Upload
others
View
1
Download
0
Embed Size (px)
Citation preview
71-4934
ARMITAGE, Donald Bruce, 1941-THE DETERMINATION AND DISTRIBUTION OFVARIOUS TRACE ELEMENTS IN NATURAL WATERS BYX-RAY FLUORESCENCE SPECTROSCOPY.
University of Hawaii, Ph.D., 1970Chemistry, analytical
University Microfilms, Inc., Ann Arbor, Michigan
MICROFILMED EXACTLY AS RECEIVEDTHIS DISSERTATION HAS BEEN
THE DETERMINATION AND DISTRIBUTION OF
VARIOUS TRACE ELEMENTS IN NATURAL WATERS
BY X-RAY FLUORESCENCE SPECTROSCOPY
A DISSERTATION SUBMITTED TO THE GRADUATE DIVISION OF THEUNIVERSITY OF HAWAII IN PARTIAL FULFILLMENT
OF THE REQUIREMENTS FOR THE DEGREE OF
DOCTOR OF PHILOSOPHY
IN CHEMISTRY
MAY 1970
By
Donald Bruce Armitage
Dissertation Committee:
Harry Zeitlin, ChairmanGeorge AndermannRobert A. DuceJohn J. NaughtonSidney J. Townsley
)
ii
ABSTRACT
A method was developed for the analysis, consecutively, of six
trace metals uranium, copper, nickel, cobalt, iron, and manganese in a
sample of fresh water and sea water through a combination of solvent
extraction with an 8-hydroxy quinoline-chloroform mixture and X-ray
fluorescence spectrometry. The primary concentration step which may be
carried out on board ship requires only three reagents and minimal
equipment, thus reducing the risk of contamination and chemical changes
due to storage. In addition, the method is nondestructive and extracted
samples evaporated on filter paper may be stored for future reference.
A pr~cision of 10% or better was obtained for the six elements with a
sample volume of 500 ml.
The analysis was applied to sea water and fresh water samples
obtained from various sources.
Coastal sea water trace element content was found to be lower than
that from mid-ocean. What appears to be significant differences in the
trace element levels were found in the water masses studied but little
variation with latitude was detected. Several of the elements, notably
uranium, displayed an increase in concentration with depth.
Examination of fresh water samples indicated that biological
activity is related to the extractable trace metal content in that
increased activity was accompanied by higher content or trace metals.
This view has as yet not been substantiated by biological studies.
Other samples showed evidence of differences which may be associated
with the water source and pollution.
TABLE OF CONTENTS
ABSTRACT •
LIST OF TABLES •
LIST OF ILLUSTRATIONS
INTRODUCTION •
EXPERIMENTAL •
Preliminary Studies •Final Analytical Method •
iii
ii
iv
vi
1
8
812
A.B.C.D.
Chemicals and ApparatusPreparation of Standards and Standard Curves •ProcedureDiscussion of Procedure
12132124
RESULTS AND CONCLUSIONS
Sea Hater DataFresh Water Data
SUMMARY
APPENDIX I. Method Using Dithizone-Ce11u1oseAcetate Pellets •
APPENDIX II. Calculation of Critical Depth for ChromiumX-Ray Radiation in the CelluloseAcetate Pellets •
APPENDIX III. Neutron Activation Detection Limits •
BIBLIOGRAPHY •
36
4061
68
70
71
73
76
Table
iv
LIST OF TABLES
I COMPARISON OF DETECTION LIMITS FOR X-RAYFLUORESCENCE, ATOMIC ABSORPTION SPECTROMETRY,AND NEUTRON ACTIVATION ANALYSIS • • • • • • • • • • • 0 10
II
III
IV
V
COMPOUNDS AND AMOUNTS USED IN PREPARATIONOF PRIMARY STANDARDS •• • • • • • • • • • • •
EXTRACTION EFFICIENCY OF THE 8-HQ-CHC13 SYSTEMFOR SPIKED SEA WATER SAMPLES • • • • • • • • •
EXTRACTION EFFICIENCY OF THE 8-HQ-CHC13 SYSTEMFOR SPIKED DEIONIZED WATER SAMPLES •• •
RELATIONSHIP OF SAMPLE VOLUME TO PERCENTEXTRACTION EFFICIENCY OF THE 8-HQ-CHC13 SYSTEM
· . . . . .4 • • • • •
· . . . . .
· . . . . .
14
25
26
27
VI RELATIONSHIP BETWEEN SAMPLE VOLUME AND PERCENTEXTRACTED BY EACH EXTRACTION STEP (8-HQ IS ADDEDIN THE FIRST AND THIRD STEPS) • • • • • • • • • • 28
VII
VIII
IX
X
XI
EFFECT OF TIME DELAY AFTER ADDITION OF 8-HQON EXTRACTION EFFICIENCY (PERCENT) ••••
PRECISION IN J.lG AND % FOR THE EXTRACTION METHODBASED ON EVAPORATED AND EXTRACTED STANDARDSFOR MAXIMUM AND MINIMUM AMOUNTS ANALYZED.AVERAGE PRECISION OF THE ACTUAL SEA WATER ANDFP~SH WATER ANALYSIS •• • • • • • • • • • •
A COMPARISON OF DATA FROM SEA WATER ANALYSES
VARIATION OF TRACE ELEMENT CONCENTRATION (j.1g/1)WITH POSITION (160 0 W) • • • • • • • • • • • • •
VARIATION OF TRACE ELEMENT CONCENTRATION (j.1g/1)WITH POSITION (125 OW) • • • • • • • • • • • • •
· . . . . .
· . . . . .
29
37
39
41
42
XII RESULTS OF SEA WATER ANALYSES (CONCENTRATION j.1g/1) 43
XII VARIATION OF TRACE ELEMENT CONCENTRATIONWITH DEPTH (160 0 W) ••••••••••• · . . . . . . . . 50
XIV VARIATION OF TRACE ELEMENT CONCENTRATIONWITH DEPTH (125 OW) ••••••••••• · . . . . . . . • 51
xv VARIATION CF,~RACE ELEMENT CONCENTRATIONWITH RESPECT TO WATER MASS (160 0 W) · . . . . . . . . 55
Table
XVI VARIATION OF TRACE ELEMENT CONCENTRATIONWITH RESPECT TO WATER MASS (125°W) · . . . . . . . .
v
57
XVII TRACE ELEMENT CONCENTRATION ABOVE, WITHIN,AND BELOW THE HALOCLINE • • • • • • • • • 59
XVIII
XIX
RESULTS OF FRESH WATER ANALYSIS(CONCENTRATION ~g/l) • • • • • •
COMPARISON OF ELEMENT TO IRON RATIO FORHAWAIIAN LAVAS, LAKE WAIAU, AND DOUGLASPERCHED WATER • • • • • • • • • • • • •
· . . . . . . . .
· . . . . . . . .
62
64
LIST OF ILLUSTRATIONS
Figure
vi
1
2
3
POSITIONS OF HYDROGRAPHIC STATIONS FORCOLLECTION OF SEA WATER SAMPLES • • • •
ISLAND OF HAWAII SHOWING LOCATION OF LAKE WAIAUAND DOUGLAS CINDER CONE • • • • • • • • •
LOCATION OF FRESH WATER SAMPLES FROMEASTERN UNITED STATES • • • • •
· . . . .
4
5
7
4 STANDARD CURVE FOR URANIUM INCLUDING BACKGROUND.SLOPE: 3350 COUNTS/~G/100 SEC. • • • • • • • •
5 STANDARD CURVE FOR COPPER INCLUDING BACKGROUND.SLOPE: 3410 COUNTS/~G/100 SEC. • • • • • • • •
6 STANDARD CURVE FOR NICKEL INCLUDING BACKGROUND.SLOPE: 3950 COUNTS/~G/100 SEC. • • • • • • • •
7 STANDARD CURVE FOR COBALT INCLUDING BACKGROUND.SLOPE: 3330 COUNTS/~G/100 SEC. • • • • • • • •
8 STANDARD CURVE FOR IRON INCLUDING BACKGROUND.SLOPE: 3000 COUNTS/~G/100 SEC. • • • . • • •
· · · · · 15
· · · · · 16
· · · · · 17
· · · · · 18
19
9
10
11
12
13
STANDARD CURVE FOR MANGANESE INCLUDING BACKGROUND.SLOPE: 2120 COUNTS/~G/100 SEC. • • • • • • ••
CONCENTRATION OF U~\NIUM, COPPER, AND NICKEL INRELATION TO DEPTH FOR COASTAL (---) ANDMID OCEAN (-) WATERS •••• • • • • • • • •
CONCENTRATION OF COBALT, IRON, AND MANGANESE INRELATION TO DEPTH FOR COASTAL (---) ANDMID OCEAN ( ) WATERS • • • • • • • • • • • • .
LOCATION AND DEPTH OF SAMPLES COLLECTED ALONG THEWEST COAST OF THE UNITED STATES (125°W).ISOHALINES ARE ALSO SHOWN WITH SALINITY IN 0/00 •
POSITION AND DEPTH OF SEA WATER SAMPLES COMPAREDTO MAJOR WATER MASSES (160 0 W). SALINITY IN °ioo
20
52
53
54
56
INTRODUCTION
The determination of trace elements in sea water is necessary to
study the geochemical properties and geographical distribution of these
elements. A method which permits the determination of a nU1TIDer of
elements in one sample of sea water without chemical separation and the
elimination of storage of sea water samples for shore analysis are most
desirous. When more than one element is determined a study Clf
relationships between elements and a comparison of the reactivities of
the elements in sea water are possible. If a single sample is used for
the analysis of all elements, then observed differences are due to
variations in reactivities not to sampling differences. Chendcal
separation of the elements can lead to contamination and loss problems,
as can storage of sea water samples.
Schutz and Turekian (29) have carried out geographical distribution
studies using neutron activation analysis but, because of interference
due to the activation of sodium chloride, extensive chemical
separations were necessary after activation. Freeze-drying was used as
the method of preconcentration. Only three elements, cobalt, nickel,
and silver, of the 18 elements analyzed are discussed in detail, because
of contamination and chemical problems.
Atomic absorption spectrometry has been used for the analysis of
sea water (3,15,19), but is not really a multi-element method. Sensitive
analysis for more than one element must be done using a separate source
lamp for each element and the appropriate lamp must be installed each
time a different element is analyzed. Problems also arise from flame
chemistry, such ass intereferences (both spectral and chemical) and
2
volatilization. Some elements, for example uranium, form refractory
oxides in the flame and thus are not volatilized, leading to high
detection limits. When atomic absorption is applied to sea water a
preconcentration-separation step is necessary to remove the trace
elements from the sea water matrix. Preconcentration is necessary
because many of the elements of geochemical interest are at or below the
detection li~its of the method. If sea water is aspirated directly into
the burner, the high solids content of the flame causes scattering of
the light source beam and leads to spurious results.
X-ray fluorescence spectroscopy is useful in multi-element analysis
because the relative simplicity of x-ray spectra yields few spectral
interferences, thus many elements can be determined without chemical
separations. Enhancement and absorption effects can be eliminated by
using a thin layer technique (10,20,23) and spectral interferences can
be predicted and easily corrected. The thin layer technique is
particularly adaptable to trace analysis. Since x-ray spectra do not
depend on the chemical state, the state need not be known in order to
perform an x-ray analysis.
X-ray fluorescence analysis has a lower detection limit of about
1 ppm, but the trace elements in sea water are in the ppb range and
therefore preconcentration by a factor of 1000 is necessary. Since sea
water contains about 3.5% dissolved solids, separation of the trace
constituents from the major constituents is also necessary.
Preconcentration-separation.tedhniques have been proposed by Natelson,
et ale (20) and Morris (18) for x-ray fluorescence analysis of sea
water. Both techniques are discussed in the Experimental section of the
3
thesis. X-ray fluorescence analysis requires only one excitation source
for the analysis of a large number of elements.
A preconcentration-separation method in conjunction with x-ray
fluorescence has been developed in this research and has been used to
make a distribution study of certain trace elements for the north
eastern Pacific Ocean. Samples were collected at various depths from
the major water masses along the 160 0 west meridian (Figure 1), as
dete~~ned by the Johns Hopkins Oceanographic Studies No.2 (28). They
were ~xamined to ascertain whether the trace element distribution can be
used as an indicator of the various water masses. Similar work has been
reported by Schutz and Turekian (29) for the world oceans for the
elements silver, nickel and cobalt.
Samples were also taken along the north western coast of the United
States (Figure 1). These samples permitted study of coastal effects on
trace element concentrations. As an example, a comparison of literature
values for uranium concentrations in open ocean (17) and coastal (1)
waters showed a marked decrease for coastal water.
The method was also applied to fresh water analysis and a number of
fresh water studies were carried out. The fresh water samples were
obtained from Lake Waiau (35), a small permanent lake at 3970 meters
elevation on the inactive volcano, Mauna Kea, on the island of Hawaii
(Figure 2). There is considerable interest in waters of this lake, as
it supports a large seasonal algal population (35) and its only source
of water is rain and snow. This study was focused on a comparison of
the trace element concentration of the water, concerning which there are
no data available, and the lava rock surrounding the lake. Weathering
o 10
CD 14
0 22
I I
FIGURE 1. POSITIONS OF HYDROGP~PHIC STATIONSFOR COLLECTION OF SEA WATER SM1PLES
4
5
FIGURE 2. ISLAJ'.m OF H...\"\.JAII SEOL-lING LOCATIONOF LAKE \vAI.AU (a) AND DOUGLAS CINDER CONE (b)
6
of the lava rock is considered to be a possible source for these elements.
Another sample studied was perched water obtained from the Douglas
cinder cone on Mauna Kea at about the same elevation as Lake Waiae
(Figure 2). Perched water is water held in an elevated position, in
this case, the depression at the top of the cinder cone. This "lake"
does not have an open surface. The water level is about 0.5 meters below
the top of the coarse material which makes up the cinder cone. The
reason for the water not rapidly draining away through the material of
the cone is not known. This sample was analyzed for comparison with
Waiau. Both bodies of water have the same environment and source of
water, but Waiau has a large seasonal algal crop and Douglas has very
little, because sufficient light does not penetrate to the water level.
Another group of samples originated from various sources in
western Pennsylvania and one sample from Lake Champlain (Figure 3). The
samples from Pennsylvania were drawn from the Shenango River Reservoir,
Conneaut Lake, Mahoning River, and a mountain spring about 20-30 miles
east of Knox, Pennsylvania. The Lake Champlain sample was obtained
about 2 miles north of Saint Albans Bay, Vermont. These samples were
analyzed to obtain the dissolved and particulate trace element content
and to compare these with the content of Waiau and Douglas.
UNITED STATES ,/
<(:
ATLAl[i'IC
/IcJ~)! ~~_
FIGmm 3. LOCATION OF FRESH HATER S.'!;"'1PLESFROM EASTEro~ UNITED STATES
a. La:<:e Champlainb. springc. Conneaut Laked. Shenango Reservoire. Mahoning River
7
EXPERIMENTAL
Preliminary Studies
Originally the Natelson Technique (20) or some modification was to
be developed into a useful method of analysis. This, however, did not
prove to be possible, although the technique did have some usable
features, especially the employment of a thin deposit on a filter paper
disk. A similar procedure has been used by other workers (10,16,23,27).
In the Nate1son technique, five milliliters of sea water were
evaporated to dryness and the residue mixed with one normal hydrochloric
aCid, glacial acetic acid, and acetic anhydride. The solution and
precipitate were mixed well, allowed to stand over night, and
centrifuged. The supernatant was evaporated to dryness and the residue
taken up in a methanol-hydrochloric acid mixture. The resulting solution
was evaporated as a spot on 37 rom filter paper using a ring over (20).
The glacial acetic acid-acetic anhydride reagent was used to
precipitate the sodium chloride from the sea ,vater and thus prevent
large sodium chloride deposits in the spotting step. Such deposits
interfered with the x-ray fluorescen~c ~lalysis by causing intense and
inconsistent scattering of the primary x-rays and, therefore aggravated
the background problem. It also reduced the sensitivity of the x-ray
method due to the thickness of the salt deposit on the disk. The
combination of chemicals used proved to be successful for the removal
of sodium chloride, but such salts as calcium chloride and magnesium
chloride are not removed (5,6). Sufficient quantities of these
materials were carried through to give hygroscopic deposits about one or
two millimeters thick which proved to be impossible to control with
9
respect to thickness, size, and shape.
An additional problem was the time involved in an analysis.
Although a number of samples were handled simultaneously, the total
process took about three days. Furthermore, the small volume of sea
water used created difficulties. Since the minimum detection limits
(Table I) of the x-ray method indicate that at least 100 milliliters of
sea water must be used to analyze with precision the elements involved,
the method could not be applied usefully to these elements. It was not
practical to increase the volume of the sea water used, since a 100 m1
sample would require the addition of 130 m1 of acetic anhydride and
would extend the evaporation time to days instead of hours. The method
was discarded because of these difficulties, but the use of the ring
oven was retained. Spots prepared with the help of the ring oven by
evaporating known volumes of methano1ic standard solutions, were very
useful in showing that thin deposits were of considerable value in
x-ray analysis.
It was decided because of the value of such deposits to employ a
method used in atomic absorption spectrometry in conjunction with x-ray
fluorescence. The solvent extraction of trace e1em8nts using ammonium
pyrro1idine dithiocarbamate (APDC) as the comp1exing agent and
methy1isobuty1ketone (MIBK) as the extracting agent has been used
successfully in atomic absorption work (3,15,19). The MIBK extract was
to be evaporated as a spot on the filter paper and then analyzed in the
x-ray instrument, but a problem was encountered in the deposition step.
The extract chemically attacked the filter paper making it very brittle,
to the extent that it fell apart when handled. Such fragility precluded
TABLE 1. COMPARISON OF DETECTION LIMITS FOR X-RAYFLUORESCENCE AND ATOMIC ABSORPTION SPECTROMETRY
AND NEUTRON ACTIVATION ANALYSIS
DETECTION LIMITS IN MICROGRAMSX-Raya Atomicb Neutronc
Element Fluorescence Absorption Activation
Uranium 0.014 180 0.002
Copper 0.026 0.030 0.005
Nickel 0.005 0.030 0.028
Cobalt 0.002 0.030 0.00005
Iron 0.005 0.030 0.28
Manganese 0.006 0.012 0.0005
aBased on experimental data for background andslope measurements, 1000 second counting time, and asignal one cr. greater than background.
bBased on detection limits given by Perkin ElmerCorp. for the 303 Atomic Absorption Spectrophotometerand the necessity of using 6 m1 of solution to analyzefor all 6 elements in the same solution.
cSee appendix III.
10
11
its use in the x-ray instrument. To rectify the problem removal of all
organics by evaporating the MIBK extract to dryness and oxidizing the
residue with nitric acid was attempted. The final residue could be
taken up in deionized water and spotted on filter paper. A publication
by Morris (18) appeared at this time which gave a similar solution to
the problem.
The published method although similar to the method just discussed
had some drawbacks. These involved need for pH adj ustment with the
attendant risk of contamination, the use of large amounts of APDC, the
requirement of special extraction equipment, and several evaporation
steps with risk of loss of metals by adsorption on the container walls.
Finally the method used by Morris (18) for presenting the sample to the
x-rays involved mixing a final residue with cellulose powder and
compression of the mixture into a 2.54 cm diameter pellet. Only about
one fourth to one third of the area of the pellet was excited by the
x-rays and penetration of the secondary x-rays was about 0.2 rom
(Appendix II), consequently, the method suffers from reduced sensitivity
since a portion of the sample is not excited.
·At this point an entirely different approach was attempted. Some
work by Carritt (4) apparently provided a method based on the use of
dithizone impregnated cellulose acetate columns for the removal of
certain trace elements from sea water. A complete description of the
column method developed is presented in Appendix I.
Although the method worked well with the standards, it could not
be applied satisfactorily to the analysis of sea water, since it did not
cover a wide enough concentration range. It worked well for zinc and
12
copper but poorly for iron and manganese and little, if at all, for
nickel, cobalt and chromium. It was then concluded, by calculation of
critical depth for secondary x-rays (Appendix II), that the method could
not be made sensitive enough for the determination of nickel, cobalt,
and chromium. Use of larger volumes of sea water would not help because
the added amounts of copper and zinc would necessitate larger columns.
For this reason there would be no gain in the metal to cellulose acetate
ratio, which was necessary to increase the sensitivity.
Following a study of the results of the calculations concerning
this problem and their significance when applied to pellets, it was
decided that thin deposits on the order of 0.1 rom were essential. The
sole method found to accomplish this was by spotting on filter paper
using the ring oven. This requirement plus the need to develop a method
sensitive enough to use in the analysis of the 120 to 240 m1 samples
available, led to the procedure finally adopted.
Final Analytical Method
The final method adopted some of the best features of the previous
work. Solvent extraction at the natural pH of sea water using a wide
spectrum extracting agent and a readily volatilized solvent were
required. The 8-hydroxyquinoline-Chloroform system fits these needs
well.
A. Chemicals and Apparatus
The chemicals used in the final method were redistilled reagent
grade chloroform, methanol, and 8-hydroxyquinoline (8-HQ). Analytical
13
reagent grade salts were used to make up standards for the elements
analyzed (Table II). Doubly distilled deionized water was used
throughout the entire work. Purified hydrochloric acid and aqueous
ammonia used for pH adjustment were made up as described in the
procedure.
The major pieces of equipment used were a kinetic clamp pump from
Sigmamotor, Inc., a ring oven fron Scientific Industries, Inc., and a
vacuum x-ray spectrometer equipped with a FA-60 tungsten target x-ray
tube and a lithium fluoride analyzing crystal from Norelco (Phillips
Electronics Instr.). Miscellaneous glassware and an 800 watt variable
hotplate were also used.
B. Preparation of Standards and Standard Curves
Standards were prepared by dissolving known quantities of reagent
grade salts of the metals in doubly distilled deionized water. A
concentration of one gram of metal per liter of standard was prepared
(Table II). Two liters of each standard were made.
The secondary standard was prepared by diluting a mixture of
appropriate volumes of primary aqueous standards to one liter using
reagent grade absolute methanol. Methanol was used for reasons
explained in the operation of the ring oven. This standard was stable
as long as it was protected from evaporation. The concentrations of
each element in the secondary standard were chosen to be: 2.00 pg/ml,
uranium; 10.0 Vg/ml, copper; 2.00 Vg/ml, nickel; 1.00 Vg/ml, cobalt;
5.00 Vg/ml, iron; 5.00 Vg/ml, m~~ganese.
Standard curves (Figures 4-9) were prepared by direct evaporation
of known quantities of the secondary standard solution on filter papers.
TABLE II. COMPOUNDS AND AMOUNTS USED INPREPARATION OF PRIMARY STANDARDS
GRAMSCOMPOUND per 2 liters
U02 (C2H302)2· 2H20 3.56
CuS04·SH20 7.68
NiS04·6H20 8.96
Co(N03)2·6H20 9.88
MnS04·H20 6.16
Fe (NH4) 2 (S04)2·6H20 14.04
14
500
'CJ 400 ,,.~oCJQ)CIl
HQ)Po 300 • ..0=
~:ICc.
----.~=! : ..c:~-,.. -"".£....-
200 ·f:>
CIl0/-1
§o
u100 ,~
~_J=_.=~....J~• ~.~<~L=_~~ ,
0.4 0.8 1.2 1.6 2.0
Micrograms of Uranium
FIGURE ll. STANDARD X-RAY FLUORESCENCE CURVE FOR URANIUH INCLUDING BACKGROUND.SLOPE 3350 COUNTS/~G/I00 SEC.
I-'VI
HQ)
P< 1200 la
'IJ 1600,....~otJQ)C/)
2000
....fl.- _~:-:.~r
800-'-~~-~" ---------~-••- ~.-l~-,~~j-""'~
C/).w§ou
400 I ...
_. v_I__-~ ..._.~ L.~_.~--L..
I 2.0 4.0 6.0
Micrograms of Copper
I ~
8.0 10.0
FJGURI.~ 5. STANDARD X-RAY FLUORESCENCE CURVE FOR COPPER INCLUDING BACKGROUND.SLOPE 3410 COUNTS/~G/100 SEC.
f-'
'"
150
120
'0l=l8 90<IJ(J)
).1<llp..
2l 60§o
u
7~
=!:5Pc u30
..._ ...~__~___ ,__ _\ I l J
f 0.4 0.8 1.2 1.6 2.0
Hicrograms of Nickel
FIGURE 6. STANDARD X-RAY FLUORESCENCE CURVE FOR NICKEL INCLUDING BACKGROUND.SLOPE 3950 COUNTS/~G/100 SEC.
l-'
'"
50
40
r-elP8 . 30''''Q)
Ul
HQ)p,
Ul 20·.j..J
§ou
10,-
=C'C:
:in6~
I 0.2
, L-~,_.. , __~_.-..:J
0.4 0.6 0.8 1.0
Hicrograms of Cobalt
FIGURE 7, STANDARD X-RAY FLUORESCENCE CURVE FOR COBALT INCLUDING BACKGROUND,SLOPE 3330 COUNTS/~G/I00 SEC.
I-'co
40 1- =-'..)=--<.,-c.. ,..;)_
J~-~, I I , ! II 1.0 2.0 3.0 4.0 5.0
200
160
rop
120 .-0tJQ)til
l--lQ)P<
til 80 ..-.jJ'p~0u
Hicrograms of Iron
FIGURE 8. STANDAPJ) X-l~Y FLUOP~SCENCE CURVE FOR IRON INCLUOING BACKGROUND.SLOPE 3000 COUNTS/~G/100 SEC.
I-'\0
15Q-
"0P8 9Q)l1J
HQ)p..
fl 60'-
Sou
30(..- T:2rC
/--J-:.c
-[ I J
LO 2.0
,__",-I_, ~~.L__
3.0 4.0----.J
5.0
Micrograms of Nanganese
FIGURE 9. STANDARD X-r-A.Y FLUORESCENCE CURVE FOR NANGANESE INCLUDING BACKGROUND.SLOPE 2120 COm~TS/~G/100 SEC.
No
21
By pumping directly from a 5 m1 buret, it was possible to measure very
easily the volume deposited on each filter paper. The buret was also
used to measure volumes of solution used in spiking both sea water and
fresh water for the determination of extraction efficiency.
Standards were checked by atomic absorption spectrometry using
independent standards prepared by dissolving known weights of the free
me ta1s • The uranium standard was checked by gravimetric means. A
known volume of the standard was treated with 8-HQ and the precipitated
uranium 8-hydroxyquinolate was dried and weighed. In all cases the
standards checked within experimental error (5%).
C. Procedure
If the sample to be analyzed was sea water, it was extracted
directly without pretreatment. ~e ~H' of a 1imno1ogica1 sample was
adjusted to between 7 and 9. If the pH exceeded 9, magnesium and
aluminum 8-hydroxyquino1ates were also formed and extracted (30), causing
difficulty in the spotting step by the formation of thick deposits. The
adj ustments of the pH were made with isopiestic hydrochloric acid and
aqueous ammonia, prepared using doubly distilled deionized water, to
avoid contamination.
(1) A 100 to 500 milliliter sample was placed in a separatory
funnel of appropriate size equipped with a Teflon stopcock and the pH
adjusted, if necessary, as described.
(2) One milliliter of 10% 8-HQ in methanol (w/v) was added to the
sample. This was mixed and allowed to stand for 5 minutes. The
solution was yellow at this point.
22
(3) Eight milliliters of chloroform were added and the mixture
shaken vigorously until there was a marked decrease in the yellow color
of the aqueous phase~ a change which required 10 to 15 seconds. After
the chloroform layer had separated, it was drained into a seven dram
glass vial. An additional 6 m1 of chloroform was added to the sample,
shaken, and drained into the vial. After the second extraction the
aqueous phase was colorless or milky white.
(4) Steps (2) and (3) were repeated and all extracts collected in
the glass vial.
(5) The combined extract was evaporated to dryness on a 70-80°C
hot plate by directing a gentle stream of air onto the surface of the
extract. This step required less time than the preparation and
extraction of the next sample. The total time for all work to this
point was on the order of 20-25 minutes. Three samples treated
together require an additional 10 minutes.
(6) The dried sample was sealed, before cooling~ in the glass vial
with a plastic cap which may be stored at least a month without change.
(7) The sample was dissolved in a minimum volume of chloroform
(1-2 ml). At this point, an internal standard of some metal not
extracted could be added as a methanolic solution, if desired. The
internal standard employed was one milliliter of a 1.00 ~g/m1
methanolic solution of Chromium (III) nitrate. The addition was found
subsequently, to be unnecessary and this step could be omitted, although
it was carried out for all samples.
(8) The sample solution was pumped by a kinetic clamp pump from
the glass vial througll Teflon tubing to a ring oven where it was
23
evaporated as a spot on 37 mIll #541 or #546 Whatman filter paper. The
glass vial was rinsed at least twice with chloroform. The pumping rate
was about 5-7 ml/hr and the ring oven was operated at a temperature of
160°C, at which temperature all unreacted 8-HQ was evaporated. At
temperatures as low as 80°C, 8-HQ evaporated readily but 160°C gave the
best overall results for spotting.
(9) The spotted filter disks were placed in 2 dram glass vials,
sealed with plastic caps. They may be stored indefinitely without
change if desired.
(10) The disks of the prescribed dimensions fit the sample holders
of the Norelco x-ray spectrometer. The following conditions for the
x-ray equipment were used for analysis: pulse height analyzer, window
25 volts, width-5 volts; tungsten target x-ray tube, 45 kilovolts and
45 milliamps, with a 0.002 inch titanium filter; scintillation counter,
1000 volts; and gas flow proportional counter, 1590 volts, with a P-10
gas flow rate of one standard cubic foot per hour. The spectrometer
was evacuated to 200 microns or better for all measurements.
The scintillation counter was used to measure the Loc radiation
intensity of uranium. The gas flow proportional counter was used for
all other elements, because the scintillation counter did not give
higher count rates. All samples were rotated at four revolutions per
minute for uniform exposure to the primary beam. The samples were
counted twice for 100 seconds and the average used. This time period
was found to give satisfactory results on the basis of counting
statistics.
24
D. Discussion of the Procedure
Complete extraction (95-100% of the elements concerned was achieved
for both fresh and sea water (Tables IV and III). There is a significant
relationship between sample volume~ e1ement~ and 8-HQ concentration
(Table V). In the case of manganese~ it was necessary to increase the
8-HQ concentration for sample volumes larger than 150 milliliters.
Although two additions of 8-HQ together with four chloroform
extractions are recommended by the procedure~ Table VI shows that 95% or
more recovery of the metals was realized in the first extraction with
one exception. Only 60-70% of the manganese was removed by the first
extraction with the remainder removed in succeeding extractions~ thus
necessitating multiple extractions.
The five minute time delay adopted in the extraction procedure was
shown to be necessary according to experiments summarized in Table VII.
Manganese~ again~ gave unexpected results for which there is no known
explanation.
In the primary evaporation step~ the vial was not permitted to
remain on the hot plate after the Chloroform had evaporated. If this
precaution was not taken most of the excess 8-HQ would also evaporate.
If this occurred~ it was doubtful whether all of the 8-hydroxyquino1ates
could be redissolved. These could be adsorbed on the glass in such a
Ban~er as to make redissolVing difficult. When they were suspended in
excess 8-HQ~ redissolving posed no difficulty. During the evaporation~
8-HQ was deposited as rings around the vial as the liquid level dropped.
After complete evaporation of the solvent~ the sides of the vial were
rinsed with a small amount of chloroform which, in turn~ was evaporated.
TABLE III. EXTRACTION EFFICIENCY OF THE 8-HQ-CHC13 SYSTEMFOR SPIKED SEA WATER SAMPLES
Element
llg added
llg recovered*
percent
Uranium
2.0
2.0
100
Copper
10
9.7
97
Nickel
2.0
2.0
100
Cobalt
l.0
l.0
100
Iron
5.0
5.0
100
Manganese
5.0
4.8
96
*Amount due to sea water has been subtracted.
NVI
TABLE IV. EXTRACTION EFFICIENCY OF THE 8-HQ-CHC13 SYSTEMFOR SPIKED DEIONIZED WATER SAMPLES
Element
~g added
~g recClvered
percent
Uranium
2.0
1.9
95
Copper
10
9.6
96
Nickel
2.0
2.0
100
Cobalt
1.0
1.0
100
Iron
5.0
4.9
98
Manganese
5.0
4.9
98
N0\
TABLE V. RELATIONSHIP OF S~IPLE VOLUME TO PERCENTEXTRACTION EFFICIENCY OF THE 8-HQ-CHC13 SYSTEM
Element Uranium Copper Nickel Cobalt Iron Manganese
Volume 500 97 96 100 100 96 45
in 250 100 95 101 100 98 80
Mi1lili ters 100 99 99 100 101 100 99
!'.'-....I
TABLE VI. RELATIONSHIP BETWEEN SAMPLE VOLUME AND PERCENT EXTRACTED IN EACH STEP(8-HQ IS ADDED IN THE FIRST AND THIRD STEPS)
Element .Urc¢ium Copper Nickel Cobalt Iron Manganese
Volume Step
500 ml 1 95 96 98 95 95 302 0 3 2 3 3 43 3 0 1 1 2 184 1 1 0 1 0 3
250 m1 1 96 96 97 97 96 502 0 4 3 3 3 43 2 0 0 1 1 204 1 1 0 0 0 5
100 ml 1 98 96 97 97 96 702 0 2 2 2 3 43 0 2 1 1 0 204 1 0 0 1 0 3
N00
TABLE VII. EFFECT OF TIME DELAY AFTER ADDITION OF 8-HQ ONEXTRACTION EFFICIENCY (PERCENT)
Element Uranium Copper Nickel Cobalt Iron Manganese
Time
in
Minutes
a
1
5
81
100
99
96
100
98
47
69
100
46
60
101
77
92
98
88
60
100
N\0
30
In redissolving, the smallest volume of chloroform possible was
used. One milliliter was usually sufficient. The smaller the volume
used, the shorter the time required for spotting. The same situation
also applied to the rinses.
The samples obtained from the primary evaporation step were stored
in the dark or in subdued light. Although the 8-hydro:h-yquinolates were
light stable, the 8-HQ in solution was somewhat unstable (30). The
stock solution was kept in a glass bottle, completely wrapped to exclude
light. All primary evaporation samples were kept in light tight boxes
of the type used to package light sensitive chart paper.
The kinetic clamp pump was very useful in the deposition step of
the method. Many schemes were tried to control the addition rate of
the samr"le solution, during this step. The problem was resolved
satisfactorily, through the use of the pump which allowed complete and
facile control of the rate. Such control was necessary for the
production of constant spot sizes using the ring oven.
The pump worked by repeatedly squeezing slugs of liquid through
resilient tubing. The rate of pumping was controlled by varying the
voltage to the direct current motor, which drove the pump.
Operation of the pump was very simple and the only difficulty
encountered was the selection of the type of tubing to be used in
pumping chloroform solutions. Gum rubber, silicone rubber,
polyvinylchloride, polyethylene, and Teflon tubing were tried. The
first three dissolved in chloroform to some extent. Polyethylene and
Teflon tubing worked well but Teflon was finally Chosen since it could
be rinsed more cleanly and more easily than polyethylene. When the
31
Teflon tubing was first tried in the pump~ it was crushed flat with
resultant loss of pumping ability following a few revolutions of the
pump. Since polyethylene had sufficient resiliency, a combination of
polyethylene and Teflon tubing was used. A short, 3 inch, section of
polyethylene tubing, 3/16 inch O.D. by 1/8 inch I.D., was slipped over a
36 inch piece of Teflon tubing, 3/32 inch O.D. by 3/64 inch I.D. The
polyethylene tubing was heated and stretched lengthwise about 100%. The
stretching caused it to shrink snugly to the Teflon, imparting the
necessary resiliency to the Teflon tubing. The combination of
polyethylene and Teflon tubing so constructed was used for pumping about
400 samples and still worked efficiently.
The ring oven was essential, since, with its use, reproducible spots
were formed. The construction of the ring oven has been discussed by
others (20). It consisted of a set of thermostatically heated rings
between which the filter paper was placed. As the solution was deposited
in the center of the filter paper and rings, it spread toward the hot
rings and evaporated before reaching them. This resulted in the
dissolved material being deposited in a spot about 1 cm in diameter in
the center of the filter paper.
The only variables in the operation of the ring oven were
temperature of the rings~ flow rate of the solution to the oven and flow
rate of the air through the central tube. The following set of
conditions gave optimum results: a temperature of 160°C, a solution
flow rate of 5-7 m1/hr, and an air flow rate which just caused the
filter paper to flutter but not float without the upper ring in place.
If the spot appeared to be too large or small, the solution flow rate
32
was adjusted with the pump. The rinses were deposited at about double
the rate of the initial solution.
X-ray fluorescence, which was used to complete the analytical
method, is usually not the method of choice for trace analysis. In
x-ray fluorescence the x-rays from the sample are excited by x-rays of a
shorter wavelength from another source. The intensity of such x-rays
is about 0.001% that obtained in electron excitation and as a result,
x-ray fluore~cence is usually not useful below the parts per million
(p.p.m.) range. Since the metals analyzed were in the parts per billion
(p.p.b.) range, it was necessary to concentrate the metals at least a
factor of a thousand to apply x-r~y fluorescence. The extraction method
already discussed more than met this requirement with a concentration
factor of about fifty thousand. This factor was based on a final
concentration in the filter paper of 0.5 parts per thousand (p.p.t.) with
the initial concentration in solution of 1 p.p.b.
X-rays arise when an inner shell electron is ejected from an atom
by a high energy electron or photon. The K~ series which was used for
all elements analyzed except uranium arises when an electron is ejected
from the K shell and this hole is filled by the transfer of an electron
from the L shell to the K shell. The energy change in the transfer is
released as an x-ray photon with energy equal to the difference between
the initial and final energy states of the transferred electron. The L
series arises from the ejection of an electron from the L shell and
subsequent filling of this hole by an electron from a higher shell. The
L~ line was employed in the analysis of uranium because the x-ray tube
used would not produce x-rays of sufficient energy to excite the ~
33
radiation of this element. The La: line is also the most intense line of
the L series.
The siQplicity of x-ray spectra provides little possibility for
spectral interference. Examination of the literature (18,20) discloses
that the only possible interference was that of the chromium Ke line
with the manganese Ka: line. Since the chromium Ke line could not be
resolved from the manganese Ka; line, it added to the manganese peak.
Chromium was not extracted under the conditions described and when added
as an internal standard, it was present in a constant amotmt,
consequent:y, its Ke radiation is constant and could be included in the
manganese background. The Ke line of an element is less intense than
the Ka: line and therefore the chromium Ke 'twuld only add. an average of
2 counts per second to the manganese backgrotmd, which is insignificant.
The maj or source of trouble in x-ray fluorescence analysis in any
analysis is the background. An increase in the background causes an
increase in ~he absolute uncertainty of the background measurement and
thus decreasing the sensitivity. In the case of most x-ray tubes the
target metal is not pure. Because of these impurities the primary
x-rays include not only lines characteristic of the target metal but
also those of the impurities. The tungsten target tube used showed such
lines for copper, nickel, manganese, and iron. A titanium filter in
the primary beam has been found very useful in decreasing such radiation
(20) • For this purpose, two layers of 0.001 inch titanium foil were
taped directly over the exit window of the x-ray tube. Both thicker~
0.005 inch, and thinner, 0.001 inch, filters have been tried by other
workers (1&,20), but the above thickness was found most effective.
34
A major advantage of the final method is the possibility of
extracting samples on board ship, as they are collected. This
eliminates or greatly reduces such problems as adsorption and desorption
of the species of interest on the container walls, biological activity,
and speciation changes, which arise when sea water is stored for shore
analysis. The method requires only simple equipment, few reagents, and
relatively little time is required to accomplish the extraction and the
primary evaporation. Such conditions are very important in ship board
work. Since the dried material obtained from the primary evaporation is
stable, sea water samples can be extracted and the dried material stored
at sea with final analysis performed ashore.
Another advantage inherent in the method is the low probability of
contamination, because few reagents are involved and no pH adjustment
or buffering are necessary.
The extraction method also does not limit the final analytical
method to x-ray fluorescence. Both atomic absorption spectroscopy and
neutron activation C~l be used, although the former is not as sensitive
on an absolute quantity basis as x-ray fluorescence (Table I).
When x-ray fluorescenc~ is used for the final analysis, other
advantages become evident. The excess 8-HQ is evaporated during the
spotting step along with the solvent, resulting in a thin deposit. The
thickness of these deposits, therefore, depends on the amount of metal
8-hydroxyquinolates extracted from the water sample and not on the
amount of 8-HQ used in the extraction.
Standards are prepared by spotting known volumes of standard
methanolic solutions of the elements of interest on filter papers.
35
Methano1ic solutions are used because they evaporate readily in the ring
oven where aqueous solutions evaporate only slowly due to the high heat
of vaporization of water. Filter papers spotted this way can be used
for standards because x-ray spectra do not depend on the chemical state
of the elements. The reagents used in the analysis do not add to the
background, consequently, the background is the same for both extracted
and direct deposition standards.
Finally, samples analyzed by x-ray fluorescence are not destroyed
nor become radioactive, and can be analyzed and stored for future
reference.
There are, of course, some disadvantages, which are not major. A
troublesome problem is the fact that the chemical speciation of the
elen~nts in sea water is in doubt. This leads to the basic question of
whether all of a certain element present in the sample is extracted or
extractable. This problem is taken up in the discussion of results.
A final difficulty, which can be avoided by careful choice of
sample volume, arises if excessively large amounts (hundreds to
thousands of micrograms) of 8-hydroxyquino1ates are deposited during the
spotting step. In this event, the layer can no longer be considered
thin and the releation between the amount of metal present and the x-ray
intensity will not be linear.
RESULTS AND DISCUSSION
The method as finally developed was capable of analyzing sea water
and fresh waterfor uranium, copper, nickel, cobalt, iron, and manganese.
Table I gives the minimum detection limits for x-ray analysis of
the elements involved. These limits are based on a 1000 second counting
time and a signal at least one (J greater than background. The background
and slope measurements necessary for the determination of the detection
limits were obtained from the standard curves. One thousand seconds was
used as a maximum counting time because it is consistent with both short
term and long term drift of the instrumentation (12).
The precision of this method depends on the element and the amount
of the element analyzed. The precision was determined by analyzing a
series of samples prepared by direct evaporation of methano1ic standards,
extracting spiked sea water, and extracting spiked deionized water. The
first two consisted of five groups of five replicates with a
concentration range for each element the same as that shavln in the stand
ard curves (Figures 4-9). The final series consisted of three groups of
five replicates over the same concentration range. The precisions
calculated for each series were the same. within experimental error.
The data are summarized in Table VIII. The first two rows of the
table give the precisions at the maximum and minimum levels of the
analysis described above. The other two rows give the precisions at the
average levels of the sea water and fresh water analysis.
In the actual determinations of the 120 ml and 240 m1 sea water
samples, a precision of 10% was obtained for copper, nickel, iron, and
manganese, out a precision of 20% and 30% was obtained for uranium and
TABLE VIII. PRECISION IN ~g AND % FOR THE EXTRACTION METHOD BASED ON EVAPORATED ANDEXTRACTED STANDARDS FOR MAXIMUM AND MINIMUM AMOUNTS ANALYZED.
AVERAGE PRECISION OF THE ACTUAL SEA WATER AND FRESH WATER ANALYSIS.
Elements Uranium Copper Nickel Cobalt Iron Manganese
Maximum 2.0±0.1 10.0±0.5 2.0±0 .1 l.0±0.05 5.0±0.25 5.0±0.255% 5% 5% 5% 5% 5%
Minimum 0.02±0.02 0.10±0.OB 0.02±0.01 0.01±0.01 0.05±0.04 0.05±0.05100% 80% 50% 100% 80% 100%
Average Precision 0.38±0.08 5.4±0.5 0.30±0.03 0.04±0.01 0.95±0.1 0.54±0.06for Sea Water 20% 10% 10% 30% 10% 10%Analysis
Average Precision 0.59±0.08 2.1±0.2 0.66±0.06 0.06±0.01 3.5±0.30 4.8±0.30for Fresh Water 15% 10% 10% 20% 9% 6%Analysis
VJ-...J
38
cobalt respectively. The reasons for the relatively poor precision of
uranium and cobalt are different. A 1-2% variation in the uranium
background can cause a 10-20% variation in the analysis result.
Variations in cobalt analysis are due to the very small amount of cobalt
analyzed (0.04-0.08 ~g). Consequently the slightest variation or
contamination will have a large effect at this level. Data are given
only to two significant figures because of the level of the precision.
Initial data were taken to four significant figures with all
calculations carried out to three.
Accuracy wC!s not known because the accuracy of a determination can
be measured only if the true value is known and, in the case of natural
water analysis, the true value is not known. Often accuracy is checked
by analyzing spiked samples. While such a check certainly applies to
the spike it contributes little about what is actually recovered from
the real system. The speciation of the spike is known but speciation in
the real system is not, especially, in the case of sea water. The
speciation of the spikes was chosen to match those given by Goldberg for
sea water (8). A check for nonextractable higher oxidation states of
analyzed elements was made by the addition of hydroxylamine hydrochloride
to sea water to provide a reducing environment. Such an environment
insured that the elements nickel, cobalt, and manganese were in the +2
oxidation state. No increase in the recovery of the metals from sea
water was noted and, thus, higher oxidation states are apparently not a
problem in the extraction of these metals.
Table IX shows the average sea water values for this analysis and
the values obtained by other workers. In the case of uranium, an
TABLE IX. COMPARISON OF DATA FROM SEA WATER ANALYSES
PRESENT WORK PREVIOUS WORKELEMENT Concentration Concentration
Location }lg/l .Location llg/l Reference
Uranium North Central 3.3 Northwest Pacific 3.3 (17)Pacific (NCP) NCUS 1.9 ( 1)
Northwest Coast of 1.7 Oceanic Average (OA) 3 ( 8)United States (NCUS) OA 3.3 (11)
Copper NCP 35 Southeast Pacific 36 (34)NCUS 29 OA 23 (11)
OA 3 ( 8)
Nickel NCP 3.2 OA 5.4 (29)NCUS 1.1 Long Island Sound 2.1 (29)
OA 6.6 (11)OA 2 ( 8)
Cobalt NCP 0.24 OA 0.27 (29)NCUS 0.13 Long Island Sound 0.048 (29)
OA 0.39 (11)OA 0.10 ( 8)
Iron NCP 6.1 OA 3.4 (11)NCUS 5.4 OA 10 ( 8)
Manganese NCP 16 OA 1.9 (11)NCUS 1.9 OA 2 ( 8)
W\0
40
estimate of the accuracy could be made by comparison with published
values (1,8,17). Good agreement, within 5%, for the overall averages of
uranium in both mid ocean and coastal waters was obtained. Other
elements were not as easily compared because there is little agreement
of literature values (8,29). Copper values are high compared with
Goldberg (8) but a paper by Whitnack (34) gives values in good
agreement for deep water. The high values for manganese in the mid
ocean are unique and could possibly be explained by the dissolving of
particulate manganese during the long storage of the samples prior to
analysis. Contamination is not believed to be the cause since all
samples were treated identically and the mid ocean manganese values
were the only high values.
Sea Water Data
Tables X - XII and Figure 1 give the position, depth and
concentration found for each element for all sea water samples. The
most notable information obtained from these tables is the difference
between the mid ocean samples (160 0 W) and the coastal samples (125°W).
Coastal samples have 10-50% lower concentrations, depending on the
element,. than the mid ocean samples. The diffe~ence might be
attributed to a relationship between sample volume and extraction
efficiency as the volumes also differ by about 50%. Table V shows that
this is not the case. Although there is a difference for manganese, it
can be eliminated as described earlier in the discussion of the final
method. Contamination is not the cause, for the values are lower not
higher than values found for mid ocean samples. The literature (1,17)
TABLE X. VARIATION OF TRACE ELEMENT CONCENTRATION (~g/l)
Location Station fI Uranium Copper Nickel Cobalt Iron Manganese
53 0 48.1' N 163 0 30.0' W 2 3.0 43 2.2 0.36 12 11
51 0 44.0' N 161 0 08.5' W 10 3.1 37 3.2 0.37 9.0 23
45 0 57.9' N 160 0 28.0' W 13 4.0 50 4.5 0.26 6.6 11
43 0 53.2' N 160 0 19.8' W 14 3.6 24 2.9 0.31 9.0 20
38 0 21.0' N 160 0 18.0' W 19 3.9 26 3.0 0.28 6.2 340
32 0 10.5' N 160 0 17.0' W 22 3.6 18 2.3 0.22 3.9 7.4
26 0 15.1' N 159 0 59.7' W 27 3.0 44 4.1 0.22 5.8 17
24 0 50.8' N 160 0 00.6' W 29 2.2 39 2.5 0.11 4.2 22
23 0 26.6' N 159 0 58.3' W 31 4.5 42 2.2 0.22 3.8 17
~
I-'
TABLE XI. VARIATION OF TRACE ELEMENT CONCENTRATION (~g/l)
-Location Station 11 Uranium Copper Nickel Cobalt Iron Manganese
42° 59.5' N 125° 00.8' W 163 1.7 32 1.2 0.14 5.6 2.0
44° 00.7' N 125° 00.0' W 164 1.6 34 1.2 0.11 5.6 1.2
45° 00.5' N 124° 59.5' W 165 2.0 31 1.2 0.18 5.3 1.7
46° 00.0' N 125° 00.0' W 166 1.5 23 0.99 0.11 5.3 0.49
47° 00.0' N 125° 00.0' W 167 1.8 32 0.90 0.16 5.2 3.2
48° 30.0' N 125° 00.0' W 168 1.4 24 1.0 0.16 6.1 1.3
~N
TABLE XII. RESULTS OF SEA WATER ANALYSES (CONCENTRATION ~g/l)*
Station /I Depth (m) Uranium Copper Nickel Cobalt Iron Manganese
2 sur 2.5 35 2.2 0.31 11 14
2 50 3.4 51 11 0.42 13 7.5
10 sur 2.7 21 2.0 0.27 8.1 22
10 400 3.1 62 4.9 0.27 9.1 21
10 1300 3.5 28 2.7 0.56 9.8 27
10 2500
13 sur 4.1 t.3 2.3 0.36 5.7 3.9
13 300 3.3 59 3.0 0.11 5.7 13
13 800 3.3 16 8.2 0.25 8.7 17
13 2500 5.2 81 4.4 0.32 6.2 10
ll. sur 3.8 38 3.4 0.52 7.2 50
ll. 400 3.0 30 3.0 0.25 11 7.5
14 800 4.3 12 2.7 0.28 6.9 1.7
14 2500 3.5 14 2.5 0.19 11 21.
.po
*See Fig. 1. w
TABLE XII. (Continued) RESULTS OF SEA WATER ANALYSES (CONCENTRATION ~g/l)*
Station II Depth (m) Uranium Copp~r Nickel Cobalt Iron Manganese
19 sur 2.6 25 2.9 0.36 8.2 44
19 500 2.6 17 2.6 0.25 7.4 18
19 800 4.3 10 3.2 0.13 4.8 20
19 2500 6.0 53 3.1 0.39 4.6 56
22 sur 5.5 26 3.1 0.18 4.6 5.7
22 400
22 600 2.5 6 2.2 0.25 3.5 10
22 2500 2.7 21 1.6 0.22 3.5 6.4
27 sur 2.2 16 LO 0.14 3.9 16
27 400 3.9 26 2.4 0.23 4.9 29
27 600 2.6 20 2.6 0.07 6.2 5.6
27 1900 3.5 82 7.2 0.42 9.1
27 2500 2.8 77 7.4 0.24 4.8 18
29 sur :.8 26 1.3 0.12 3.3 24
29 400 4.3 47 2.1 0.14 3.2 4.8.p-.p-
TABLE XII. (Continued) RESULTS OF SEA WATER ANALYSES (CONCENTRATION ~g/l)*
Station tI Depth (m) Uranium Copper Nickel Cobalt 'Iron Manganese
29 800 1.8 21 3.8 0.12 5.8 55
29 2500 0.8 61 2.8 0.07 3.9 4.7
31 sur 2.1 60 2.3 0.13 3.3 2.7
31 400 2.9 13 1.9 0.27 4.2 21
31 1300 5.8 16 1.8 0.22 4.0 41
31 2500 7.1 78 2.7 0.28 3.6 4.5
OVERALL AVERAGE 3.3 35 3.2 0.24 6.1 16~
163 sur 1.5 32 1.8 0.11 6.3 1.4
163 100 1.9 38 1.4 0.27 9.3 4.4
163 200
163 400 1.4 11 0.63 0.16 3.7 1.1
163 800 2.0 18 1.3 0.17 4.2 4.6
163 1000 1.4 34 0.80 0.08 3.4 0.22
163 1240 1.9 57 1.2 0.04 6.4 0.44~
164 sur 1.9 60 1.5 0.16 4.7 1.3 VI
TABLE XII. (Continued) RESULTS OF SEA WATER ANALYSES (CONCENTRATION ~g/l)*
Station 11 Depth (m) Uranium Copper. Nickel Cobalt Iron Manganese
164 100 1.6 19 1.3 0.07 5.0 2.7
164 200 2.0 31 1.3 0.05 6.2 1.2
164 300 1.4 51 1.2 0.09 5.1 0.32
164 400 L8 18 1.3 0.12 7.1 0.74
16Lf 790 1.0 18 0.80 0.14 5.7 2.0
164 940 L7 42 1.0 0.16 5.4 0.50
165 sur LO 50 0.89 0.15 3.9 2.8
165 100 1.9 24 0.64 0.15 5.2 1.9
165 200 1.4 19 0.34 0.13 4.5 0.21
165 400 1.5 16 1.5 0.10 5.0 1.0
165 700 2.3 51 2.5 0.32 8.4 13
165 940 4.0 27 1.1 0.24 4.8 2.5
166 sur 1.9 25 0.59 0.10 6.3 O. Lr5
166 100 1.3 7.7 0.77 0.13 6.0 0.91
166 200 0.8 25 0.45 0.10 4.9 0.49 ~0\
TABLE XII. (Continued) RESULTS OF SEA WATER ANALYSES (CONCENTRATION ~g/l)*
-Station It Depth (m) Uranium Copper Nickel Cobalt Iron Manganese
166 400 1.6 39 0.86 0.17 5.6 0.29
166 600 1.6 14 0.78 0.01 4.5 0.26
166 800 1.9 21 2.1 0.09 4.9 0.53
166 1000 1.4 27 1.4 0.11 4.7 <0.2
166 1240
167 sur 1.4 38 0.80 0.19 5.8 2.4
167 50
167 100
167 200 1.8 24 0.49 0.09 2.8 4.3
167 225 2.5 41 1.5 0.17 5.9 5.1
168 sur 1.1 21 0.46 ---- 4.4 1.2
168 50 1.4 32 1.6 0.18 6.1 1.6
168 78 1.6 20 5.0 0.15 7.8 1.1
OVERALL AVERAGE 1.7 29 1.1 0.13 5.4 1.9~(Surface values from 1-3 meters deep.) "
48
contains some evidence that a real difference could exist (Table IX).
No clear-cut mechanism has been proposed to explain the difference.
Jenne (13) proposed hydrous oxides of iron and manganese as a possible
control by coprecipitation for the amount of dissolved iron, manganese,
copper, cobalt, and nickel in soils and fresh water. River and stream
inputs from the Straits of Juan de Fuca and the Columbia River contain
these hydrous oxides and probably form more on mixing with sea water,
thus providing a source for the hydrous oxides. It seems likely
therefore, that the mechanism may also apply to sea water. Simple
dilution effects are not enough to explain the decrease. Salinity
changes only 1-10% but the element concentrations change from 10-50%
between coastal and mid ocean samples. The above mechanism may not
explain the entire decrease, as organic and sulfide complexing,
precipitation, and adsorption may also contribute to the removal. These
are thought to be the major factors in the removal of trace elements in
Long Island SOlIDd (29). Although no complete explanation is known, the
difference does exist according to the data and provides an opportunity
for further productive research.
Tables X and XI show how the trace element concentration varies
with latitude for each water column. The coastal and mid ocean samples
are treated separately because of the differences already discussed.
Little regular change with latitude is observed, but some trends are
evident. Iron and cobalt show a decrease with decreasing latitude for
the mid ocean samples. Changes are not observed for coastal samples
because of the relatively small area sampled (Figure 1). There seems
to be no correlation with latitude for any element from coastal
49
sampling.
Tables XIII and XIV show variation of concentration with depth.
There is a definite increase in uranium and nickel with depth for the
mid ocean samples (also see Figures 10 and 11). TIle other elements do
not show a regular variation with depth. The variation is still
evident for uranium in the coastal samples. Biological activity in the
form of incorporation of uranium in the calcareous tests of various
microorganisms (1,2) is the probable explanation for the uranium
variations. When the microorganism dies, its test sinks down the water
column and begins to dissolve (22). In dissolving it will release the
uranium and thus cause a transport of uranium from upper water levels to
deeper ones. Nickel is also concentrated by planktonic organisms (9)
and is released both through excretion and decomposition upon death of
the organism. The latter process could yield a net transport of nickel
from upper to lower water levels. Other metals, such as copper and
cobalt are also concentrated in organisms. It is not known why these
do not show similar trends.
Tables XV and XVI show concentration variations with water mass.
Figures 12 and 13 show samples in relation to water mass. Figure 12
was prepared from Johns Hopkins Oceanographic Studies No.2 (28).
Figure 13 was prepared by assembling data from a number of sources
(7,21,24,25,26). In the case of the latter figure, there is a time
-dependence for the water masses. From late spring until early fall,
the Columbia River plume extends out and then curves south along the
coast. It is separated from the coast by another coastal current (21).
In late fall to early spring most of the plume is blown north by the
TABLE XIII. VARIATION OF TRACE ELEMENT CONCENTRATION WITH DEPTH (160 0 W)
Depth in Elements concentration ~g/liter
Meters Uranium Copper Nickel Cobalt Iron Manganese
Surface* 3.0 32 2.3 0.27 6.1 20
50-400 3.2 35 3.5 0.22 6.7 14
500-1300 3.5 16 3.4 0.24 6.2 22
1900-2500 3.7 54 3.7 0.25 5.5 15
*Surface means 1 to 3 meters depth.
V1o
TABLE XIV. VARIATION OF TRACE ELEMENT CONCENTRATION WITH DEPTH (125°W)
Depth in ELEMENT (concentration in ~g/liter)
Meters Uranium· .COpper .. Nickel· .Cobalt .Iron Manganese
Surface* 1.5 38 1.0 0.14 5.2 1.6
50-100 1.4 25 1.5 0.14 5.8 2.1
200-400 1.6 28 0.97 0.12 5.1 1.5
600-800 1.7 25 1.5 0.16 5.5 4.3
900-·1200 1.9 33 1.1 0.11 4.4 0.70
*Surface means 1 to 3 meters depth.
VII-'
NickellJg/l 4
~=='r-~a ~""':'\..\'~...:.:; .
-'..J<->,4
\, -r-¢- ......'-=0,,,
n _~
o
500 [::2
1000
2000 f:.<o
2500
(J)}-lOJ.wOJ~
P.r! 1500 I."
.d.w~
A
2500
200) 1=
Copperpg/1
o 20 40o r ~" ...- "C'~=~~'-D::''':~~\'«}~='':''''''':
'-./,~r-
, ~ "'='
500(",. VA~-
.;-~.rc-.z....~!";%.;n~'","1000 [=..., \. -b-
1500 k~
(J)}-l(j).wOJ~
.~
-Ep,OJA
eu=-=-0....~-~~·
UraniumlJ8/ 1
024oI- -,,, ,c -_. -~--~_: c'-r- ~'OU'=-'\)=~~i!~-=-~/:~~
\'\
cr.?=-,:,--=q- \.
, cn=z={)~n,.",.n,~~
500
I2500 It."
1000 ,."
(J)
I}-lOJ.w I<V~,
l.~ 1500.d I.wp,OJ IA I
II
2000lr
FIGURE 10. CONcmfr:~TION OF URANIUM, COPPER, AND NICKEL IN RELATIONTO DEPTH FOR COASTAL (---) AND NID OCEAN (~) HATERS.
Intv
500 I=»
ar..:('-;'-'=.~u-~
o
15001=
2000["
·2500 '=>
UlHoJ~
...~.....,
.~
.r:i~
PIOJ
t=1
Ironllg/l
4 8oOJ""'"'-.."tt '·_~"'U~O;~~~~--'v L _. .,
--J-,,,,\r,
C'\.;~ I'._r,\.c.o:a-, '-'",
~~~
500 ~'u>
2000 htl
2500 0,
~ 1000 I'"OJ~
OJ;:E:
s::.,-j
.d J.500 1'0:>~
~t=1
Cobaltllg/l
o 0.2 0.4o r..,,~,~,u,~,,-,('.;n=U~l--=-'~-U~~
_ .. r\.a.;.»yI
-<in,
\-1-~,"-l.-
~"' r_~. ",,
2000 1=
-u-2500 c.,
~ 1000 (zo ~-d~-OJ~
qj::>-1
s::'d 1500 I','
.c~p.OJ
t=1
FIGURE 11. CONCENTRATION OF COBALT, IRON, AND MANGANESE IN RELATIONTO DEPTH FOR COASTAL (---) AND HID OCEAN (_) HATERS.
\JlW
Degrees North Latitude 54
_200
~r600
~t,.800
o
II
00o
~Llooo~
0 ,,!
I _2000
0 00 0
3000
o
o
Geo 0
000
20
~--O-C<J>--..:J-;:>-,-~~~-\
IV 1 VI 35.2
FIGURE 12. POSITION AND DEPTn OT? SEA T'!ATER SAHPLESCOHPARED TO THE MAJOR HATER Y~SSES
SALINIl:Y iN 0/00
TABLE XV. VARIATION OF TRACE ELEMENT CONCENTRATION WITHRESPECT TO WATER MASS (160 0 W)
S %0 Water ELEMENT cortcerttratiort"irtug/1iterRange Mass* Uranium Copper Nickel Cobalt ,
Iron Manganese
34.4-34.8 I 5.0±0.5 51±9 3.6±0.6 0.32±O.O3 6.0±0.9 21±5
34.0-34.4 II 3.4±0.3 26±6 3.6±0.6 0.23±0.03 6.2±0.7 24±5
33.6-34.0 III 2.8±0.1 26±8 2. 7±0.1 0.19±0.04 6.8±1.1 11±2
34.8-35.2 IV 2.1±0.4 60±6 2.3±0.3 0.13±0.04 3.3±0.3 2.7±0.3
35.2-35.4 V 3.2±1.0 23±3 1.8±0.5 0.15±0.01 3. 9±0. 3 15±4
33.2-33.6 VI 3.8±0.8 38±4 3.4±0.3 0.52±0.15 7.2±0.7 50±5
32.8-33.2 VII 3.8±0.3 47±3 2.2±0.1 0.39±0.02 9.4±2.5 5.7±1.3
32.4-32.8 VIII 2.6±0.1 28±5 2.1±0.1 0.29±0.01 9.5±1.0 18±3
*See Figure 12.
V1V1
56Degrees North Latitude
50 49 48 47 46 45 44 43 42
~i.I 1((31r'1
. ) D1"'1 ----r-
33 ......
0 20034
0
0 0 0 0 400
B
UJl-l
0 600 aJ.waJ......
0"-<
34.5 _ ~ ~(} ,,-1
I ..c! .wi P-
OaJ
0 0 800 A
A
1000
--1200
I1-1------------------.....1-1400
FIGURE 13. LOCATION AND DEPTH OF SA~LES COLLECTEDALONG THE WEST COAST OF TIill UNITED STATES (125°W).
ISOHP.LINES ARE ALSO SHOWN WITH SALINITY IN 0/00.
"
TABLE XVI. VARIATION OF TRACE ELEMENT CONCENTRATION WITHRESPECT TO WATER MASS (12SoW)
S 0/00 Water ELEMENT concentration in pg/liter-Range Mass* Uranium Copper Nickel Cobalt Iron Manganese
34.5-35.0 A 1.9±0. 3 33±5 1.4±0.2 O.lS±0.03 5.3±0.S 2.9±1.4
34.0-34.5 B 1. 7±0.1 27±6 1.1±0.1 0.14±0.01 5.4±0.4 0.64±0.1
33.0-34.0 C 1.S±0.2 2S±2 0.64±0.2 0.09±0.02 4.6±0.6 1. 6±0. 8
32.0-33.0 D 1.6±0 .1 24±4 1. 2±0. 2 0.lS±0.03 6.4±0.7 2.3±0.S
29.0-30.0 F 1.4±0.3 38±8 0.74±0.1 0.12±0.01 S.1±0.8 1.6±0.8
31.0-32.0 H 1.6±0.1 39±9 1.2±0.2 0.17±0.01 6.l±0.8 1. 6±0. 3
30.0-31.0 I 1. 2±0.1 26±4 1.0±0.4 0.18±0.OS S.2±0.8 1.4±0.1
*See Figure 13.
Ul-....J
58
winds. Since the samples were collected in mid-October, 1967, the data
for the figure were averaged over the years 1963 to 1966 for this time
of year. The data are representative of the isohalines in the upper
100 meters, but some variation would be expected as the plume is not in
a reproducible area each year.
In addition to the Columbia River plume, there is another very
important water structure known as a halocline, off the west coast of
the United States (7). A halocline is a water "layer showing a rapid
increase in salinity with depth. The top of the halo cline is at 100
meters and has a salinity of 33 0/00 and the bottom is at 200 meters
with a salinity of 34 0/00. Since the halocline is stable with respect
to time, water above the halocline can mix only slowly, if at all with
water below it. This isolation from mixing should yield a difference
between the two regions. Table XVII shows there is a difference in the
concentrations of the trace elements, except for manganese but this
difference is small compared to the data spread in eaCh region. The low
trace element concentrations found within the halocline (Table XVII)
are possibly due to the high productivity associated with such an area
(32).
The Columbia River plume is represented in Figure 13 by water
masses E, F, and G. Water mass H is probably a mixture of low salinity
water from the Straits of Juan de Fuca and the Columbia River. One
source has described the Columbia River plume as water with a salinity
less than 32.5 0/00 (20). In Figure 13, water with a salinity less
than 32 0/00 clearly shows a cross section of the plume between 46°N and
44°N. Only two samples were obtained from this area, both from water
TABLE XVII. TRACE ELEMENT CONCENTRATION ABOVE, WITHIN, AND BELOW THE HALOCLINE
Position with respect ELEMENT concentration in ~g/l
_____t_o_Ha1oc1ine Uranium Copper Nickel Cobalt Iron Manganese
r{:~
Above
Within
Below
1.4±0.1
1.3±0.1
1. 7±0.2
32±6
24±3
28±3
1.3±0.2
0.83±0.2
1.5±0.1
0.15±0.01
0.13±0.01
0.13±0.02
5.7±0.5
5.4±0.5
5.1±0.3
1. 7±0.3
2.0±0.7
1. 7±0. 7
U11.0
60
mass F. Table XVI shows F to be low in all elements except copper which
is high. Water mass I is also low including copper. Water masses A,
B, C, and D show a trace element distribution similar to the depth
distribution, as expected, as approximately the same grouping of samples
was used for each. It is interesting to note that D and H could be
considered very similar and indeed, the uranium, nickel, cobalt, and
iron content is very similar. In general, there was a sm~ll but
observable difference in certain trace element concentrations between
water masses for the coastal waters.
The differences in the mid ocean waters are more readily observable
as Figure 12 and Table XV show. The m03t obvious difference is between
water masses II and III. Samples from III are from approximately the
same depth as II and yet the difference is distinct for all elements but
copper. Copper and manganese values are extremely variable and
differences given in Table XV mayor may not be reaL The copper value
of IV and the manganese value of VI ~re thought to be anomalously high.
Water masses VI and VII have higher trace element concentrations in
general than IV and V even though the latter have higher salinities.
This indicates a latitude relation which may have been masked by deep
water samples included in Table IX. High latitude samples also have a
higher iron content than deep water samples, and there also seems to be
an inverse relationship between the other elements and iron for VI, VII,
and VIII. In general, for the mid ocean samples, there is a distinct
difference between water masses which appear significantly larger than
differences in salinity.
61
Fresh Water Data
The fresh water samples were analyzed to ascertain their dissolved
and particulate trace element content. Table XVIII shows the results of
the analysis of these samples for filtered and unfiltered water and
particulate matter. Each sample was analyzed twice, first a 500 ml
unfiltered sample followed by a 500 ml sample filtered through a 0.45
micron pore size membrane filter. The filters were later analyzed
directly by x-ray fluorescence spectrometry. The particulate values
were estimated from the total number of counts, the area excited by the
primary beam, the total area covered by the particulate matter, and the
counts per microgram obtained from the standards. The background for
each element was obtained by measuring the background of an unused
membrane filter. Although the above is an estimate, it is probably
accurate within ±20%.
Both filtered and unfiltered samples were analyzed to determine if
the same amount of metal was extracted in each case. Table XVIII shows
unfiltered sample values are higher than filtered values in most CL:.1':'8.
Thus comparisons between analyses must be made only between filt~ -.'"..:
samples or unfiltered samples.
Lake Waiau was analyzed and was found to have very high part'ic"~;;'~"~·
values for iron and manganese, and relatively high values for the
unfiltered sample, at least, when compared to water from the Douglas
cinder cone. In fact all elements except uranium are higher in Lake
Waiau than in Douglas. Since both Waiau and Douglas have the same
water source, rain and snow, the higher extractable trace element
content of Waiau may be due to the larger algal population of Waiau.
TABLE XVIII. RESULTS OF FRESH WATER ANALYSIS(CONCENTRATION ~g/l)
62
Uranium Copper Nickel Cobalt Iron Manganese
Lake Waiau
Particulate 1.2 740 52Unfiltered 1.2 9.8 1.4 0.14 26 11Filtered 1.6 9.6 1.2 0.07 4.7 1.5
Perched water (Douglas)
Unfiltered 1.2 5.6 0.48 0.07 1.6 0.24
Lake Champlain
Particulate 18 3.2 12 142 30Unfiltered 1.6 3.4 0.92 0.26 14 18Filtered 1.0 3.2 0.78 0.06 1.4 1.7
Conneaut Lake
Particulate 2.2 0.20 0.45 6.0 17Unfiltered 0.6 1.8 1.6 0.14 5.5 21Filtered 1.3 1.6 0.52 0.12 1.6 4.6
Mahoning River
Particulate 2.9 2.5 6.7 104 10Unfiltered 2.0 0.2 35 0.58 12 350Filtered 1.8 1.8 33 0.62 16 360
Shenango River Reservoir
Particulate 2.7 0.60 1.4 22 28Unfiltered 0.7 3.4 2.0 0.06 6.1 37Filtered 1.1 2.4 1.2 0.28 0.65 7.6
Spring water
Particulate 2.2 0.25 0.32 2.8 0.45Unfiltered 0.5 2.4 0.02 1.4 0.76Filtered 0.6 6.8 2.0 0.02 0.58 2.1
63
A possible reason for the difference in algal populations is given in
tae Introduction but not yet been substantiated. It may be argued that
if this were not the case, one would expect approximately the same trace
element concentrations in both lakes, as the source of trace elements
for each must be similar, if not identical.
There seems to be some correlation between dissolved trace element
concentrations and the concentrations of the elements in the lava.
Hawaiian lavas are about 6-9% by weight iron as FeO and 0.1-0.2%
manganese as MIlO with other elements in the parts per million range
(32). This, of course, refers only to the elements considered in the
study. The high values for iron and manganese should be reflected in
the waters associated with the lava. The effect is noted to some
extent for dissolved material in Waiau, but is much more evident for
particulate material. Table XIX compares the element to iron ratio of
lavas and the particulate and dissolved material for Waiau and Douglas.
All metals in the table show an enrichment with respect to iron,
especially copper. The ratios of the lake waters, except copper, agree
within a factor of 10 to 50 with the ratios of the lavas, thus,
indicating that the lavas play a role in the trace element supply for
these waters. The high copper ratios are interesting and warrant
further research.
The other fresh water samples were chosen to represent as wide a
variety of bodies of water as possible, to test the applicability of the
method to various waters. Their trace element concentrations are shown
in Table XVIII and the locations are shown in Figure 3. Lake Champlain
is a large lake about 100 miles long and 1-10 miles wide with little
TABLE XIX. COMPARISON OF ELEMENT TO IRON RATIO FOR HAWAIIAN LAVAS,LAKE WAIAU, AND DOUGLAS PERCHED 'vATER
Hawaiian Waiau Waiau Waiau DouglasRatio, Lavas Particulate Unfiltered Filtered Unfiltered
Mn/Fe 1. 6x10- 2 7.0x10-2 4.0x10- 1 3.0x10- 1 1.5x10- 1
Ni/Fe 6.4x10- 3 --- 5.4x10- 2 2.5x10- 1 3.0x10-2
Co/Fe 5.6x10- lf 1.6x10- 3 5.4x10- 3 1.4x10-2 4.3x10- 2
CufFe 1.7x10- 3 --- 2.0 2.0 3.5
0'~
65
heavy industry bordering it and only moderate recreational use of its
surface area is ~dde. Conneaut Lake is a small lake about 3 miles long
and I mile wide with heavy recreational use for its surface area in the
summer which is surrounded by a large number of both permanent and
summer homes. The Mahoning River is a small river which flows through
the industrial complex of Warren and Youngstown, Ohio, and New Castle,
Pennsylvania. The Shenango River Reservoir is a three year old man-made
lake about 15 miles long and with a maximum width of less than a mile.
The reservoir is formed before the Shenango River flows through any
heavy industry. The spring is located in the mountains of Western
Pennsylvania and has a flow rate of about 30 gallons per hour.
Since the sample from Lake Champlain was collected near shore while
the lake was rough, there was considerable suspended sand, organic
matter and clays in it. Some of this material settled quickly but the
sample was shaken before filtering to get an overall sample of the
suspended matter. The presence of the sand particles is the probable
cause of the high values for the particulate analysis of the lake. This
material will cause increased scattering of the primary x-rays and
therefore an apparent increase in the intensity for each element. The
uranium value of 18 ~g/l is highly suspect. The ~ radiation of the
particulate and standard samples was counted and indications were that
the actual uranium content is about an order of magnitude less. Good
~ spectra were impossible to obtain because of the large ~ energy
absorption of the samples. There seems to be little distinct
difference between the filtered samples of this lake and Conneaut Lake
despite the different lake environments.
66
The Shenango River Reservoir has generally more dissolved and
particulate matter than Conneaut Lake. Both bodies of water were in
late summer algal bloom) but the reservoir population was estimated to
be 4 times greater than the lake population. Reflectance spectra of
particulate matter on the filters have been used to make the estimate
(31). The difference may explain part of the trace element content
variation between the bodies of water) but most of it is probably due
to the different water sources for each. Conneaut Lake is both spring
and stream fed) whereas, the reservoir is river fed. Because the river
carries a higher dissolved and sediment load, one would expect the
reservoir to contain more dissolved and particulate material. The
recent nature of the reservoir may also be a factor in the difference.
The spring water is clear, cold, and excellent drinking water
serving a group of hunting and summer cabins (about 15), 80-90 miles
north of Pittsburgh, Pennsylvania. The Mahoning River is used for
dumping raw and treated sewage, steel mill wastes) and as cooling water
for steel mills and other industry along about one fourth of its entire
length. The effect of this use can be seen in the trace element
content. The high particulate iron and very high dissolved manganese
and nickel values could probably be traced to the iron and steel
industry. The sample was collected about 10 miles below the last steel
mill and about 3 miles above New Castle, Pennsylvania. It would be
most informative to sample this river every quarter mile to learn the
source of the metals and how long the material stays in the water. The
spring water is low in all elements except copper and nickel.
67
The work with f1"esh water samples indicates that the extraction
method can be used to trace certain types of pollution and possibly to
characterize water sources by trace element content.
SUMMARY
A method was developed to analyze for uranium, copper, nickel,
cobalt, iron, and manganese in both fresh and sea water. An 8-hydroxy
qUinoline-chloroform extraction and x-ray fluorescence spectrometry
were used in the analysis. Absolute methanol, 8-hydroxyquinoline,
and chlorofo~ were the only reagents needed for sea water analysis and
the equipment needed for the extraction and primary evaporation was
simple and portable, thus, shipboard and field work could be done.
The precision of the method depended on the element and the
absolute amount of the element being analyzed. The analysis of a 500 m1
sample of sea water had a precision of 5% for all elements except
uranium and cobalt, which were 10%. AlSO m1 sample had a precision of
10% for all elements except uranium and cobalt, which were 20% and 30%
respectively.
The actual sea water analyses for this research were carried out
on 120 m1 and 240 m1 samples from, respectively, the mid North Pacific
Ocean off the Northwest Coast of the United States (125°W). Coastal
water trace element content was found to be lower than mid ocean content.
Significant differences in trace element content were also found between
water masses of differing salinity, but little regular variation with
latitude could be found. Some elements, notably uranium, showed an
increase in concentration with depth.
The method proved to be applicable to a wide variety of fresh
waters, ranging from spring water to polluted river water. The large
algal population apparently present in Lake Waiau appeared to have the
effect of increasing the extractable trace element content of the lake
as compared to Douglas perched water, where such a population was
absent. Other fresh water samples showed evidence of differences
related to the water source and possible pollution.
69
APPENDIX I
METHOD USING DITHIZONE-CELLULOSE ACETATE COLUMNS
Cellulose acetate (Fisher Scientific Co.) with a particle size of
0.4-0.8 rom is treated with a 0.01% solution of dithizone in carbon
tetrachloride and the carbon tetrachloride removed in a vacuum rotary
evaporator. This material was used to make columns which were
approximately 2 cm in length and 1 cm in diameter with a 3 rom thick
layer of powdered cellulose on the bottom. A 2 m1 filtering funnel
made an excellent container for the columns. The column was wet with
about 0.5 m1 of carbon tetrachloride, washed with 50-60 m1 of one normal
hydrochloric acid, and rinsed with deionized water. The hydrochloric
acid wash was necessary since recovery was very poor without it.
The water sample was adjusted to a pH of 7.00 ± 0.05 and passed
through the column at a rate of one to two liters per hour. The bulk
of the carbon tetrachloride was removed by drawing warm air through the
column for several minutes. The column material was removed from the
filtering funnel using a Teflon coated spatula and placed in a glass
vial. It was dried on a 100°C hot plate. The dried material was
transferred to a mortar and ground to a powder, which was compressed
into a 1.27 cm pellet about 3 rom thick at a pressure of 30 T/in2 •
Since the pellets were too small to be held by the sample holder of the
x-ray instrument, a set of Teflon rings of the proper size was
constructed to accommodate and position the pellets.
APPENDIX II
CALCULATION OF CRITICAL DEPTH FOR CHROMIUM X-RAYRADIATION IN THE CELLULOSE ACETATE PELLET
This calculation is based on an equation derived by Liebhafsky,
et ale (14).
(1) Id = 1 _ e-apd
100
Where: Id = intensity from a sample of thickness d
I = intensity from an infinitely thick sample00
a = 111 csc8l + 112 csc62
111 = average mass absorption coefficient for incomingbeam
112 = average mass absorption coefficient for outgoingbeam
81 = angle of incidence
62 = angle of emergence
p = density of matrix
d = depth in cm.
For purposes of calculation the following assumptions are made:
1. Only absorption effects are considered
2. The matrix is effectively 100% cellulose acetate
The other quantities in the equation have the following values:
(]
72
].11 = 0.1
].12 = 26
81 = 67 0
82 =nnOL:.J
p 1.0 g/cm3
Upon substitution of the above values into equation (1), the
critical depth is found to be 0.1 rom for chromium radiation. The
critical depth will increase with increasing atomic number. In pellet
work a maximum depth will be reached for the element zinc and will be
aoout 0.2 rom.
When these values are compared to the total thickness of the
cellulose acetate pellets (3 mm), it is clearly shown that only a small
percentage of the total pellet (3%) is excited by the x-rays. Since a
pellet weighs approximately 0.5 grams and the minimum amount of cobalt
that can be analyzed with precision is 0.02 ~g, the concentration of
cobalt in the pellet would be 1.2 ppm or 0.6 ].Ig in absolute amount.
This would require a 2 liter sample of sea water based on the mid ocean
value found and the amount of zinc and copper in such an amount would
completely swamp the column. About 500 m1 of sea water is the most
that can be analyzed for copper and zinc. It is, therefore, impossible
to use this method to analyze for cobalt. The same type of argument
may be applied to nickel and chromium, so the pellet method was
abandoned.
APPENDIX III
NEUTRON ACTIVATION DETECTION LIMITS
The detection limits for neutron activation analysis were
calculated from the following equation:
(1) A = N 0 a % abundance (1 _ e-At )100
A = activity in disintegrations per minute
N = number of atoms
o = neutron flux in neutrons/cm2 /sec
a = cross section in cm2
A = decay constant
t = irradiation time in hours
A number of assumptions must be made in order to use the above
equation.
A = 10 dpm
N grams x 6.0xl0 23
Atomic Weight
f/J = 5xlO 12n/cm2 /sec
a = barns x 10-2 4 cm2 /b arms
A _ 0.69 • t 1/2 = half-life in hours--~
t 1/2
t = 0.082 hours
An irradiation time of five minutes is us<?·d to prevEmt any sodium
chloride carried through the procedure from becomin~~too radioactive.
74
The detection limits of all elements except Fe58 would increase with
longer irradiation times. Iron 58 would not increase because of the
long half-life of Fe59 • An element reaches one half maximum activity
when irradiated for one half-life and an infinitely longer irradiation
only doubles the activity. For this reason irradiations longer than
one half-life are not useful.
Uranium analysis is assumed to be by the n,Y reaction not by
fission, although fission will certainly take place. In the case of
Fe 59 decay takes place by both Sand Y emission in about equal parts
with a further equal split in the gamma energies, therefore, the
detection limit is four times higher than calculated from equation (1).
75
ISOTOPE % CROSSELEMENT ACTIVATED ABUNDANCE SECTION
uranium U238 99 2.7 barns
copper Cu63 69 4.5 "nickel Ni64 1.1 1.5 "
cobalt Co 59 100 18 "iron Fe 58 0.33 1.2 "manganese Mn 55 100 13.3 "
ISOTOPEELEHENT produced in n, a HALF LIFE
REACTION
uranium U239 23.5 min
copper Cu64 12.9 hr
nickel Ni65 2.56 hr
cobalt Co 6O 10.5 min
iron Fe 59 45 d
manganese Mu 55 2.58 hr
The above tables give the information needed to use equation (1) to
calculate the data given in Table I.
BIBLIOGRAPHY
1. Blanchard, R. L., U234 jU238 Ratios in Coastal Marine Haters and
Calcium Carbonates, J. Geophys. Res. 70, 4055-61 (1965).
2. Blanchard, R. L. and D. Oakes, Relationships between Uranium and
Radium in Coastal Marine Shells and Their Environment, J. Geophys.
Res. 70, 2911-21 (1965).
3. Brooks, R. R., B. J. Presley, and R. I. Kaplan, APDC-MIBK
Extraction System for the Determination of Trace Elements in Saline
Waters by Atomic-Absorption Spectrophotometry, Ta1anta 14, 809-16
(1967).
4. Carritt, D., Separation and Concentration of Trace Metals from
Natural Waters, Anal. Chern. 25, 1927 (1953).
5. Davidson, A. W., Solutions of Salts in Pure Acetic Acid. I.
Preliminary Paper, J. Am. Chem. Soc. 50, 1890-95 (1928).
6. Davidson, A. W. and W. H. McAllister, Solution of Salts in Pure
Acetic Acid. II. Solubilities of Acetates, J. Am. Chem. Soc. 52,
507-19 (1930).
7. Fleming, R. H., Notes Concerning the Ha1oc1ine in the Northeast
Pacific Ocean, J. Mar. Res. 17, 158-73 (1958).
8. Goldberg, E., Minor Elements in Sea Water, Chemical Oceanography,
J. Riley, and G. Skirrow, ed., Vol. 1, 164-5, New York (1965).
9. Goldberg, E., Minor Elements in Sea Water, Che~ic~l Oce~cgraph~,
J. Riley and G. Skirrow, ed., Vol. 1,183-7, New York (1965).
10. Gunn, E. L., X-Ray Fluorescence Intensity of Elements Evaporated
from Solution onto Thin Film, Anal. Chem. 33, 921-7 (1961).
77
11. Holland, H. D., The Chemical Evolution of the Earth1 s Atmosphere
and Oceans, unpublished manuscript (1968).
12. Jenkins, R. and J. L. De Vries, Instrumental Factors in the
Detection of Low Concentrations by X-Ray Fluorescence Spectrometry,
Analyst 94, 447-56 (1969).
13. Jenne, E. A., Controls on Mn, Fe, Co, Ni, Cu, and Zn Concentration
in Soils and Waters: the Significant Role of Hydrous Mn and Fe
Oxides, Trace Inorganics in Water Advances in Chemistry Series No.
11, Robert F. Gould, ed., 337-87, Washington (1968).
14. Liebhafsky, H. A., H. G. Pfeiffer, E. H. Winslow, and P. D. Zemany,
X-Ray Absorption and Emission in Analytical Chemistry, 149-52,
New York (1960).
15. Mansell, R. E. and H. W. Emmel, Trace-Metal Extractions from Brine
with APDC and Oxine, Atomic Absorption News1~ 4, 365-6 (1965).
16. Marcie, F. J., X-Ray Determination of Trace Toxic Elements in
Water, Envir. Sci. TeCh. 1, 164-6 (1967).
17. Miyake, Y., Y. Sugimura, and T. UchiG~, Ratio U234 /U238 and the
Uranium Concentration in Seawater in the Western North Pacific,
J. Geophys. Res. 71, 3083-7 (1966).
18. Morris, A. W., The Simultaneous Determination of Vanadium,
Chromium, Manganese, Iron, Cobalt, Nickel, Copper, and Zinc in Sea
Water by X-Ray Fluorescence Spectroscopy, Anal. Chim. Acta 42,
397-406 (1968).
19. Mulford, C. E., Solvent Extraction Techniques for Atomic
Absorption Spectroscopy, Atomic Absorption Newsletter 5, 88-90
(1966).
78
20. Natelson, S., D. Leighton, and C. Calas, Assay for the Elements
Chromium, ~langanese, Iron, Cobalt, Copper, and Zinc Simultaneously
in Human Serum and Sea Water by X-Ray Spectroscopy,Microchem. J.
6, 539-56 (1962).
21. Park, K., Alkalinity and pH off the Coast of Oregon, Deep-Sea
Research 15, 171-83 (1968).
22. Peterson, M. N. A., Calcite Rates of Dissolution in a Vertical
Profile in the Central Pacific; Science 154, 1542-4 (1966).
23. Pfeiffer, H. G. and P. D. Zemany, Trace Analysis by X-Ray Emission
Spectrography, Nature 174, 397 (1954).
24. Physical, Chemical, and Biological Data from the Northeast Pacific
Ocean: Columbia Effluent Area, Tech. Report No. l5g. Vol. II, III,
University of Washington (1963).
25. Physical, Chemical, and Biological Data from the Northeast Pacific
Ocean: Columbia River Effluent Area, Tech. Report No. 182, Vol. I,
University of Washington (1965).
26. Physical, Chemical, and Biological Data from the Northeast Pacific
Ocean: Columbia River Effluent Area, Tech. Report No. 186,
University of Washington (1966).
27. Pueschel, R., Application of X-Ray Fluorescence to Trace Analysis.
I. Enrichment of Trace Elements by Extraction, Mickrochim. Ichnoanal.
Acta (4) 770-86 (1968).
28. Reid, J., Jr., Intermediate Waters of the Pacific Ocean, 55-8,
Baltimore (1965).
79
29. Schutz, D. F. and K. K. Turekian, The Investigation of the
Geographical and Vertical Distribution of Several Trace Elements
in Sea Water Using Neutron Activation Analysis, Geochim. Cosmochim.
~ 29, 259-313 (1965).
30. Stary, J., The Solvent Extraction of Metal Chelates, 80-94, New
York (1964).
31. Strickland, J. D. H., Production of Organic Matter in the Primary
Stages of the Marine Food Chain, Chemical Oceanography, J. Riley
fu.d G. Skirrow, ed., Vol. 1, 501, New York (1965).
32. Strickland, J. D. H., Production of Organic Matter in the Primary
Stages of the rrarine Food Chain, Chemical Oceanography, J. Riley
and G. Skirrow, ed., Vol. 1, 552, New York (1965).
33. Wager, L. R. and R. L. Mitchell, Trace Elements in a Suite of
Hawaiian Lavas, Geochim. Cosmochim. Acta, 3, 217-23 (1953).
34. Whitnack, G. C., Single-Sweep Polarographic Study of Some Trace
Elements in South American Pacific Ocean Waters, Naval Weapons
Center Publication 4467 (1967).
35. Woodcock, A. H., M. Rubin, and R. A. Duce, Deep Layer Sediments in
Alpine Lake in the Tropical Mid-Pacific, Science 154, 647-8 (1966).