE 0.6. Sediment Column Leakage of Waste Components Disposed to 216-A-360 Crib

Monitoring We1 1 Organics Identified in Groundwater

TOX

2-propanol , acetone TOX

Bis(2-ethyl hexyl)phthalate, methylene chloride, TOX

Acetone, methylene chloride, TOX

Trichlorofluoromethane

Radionuclides Identified in Groundwater

Carbon-14, cesium-137, cobalt-60, iodine-129, ruthenium-106, strontium-90, tritium

Cesium-134, cobalt-60, iodine-129, ruthenium-106, strontium-90, technetium-99, tritium

Cobalt-60, iodine-129, ruthenium-106, strontium-90, technetium-99, tritium

Cobalt-60, ruthenium-106, strontium-90, technetium-99, tritium

Cobalt-60, iodine-129, technetium-99, tritium

tritium

LEGEND:

GROUND-WATER MONITORING WELLS

FIGURE B.9. Monitoring Well Locations at 216-A-37-1 Crib

TABLE B.7. Sediment Column Leakage of Waste Components Disposed to 216-A-37-A Crib (216-A-37-1)

Monitoring We1 1 Organics Identified in Groundwater

299-E25-17 None

299-E25-18 Acetone, TOX

299-E25-19 Methyl ethyl ketone, TOX

299-E25-20 None

Radionucl ides Identified in Groundwater

Cesium-137, cobalt-60, strontium-90, tritium

Cesium-137, cobalt-60, ruthenium-106, strontium-90, technetium-99, tritium

Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

Cesium-137, cobalt-60, ruthenium-106, technetium-99, tritium

W A R I T M U TOO C U T TO aLI(1NUP O I O U ( I D W A T L I R O W OlMClWM

FIGURE 0.10. Monitoring Well Locations at 216-A-37-2 Crib

TABLE 0.8. Sediment Column Leakage of Waste Components Disposed to 216-A-37-2 Crib (216-A-37-2)

Monitoring We1 1 Organics Identified in Groundwater

299-E25-21 None

299-E25-22 None

299-E25-23 Styrene

299-E25-24 None

Radionuclides Identified in Groundwater

299-E25-21 Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

299-E25-22 Cesium-137, cobalt-60, ruthenium-106, technetium-99, tritium

299-E25-23 Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

299-E25-24 Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

LEGEND

GROUND-WATER MONITORING WELLS

FIGURE B. 11. Monitoring We1 1 Locations at 216-A-45 Crib

TABLE B.9. Sediment Column Leakage of Waste Components Disposed to 216-A-45 Crib (216-A-45)

Monitoring We1 1

299-E17-12 299-E17-13

Organics Identified in Groundwater None None

Radionuclides Identified in Groundwater

Cesium-137, cobal t-60, iodine-129, plutonium-239140, ruthenium-106, technetium-99, tritium

Cesium-137, cobalt-60, plutonium-239140, ruthenium-106, strontium-90, technetium-99, tritium

a 9 3 4 4 - 4 2 B POND

' h - A - 2 9 DITCH

a 216-0-3A POND

216-0-30 -qq 699-42-4OA AND B

216.0-3C

FIGURE B.12. Monitoring Well Locations at B Pond

TABLE B.lO.

Monitoring We1 1

699-42-40A

699-42-40B

699-42-42B

699-42-425

699-43-43

699-44-42

Sediment Column Leakage of Waste Components Disposed to B Pond System

Organics Identified in Groundwater

TOX

TOX

TOX

Acetone

TOX

TOX

Radionuclides Identified as Groundwater

Cesium-137, cobalt-60, ruthenium-106, tritium

Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

Tritium

Tritium

Tritium

Tritium

W A T U T U U TOO C U T TO O W U I L P I ~~OUI(D.WATU ROW oncmom

GROUND-WAT ER MONITORING WELLS

FIGURE B.13. Monitoring Well Locations At 216-B-55 Crib

TABLE 6.11. Sediment Column Leakage of Waste Components Disposed to 216-6-55 Crib (216-B-55)

Monitoring We1 1 Organics Identified in Groundwater

None

TOX

Radionuclides Identified in Groundwater

Cesium-137, cobalt-60, ruthenium-106, tritium

Cesium-137, cobalt-60, ruthenium-106, tritium

W A T L l l 1 I . U TOO N T TO 0 C . m - W A l U R O W DIII1CT)ON .

* ( GROUND-WATER MONITORING WELLS 1

FIGURE B.14. Monitoring Well Locations at 216-B-62 Crib

TABLE B.12. Sediment Column Leakage of Waste Components Disposed to 216-B-62 Crib (216-B-62)

Monitoring We1 1

299-E28-18

299-E28-21

Organics Identified in Groundwater

None

TOX

Radionuclides Identified in Groundwater

Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

FIGURE B.15. Monitoring Well at 216-S-26 Crib

TABLE B.13. Sediment Column Leakage of Waste Components Disposed to 216-S-26 Crib (216-S-26)

Monitoring We1 1 Organics Identified in Groundwater

299-W27-1 Chl oroform

Radi onucl ides Identified in Groundwater

299-W27-1 Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

I GROUND-WATER MONITORING WELL --I

FIGURE B.16. Mon i to r ing Well Locat ions a t 216-U-14 D i t c h

TABLE 6.14. Sediment Column Leakage o f Waste Components Disposed t o 216-U-14 D i t c h (216-U-14)

Mon i to r i ng We1 1 Organics I d e n t i f i e d i n Groundwater

299-W19-1 None

299-W19-21 None

299-W19-27 None

Radionucl ides I d e n t i f i e d i n Groundwater

Technetium-99

Cesium-137, plutonium-239/40, ruthenium-106

Ruthenium-106

21 6-U-17 CRIB

FIGURE B. 17. Mon i to r i ng We1 1 Locat ions a t 216-U-17 C r ib

TABLE B. 15. Sediment Col umn Leakage of Waste Components Disposed to 216-U-17 Crib (216-U-17)

Monitoring We1 1 Organics Identified in Groundwater

299-W19-19 None

299-W19-20 TOX

299-W19-23 None

299-W19-24 TOX

299-W19-25 None

299-W19-26 None

Radionuclides Identified in Groundwater

299-W19-19 Cesium-137, cobalt-60, ruthenium-106, strontium-90, technetium-99, tritium

299-W19-20 Cesium-137, cobalt-60, ruthenium-106, strontium-90, technetium-99, tritium

299-W19-23 Cesi um-137, pl utoni um-238, pl utoni um-239140, ruthenium-106, technetium-99, tritium

299-W19-24 Cobal t-60, pl utonium-238, pl utonium-239140, ruthenium-106, strontium-90, technetium-99, tritium

299-W19-25 Cesium-137, cobal t-60, pl utonium-238, pl utonium-239/40, ruthenium-106, technetium-99, tritium

299-W19-26 Cesium-137, cobalt-60, technetium-99, tritium

21 6-W-LCW CRIB

FIGURE B.18. Monitoring Well Location at 216-W-LCW Crib

TABLE B.16. Sediment column Leakage of Waste Components Disposed to 216-W-LCW Crib (216-W-LC)

Monitoring We1 1

299-W14-10

Organics Identified in Groundwater

None

Radionuclides Identified in Groundwater

Cesium-137, cobalt-60, ruthenium-106, strontium-90, tritium

299-W18-20

m I Z Q DIRECTION OF GRMMD-WATER ROI

299-W18-17

GROUND-WATER MONITORING WELLS I.

FIGURE 0.19. Monitoring Well Locations at 216-2-20 Crib

TABLE 0.17. Sediment Column Leakage of Waste Components Disposed to 216-2-20 Crib (216-2-20) t.

Monitoring We1 1 Organics Identified in Groundwater

299-W18-17 Acetone, carbon tetrachloride, TOX, chloroform 299-W18-18 None

299-W18-19 None 299-W18-20 None

Radionuclides Identified in Groundwater

299-W18-17 Cobalt-60, ruthenium-106, tritium

299-W18-18 Cesium-137, cobalt-60, ruthenium-106, tritium

299-W18-19 Cesium-137, cobalt-60, ruthenium-106, tritium

299-W18-20 Cesium-137, cobalt-60, ruthenium-106, tritium

GROUND-WATER MONITORING WELL

BERM

l k I(/ 12 W T E N CULVERT

21 01 -M POND (.-J J)q =I5?

m ' EFFLUENT l l l l m l DRAIN 5-n H I G Y BERM 1111R1

ESTIMATED FLOW DIRECTION

/ CORRUGATED

k-"lp€

- - -- DIRT ROAD

FIGURE B.20. Mon i to r i ng Well Locat ions a t 2101-M Pond

TABLE B.18. Sediment Column Leakage o f Waste Components Disposed t o 2101-M Pond

Mon i to r i ng We1 1 Organics I d e n t i f i e d i n Groundwater

299-E18-1 None

299-E18-2 Acetone, TOX

299-E18-3 TOX

299-E18-4 TOX

Radionucl ides I d e n t i f i e d i n Groundwater

None

None

None

None

Note a l l wells 399-x-x or 399-x-xx

I I 1 I 1 1 1 I l l I 1 1 1 I

- 8 - 1 'Welt Location

- 699-S29-€12 Wel l Location Outside 300 Area

- Fence

- Stevens Drive

FIGURE B.21. Monitoring Well Locations a t the 300 Area Process Trenches

I 1 I I I I I I I I I I 1

8-2 - - -

-

- 699-S19-El3 -

1-18 A,B,C-

El 5000 -

'-Process Water

- George Washington Way 1 ; -

699-S30-El54 - -

- . Columbia River

-

TABLE B.19.

Monitoring We1 1

399-1-1

Sediment Column Leakage of Waste Components Disposed to 300 Area Process Trenches (316-5)

Organics Identified in Groundwater Chloroform, methylene chloride, TOX

Chloroform, hexane, methylene chloride, tetrachlorethane, TOX

Chloroform, methyl ene chloride, TOX

Chloroform, methylene chloride, thiourea, TOX

Acetone, chloroform, methylene chloride, tetrachloro- ethylene, te t rae thy lpy rophosphate , TOX

2,6-bis(1,l-dimethylethy1)-4-methyl phen, chloroform, methylene chloride, phenol, TOX

Chloroform, methylene chloride, l,l,l-trichloroethane, 1,2-dichloroethane, TOX

Chloroform, 1,2-dichloroethane, methylene chloride, TOX, l,l,l-trichloroethane

Chloroform, TOX

Methyl ethyl ketone, TOX

Chloroform, methylene chloride, TOX

Acetone, chloroform, methylene chloride, TOX

Chloroform, methyl ethyl ketone, TOX

Methyl ethyl ketone, TOX, trans-1,2-dichloroethene, trichloroethylene

Trans-1,2-dichloroethene, trichloroethylene

Chloroform, l,l,l-trichloroethane, tetrachloroethylene, TOX

Methylene chloride, trans-1,2-dichloroethene, TOX

TOX

TABLE B.19. (contd)

Monitoring We1 1

399-1-18A Organics Identified in Groundwater

Carbon tetrachloride, methyl ethyl ketone

Methyl ethyl ketone

Methyl ethyl ketone

Chloroform, tetrachloroethylene, trichloroethylene, l,l,l-trichloroethane, TOX

Chloroform, methylene chloride, tetrachloroethylene, tetrahydrofuran, TOX

Chloroform, methylene chloride, trichloroethylene, TOX

Chloroform, methylene chloride, tetrachloroethylene, l,l,l-trichloroethane, TOX

Chloroform, TOX

Bis(2-ethylhexyl)phthalate, chloroform, methylene chloride, phenol, tetrachloroethylene, TOX

Acetone, chloroform, 2-hexanone, phenol, TOX, 1,12-trichloroethane, trichloroethylene

1,2-benzene dicarboxylic acid, chloroform, hexane, methylene chloride, phenol, TOX

Chloroform, TOX, trichloroethylene

TOX

Methylene chloride, phenol, tetrachloroethylene, TOX, l,l,l-trichloroethane

Chloroform, methylene chloride, TOX

Chloroform, methylene chloride, tetrachloroethylene, TOX, l,l, 1-trichloroethane

Methyl ethyl ketone, phenol, tetrahydrofuran, TOX

Radionuclides Identified in Groundwater

Cobalt-60, ruthenium-106, technetium-99, tritium

Cobalt-60, ruthenium-106, technetium-99, tritium

TABLE B.19. (contd)

Monitoring We1 1 Radionucl ides Identified in Groundwater

Cobal t-60, tritium

Cesium-137, cobalt-60, tritium

None

None

None

None

None

Tritium

Tritium

Tritium

Tritium

None

None

None

Cobal t-60, strontium-90

None

Tritium

Tritium

Tritium

None

Cobalt-60, technetium-99, tritium

Cobalt-60, strontium-90, ruthenium-106, technetium-99

Cesium-137, cobalt-60, tritium

Cobalt-60, strontium-90, technetium-99, tritium

TABLE B.19. (contd)

Monitoring We1 1 Radionuclides Identified in Groundwater

Cesium-137, cobal t-60, strontium-90, tritium

Cesium-137, cobalt-60, ruthenium-106, tritium

Cesium-137, cobalt-60, technetium-99, tritium

Tritium

Cesium-137, cobalt-60, ruthenium-106, tritium

Cobal t-60

Cesium-137, cobalt-60, ruthenium-106, tritium

Cesium-137, cobalt-60, ruthenium-106, tritium

Tri tium

400 AREA PERCOLATIO PONDS

N 1,650 -

FIGURE B.22. Monitoring Well Location at 400 Area Percolation Ponds

TABLE 8.20. Sediment Column Leakage of Waste Component Disposed to 400 Area Percolation Ponds (400 Area Process Pond and Sewer System)

Monitoring We1 1 Organics Identified in Groundwater

699-2-7 None

Radionuclides Identified in Groundwater

699-2-7 Tritium

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