CORE – Aggregating the world’s open access research papers · Dr. Mohammad Ajmal Environmental Research Lab. Deptt. of Applied Chemistry Z.U. College of Engg.&Tech. Aligarh Muslim

STUDIES ON THE DISPOSAL AND TREATMENT OF SOME

INDUSTRIAL WASTES

DISSERTATION SUBMITTED IN PARTIAL FULFILMENT OF THE REQUIREMENTS

FOR THE AWARD OF THE DEGREE OF

ilgiidIP @ff P)[h)QO@g@p(h)Si' IN

CHEMISTRY

AKHTAR HUSSAIN KHAN

DEPARTMENT OF CHEMISTRY ALIGARH MUSLIM UNIVERSITY

ALIGARH (INDIA)

1 9 8 8

DS1280

Dr. Mohammad Ajmal Environmental Research Lab. Deptt. of Applied Chemistry Z.U. College of Engg.&Tech. Aligarh Muslim University Aligarh - 202 002 iIndia)

Dated . k: JP.. ^.'^. . .

C E R T I F I C A T E

This is to certify that the work described

in this dissertation entitled "Studies on the Disposal

and Treatment of some Industrial Wastes" is the original

work of Mr. Akhtar Hussain Khan, carried out under my

supervision and guidance. The work included in this disser

tation has not been submitted elsewhere for any other

degree or diploma of any university.

MOHAMMAD AJMAL (Supervisor)

A C K N O W L E D G E M E N T

I am highly thankful to Dr. Mohammad Ajmal, Reader,

Department of Applied Chemistry, Aligarh Muslim University.

Aligarh for his guidance, healthy criticism and worthy

suggestions.

My special thanks are also due to Prof. K.T. Naseem

Chairman, Department of Applied Chemistry, A.M.U, Aligarh,

for providing me all the requisite research facilities

available in the department.

I also render my sincerest thanks to

Dr. Ali Mohammad and Dr. Naim Fatima for their kind and

valuable help and suggestions during these studies.

I am indebted to my senior colleagues

Drs. Sultan Ahmad, Ahsanullah Khan, Mujahid A. Khan,

Raziuddin, Nadeem A. Siddiqui and Abdul Jabbar Khan

for their advice, affections and encouragement from time

to time during the all stages of assignment.

I am also sincerely grateful to my colleagues

Rubina Chaudhry and Shamim Ahmad for their moral support

and all round co-operation during the entire period of

studies.

I am no less thankful to my fellow research scho

lars Shahreer Ahmad, Rais Ahmad and Jamal A. Khan for

their assistance and co-operation.

I express heartfelt regards and reverence to my

parents whose good wishes and love have always been

a great source of inspiration in accomplishing this task.

I, indeed feel proud of dedicating this research work

to them.

v - V ^ . v l i > v y ^ ^ - -

(AKHTAR HUSSAIN KHAN)

CONTENTS

Chapter I GENERAL INTRODUCTION

Chapter II SURVEY OF LITERATURES

Chapter III REVERSED PHASE THIN LAYER CHROMATOGRAPHIC SEPARATION OF HEAVY METAL IONS ON SILICA GEL LAYERS LOADED WITH TRIBUTYLAMINE

Introduction

Experimental

Resvilts and Discussion

Chapter IV USE OF ACIDIFIED SILICA GEL LAYERS AS AN ADSORBENT IN CHROMATOGRAPHIC SEPARATION OF SOME METAL IONS

Introduction

Experimental

Results and Discussion

Chapter V SUMMARY

REFERENCES

Page

1-25

26-48

49-55

54-57

58-82

83

84-86

86-97

98-100

101-104

PUBLICATION

1. Reversed Phase Thin Layer Chromatographic

Separation of Heavy Metal Ions on Silica

Gel Layers Loaded with Tributylamine.

Journal of Planar Chromatography

Volume-1, No. 2, pp. 128-15A (1988).

C H A P T E R - I

GENERAL INTRODUCTION

C H A P T E R I

GENERAL INTRODUCTION

It is difficult to define Environmental pollution

and its defination may change not only from country to

country but also from area to area within the same

country. It is, however, less difficult to describe

Environmental Pollution. Such a pollution inclxjdes the

release of substances, which harm the quality of air,

water or soil into the environment which upset the

biological cycles linking man to animals or plants even

when this damage is subtle and causes no deaths or does

not manifest itself for several decades or generations.

Pollution such as noise and smell which often irritates

is also hazardous to health.

We are on stronger ground if we relate pollution

to the natural cycles of growth and decay which, govern

all life on the planet. Where man's activities feed

into and are accomodated within these cycles, he is not

causing pollution. For example, the discharge of carbon

monoxide into the atmosphere by motor vehicles is unli

kely to cause serious overall damage, because natural

bacteria in the soil can feed on it and convert it to

harmless compounds. Provided we do not release so much

carbon monoxide that there are not sufficient bacteria to

break it down, then pollution cannot be said to occur.

On the other hand, the chemicals xxsed as propellants

in domestic and industrial aerosols are not, so far as

we know, attacked by any bacteria and so do not decay

naturally. They cannot slot into any natural cycles

and are therefore steadily building up in the atmos

phere. While there seems no suggestion that they are in

any way dangeroiis at present, they are most certainly

a form of pollution.

Sometimes man's waste products do not merely fail

to form part of the natural cycle, but positively

overwhelm or poison it. Our rivers for example are well

used to receiving natural organic matter and breaking it

down to compounds which can once again become the buil

ding blocks of new plant and animal tissue. When man

adds moderate quantities of domestic sewage, he merely

increases the total load of organic matter to be decayed.

But the bacteria which mainly bring this about need

oxygen to survive and the more the sewage is added the

more oxygen is consumed. Within limits the river natu

rally reaerates itself. But if too much organic matter

is added, the water becomes totally devoid of oxygen.

Not only do fish and other aquatic life die, but so do the

every bacteria which carryout the decaying process. They

are sometimes replaced by other species of bacteria, which

can survive without oxygen, and which can trigger off

different and often dangerous ecological cycles. Either

way, the river has been overwhelmed by pollution.

Some pollutants are indisputably dangerous either

to human health and welfare or to ecological cycles on

which man depends for his survival. I would like to

stress the point that it is quite inadequate to think

of harm to human beings or human health. Man is integral

part of the highly complex web of living organisms which

we call biosphere. Harm done to any part of the biosphere

may have reperexjssions on human welfare, for man relies

on it for food and other raw materials. Many pollutants

have already damaged agriculture and fisheries. We may

conclude that any substance which weakens any link in

nature s network is potentially harmfvil. Pollutants can

be harmful, harmless or even beneficial depending on

their concentration. Carbon dioxide for example, is

essential for green plants, so are the traces of some

heavy materials, so, probably, are small amounts of sulphur

dioxide. Yet large quantities of any of these can skill

plant or animal life.

Again it is easy to determine the effects of a

single pollutants in the laboratory. But in real life

there are usually many pollutants and they may sometimes

have synergistic effects on one another (combined effect

is much greater than the sum of their individual

effects). For example, nitrogen oxides and hydro

carbons emitted from motor car exhausts are relatively

harmless. Together, under the influence of intense

sxjnlight, they can combine to form an eye-smarting

photochemical smog.

One of the important aspects of pollution

abatement pollutes is to strike a balance. On the one

hand we wish to avoid a pollutant reaching a dangerovis

level. On the other than we must not suppress at

great expense which at present is nowhere near a

harmftil level. However, there are certain pollutants

about which there is no controversy. Any pollution

abatement policy shoxjld concentrate upon them.

The Origin of Waste:

One characteristics peculiar to Man is that he

progressively changes his environment to meet his

biological and social needs. On a socially organized

basis Man provides himself with the materials necessary

of life which he removes initially as raw material

from his environment. It is in the provision and

utilization of these material necessities, that worthless

and sometimes harmful by-products originate. Such pro

ducts comprise wastes of ail descriptions and they are

inev i tab le r e s u l t of Man's i n t e rac t ion with h i s physical

and bio logica l sorroundings. To separa te waste from

environment has been one of Man's o ldes t a c t i v i t i e s .

His tor ica l and Cultural Background:

In primit ive nomad s o c i t i e s the problem of waste

d isposal is a t i t s l e a s t . The nomad separa tes waste

from environment by changing his sorroundings. I t i s

when Man ex i s t in permanent communities t h a t the

removal of his waste products must be condixjted on

an organised bas i s . I t i s of i n t e r e s t t o note t h a t

i t was the t r ans i t i on from Pa laeo l i th ic Society based

on hunting and gathering to Neoli thic soc ie ty based on

farming and agricultixre which heralded the need for

waste d isposal . But i t has been the excesses of the

Indus t r i a l Revolution and i t s aftermath upto the

present day which has resul ted in a q u a l i t a t i v e l y

d i f f e ren t type of problem. Although waste disposal

must, as a minimum requirement, conserve the environ

ment's a b i l i t y to sustain human l i f e , the degree to

which i t practised at levels above t h i s rainimtjm depends

on the economic, p o l i t i c a l , cu l t u r a l and aes the t i c

values of the waste producing soc ie ty .

Pollutants.:

Wastes are not necessarily pollutants in them

selves but all have the capacity to be so - A waste

becomes a pollutant when it occurs in a wrong place.

It will be appreciated that production of waste is an

inevitable consequence of the first and second laws

of thermodynamics. The production of actual pollutants

is far from inevitable,

Fredrick Werner (1975) defined a pollutant as

"A substance or effect is normally considered to be a

pollutant if it adversely alters the environment by

changing the growth rate of a species, interferes with

the food chain, is toxic, or interferes with health,

comfort, amenities, or property values of people.

Generally a pollutant is a substqnce or effect intro

duced into the environment in significant amounts as

sewage, waste, accidental discharge, or as a by product

of a manufacturing process or other human activity. A

polluting substance can be a solid, semi-solid, liquid,

gas or sub-molecular particle. A polluting effect is

normally some kind of waste energy such as heat, noise,

or vibration.

Pollution ;

pollution is the result of the action or presence

7

of a pollutant in a part of the environment where it

is considered to have deleterious affects.

In the statement by Darling (1970) : 'Pollution

comes from getting rid of wastes at the least possible

cost.

Odum (1971) says in his own words "Pollution is

an undesirable change in the physical, chemical or

biological characteristics of our air, land and water

that may or will waste or deteriorate our raw material

resources.**

Industrial Wastes:

As a consequences of rapid industrialization in

the post—independence period prior to which our

economy was largely, agrarian, the problem of indus

trial effluent has grown into a significant magnitude.

Since a large majority of indxjstries is water based,

considerable volxme of wastewater emanate from the

indtistries. As the industrial effluents are as

varied in nature as the industry itself, the problem

gets further aggrevated as no standard procedure for

treatment can be recommended. Because of a variety of

reasons the industrial effluents are generally discharged

into water course either untreated or inadeqioately trea-

8

ted. The situation therefore has created a problem of

surface and subsoil water pollution. The pressure on

our water resources is therefore two fold.

(i) Requirement of large volume of water for the

industry and

(ii) Inavailability of clean water because of the

pollution due to the discharge of wastewaters.

In the light of the above it becomes therefore

imperative that the Industrial effluents are

adequately treated so as to become largely inno

cuous. However before the various methods of

treatment and disposal are considered it is

desirable to have a look at the nature of

effluents from various industries.

The growth pattern of some industries in India

which releases hazardous substances which are not bio

logically degradable indicates the increasing serious

ness of the problem is given in the following table.

Characteristics of the Industrial Wastes :

Unlike the domestic sewage, the industrial

wastes are very difficult to generalize. The charac

teristics of the industrial wastes not only vary with

Growth pattern of Some Industries in India :

Production x 10 tonnes

1950

NA

NA

0.25

200

18

I960

1.46*

1.15

1.23

580

153

1970

3.00

13.55

1.79

17,100

1,059

1980

1*0.e&

30.85

5.07

24,100

3,005

Pesticides

Dyes and Pigments

Pharmaceuticals

Organic Chemicals including Petrochemicals

Fertilizers (Nitrogenous and Phosphatic)

Steel ingots

Non-ferrous metals

Copper

Lead

Zinc

Caustic soda

15x10^ 3.4x10^ 6.5x10^ 8.0x10^

NA

NA

NA

11

8.500

NA

NA

101

9.30

1.86

23.41

304

18.80

11.40

52.70

457

+ DDT only ; NA = Not available.

Ref. : Sundaresan, B.B.-, Subrahmanyam, P.V.R.;

I.A.W.P.C. Newsletter, July 1983.

lo

the type of the industry, but also from plant to

plant producing same type of end prodixjts. Different

types of liquid wastes originate from various tjrpes of

industrial processes. The pollutants include the raw

materials, process chemicals, final products, process

intermediates, process by-products, and impurities in

raw materials and process chemicals. Broadly, these

pollutants can be classified as follows :

(i) Organic substances that deplete the oxygen

content of the receiving streams and impose a great

load on the biological units of the sewage treatment

plant.

(ii) Inorganic substances like carbonates, chlorides,

nitrogen etc. that render the water body unfit for

further use and sometimes incourage the growth of some

undesirable micro-plants in the body of water.

(iii) Acids or alkalis which make the receiving stream

unsuitable for the growth of fish and other aquatic life

there, and cause serious difficulties in the operation

of sewage treatment plants.

(iv) Toxic substances like cyanides, sulphides, acety

lene, alcohol, petrol etc. which cause damage to the

flora and fauna of the receiving streams, affect the

11

municipal treatment processes and sometimes endanger

the safety of the workmen.

(v) Colour-prodiicing substances like dyes, which

though not toxic, are aesthetically objectionable when

present in the water sijpplies.

(vi) Oil and other floating substances, which not

only render the streams unsightly but interfere with

the self purification of the same, and the operations

of the sewage treatment plants. A general view of the

natijre of effluents can be had from the following table.

Pollution Characteristics of Different

Industries

Industry Pollution Character- Suggested treat-is tics ment Methods

1. Paper and Strong colour Chemicals recovery pulp

High BOD, Lime Treatment for

High COD/BOD ratio, Colour,

Highly alkaline. Biological Treatment

High sodium content.

12

Industry Pollut ion Character is t ics

Sviggested Treatment Methods

2. Tannery Strong colour, Chemical Treatment ,

High salt content, Biological Treatment

High BOD,

High dissolved s o l i d s ,

Presence of s u l f i d e s ,

Lime and Chromium.

3. Textile Highly alkaline, Chemical and

(a) Cotton High BOD, Biological Treatment

High suspended solids.

High pH .

(b) Synth- Low pH . etic

High dissolved solids.

Toxic organics•

U. Distillary Strong Colour,

and Brewery High chloride ,

High sulphate,

Very high BOD »

and COD, low pH-

Biological

Treatment

5. Petrochemicals

Mineral oils in Chemical Treatment,

various forms. Biological Treatment.

High BOD and COD,

High total solids-

13

Industry Pollution Characteristics

Suggested Treatment Methods

5. Pharmaceuticals

7. Coke oven

8. Oil refin

eries

9. Fertilizer

(a) Nitrogenous

High total solids, Chenical Treatment,

High COD, High Biological Treatment

COD/BOD ratio,

either acidic or

alkaline•

Chemical Treatment,

Biological Treatment

High ammonia.

High pH, High

Phenol content.

High BOD, High

cyanide and

cyanates,Low

suspended solids.

Free and emulsi

fied oil, acids,

alkalis, salts,

phenols, Soaps

and resinoxis or

tarry materials -

High Nitrogen Biological Treatment

content. High pH ,

Oil separation.

Chemical Treatment,

Biological Treatment.

14

Industry Pollution Characteristics

Suggested Treatment Methods

9.(b) Phos-phatic

10. Dairy

11. Sugar

12. Electroplating

High Fluoride

content •

High dissolved

solids, High

suspended solids,

HighBOD, Presence

of oil and grease.

Odors on stagnation*

High BOD, High

Volatile solids.

Low pH .



Alkaline, Low BOD, Chemical Treatment •

Toxic metals,

cyanides.

Ref. Rao, M.N., Datta, A.K., Waste Water Treatment Oxford IBH Publishing Co. 1979.

From the foregoing table it can be conceived

that the indxjstrial effluents can be categorized into

three broad categories.

( i ) Organic effluents including dairy wastes,

d i s t i l l e ry wastes, tannery wastes etc•

( i i ) Inorganic wastes including electro-plating wastes.

15

Synthetic yarm wastes etc. and

(iii) Toxic wastes covering pesticide wastes, organic

chemical waustes, antibiotic wastes etc. It must however

be mentioned that the categorization is rather arbitrary

and one category does considerably overlape to other.

Volumes of waste waters again vary considerably

from indiastry to industry. A general idea of the

volumes can be had from the following table :

Industry Unit Volumes of waste water per vnit product manufacture

•M57 Gallons/ Unit Unit

1. Pulp and paper

Tonne of paper 50,000 to 227

1000,000 455

2. Straw board Tonne of board 20,000 100

3. Tannery 100 Kg of hide 750 processed

5.^

k. Cotton Textile

1000 meters of Cloth

440-1760 2-8

5. D i s t i l l e r y Tonne of molasses 1320 processed

6. Dairy 1000 l i t r e s of milk processed

440-1760 2-8

16

7.

8.

9.

1

Steel Mill :

Coke oven

Steel (finished)

Refinery-

Fertilizer

Ammonia

Urea

2

Tonne of steel

-do-

Tonne of oil processed

Tonne of NH,

Tonne of Urea

3

125-155

530-650

350-400

2000

1500

h

0.51-0.70

2.^3.0

1.6-1.8

9

7

Ref. : Arora, H.C.

Environmental Pollution Monitoring and Control. Vol. No. 2, HBTI, KanpxjT.

Treatment of Industrial Wastes

Industrial activity is increasingly releasing

gaseous, liquid and solid wastes which are traditionally

discharged to the atmosphere, water bodies including

ocean fronts, or to land, considerably, affecting the

environment.

Some of the main industries are mentioned here

according to the type of pollution and therefore accor

ding to treatability.

- Agriculture and food industries which include

17

sugar refineries, breweries, dairies, cheese dairies.

Slaughter-houses, meat or vegetable preserving plants

cause considerable biodegradable pollution.

The effluents from these industries are laden

with vegetable or animal waste (fibre, fur, hair, fat,

etc.) which block pipes, cause fermentable deposits

and blockages. These also often contain colloidal

or dissolved organic matter which constitutes an

ideal medium fcr fermentation. In some cases, the

waste water contains bacteria or yeast from the manu

facturing process. Effluents from fish canneries and

curing plant may be heavily polluted with salt.

The composition of the effluents often varies

considerably over a period and it may be advantageous

to install buffer tanks for storage and homogenisation.

The biological treatment processes used for

these effluents are generally the same as for domestic

sewage, but high purification efficiency is required

because of the large amount of pollution to be treated.

Furthermore the presence of glueids and rapidly fermen

table products encourages the development of some

types of microorganisms which may interfere with the

efficient operation of the treatment plant.

18

Low rate treatment processes are therefore used.

Secondry clarifiers are generously scaled and pretreat-

ment processes such as grit and grease removal by

static means or by air injection fine screening or

microstraining must be particularly efficient. Aerated

lagoons, providing extensive storage facilities though

wasteful of energy, are particiiLarly recommended for

these indxostries on conditions that preliminary treat

ment processes are carefully planned and the lagoons and

aerators designed for maximun reliability.

The manxifacturing circuits should be studied

in detail before a treatment plant is constructed, as

it is advantageous to separate certain heavily -

polluting effluents sxochas mother liquor and serums at

the source, since the very considerable and specific

pollution involved may require separate recovery or

destruction (e.g. methanation).

Stabilization and dewatering of the biological

sludge is an essential adjunct to purification. The

most modern processes should be used so as to reduce

the relatively high operating costs in this type of

indvistry.

The paper-making industry is the third largest

19

source of i ndus t r i a l organic po l lu t ion a f t e r stock

breeding and the food indxjstr ies, the po l lu t ion i t

produces representing 10 percent of a l l indxjstrial

po l lu t ion in advanced coun t r i e s .

About one t h i r d of t h i s po l lu t ion cons is t s of

the white water from the actxial manufacture of paper,

while the other two-thirds a r i s e from the manufacture

of the various mechanical, semichemical, b i s u l p h i t e ,

k r a f t , unbleached or bleached piilps.

Though simple physico-chemical treatment of the

the white water by f loccula t ion and s e t t l i n g or f loa

t a t i on can eleminate the considerable suspended sol ids

and 50 to 70 percent of the BOD, treatment of the pulp

manufacturing eff luents presents d i f f i c i i l t i e s l inked

to t h e i r colour due to l i gn in and t o the presence of

other compounds which are not eas i ly biodegradable.

I t requires complicated pretreatment (removal of colour

by the Degremont aluminium sulphate process from the

bleached kraf t piilp ef f luent , removal of sulphides

from the unbleached kraf t puLp eff luent e t c . ) . In a l l

cases, high r a t e b io logica l treatment should remove

the BOD which can vary from 10 Kg/t in the case of

mechanical pulp to 250 Kg/t in the case of Kraft pulps

without l iquor recovery.

20

The polluted effluents from the various manu

facturing processes in the automobile and metal fini

shing industries may be classified under three cate

gories according to source electroplating and heat

treatment shops, chemical deposition or etching,

picking plant, paint shops, and machining, grinding

or screw-cutting shops (soluble oils).

The first type consists of acid or basic inor

ganic pollutants or toxic pollutants (cyanides, hexa-

valent chromium, fluorides and heavy metals and

small quantities of organic surface active) pollutants.

Whether these effluents are discharged direct

or recycled via an ion exchange unit, it is necessary

to detoxify the final effluent by neutralisation, pre

cipitation of metal hydroxides, oxidation of toxic

hexavalent chromium. The organic matter can be fixed

on adsorbents.

Metal concentrations in acid baths can be

stabilised by ion exchange.

The second type of effluent corresponds in the

application of three successive coats of point-primer,

londercoat and the glass. The development of the

primer from electrophoresis (anaphoresis and cata-

phoresis) produces specific effluents which are treated

21

by floccialation and floatation in special Defire-

ment floatation units. The more highly polluted

effluents from the point slops are salted out in

situ by flocculants after which they are briefly

clarified and recycled. The recycled effluent must,

however, be deconcentrated and the blowdown treated

by flocculation and floatation.

Soluble oils are difficult to treat as the

paths used in this industry are highly concentrated

and have to be treated in plants varying greatly in size

and equipment. This type of effluent is treated by the

following processes : flocculation-floatation, ultra

filtration, reverse osmosis, possibly hot breaking or

incineration in exceptional cases. The process is

chosen according to the formula of the lubricants used.

The effluents from the petroleum refining and

petrochemical industries, which are separated according

to origin from the units or drains are treated in two

or three stages according to the nature and concentra

tion of the pollutants. These are mainly aliphatic or

aromatic hydrocarbons plus a wide variety of organic

and mineral compounds (phenols, mercaptans, sxilphides,

fluorides, organic acids, etc.).

The first stage consists of preliminary oil

22

removal by gravi ty separa t ion in two successive phases

intended to recover the free o i l s (Degremout c i r c u l a r

o i l removal u n i t ) .

The second or physical-chemical s tage ensures

coagulation of the emulsified o i l s by means of e i t he r

an organic coagulant or a metal hydroxide and poss ible

p rec ip i t a t i on or oxidation of the sulphides . The f loe

formed can be separated with excel lent r e su l t s in Flotazur

or sed i f lo tazur f l oa t a t ion tanks . In some cases o i l may

be removed by f i l t r a t i o n throi:igh sand or dual media

f U t e r .

The th i rd s tage i s necessary only when elemina-

t ing res idual BOD or phenol compounds. I t cons is t s of

b iological piorification carr ied out by Degremont in

three ways according to the nature and concentrat ion

of the soluble BODc- by high r a t e act ivated sludge

treatment, or by extended aera t ion;

By coordinated-material b io log ica l f i l t e r s ;

by pressiorised b io logica l f i l t e r s , or p i o l i t e

f i l t e r s -

Among other i ndus t r i e s , the iron and s t e e l

industry h i the r to produced p l lu t an t s in the form of

eas i ly separate suspended s o l i d s . However, advanced

technology i s tending to cause addi t iona l po l lu t ion by

dissolved s a l t s or o i l .

23

In the chemical and pharmaceutical industries,

where the manufacturing process is often intermittent,

rapidly changing technology necessitates constant

rethinking on treatability and often requires specific

pretreatment in the treatment units or special preli

minary techniques (e.g. stripping, carbonate removal,

oil removal etc.).

The textile manufacturing indvistries present

spacial problems in the reduction of colour and soluble

CX)D.

In fossil fuel and nuclear power station, where

waste streams produce pollution which often passes

unnoticed but which requires special treatment, such

effluents can often be recycled.

Disposal of Industrial Wastes

The treated effluents can be discharged into

surface water courses, sewers and onto land. The mode

of disposal however has to depend on the merits of

the case so that the problem of pollution can be mini

mized if not totally eleminated. It is important to

bear in mind that some of the stabilized industrial

effluents have a good manurial potential which should be

exploited. This practice will not only be useful for

our soil but also would be a good step towards minimizing

24

pollution. Neverthless it has to be ensured that the

treated effluent is safe enough to be lised for irriga

tion purposes.

Wastes are disposed off on land in two forms,

the solid wastes and the liquid wastes. The liquid

wastes include, sewage, sewage effluents and industrial

effluents. The disposal of these liquid wastes on land

is done by two distinct methods.

(i) Irrigation - wherein sewage or industrial waste

waters are utilized in raising profitable crops while

simultaneously affording satisfactory hygenic disposal.

(ii) Infiltration - of sewage or industrial waste

waters on land prepared for mere infiltration and dis

posal without any profitable crop raising, such vegeta

tion as may be permitted on the infiltration area should

be only for the purpose of facilitating or increasing

the rate of disposal by improving the conditions for

the dissipation of sewage or industrial effluents by

the action of roots and axjgmenting the rate of overall

disposal per unit of area by evapotranspiration losses

induced vegetation.

The harmful effect or infertility of sewage or

industrial waste - irrigated soils is due to any one

or combination of the following factors.

25

(i) Difficulty of carrying out agriciiltiiral

operation.

(ii) Anaerobic conditions in soil,

(iii) Restriction of root zone of plants.

(iv) Smothering of the crops by the flora of water -

logged lands.

(v) Possibility of a high concentration of salts

particularly sodium salts.

Salt may retard absorption of nutrients and water,

may themselves be toxic, or lead to alkailine conditions.

Anaerobic conditions also retard the bacterial activity

which is essential for nitrification.

Scientists are continuously assessing the possi

bilities of disposing of sewage sludge, municipal waste

water and the trade wastes on the land and on the utili

zation of the nutrients present in these wastes by the

crops.

C H A P T E R - II

SURVEY OF LITERATURES

26

C H A P T E R 2

SURVEY OF LITERATURE

Sco t t (1980) r epo r t ed a su lph ide p r e c i p i t a t i o n

process t h a t can be ijsed t o remove heavy meta ls from

waste s t reams and y i e l d s a su lph ide s ludge s u i t a b l e fo r

l a n d f i l l . The waste t r ea tment system c o n s i s t s of nex>-

t r a l i z a t i o n , p r e c i p i t a t i o n , c l a r i f i c a t i o n , f i l t r a t i o n

and s ludge dewate r ing .

Lead, Germanium and Zirconium in was tewate r

from semiconductor manufacture o r a n u c l e a r r e a c t o r

a re removed by p r e c i p i t a t i o n (Kosaku, 1980) . The

wastewater i s a e r a t e d a t pH 7-9 in t h e p re sence of a

c a r b o n a t e , then a f e r rous s a l t and an a l k a l i n e

compound a r e added ( t o pH 9-11) t o p r e c i p i t a t e t h e

m e t a l s . Thus a wastewater (pH 8.02) con ta in ing

75 .5 ppm germanium and 3360 ppm F luor ide was a e r a t e d

in t h e p resence of Na2C0,, and an FeSO^ s o l u t i o n was

added. Calcium Hydroxide was then added t o pH 1 0 , and

an an ion ic polymer coagulant was added, fol lowed by

n e u t r a l i z a t i o n . The superna tan t l i q u i d con ta ined no

germanium.

Kotani e t a l s (1980) t r e a t e d t h e l ead c o n t a i n i n g

wastewater by s o l i d i f i c a t i o n with c o n c r e t e or cement in

21

the presence of a harmless metal sialfate. Thus lead

containing pigment slvxige was mixed with aluminium

sulphate and cement. No lead was leached out a f t e r

five weeks.

Lyubman e t a l s . (1981) car r ied out the p r ec ip i -5 + t a t i on of As from water solut ions containing sulphuric

acid and arsenic and determined the optimum conditions

for the most e f fec t ive p r e c i p i t a t i o n of As- from sxol-

phuric acid and As-containing waste waters. The most 5+ effect ive p r e c i p i t a t i o n of As was achieved when calcium

hydroxide was lised as a p r e c i p i t a t i n g agent a t 80° and

a t pH 12.0-12.5 .

Electro-plating wastewater containing cyanide is

treated with sodium hypochlorite, (Thomas et als, 1981)

for conversion of cyanide to cyanate, and to carbondi-

oxide and nitrogen. The cyanide concentrations before

and after the treatment are 30 and 0.50 mg/L, respec

tively. The cyanide free wastewater containing metals

is treated with sodium hydroxide in two stages for proper

metal hydroxide precipitation followed by flocculation

for copper and nickel, the removal rates are /N-< 95 percent,

for silver and tin, '•>^ 75 percent.

Teslya et als. (1981) suggested the removal of

heavy metals from wastewater giving reduced amounts of

28

toxic wastes and reiJsable water by treating at pH 4-5

with the reaction product of a fayalite slag and a>SO^

and increasing the pH to 7-8.5 to precipitate the heavy

metals.

Higgins et als. (1982) suggested the treatment

of heavy metals wastewater by alkaline ferrous reduction

of chromium and sulfide precipitation. Ferrous sulphate

reduces rapidly and stoichiometrically the Cr(VI) in

synthetic plating rinse waters at a pH 7-10. Sodium

sulphide and ferrous sulphate act synergistically. The

oxidized Fe(II) ion coagxilates colloidal metal sxalfides.

Alkyl and EDTA, but not Ca hardness interfere with Cr

reduction, floe formation, and removal. Treatment

using FeSO^ and Na^S precipitation/coagulation followed

by direct upflow filtration provides effective removal

of chromium and cadmium from the rinse water.

The mechanism of adsorption of Iron on activa

ted carbon has been studied by Nakamori et als. (1982).

The adsorption isotherms conform to the Freundlich

equation. The amount of iron adsorbed is a function

of the H concentration. Iron is not adsorbed as

Fe- . Fe is not adsorbed from a O.Cl N H d soln. on

activated carbon. Fe(0H)2 is the adsorbed species.

Balykin (1982) reported the removal of mercury

29

from wastewater by filtering through activated carbon

is improved by pretreating the activated carbon with

a 20-25 percent solution of sodium thiosiilphate and

pH adjustment of the wastewater, frcxn 1 to 7.

Gregory et als. (1982) sioggested that, adsorbing

colloid foam floatation can be effectively x;>sed in

industrial wastewater treatment to remove copper, zinc,

chromium and mixtures thereof. Thus under optimal

conditions in pilot plant treatment, the copper (II)

and zinc (II) concentration in the treated effluent

was 0.1-0.3 and 0,5 mg/L respectively. Treatment of

electroplating wastewater containing copper (II), zinc

(II) and chromium (III) in concentrations of 20 mg each/L

produced effluent containing < 0.1 mg copper (II),

< 0.5 mg Zinc (II), and 1 0.2 mg chromium (III)/L.

The method was found to be more economically and advan

tageous than other conventional methods.

Mercury was effectively removed from industrial

wastewaters by precipitation with NaHS and subsequent

oxidation of excess NaHS with ferric chloride to prevent

the formation of ferrous si£Lphide and zinc sulphide

which could produce HpS after landfilling of the sludge

(Gechmann and Hennings, 1982).

Chisso Corp. (1982) reported that a wastewater

30

containing chromium (VI) and f luor ide i s reduced,

neutra l ized with calcium hydroxide, then, the resu l t ing

sl\jrry i s so l i d i f i ed with gypsum. The method can t r e a t

a Cr "*" and f luoride containing wastewater simxaltaneously.

Thus a wastewater containing Cr and sulphxjric acid was fit 2 t

t rea ted with MeOH to reduce Cr to Cr- , then t rea ted

with calcium hydroxide. Another wastewater containing

Cr and F was reduced with MeOH, then t rea ted with

calcium hydroxide. The two re su l t ing s l u r r i e s were

molded and cured for d isposal .

Petryaev et a l s . (1982) s t i r l ied the removal of

arsenic by passing NaÔOa-containing wastewater through

a cation exchanger r esu l t ing in the formation of HpCO r

and through an anion exchanger to remove carbonate.

The degree of pur i f i ca t ion is increased by aerat ing

wastewater a f te r passing through the cat ion exchangev

with a res idual concentration of 20-30 mg HÔO^/L.

Konkova (19B3) reported the use of indiostrial

wastes for the removal of heaA/y metal ions and petroleum

products from indus t r i a l wastewater. The removal of iron

and copper from wastewater using sawdust and an th rac i t e

wastes at various pH was much f a s t e r with than without

mixing, a t pH 3 with an adsorbent dose of 5 g/L. Iron

removal of 7^ percent was achieved in 3 h with and 18 h

31

without mixing. The dynamics of adsorption of the ions

were calcxiLated and xxsed to design an apparatus and

procedure. The optimal pH is 7 which requires only 2

adsorbers with a diameter of 5 m and a saw dust layer

thickness of 3 m Vs. pH 5 which requires 28 adsorbers with

the same diameter and 1,6 m.

Antimony (III) in small concentration is removed

from wastewater by adsorption on hydroxyl-apatite preci

pitates, (Treshchina et eils, 1983) in the presence of

calcium and phosphate with '-^ 100 percent precipitation

at pH 'N 12.0. The presence of chloride or nitrate at

15-20 mg/L did not interfere but the presence of oxide

and sulphate decreases adsorption of Sb(III) on the

hydroxyl apatite precipitates.

A wastewater containing arsenic is treated with

a titanium compound to fonn titanic acid which forms a

Co- precipitate with aresenic, (Anon 1983). Thus a synthe

tic wastewater pH 2-8 containing 97.08 ug As/ml was

treated with Ti(iso-PrO)^, stirred for 16 h at ^ ° , and

filtered. The filtrate contained 0.025-0.05^ Ug As/ral.

A very similar study was carried out for the

treatment of arsenic containing wastewater. A waste

water containing As is precipitated, oxidized and

treated with an amphoteric metal hydrooxide to remove

32

arsenic. Thus a synthetic wastewater containing

5 ppm As and 20 ppm PO^^ was treated with Fed,,

and the resulting siQ>ematant containing 0.5 ppm As

and 0.9 ppni PO^ was passed through a titanium hydro-

oxide containing column. The effluent contained 5 ppb

aresenic. The titanium hydroxide was prepared by trea

ting Ti0(0H)2 with sulfuric acid, palletizing and neu

tralizing with sodium hydroxide.

Hiroaki et als. (1983) studied on selective

adsorption resins. A macro nuclear chelating resin

(RMH) containing hydrazine groxqjs showed a good

affinity for chromium (III) at pH 5.8-7.5 in batch

e3q)eriments. The adsorption of chromium (III) on the

RMH was not influenced by the presence of Ca over the

concentrations range of 0.01-0.1 mol/L. In the column

method, chromium (III) in an aqueous solution was

favourably adsorbed on the FJMH, when a chromiim nitrate

solution (pH 3.8 and containing either 1 or 10 mg

Cr (III)/L) was passed thro\Agh the column. Chromium

(III) was effectively eluted by passing 20 bed volumes

of 4 mol sodium hydroxide over the resin at a space

velocity of 7.5 h.

The uptake of cadmium (II) and copper (II) from

aqueous solutions at 40° was investigated (Hideki et als,

1983), on slightly soluble hydroxyapatite (HAP), Octa-

calcium phosphate (OCP), and brushite (DCPD). The

33

uptake of M " (ca '*' or Cu "*") proceeded Initially

through an ion exchange reaction Ca "*" 7-^ M"*" and

then through subsequent reactions accompanying the

formation of either Cd-iUCPO^)^.^!^© or, presumably

2+ Ca -dissolving Cu,(P0/^)2»3H20. Exchange fractions of

M"*" were established to be > 10 Cd or > 8 mol percent

Cu "*" for HAP, 2. Cd '*' or 2 9 mol percent Cu " for OCP

and 2 6 mol percent M"*" for DCPD. The reactivity was

in the order HAP < OCP < DCPD, and Cu ' -i9)take occurred

more easily than Cd - iq)take.

Heavy metal ions were removed from solutions

modelling machinery factory wastewaters ixsing coal

as an adsorbent, (Rodionov et als. (1983), Zinc remo

vals of 99 percent were obtained at pH 6 at coal dosages

of 20 g/L, copper (II) and chromium (III) were decreased

to permissible limits at lower pH and adsorbent dosages.

Results were verified with real wastewaters and a scheme

involving 2-stage coal adsorption was developed for

local wastewater treatment.

The reaction of model solutions of chromium

(VI), iron (III), chromium (III) and sulphate with saw

dust was studied by Militsa and Zalesina (1983), to

develop a combined method for treating concentrated

spent solutions from electrolytic chrome plating using

wood wastes. Air-dried sawdust was successfiiL in remo-

3A

ving chromium (YI) at an optimal solid/liquid ratio of

1:8:85 and contact time of 10 mln. in preliminary tests.

The best removals of chromium (VI), chromium (III) and

iron (III) were obtained using saw dust pretreated with

sulphuric acid solution. A 7-stage scheme was developed

for treatment of electroplating wastewater with treated

saw dust.

Frederick et als (1984)reported the removal of

cadmium, copper and lead from wastewaters by 3 algal

species with a concentration factor (CF) on the order

of magnituie of 10^, for zinc, CF is 300-800.

A process was developed to remove CN and COD

(Koichi, 1984), components from metal plating and coati3Tg

wastewater. Cyanide was decomposed with NaClO, and then

residual CN was further removed by precipitation as zinc

cyanide complex. The COD components were removed by

ion exchange, activated carbon, or inorganic adsorbent

but the use of a suitable activated carbon was found

the best.

Low sulphide stockpile leachate was treated in an

unsaturated failing bed to remove trace metals (copper,

nickel, cobalt, zinc), Leachate (28,000 L) passed through

the bed at flow rates of 50-3300 L/day, at pH 6.5-7.1.

Trace metal overall removal was 25 percent, copper 75-90,

35

nickel 23-58, cobalt 3^70 and zinc 12-75 'L

Barbara and Alexander (1984) sxjggested a new

indijstrial wastewater treatment method for the removal

of organic and inorganic contaminants in aqueoi;u5 solxi-

tions by adsorption in a single step, resulting in a

dry, stable sludge.Copper, nickel,zinc, chromium and

iron are removed from a chelated wastewater with 97-100

percent,efficiency.

Hartl et. als (1984) reported the wastewater

treatment for copper, nickel and lead removal by flo-

cculation-sedimentation. The treated wastewater

contains copper, nickel and lead in the amounts < 0.79,

< 1.6 and < 3.4 mg/L, respectively. The metal contents

in the sludge are'^ 50 '/. below the maximum allowed values,

the solid content in the dewatered sludge cake is 60-70 '/.

Ferdinand et.als. (1984) eleminated cyanides in

wastewater, using formaldehyde. Mixing of 2 wastewater

streams, 1 containing cyanide and the other amino acids,

hydroxy acids, and their salts. The reaction rate was

pH dependent and its completeness depended on the CN-

HCHO mol. ratio (R). A complete cyanide removal was

obtained at pH 8-9 and R = 1.5.

Ozonation of electroplating wastewaters containing

OOD 28,200, total organic carbon 6230, chloride 2300,

36

sulphate 720, total nitrogen 3240, nickel(ll) 387, and

other metals 142 mg/L resxilts in an effluent which can

be biologically oxidized with acclimated sludge after

addition of a nutrient solution. The COD was redixed

to 150 mg/L.

Anon (1984) used a strongly magnetic FeO.OH for

treating metal containing wastewaters. Iron (II) in a

solution at pH : 8 is oxidized with air or other oxi

dant, then additional iron (II) and alkaline compound

are added to the solution to pH 7 with further aeration

to prepare FeO-OH-coated magnetite. Wastewater (0.9 L)

containing metal was mixed with 0.7 g magnetite sludge

and 0.1 L water and then stirred at pH 10.5 for 2 h.

No metals were observed in 0.8 L of supernatant. The

magnetite was then regenerated.

Jeffrey (1985) reported the control of heavy

metal discharge in the printed circtiit industry contain

ing copper using NaBH. only, as opposed to NapS20^ and

NaBH. , resulted in lower volumes of sludge which contained

a high copper content (85-95 percent on a dry basis) mak

ing metal recovery completely feasible. Sodium bisulphite

was used prior to NaBH. application when the wastewater

contained ammonium persulfate. The slixige settled

easily, and the effluent contained Cu < 1 mg/L.

37

Toyaki et als. (1985) reported the recovery of

chromium (VI) from wastewater with Iron (H) hydroxide.

Chromium (VI) was selectively recovered containing Cd(ll),

Pb(II), Zn(II), Cu(II) and Cr (III) by adsorption on

iron hydroxide at pH 4,5 and, after separation of the

precipitate, desorption in alkaline solution (pH 10.5).

Phosphate interference was suppressed by increasing the

amount of iron hydroxide and the sulphate interference

was appreciably suppressed by the use of calcium hydroxide

instead of sodium hydroxide as a neutralizing agent.

A thermodynamic analysis of an aq. Hg(II)-Cl~

system showed that decreased chloride concentrations,

are favourable for mercxary removal from the solution by

the neutralizing hydrolysis method. However in the

dilvrte brine from chlor-alkali plant, a certain amount

of free chloride prevents mercury (II) precipitation

and subsequent secondry pollution by Hg-containing salt

sludge .

Showa Denko (1985) reported the removal of

chromium compounds from aqueous electrolytic solutions,

chromium, compounds are adsorbed on iron hydroxide and

removed by filtration.

Walter (1985) proposed a method and apparatus

for removing environmentally unfavourable metal ions from

rinse waters by ion exchange by placing a by pass in the

38

rinse cycle e.g. of an etching apparatus, to feed a

part of the circulating rinsing agent through an ion

exchanger.

Kiyoshi et als (1985) suggested the removal and

recovery of nickel in wastewater from chemical plating

using a strong-base anion-exchange resin (in chloride

form) and a chelate resin (in H form). This method

was proved effective for the removal and recovery of

nickel from the waste rinse water from chemical nickel

plating. The adsorbed nickel on these resins could be

eluted efficiently by 2N hydrochloric acid.

Wastewater containing atleast iron (II) in high

concentration is treated in an oxidation tank with

Fe-oxidizing bacteria, cultivated in highly concentra

ted liquid containing impurities, to oxidize Fe * to

Fe "*", and the generated slvidge containing Fe-oxidizing

bacteria is repeatedly used in the oxidation tank.

(Anon 1985).

Douglas (1985) studied the removal of heavy

metals from wastewater at near neutral pH and without

the addition of large amounts of alkaline chemicals,

by coprecipitation with carrier precipitate precursor

cations (Fe(OH),) and anions (aq. NH,). After preci

pitation, removal by filtration, the cadmium, chromium

39

copper, iron, nickel, lead and zinc concentrations

decreased from 0.6, 2.3, 5, 50, 3.5, 106 and 953

respectively to < 0.1, < 0.1, 1.4, < o.l, 0.2, < 0.5

and 2.8 ppm respectively.

Manfred (1986) suggested the removal of heavy

metals from wastewater by anaerobic biosorption. An

anaerobic sludge-bed reactor removed copper, nickel,

zinc and mercury 99.5, chromium 75, and sulphate

35-40 percent, from vinasse.

Lortie et al (1986) reported the adsorption of

Cr^* on freshly prepared Ti(0H)i . They found that the

temperatiore and ionic strength have little influence on

the adsorption of chromium (III) on titaniiim hydroxide.

Takashi et al. (1986) suggested the treatment of

mercury containing wastewater by reducing Hg ions to

Hg metal, volatilizing the Hg metal with volatile gases,

and cooling to recover the Hg vapor with the gases

recycled for rexise. The recycling of the volatile gases

is effective in preventing Hg diffusion to protect the

environment.

Masao et al. (1986) proposed the treatment method

of dust containing chlorides of heavy metals produced

during melting of flyash, mixed with an alkali metal

40

phosphate in an amount at least equal to that of chlo

rides, melted and solidified. Thus 10 parts dust

(separated from flyash and containing Cd, Pb, Cr , Zn,

Hg, SO^ , CI, Na, K, and Ca) was mixed with 7 parts

Na2HP0^, melted at 600° and solidified. The solid was

completely glassy showed volume decreases 6o percent,

and significantly low elution of heavy metals (Od, Pb,

Cr , Zn, Cu, Hg), and SO^ ~ in leaching test.

Sadhana et al. (1986) extracted chromium (III)

from wastewater in the presence of NaClO^ as a salting

agent, The chromium (III) removal was maximum at a pH

of 2.8 and concentration of Triisoamyl phosphate 30 7

with an initial chromium (III) concentration of 1.5 x

10"^ mol. At Cr(III) concentrations of 0.75-5.0 mg/L,

the removal efficiency was 98.7 percent. The removal

of Cr(III) is significantly affected by the presence of

metals such as Mn(II), Al, and Fe (III).

Licsko and Takaes (1986) reported the removal of

heavy metals in the presence of colloid-stabilizing

organic material and complexing agents. The removal of

heavy metals is improved by Mg addition and adjusting

the pH. The pH that is necessary for destabilizing a

colloid is lowered by increasing the Mg"*" concentration.

The method can be used for the combined removal of

1

different heavy metals (e.g., copper, zinc, cadmium etc.)

In the presence of ammonium salts, some heavy metals

(copper, zinc, nickel) produce stable heavy metal-amine

complexes. The Cu-tetramine complexes formed are stable

and satisfactory heavy metal removal is attained only

at pH 10.5-11.0 since the Mg can only improve the heavy

metal removal to a small degree.

Music (1986) studied the sorption of chromium

( VI) and chromium (III) on aluminium hydroxide. The

factors that influence the sorption of Cr (VI) and

Cr (III) were investigated. The mechanism of sorption

was also interpreted. The best conditions for the

fixation of Cr (VI) and Cr (III) by aluminium hydroxide

are presented.

Makhmetov et al (1986) suggested the method for

removal of arsenic from wastewater by adding a mixture

of V-containing and P-containing slags in a 1:(1-1.5)

ratio as oxidizing and precipitating reagents respectively

and then removing the resultant precipitate.

Tsodikov et al. (1986) stuiied the removal of

lead ions from wastewater, by adding an alkaline earth

metal nitrate and an ammonium salt. The degree of

purification is increased and the procedure is simpli

fied by using ammonium orthophosphate as the ammonium

42

salt at a wt. ratio of lead, alkaline earth metal,

and ammoniim orthophosphate of 1:3-200:3-200. They

have found that stroncium and calcium may be used as

the alkaline earth metal.

Removal of heavy metals from wastewater was

done by mixing an aq. Na aluminate solution with NaÔ-

AlpO, mol. ratio > 1, and the heavy metal compounds

precipitated at pH : 7 and are removed from the water

(Volker, 1986).

Shugxii and Guangwei (1987) studied the effective

ness of removing lead, cadmium and chromium from waste

water by water hyacinths. The experiments conducted

were (l) determination of the removal rates of the metals

under different initial concentrations and various pH

values (2) detection of the accumulation and release of

the metals and (3) detection of the removal of lead,

cadmium and chromium from waste-water samples. Water

hyacinths were effective for removing these heavy metals

from wastewater and their effectiveness was in the order

Pb > Cr > Cd. In 6 days, the purification lo^d and the

purification efficiency for Pb, Cd, and Cr were 0.076-

0.496 and 71.21-85.96, 0.008-0.041 and 61.54-83.33, and

0.022-0.056 g/kg (dry wt.)-day and 29.52-58.65 percent

respectively.

43

A similar stxady was carried out by Mario et al.

(1987). The average concentration of silver in dried

material from water hyacinth was 9 ng/g. The plants

were kept for 24 hr in a solution containing 40 mg/L

silver. The silver uptake was 70 percent. The process

can be used for wastewater treatment of Ag-containing

effluents, the water hyacinth used for biogas generation,

and the fermentation residual processed for silver

recovery.

Gudekar and Trivedy (1987) suggested the treatment

of engineering industry waste using water hyacinth.

Refrigeration compressor manufacturing wastewater treat

ment with Sichhomia crassipes resulted in OOD, TSS, and

BOD removal efficiencies of <: 94.15, 9B.07, and 90 percent

respectively. The roots of the E. crassipes contained

maximum concentration of nutrients.

Kalalova et al, (1987) reported the râoval of

heavy metals from industrial wastewater. The ammoniation

of ethylene dimethylaerylate-glycidyl methacrylate copo-

lymer gave a macroporus resin (sp. surface area 60 m /g

which is able to complex metals. This resin was-used

as a chemisorbent for the removal of Ag, Cu, Ni, and Zn

from wastewater. In the case of Ag (main pollutant) the

resin had 0,8-1 mmol/g capacity at pH 6.

kk

Schultz et al (1987) stxadied the adsorption and

desorption of metals on ferrihydrite. Metal ions are

removed from dilute solution by sorption onto ferrihydrite

and are then desorbed into a more concentrated solution,

at lower pH, the heavy metals Cu, Pb, Ni, 2n, Cd and

Cr (III) can be quantitatively sorbed from a simulated

plating solution onto ferrihydrite at pH 9.5. Lowering

the pH to 4.5 substantially desorbs the metals.

Krishnan et al (1987) used the natural materials

s\ich as hair and certain plants, which are inexpensive

for the absorption and hence the cleaniip of heavy ele

ments from polluted water was observed. These natural

materials effectively removed the heavy elements concen

tration to the extent of ^ 500. The contact time required

is on the order of several hours. The capacities of

absorption varies from r^ \ to r\j 5 g/kg for mercury and

are lower for arsenic and cadmium. The results show

that with hair, nearly 10,000 L of Hg contaminated water,

a typical output from a 100 ton chior-alkali, plant,

can be treated with >^ 1/2 Kg of hair valued at nJ 25

cents. This makes the process extremely cos-effective

compared to the conventional processes now in use.

Clinoptilolite is an effective sorbent for the

mercury removal from wastewaters in the manufacture of

45

acetic acid (Horvathova and Stefan, 1987), however it

is quickly clogged by colloidal substances and for this

reason, is not suitable for the removal of palladium

from wastewaters in the manufacture of an antioxidant.

Palladium can be adsorbed by clinoptilolite in the abs

ence of colloidal impurities. The following order of

decreasing sorption capacity of clinoptilolite was

obtained : Cs > Pb > Fe > Cu > Zn, Sr, Cd, Al, Co >

Ni > Mn > Cr.

Kenichi et al. (1987) reported the ranoval of heavy

metals from sewage sludge by aeration and extraction with

aq. HNO^ and aq. HCl to remove ^ 75 percent of the copper

zinc, cadmium and lead. Aeration and addition of

hydrogen peroxide increased the efficiency of removal.

Kaiser et al. (1988) suggested the method for the

removal of arsenic from wastewater of the lead glass

industry. Iron (III) in combination with hydrogen peroxide

was used, resulting in an effluent containing < 0.1 mg

As/L. Lead removal by carbondioxide was not affected

with the arsenic removal process.

Slocum et al. (1988) reported the treatment of

metal finishing wastewater with peatmoss contact columns.

Peat moss was effective in the removal of metals and

cyanide. Minimum effluent cyanide concentration was 9.6-

6

12 percent of influent cyanide concentration. Aera

tion of the peat columns increased CN removal capacity

by 27 percent.

Mc-Kay et al. (1988) carried out the sorption

of metal ions by Chitosan. Equilibrium isotherms were

determined of copper (II) and mercury (II) sorption

from aqueous solution by chitosan and kinetics of the

process was studied to evaluate the usefulness of this

material in wastewater treatment.

Mashima et al. (1988) examined the adsorption

of chromium (VI) using a column packed with polyamine

chelating resin. Adsorption of chromixam (VO was 53.6

mg/ml of resin at a Cr(VI) concentration of 100 mg/L,

and 164 mg/ml of resin at a Cr(VI) concentration of

13.3 g/L. Regeneration of resin was achieved by reduc

tion and elution of Cr(VI) with 0.1 percent, hydroxyl-

araine ssLLt aqueous solution at pH 1. Other metal ions

were not eluted.

Henning et al. (1988) studied the removal of

mercury by activated carbon process. The adsorption was

done on activated carbon impregnated with potassium

iodide or sulphuric acid.

Stewart et al. (1988) suggested reverse osmosis

kl

to remove cadmltuB from a metal processing waste stream.

Cd concentration was reduced from I65 to 0.003 mg/L.

Juergen et als (1988) reported the treatment and

recovery of the metals from wastewater. Pb and/or Cu

are selectively recovered from metal processing effluents

containing iron, e.g. wire drawing in a mtdtistage pro

cess comprising precipitation at pH 1.5-2.5 with excess

aq. 10 / sodium sulphide solution, precipitation at pH

3.5-^.5 with 5-10 percent calcixom hydroxide or sodivun

hydroxide and precipitation of remaining Fe ions at pH

8.0-9.5 with NaOH or Ca(OH)p. The precipitates contain

ing Pb and/or Cu are treated to recover the metals.

Diane and Thomas (1988) stiidied the removal of

manganese from aquoxjs industrial waste effluents.

Manganese and/or F and heavy metals are precipitated

from washing effluents from aluminium and tin-coated

steel can manufacturing by the addition of phosphate

in acid medium followed by the addition of Ca in

alkaline medium, where the PO '/Ca "*" ratio is 3:1 to 1:2:5,

at pH 8-9.

Phenols and heavy metals, e.g., Zn, Cu, Cd, Ni,

Pb, Hg, Mn, Cr in a wastewater from ore refining are

removed by mixing with sintered powdered desulfuriza-

tion slag containing Fe oxides 45-48 (Fe basis), CaO

48

and CaS 10-15 (Ca basis), and S compoxmds, 1.5-1.6 */

(S.basis) and then by separating the resulting deposit

from the treated effluent. The resulting supernatant

is discharged. This method is economical to operate.

(Smith 1988).

It appears from the available literature that

several attempts have been made to achieve the separa

tion of 2n (II) from Cd (II) by using different tech

niques, but no work has yet been done and reported on

reversed phase thin layer chromatography (TLC) for the

above mentioned separation. The work presented in this

dissertation describes the chromatographic behavioxor

of some heavy metal ions and their separations. Silica

gel loaded with tributyl amine (TBA) was found to be a

suitable adsorbent for the separation of some toxic metal

ions.

C H A P T E R - III

REVERSED PHASE THIN LAYER CHROMATOGRAPHIC

SEPARATION OF HEAVY METAL IONS ON SILICA

GEL LAYERS LOADED WITH TRIBUTYL AMINE

49

C H A P T E R 3

I N T R O D U C T I O N

The discharge of heavy metals which are non

biodegradable pollutants often contained in the

industrial waste water has been the subject of great

concern in recent years. The heavy metals cause

adverse effects on the living organisms whereas some

are lethal even at very low concentration. Therefore

the presence of sixih substances in water beyond permi

ssible levels may constitute chemical hazard and

render the water unfit for benificial uses. Among

the analytical techniques, the thin layer chromato

graphy is an important tool for the detection and

separation of heavy metals in the field of Environmental

Chemistry.

Description of the Planar Chromatography :

Planar chromatography takes two forms. In thin

layer chromatography, separation takes place on a layer

of a finely divided solid that is fixed on a flat surface.

A sheet or strip of heavy filter paper serves as the

separatory medium for paper chromatography. Thin-layer

chromatography was developed in the late 1950s and by

now has become the more important of the two planer

methods.

50

Thin-layer chromatography provides remarkably

simple and inescpensive means for separating and iden

tifying the components of small samples of complex

inorganic, organic, and biochemical substances. F\jr-

thermore, the methods permit reasonably accurate

quantitative determination of the concentrations of

the components of such mixtures.

General Considerations-.

In planar chromatography, a drop of a solution

containing the sample is introduced at some point on

the planar surface of the stationary phase. After

evaporation of the solvent, the chromatogram is developed

by the flow of a mobile phase (the developer) across the

surface. Movement of the developer is caused by capillary

forces. In ascending development, the motion of the

mobile phase is upward, in radial development, it is

outward from a central spot. Gravity also contributes

to solvent flow in descending development, where move

ment is in a downward direction.

The general principles developed earlier for

column chromatography appear to apply equally well to

paper and thin-layer media. Within these media,

repeated transfer of solute between the stationary and

51

mobile phases occurs. The rate of movement of the solute

depends upon its partition coefficient -

K » C, s/^

It is customary to describe the travel of a particular

solute in terms of its retardation factor R-, which is

defined as

distance of solute motion R >

distance of solvent motion

To compensate for uncontrolled variables, the

distance travelled by a solute is frequently compared

with that for a standard substance under identical con

ditions. The ratio of these distances are designated as

std.

Thin-Layer Chromatography;

Sta t ionary Phase : The so l id absorbents (or sometimos

adsorbents) employed in th in- layer chromatography are

s imi la r in chemical composition and p a r t i c l e s ize to those

of the various types of column chromatography. The most

widely used substances is s i l i c a ge l , which often func

t ions as a support for water or other polar solvents for

p a r t i t i o n chromatography. If, however, the s i l i c a layers

i s oven dried a f te r preparat ion, much of the moisture is

52

lost and the surface becomes a predominately solid one

that serves as an adsorbent for adsorption chromato

graphy.

Thin layer chromatography (TLC) of heavy metal

ions on silica gel (SG) layers offers interesting

possibilities which are greatly enhanced when these

layers are loaded with high molecular weight extrac-

tants. Silica gel retains solutes almost exclusively

on the basis of polarity and thus the separation of

solutes with close polarity even with different molecular

weights is difficult. The selectivity in such cases can

be effected only by varied choice of mobile phases.

Reversed phase-TLC offers some distinct advantages

over normal phase TLC by providing several factors such

as organization of the hydrocarbon ligands on the silica

surface, intercalation of solvent into the bonded layer

and the activity of residual silanols on the solid supp

ort. All these factors influence the selectivity of

the medium in a peculiar manner. Thus, in reversed

phase-TLC the selectivity of a medium can be altered by

varied choice of mobile phases or sorbents, as well as

by surface modifications involving the reaction between

silica support and reactive organo silanes of varying

chain lengths.

53

Because of its simplicity and better resolution

power, reversed phase chromatography has grown to be

a widely used method for chemical analysis of complica

ted mixtures. As a result a ntunber of studies have

been reported on the separation of metal ions using

1-14 various mobile and stationary phases. Most of these

reversed phase studies are based on the use of paper and

column chromatography and little attention has been paid

to the use of TLCp-^'^^,

Separation of Zn(II) from Cd(II) is of great interest

because of close resemblance in their chromatographic

behaviour. Several attempts have been made to achieve

their mutual separation by using normal and reversed

phase paper chromatography^^" , ion exchange chromato-

?? 25 Û graphy , solvent extraction -^, normal phase TLCr and

25 by precipitation . It is surprising that no work has

been reported on reversed phase TLC for the separation

of Zn(II) from Cd (II). It was therefore decided to

evolve optimum conditions for the separation of 2n(II)

from Cd(II), Ni( II) and Co(II) by reversed phase-TLC

using tributylamine (TBA) as stationary phase on SG

support. Aqueous solvent systems containing variable

concentration of formic acid and sodium formate were

used as mobile phases.

3k

EXPERIMENTAL

^paratus:

A thin layer chromatography apparatus (Toshniwal,

India) for the preparation of silica gel thin layers on

20 X 3 cm glass plates was used. The chromatography

•was performed in 2^ x 6 cm glass oars. Elico pH meter

was used for pH measurements.

Reaj ents :

Silica gel G (BDH)

Tributyl amine (TBA) of Fluka

Sodium formate (SF) and formic acid

(FA) of E. Merck were used.

All other reagents were of analytical grade.

Test Solutions and Detectors:

The 0.1 M solutions of aitrates, chlorides or

sulphates of most of cations were prepared in 0.1 M

?6 solutions of the corresponding acids as described earlier .

Various known volumes of standard solutions of metal ions

were taken to study the effect of loading on the Rp

values. To study the effect of pH of metal solutions

on the Rp value of cations. The pH of the sample solu

tions were brought to the required value by the addition

of either dilute NaOH or dilute HCl.

55

The metal ions were detected by xjsing conventional

spot test reagents.

Metal ions Detectors

VO^*, Cu " , Fe^*, Uol* Potassium ferrocyanide

p + Fe Potassium ferricyanide 4+

Ti Chromotropic acid

Al" Aluminon

^- Pyrogallol

Ni^*, Co^* Dimethyl glyoxime

Zn^*, Cd^*, Mn "*", Cr " Dithizone

Ag*,Bi^"^,Pb^*,Tl"^,Tl^*,Hg^"*" Yellow ammonium sulphide

Ta "*", La "*", Zr^* Alizarine red S

Se Stannous chloride

Th Thoron

Preparation of chromatopiates:

(a) Preparation of Plain SG Thin Layer Plates :

SG was slurried with demineralized water in the

ratio of 1:3 with constant shaking for 5 minutes. The

resulting slurry was coated on clean glass plates with

the help of an applicator to give a layer of 0.25 mm.

The plates were air dried first and then kept at 100° +

56

5°C for 1 h in an electrically controlled oven. The

plates were cooled to room temperatiare by keeping tbem

in a closed chamber before use.

(b) Preparation of TBA Impregnated SG Thin Layers :

Impregnated silica gel thin layers were prepared

by using two methods.

(i) Direct Impregnation Method :

20 gms of silica gel was shaken in a conical

flask with 60 ml of 10-70 percent TBA solution in benzene

(V/v) to obtain a homogeneous slurry. The resultant

slurry was spread over glass plates to form a layer of

uniform thickness {r>^ 0.25 mm). Benzene was allowed to

evaporate at room temperature. The plates were heated

at 100 _+ 5°C for 1 h. and then cooled to room temperature

by keeping in a closed chamber.

(ii) Indirect Impregnation Method :

The plain SG plates were first prepared by adopting

a method as mentioned above and then were impregnated by

placing in chromatographic Jars for development containiiTg

a 10-70 percent TBA solution in benzene (V/V). Benzene

was allowed to evaporate at room temperature and then the

plates were heated at 100°_+ 5°C for 1 h in an electrically

controlled oven. The plates were cooled to room tempera-

57

ture by keeping in a closed chamber and then used

as such.

Solvent SystemsUsed :

(i) Aqueous FA (10"^, 10"^, 0.1, 1.0, 5.0, 10.0,

and 20.0 M)

(ii) Aqueous SF (10"^, 10~^, 0.1, 1.0, 2.0, 5.0 M)

(iii) Mixtures of 1.0 M aq. FA and 1.0 M aq. SF in

8:2, 6:4, 1:1, 4:6 and 2:8 ratio)

Procedure :

The sample solution (3-5 yd) was loaded on plain

or TBA impregnated SG chromoplates with the help of

micropipette. The spots were dried at room temperature

before proceeding for development. The glass Jars cont

aining mobile phase were covered with lids and left for

10 minutes before placing the plates for development.

The plates were developed in a chosen mobile phase by

an ascending technique with a solvent run to 10 cm in

all cases unless otherwise stated. After the develop

ment was over, the plates were air dried and the cations

were detected by spraying appropriate coloring reagents.

The R^ values were calculated from the values of R,

(R^ of leading front and R^ (R^ of trailing front).

58

RESULTS AND DISCUSSION

Results of this study have been sununarized in

figxires 1-4 and tables 1-6,

Reversed phase chromatography on SG impregnated

TBA gave excellent results. The thin layers were of good

quality. However the plates prepared by direct impreg

nation method were found to be better than those obtained

by indirect impregnation method. The time of development

ranged from 1-2 h depending upon the composition of the

mobile phase used. The spots were compact and well

formed in all solvent systems and at all percent impreg-

nations (10-70 percent) of TBA. However, Cd , Ag ,

Hg2* and Hg^* showed some tailing (R -Rj,) > 0.3) in some

solvent systans. The R- values of metal ions were found

to depend \5)on the time and tenperature of drying of

impregnated SG plates. The plates were quite stable in

acidic developers and also in 1.0 M SF but at a higher

pH of mobile phase, the plates were deformed on drying.

As a result, the plates developed in 5.0 M aqueous SF

(pH = 7.75) get deformed on drying. The effect of

various factors on the chromatographic behaviour of metal

ions is given below.

1. Effect of Aqueous SF Concentration on the Mobility

of Metal Ions:

On the basis of chromatographic behaviour on SG

59

layers impregnated with 40 percent TBA in varying con

centrations of SF (O.OOl to 5.0 M), the metal ions

can be classified into the following groups :

(i) Metal ions such as \J0^^*, Fe^*, Al "*", Ag*, Pb " ,

Bi" , Tl^ and Ti did not show any mobility over the

entire range of SF concentrations. The low R- value

for these metal ions may be attributed to the formation

of anionic/neutral complexes with SF similar to those

reported by Qureshi et al for few cations. Hg^ and

Hg produced tailed spots starting from the point of

application.

(ii) Ni and Co moved with the solvent front giving

high R„ (/->.J0.9) over the whole concentration range.

The absence of sorption in these cases may be attributed

to the lack of formation of anionic metal formate

complexes.

(iii) Metal ions like Tl and Cd' ' showed an increase

in mobility with the increase in SF concentration giving

R^ equal to 0.9 in 5 M SF. The increase in R- value

with the increase in SF concentration may be probably

due to increased complexation at higher pH.

(iv) Cu "*" and Zn "*" did not move in solvents containing

upto 1.0 M SF. However a sudden increase in their R-

values in 2.0 M and 5.0 M SF was observed.

60

All the metal ions were detected satisfactorily

at all SF concentrations (0.001-5.0 M). The development

time increases with the increase in molar concentration

of SF until it reaches to 2 h in 5.0 M SF.

2. Effect of FA concentration on the Mobility of

Metal ions:

The study of chromatographic behaviour of metal

ions on ^0 percent TBA impregnated SG plates in acidic

developers containing varying molar concentrations of

aqueous FA (0.001-20.0 M) gave some interesting results.

The main points emerged out of this stixiy are as follows ;

(i) Hgp^ formed elongated spots at all FA concentra

tions while Bi "*" and Cd produced tailed spots (starting

from the origin) in 5-20 M and 0.001 M - 0.1 M FA respec

tively.

(ii) Ag"*", Pb "*" and Ti " remained at the point of

application at all FA concentrations losed. Conversely,

2+ 2 + Ni and Co moved with the solvent front probably due

to the solvation of these ions/complexes by the mobile

phase.

(iii) Uo|"*", Fe "*", Al "", Bi " , Zn - , Cr "", Cu^^ and Cd ""

did not move in mobile phases containing upto 0.1 M FA.

On further increase in acid concentrations these metal

61

ions show significant mobility giving R- 0.7-0.9 in

1.0 M FA. The R- values reach a maxiniiin (R^ = l.O)

at higher FA concentrations (i.e. 5-20 M). The higher

FA concentration was found unsuitable because of (i)

spreading of spots (ii) greater development time

(iii) less sharp detection of most of the metal ions.

The increase in R^ with increase in molar concen

tration of FA is attributed to the increase in the

number of H^ ions competing with the cations/or cationic

complexes, for the exchange sites.

3. Effect of TBA Impregnation on the Mobility of

Metal ions -.

Fig. 1 shows that TBA impregnated SG layers are

more strongly sorbing than unimpregnated or plain SG

layers for most of the metal ions as indicated by posi

tive values of AR-.. Here AR- is the measure of the

difference in the R« values of metal ions on unimpreg

nated and impregnated SG layers i.e. AR- = R^ on unim

pregnated SG layers- R» on impregnated SG layers. Thus,

TBA impregnation enhances the selectivity of the plain

SG layers.

Fig. 2 shows the effect of degree of impregnation

of TBA on the R^ values of metal ions in 1.0 M FA and

in 1.0 M FA + 1.0 M SF (2:8) solvent systems. The R^

62

--• 1-OM SF

-® l-OMSF + 1 OM FA (1:1)

+ 1-0 r

-y. 1-OM FA

-A O lM FA

< > O U . U . O Z O N < O X X | - » - Q . C D I D I -

cations

F i g . l :

Comparison of selectivitles of TBA^lmpregnated

and tminqpregnated silica gel layers in different

solvent systems.

63

values for only those cations which gave compact spots

were taken for plotting the figxires. It is evident

from fig. (2) that in 1.0 M FA, the R^ values generally

decrease with the increase in degree of impregnation.

However, Cd and Bi-"*" showed constancy in R- values at

2+ all degrees of impregnation. 2n showed significant

tailing (R^ » 0.0-0.6), over 10-20 percent impregnation.

In solvent system containing the mixture of 1.0 M

FA and 1.0 M SF in 2:8 ratio, the plots (fig. 2) showed

frequent fluctuations over the entire range of TBA impreg

nation. Interestingly, a few cations showed stronger

sorption at 30 percent TBA impregnation. Detection of

all metal ions were very clean and sharp at all degrees

of impregnation but the spots were more compact at higher

degrees of impregnation. The shapes of these curves can

be tentatively explained on the basis of the existence of

a neutral, positive, or negative species as well as the

possibility of formation of less adsorbed higher charged

negative complexes. Some other phenomena such as the

adsorption in the network of the support, precipitation

in the network of the support, precipitation, hydrolysis

and solvent solvent interactions, may play an important

role to effect the sorption behaviour of metal ions on

impregnated SG layers.

1-0

0-8

j 0-6

Rf 0-6

0-2

0-0

2+ Cd

-I 1 I 1 I I I

10 20 30 60 50 60 70 Vo impregnation wi th TBA

I I 1 ! I 1 i -

- O -

- ® -

Zn 2 +

J ! 1 I 1 1 L.

- O -

ô«..

Ni •2 +

J I 1 L 10 20 30 40 50 60 70 % impregnation wi th TBA

Fig . 2a and 2b :

P l o t of R^ Vs. pe r cen t age impregnation of TBA in benzene^

8 '& 1.0 M FA G 0 1.0 M FA + 1.0 M SF (2 :8 )

65

1.0 r

0 8

' O.G

Rf 0.^

0-2

00

10

0-8 \-

" 0.6

Rf 0.6 -

0-2 -

0-0

1-0 r

0-8

0-6 H

Rf 0.4

0.2 h

0-0

1.0

0 8

0-6

Rf 0.4

0-2 h

0-0

Co' 2 +

Mn 2 +

O-- - O - O — - O

Tl 3 +

O , . 'ô-^~^^^^.-^-o

Pb 2 +

-C t ^ -^--^-.^^^ 10 20 30 40 50 60 70

Vo impregnadon with TBA

J3—0-O iD -

- O ' '<y

Bi 3 +

- ^ - O — - r r r - - ^ Q - - O

- - 0 -

Tl

1 1

2 + Hg

1 1

o

1 1

10 20 30 40 50 60 70 Vo impregnation with TBA

2b

66

4. Effect of Mixed Solvent Systems Containing Mixture

of 1.0 M FA and 1.0 M SF on the Mobility of Metal

Ions :

It is clear from Fig. 3a that 1.0 M SF is the

best solvent for the separation of Zrr'^ from Cd , Ni "*"

2 + and Co on 60 percent TBA impregnated SG layers. Though

7+ ? +

the separation of Cd from Zrr in this solvent is also

possible on UO percent impregnated plates but the higher

tailing of Cd decreases the resolution of its separa

tion from Zn^* (Fig. 3b). It is clear from Fig. 3b that

1.0 M SF behaved differently than 1.0 M FA as a mobile

phase. Most of the cations move faster in FA and produce 2+ 2 + more compact spots compared to SF. Ni and Co showed

identical behaviour in both the solvent systems and

moved with the solvent front. Figs. 3c-d summarize the

chromatographic behaviour of metal ions in solvent systems

containing mixtures of 1.0 M FA ani 1,0 M SF in different

molar ratios. It is evident from these curves that most

of the metal ions showed relatively greater mobility and

higher compactness in solvents containing higher percen

tage of FA.

5. Sffect of pH of Metal Solutions on the separation

of Zn " from Ni " , Co " and Cd "*";

It is clear from Fig. that the R- values of

67

R 0 6

l O M SF

A = 1 0 M SF B = 1-0M FA

(C ) A=1-0M SF + lOM FA{8

8=1-0M SF + 1 0 M F A ( 2

C = 1-0M SF + 1-OM FA(1

2) 8) 1)

A = 1 0 M SF + VOM FA(6:A)

B=1-0M S F + l O M FA(/i-6)

— l_ 4( » o — ^ C 0> Tj 0> W» m ,0 .—

< > o u . u . o 2 o r N 4 < o x i f l p a . C D r ) » : i cations

Fig. 3 : Plot of R- Vs metal ions in different solvent systems

a - 60 '/ TBA impregnated silica gel layers.

b,c,d = 40 •/ TBA Impregnated silica gel layers.

• • compact spots; A A Tailed spots with

0- -G Tailed spots with RT-R^P < 0.4.

68

1-0

0-8

0-6

Rf 0-A

0-2

O'O 0

Cd ,'*' Ni ' ônd Co^"^

1 2 3 ii pH of metal solutions

Fig. 4 :-

Plot of pH of metal solxitions Vs R^ on silica

gel layers impregnated with 60 •/ TBA in solvent

system containing 1.0 M sodium formate and 1..0 M

formic acid in an 8:2 ratio.

69

Zn "*", Ni " , Co "*" and Cd "*" are independent of the pH

of the sample solution in the pH range of 1-5. Thus

2 + a good separation of Zn from these metal ions can be

obtained on 60 percent TBA impregnated SG layers in

mobile phase containing a mixture of 1.0 M SF and 1.0 M

FA in 8:2 by using unbxiffered sample solutions without

adhering to the close control of the sample pH.

The enhancement in the selectivity of SG layers on

impregnation with TBA provides an opportunity in achiev

ing many analytically important separations. Many such

separations have been actually realized and have been

2+ tabulated in tables 1-4. The separations such as Zn -

Cd 2*, Al5*-Cu2\ VD2•^-Tl5^ ^0^^.^\ Th'^^-Zr'^^ Fe^*-

Tl5^ Al5^-Cu2*-Ni2*-Ti^^ Cr^^-Bi5*-Cd2'^-Co2^ Zn - -Cd " -

Pb " and Zn2"*"-Tl* -Pb "*" are worth mentioning.

Table 5 summarizes the results of the effect of

loading on the R- values and the lowest possible detec

table amount of metal ions on the chromatopiates. It

is evident that TBA impregnated SG layers gave highly

compact spots over a wide range of loading amount of

the metal ions. 0.5 pg of Ni gave R„ equal to 0.9^

while it is 1.0 for 400 ug of Ni "*".

In order to bring out a more clear picture

regarding the separation of Zn "*" from Cd "*", Ni "*", and

70

Co , some TLC parameters such as AR- (R^ of separating

metal ion-R- of Zn ), separation factor (a) and reso

lution (Rs) have been calcialated. These data have been

presented in table 6. The values for a and Rs have been

calculated by using the following relationships.

(M » separating metal) ( i ) a = KZn/Kj^

/ 1 - R-

/ where K is a capacity factor which measures the degree

of retention of a solute compared to the solvent.

R : s 1/2 (d- -Hi2)

where AX is the distance between the centres of spots

and d-. , d„ are their respective diameters. Two solutes

are just separated if Rs is equal to 1. It is clear

from table 6 that a good separation of Zn from Cd ,

Ni and Co can be carried out by using the proposed

method. The AR- value is always greater than 0.5.

A high value of separation factor and well resolved

spots with R_ >, 5 are the added advantages of this

study.

The proposed method consisting the use of 40-50"/

TBA impregnated SG layer and a mixture of 1.0 M SF and

71

1.0 M FA in 8:2 ratio as developer is very reliable and

reproducible for achieving the separation of a particular

cation from others in general. It is particularly more

usefiiL if one needed sharper and clearer ternary and

quarteraary separations. The spots are so well formed

and compact that good quartemary separations are always

possible. It is a very reliable method to separate Zn

from over a reasonable pH range of sample solutions.

72

+> c 0) o t l 0) o,

s A •P •H

TJ 0)

-P CO

c bO 0)

^

ra t Q) >, CO -3

rH

a)

CO o •H f H •H CO

C O

n 0) >

•H Si o <

to C o •H

• P CO U CO a Q) CO

>> U CO c •H OQ

• »

CO rH

0) H X> CO H

• 0} 0 0) P (0 > . CO

p C (U > H O

CO

P C 0) ^ (D M M •H a c •H

< 03 H

,»-v

oT 1

cr: •^-^

•o ^ > 0)

:d <

CO

o •H P CO

CO a 0) to

CO

a <D p CO

CO

p

CD >

rH O

CO 1

» ^ t^

« o

• o

v_x

4-K>>

^

(< O

o o 1 o

• o

+ ^

•H

1

ir> (H

• o 1

K>i

O

+ fM

O >

s:

o • H

^ - N

00 •

o 1

o • H

N.^'

+ CM

•H 2

tu o

o o 1 o

• o

+ ^

1

i n H

• o

1 r O

+ cv

^

o o 1

o •

o

+ <r •H

EH

1

i n •

o 1

vO

O

+ K^

^

o o 1 o

• o

+ 4-

1

i n •

o 1

t ^

o

+ K>

(U

c o 1

cr> •

o

+ eg

•H 2

1

O •

o 1

o o

+ J-

•H

>^-s OvJ

•

o 1 i n

• o

\—y

+ CM P >

U o

o o 1 o

• o

+ -d-

•H EH

1

vO •

o cA o

+ cvyvj

+ CM

O O

+ CM

•H 2 :

<H

o CO

o ^

•H

a 1

o •

o 1

o o

+ f<^

Ct4 CO

s o • rH

< ^ o

• o 1

H • o

V . X

+ »n

0) tL,

u o

, -x CM

• O

1 K^

• o ^ ^

+ ^ 3 o

t

00 •

o 1

o rH

+ CM

^-^ O

• o 1 in

o •

o v--*

- » •

CM C N

U o

^'^ o

•

o 1

H •

o

+ rn

•H CQ

1

00 •

O »

o rH

+ CM

^

1

73

KN

H a:

1 • J

oc

n 0) > 0)

:d o <:

C o •H + CO u ca o, 0) t o

/ " • ^

t ^ •

o cA o

+ C\J o o

1

,--> CO CM

• o 1 i n CM

• o

• o (A

• o

+ CM

o u o

^^s vO CM •

o 1

K>

o

+ f ^ w

:3 o

1

^ - N

H •

O 1

CM •

O

^ • v

cn •

o 1

o H

+ CM •H

z 1

^ - x H

• O 1

CM

O

y - ^

vD •^

• O

a!,

o

- » •

CM

s 1

(• '-^ c>-H

• O

cA CM

O

, — N

o •

o 1

o o

+ 4-

1

, . ^ k

K^ ^f^

• O

1 vO K>

O

o 1

i n

• o

+ i n

CO

o /• ^ CM

• o 1

CM ^

o

+ K^

• o 1

i n CM •

o

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C H A P T E R - IV

USE OF ACIDIFIED SILICA GEL LAYERS AS AN

ADSORBENT IN CHROMATOGRAPHIC SEPARATION

OF SOME METAL IONS

83

C H A P T E R IV

INTRODUCTION

In c o n t i n u a t i o n of oxxr p rev ious work ^ ,

we have used ca rboxy l i c and mineral ac ids as impre-

gnants on s i l i c a ge l l a y e r s in o rde r t o unders tand t h e

r e t e n t i o n behaviour of some metal i o n s . As a r e s u l t

we have achieved some important s e p a r a t i o n s which a r e

d i s cus sed i n t h i s c h a p t e r . However, some more work

i s r e q u i r e d t o pu t t h e s e r e s u l t s fo r more p r a c t i c a l use .

In t h i s d i r e c t i o n , t h e q u a n t i t a t i v e s e p a r a t i o n of

d i f f e r e n t va lence s t a t e s of mercury i s i n p r o g r e s s .

The s e p a r a t i o n of Hg(II) from some metal ions on t h i n

l a y e r s of s y n t h e t i c i no rgan ic ion exchangers has been

31-36 e a r l i e r a t tempted by some workers-'^ -^ .

However t h e i r s t u d i e s s u f f e r t he fol lowing

l i m i t a t i o n s .

( i ) Effec t of anions on t h e s e p a r a t i o n of m e r c u r y ( l l )

from o t h e r ions has no t been examined.

( i i ) Loading e f f e c t of s e p a r a t i n g ions has no t been

s t u d i e d .

Therefore i t was thoughtworthwhile t o op t imize

t h e c o n d i t i o n for t h e s e p a r a t i o n of mercury ( I I ) from

s e v e r a l metal ions

&k

EXPERIMENTAL

Apparatus

Toshniwal TLC apparatus was used for the p re -

paucation of s i l i c a gel l aye r s .

Reagents

Silica gel G of BDH India and all other reagents

were of analytical grade.

Impregnants

Following aqueous impregnants whose concentra

tions are given in parenthesis were used.

(i) Oxalic acid (0,1, 0.5, 1.0, 2.0 and 10 /)

(ii) Citric acid (0.5 '/)

(iii) Tartaric acid (0.5 /)

(iv) Formic acid (0.5, 1.0, and 2.0 'A)

(v) Hydrochloric acid (O.l, 2.0, 5.0 and 10 '/)

(vi) Nitric acid (2.0 /)

(vii) Perchloric acid(2.0 and 5.0 "/)

Solvent Systems Used

The solvent systems used are given below.

85

Solvent System Composition EA-Acetone-FA-Water

10

8

7

2 : 1

6 : 1

8

10 : 1

k : 1

Preparation of silica gel plates:

Plain silica gel thin layers were prepared as

discussed earlier. For the preparation of acid impreg

nated silica gel layers 20 gram of silica gel was

shaken in a conical flask with 60 ml of 0.1-10 /. aqueous

solutions of various acids to obtain a homogeneous slurry.

The resultant slurry was spread over glass plates to

form a layers of uniform thickness ('~ 0.25 mm). The

plates were heated at 100 ± 5°C for 1 h, and then

cooled to room temperature by keeping in a closed

chamber.

Test Solutions and Detectors ;

Test solutions and detectors used were the same

as earlier.

86

Procedure

Plates were developed xjsing ascending technique

as discussed earlier and the ascent was kept 10 cm in

all cases.

RESULTS AND DISCUSSIONS

The results obtained have been shown in figs.

5-7 and tables 7-10. The silica gel layers impregna

ted with carboxylic and mineral acids provide some

new separations. Silica gel layers impregnated with

acids were found more selective to most of the metal

ions compared to plain silica gel layers. The R^

value of metal ions remained almost constant in the

range of 0.1 - 2 / oxalic acid impregnation. It is

evident from fig. 5 that oxalic acid impregnated

silica gel layers retained the metal ions more

strongly than the plain silica gel layers. Cr, Mn

and V are only the exceptions which showed strong

adsorption on plain silica gel layers. The chromato

graphic behaviour of metal ions on mineral acids and

carboxylic acids impregnated silica gel layers have

been summarized in fig. 6(a) and (b). The mobility

of the most of the cations was higher in formic acid

impregnated plates compared to oxalic acid impregnated

plates (fig. 6b) showing the stronger complexing

87

< I— ^c:>5îi 11 o 2 - X I—»— < } — > o 2 : i j L U . o 2 o f ^ 2 o > X I—»—

Metal ions »

Fig. 5 :

Plot of AR^ (R^ on plain silica gel layers

Rf on Impregnated layers) Vs metal ions.

88

a)

'mpregnants:

o 2 / HCI

X 2 / HGO^

A 2/ HNO3

. 5/ HCIO,

(b)

 o l l 2 £ S z 5 . 5 M ^ S ^ f ^ x P f e ^ ^ 3

o 2/ FA

® 2 / Ox Ac

Metal ions

Fig. 6(a) and (b)

Mobility of metal ions on mineral acid and carboxylic acids impregnated s i l i c a gel l aye r s in ethyl ace ta t e -acetone-formic acid-water so lvent system.

89

tendency of oxalic acid. Amongst the mineral acids(Fig.7)

xjsed, perchloric acid and hydrochloric acid were found

better impregnants. The optimiam impregnant concentra

tion was found to be 5 percent for HCl or HCIO^ and

2 percent for oxalic acid. Almost all the cations

tailed on silica gel layers impregnated with 0.5 'A

oxalic acid, citric acid or tartaric acid. 5 percent

perchloric acid impregnated silica gel layers gave

more compact spots compared to 5 percent hydrochloric

acid impregnated plates. Ni "*", Cd^*, Zn "*" and Fe^*

tailed at all HCl concentrations (O.l - 10 percent).

Th " , Bi^*, Ag*, Pb " , Tl"*" , remained at the point of

application, while Cu " , Uo|*, Fe moved with the

solvent system at all HCl concentrations. However,

the R- of Co increases with the HCl concentrations.

The substitution of water by 1.0 M aqueous sodium

formate solution in solvent system leads to the

formation of tailed spots for most of cations. The

R- values of cations were found to be dependent on

the concentration ( /. volume) of formic acid or water.

Several important separations achieved on acid

impregnated silica gel layers have been summarized in

tables 7-lC.

The separation of Hg "*" from Hg " and of Th "

from UOp using 2 percent oxalic acid and 5 percent

perchloric acid as impregnants respectively was carried

90

© ® 5 •/ HCl

O O 5 •/ HCIO^

C E ^. -J C t- 0>-r3-^*CTib>+ X5—r-—, (- ±: 0; a* ovz . 3 ^ ' . < ^r>02:LL l i_oZ O MM

Metal ions

Fig. 7 Comparison of hydrochloric acid and perchloric acid

as impregnant on the mobility of cations in ethyl

acetate-acetone-formic acid-water solvent system.

91

2- — -out in the presence of certain anions. OOt , BrO,, I ,

lor, Br", NO2, NOl, CI"", CrÔrj^'f and CrO^" do not hurt

the above separations. The A R^ values for Hg - Hg^

4+ 2-f and Th - UOp separations were found to be 0.85 and

0.68 respectively. The loading effect of separating

metal ions has also been studied and the separation

of 10 yig of Hg(ll) fromlmgof Cu(II), 1 mg of Ni(ll),

10 mg of Pb(II) and 50 yg of Hg(I) has been successfully

achieved.

Apart from the qualitative separations, the second

aspect of this problem is the quantitative separation

of Hg(II) from other metal ions such as copper (II),

nickel (II), lead (II) and mercury (I). The quanti

tative separation of mercuric ion from mercurous ion

is important from analytical as well as theoretical

point of view.

It is also aimed to apply the method developed

for the quantitative separation of mercury (II) on

industrial wastes containing mercuric salts.

92

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97

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S U M M A R Y

98

C H A P T E R V

S U M M A R Y

This d i s s e r t a t i o n e n t i t l e d , Studies on the Disposal

and Treatment of some Indi is t r ia l Wastes, mainly com

pr ises of four chap te rs . The f i r s t chapter i s the

introductory par t giving a general idea regarding

environmental po l lu t ion and nature and cha rac t e r i s t i c s

of i ndus t r i a l eff luent which plays a important ro l e in

degrading the qual i ty of the environment. As the rapid

i ndus t r i a l i za t i on i s taking p lace , there has been an

appreciable increase in the volume of the indus t r i a l

e f f luents , containing several tox ic substances and

often heavy metals which causes an adverse effect on

aquatic l i f e when dischairged in to the water body.

Relevant to t h i s subjec t , in the second chapter,

a de ta i led and upto date l i t e r a t u r e on the treatment

and disposal of i ndus t r i a l wastes, has been reviewed.

In addi t ion, the d i f fe ren t methods for the ranoval

and recovery of heavy metals from indus t r i a l effluents

have also been described. Among the ana ly t ica l tech

niques used for the de tec t ion and separation of heavy

metals (qua l i t a t i ve and quant i ta t ive) the th in layer

chromatographic method has been found to be much more

accurate , r e l i a b l e and inexpensive. This method i s

99

foxmd to be very sensitive even upto the microgram

quantity. Therefore, it was thought to optimize the

different conditions adopting thin layer chromatogra

phic method using silica gel as an adsorbent,by preparing

a synthetic industrial waste containing toxic metal

ions and finally to apply the optimized method on

wastes from different industries.

The third chapter deals with the study of thin

layer chromatographic separation of heavy metal ions

on silica gel layers loaded with tributylamine. The

chromatographic behaviour of some heavy metal ions has

been stixiied in formic acid sodium formate system.

Several important binary,ternary and quarternary sepa

rations have been achieved. The separations such as

2n2*-Cd2^ Al5-^-Cu2*, YO^^-Tl^^ VO^^-W ^t Th -Zr" "-

Fe5^-Tl5% Al5^-Cu2*-Ni2-^-Ti'^\ Cr5^-Bi5•^-Cd2^-Co2^

Zn '*"-Cd ' -Pb ' , and Zn^^-Tl"^ -Pb "*" are very important

from theoretical as well as analytical point of view.

The effect of various factors such as (i)varying

concentration of aqueous sodium formate (.001 to 5.0 M),

(ii) Varying molar concentration of aqueous formic acid.

(.CC1-2C.0 M), (lii) percent impregnation of trlbuty-

lamine (10-70 / ) , (iv) mixed solvent systems containing

mixture of 1.0 M formic acid and 1.0 M soidium formate,

, (v) pH of metal solutions, (vi) and loading amount

of metal ions were studied on the mobility of metal ions.

The lower detectability level of some of the metal ions

100

playing an important roie in water quality is foimd

Cu "" (1.0 ^ ) , Ni^^ (0.5 pg), Co^* (10.0 pg), Zn^*

(0.3 ys)f and for Cd (l.O pg). Hence the proposed

method consisting the vse of -60 percent TBA impre

gnated silica gel layers and a mixture of 1.0 M

sodium formate and 1.0 M formic acid in 8:2 ratio as

developer is very reliable and reproducible for achi

eving the separation of a perticular cation from others

in general.

In the last chapter a comparative study of plain

and acids impregnated silica gel layers towards the

adsorption of some metal ions was carried out and some

new separations were achieved. It was found that acid

impregnated silica gel layers were more selective for

most of the metal ions compared to plain silica gel

layers. Oxalic acid impregnated layers retained the

metal ions more strongly. Amongst the mineral acids

used, hydrochloric and perchloric acids were found

better impregnants. Concentrations of carboxylic and

mineral acids as impregnants were established.

R E F E R E N C E S

101

REFERENCES

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Reviews, Vol, 6, Elsevier, Amsterdam, 129, 1964,

2. Cerrai, E.; and Ghersini, G,; J. Chromatog., l6,

258, 196if.

3. Cerrai, E,; and Ghersini", J. Chromatog. 18,12^,

1965.

4. Yu Mxorinov, I.*, Kartavtseva, A.G.; and Yu Nikitin,

E.', Zh analyt. Khim, 32, 904, 1977.

5. Przeszlakowski, S.; and Soczewinski, E.; Chem.

Analit, 11, 895, (1966).

6. De, A.K,;and Sarkar, S.K.; Sep. Sci. 9, 431, 1974.

7. Yedi, C.G. and Shinde, V,M,; Analyst, 101, 993T5 ,

1984.

8. Yeole, C.G.;and Shinde, V.M.; Indian J. Chem.

23A, 1053. 1984.

9. Brinkman, U.A.Th.; De Vries, G.;and Van Dal en, E.',

J. Chromatogr., 22, 407, 1966.

10. Brinkman, U.A.Th.; DeVries, G.;and Van Dalen, E.;

J. Chromatogr., 23, 237, 1966.

11. Cerrai, E.", and Testa, C.; J. Chromatogr., 6, 443,

1961.

102

12. Heldur, R. B.; and Khopkar, S.M.; J. Liq, Chromatog.

8(1), 95. 1985.

15. Heldur, R.B.; and Khopkar, S.M.; Analyst, 109 (11),

1493, 1984.

14. Bhosale, S.N.; and Khopkar, S.M.; Talanta, 32(2),

155-7, 1985.

15. QiJreshi, M.-, Sethi, B.M.; and Sharma, S.D.-, J. Liq.

Chromatogr. 6(1), 163, 1983.

16. Qiireshi, M.; Mohammad, A.i and Fatimaj N., J. Liq.

Chromatogr., 8(7), 1279-92, 1985.

17. Muchova, A. i and Jokl, V.; Chem. Zvesti, 30(5), 629,

1976.

18. Muchova, A.-, and Jokl, V.; Acta, Fac, Pharm.

Univ., Cominianae, 26, 9 (1974).

19. Krausz, I." and Orban, M.; Magyarkem Poly, 69,

493, 1963.

20. Pollard, F.H.; Banister, A.J.-, Geary, W.J;

and Nickless, G. •, J. Chromatogr., 2, 372, 1959.

21. Yede, C.G; and Shinde, V.M.-, J. Indian Chem. Soc.

23A, 1053, 1984.

22. Ser.ja, S.D.L, and TaOhui Le", Fenxi Huaxue; 12,

934, 198/+, CA : 102(8), 71950V, 1985.

23. Sasaki,Y.; Anal. Chim. Acta, 127, 209, 1981.

103

2^ . Qiireshi, M.; and Thakur, J . S . ; Sepn. S c i . , 1 1 ,

46U, 1976.

25 . Wang, Zhikeng; L i , Guangzu Hijaxue Tongbao; 1 ,

52 , 1985.

26 . Qureshi , M.; Varshney, K.Gj and Ra jpu t , R.P.S.- ,

Anal. Chem., ^ 7 , 1520, 1975.

27 . Qureshi , M. v Varshney, K.G; and Katjshik, R.C. i

Anal. Chem., ^ 5 , 2^33, 1973.

28 . FatLma, N.i Mohammad, A.; Sep. S c i . Technol , 19 ,

Z+29-^^3, 1984.

29 . Ajmal, M.; Mohammad, A.; Fat ima, N; ,J.Liq. Chroma-

t o g r . , 9 , 1877-1909, 1986.

50. Quresh i , M.', Mohammad, A.; Fat ima, N. ; J . Liq .

Chromatogr. , 8, 1279-1292, 1985.

5 1 . Qtireshi , M. ; Varshney, K.G.', Fat ima, N . ; Sep. «

S c i . 12 , 321-328, 1977.

32. De, A.K.i Pal, B.K.; Sep. Sci. 15, 1271-1275, 1980.

33. Sen, A.K., Ghosh, Ch.U.; J. Liq. Chromatog., 3,

71-79 (1980).

34. Sen, A.K., Das,S.B.; Ghosh, U. C., J. Liq. Chromatog.

8, 2999-3008, (1985).

lOA

35. De, A.K,; Chakraborty, P.; J. Liq. Chromatogr.»

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Off.Anal. Chem., 64, 792-732 (1981).

P 3593 F

Joiipiial of Planar Chromatograpliy —Modern TLC

DYNORPHIN (1-10)/SORBITOL IN SIMS BLOT nj/2 ,235

m/z 12 36 [] tlf'-'

.:^~,'

Secondary ion mass spectrometry in imaging analysis. See page 738

2/88 A Publication of iQj H t t t M g

Reversed Phase Thin Layer Chromatographic Separation of Heavy Metal Ions on Silica Gel Layers Loaded with Tributylamine

Mohammad Ajmal*, A. Mohammad, N. Fatima, and Akhtar H. Khan

Key Words:

Thin layer chromatography, TLC Heavy metal ions Tributylamine loaded silica Reversed phase

Summary

Chromatographic behavior of some heavy metal Ions on silica gel layers loaded with tritrntylamine has been studied in formic acid-sodium formate systems. Several important binary, ternary and quartemary separations have t>een achieved. Zn has t>een successfully separated from Cd, Ni, and Co. Some TLC parameters for Zn-Cd, Zn-Ni and Zn-Co separations have also t>een calculated.

1 Introduction

The discharge of heavy metals, which are nondegradable pollutants often contained in industrial waste water, has been the subject of great concern in recent years. Heavy metals cause adverse effects on living organisms, and some are lethal even at very low concentration. Therefore, the presence of such substance in water beyond permissible levels may constitute a chemical hazard and render the water unfit for many uses. Among the analytical techniques available, thin layer chromatography is an important tool for detection and separation of heavy metals in the field of environmental chemistry.

Reversed phase TLC offers some distinct advantages over normal phase TLC by providing several special features, such as organization of the hydrocarbon ligands on the silica surface, intercalation of solvent into the bonded layer, and the activity of residual silanois on the solid support. All these factors influence the selectivity of the medium in a specific manner. Thus, in reversed phase TLC the selectivity of a medium can be altered by varying the mobile phases or sor-bents, as well as by surface modifications involving reaction between silica support and reactive organosilanes of varying chain lengths.

Because of its simplicity and better resolution power, reversed phase chromatography has become a widely used method for chemical analysis of complicated mixtures. As a

M. Ajmal, A. Mohammad, N. Fatima, A. H Khan, Environmental Research Laboratory, Department of Applied Chemistry, Z H. College of Engg. and Technology, Aligarti Muslim University, Aligarh 202 002. India

result, a number of studies have been reported on the separation of metal ions using various mobile and slationary phases [1-14]. Most of these reversed phase studies are based on the use of paper and column chromatography and little attention has been paid to the use of TLC [15-1^ .

Separation of Zn(ll) from Cd(ll) is of great interest because of close resemblance in their chromatographic behavior. Several attempts have been made to achieve their mutual separation by using normal and reversed phase paper chromatography [19-21], ion exchange chromatography (22), solvent extraction [23), normal phase TLC [24], and by precipitation [25]. It is surprising that no work has been reported on reversed phase TLC for the separation of Zn(ll) from Cd(ll). It was therefore decided to establish optimum conditions for the separation of Zn(ll) from Cd(ll), Ni(ll), and Co(ll) by reversed phase TLC using tributylamine (TBA) as stationary phase on a silica gel (SG) support. Aqueous solvent systems containing variable concentrations of fonnic acid and sodium formate were used as mobile phases.

2 Experimental

2.1 Apparatus

A thin layer chromatography apparatus (Toshniwal, India) for the preparation of silica gel thin layers on 20 x 3 cm glass plates was used. Chromatography was performed in 24 x 6 cm glass jars. An Elico pH meter was used for pH measurements.

2.2 Reagents

Silica gel G from BDH, TBA from Fluka, sodium formate (SF) and formic acid (FA) from E. Merck (India) were used. All other reagents were of analytical grade.

2.3 Test Solutions and Detectors

The 0,1 M solutions of nitrates, chlorides, or sulfates of most of cations were prepared in 0.1 M solutions of the corresponding acids. Various known volumes of standard solu-

128 Journal of Planar Chromatography 1988 Dr. Alfred Huethig PuDlisêrs

RP-TLC o' Heavy Mel.il Ions

tions of metal ions were taken to study the effect of loading on tfie flf values. To study tfie effect of pH of metal solutions on the R, value of cations, the pH of the sample solutions were brought to the required value by the addition of either dilute NaOH or dilute HCI. Zn^' and Cd^* were detected with difhizone solution and other metal ions were detected by using conventional spot test reagents [26].

2.4 Preparation of Chromatoplates

2.4.1 Preparation of Plain SG Thin Layer Plates

SG was slurried with demineralized water in the ratio of 1:3 with constant shaking for 5 minutes. The resulting slurry was coated on clean glass plates with the help of an applicator to give a layer of 0.25 mm. The plates were air dried first and then kept at 100°±5''C for 1 h in an electrically controlled oven. Tlie plates were cooled to room temperature in a closed chamber before use.

2.4.2 Preparation of TBA Impregnated SG Thin Layers

Impregnated silica gel thin layers were prepared by two methods.

Direct Impregnation Method: 20 g of silica gel was shaken in a conical flask with 60 ml of 10-70% TBA solution in benzene (V/V) to obtain a homogeneous slurry. The resultant slurry was spread over glass plates to form a layer of uniform thickness (= 0.25 mm). Benzene was allowed to evaporate at room temperature. The plates were heated at 100 ± 5°C for 1 h and then cooled to room temperature in a closed chamtjer.

Indirect Impregnation Method: The plain SG plates were first prepared by adopting a method as mentioned above and then were impregnated by placing them in chromatographic jars for development containing a 10-70% TBA solution in benzene (V/V). Benzene was allowed to evaporate at room temperature and then the plates were heated at 100°± 5°C for 1 h in an electrically controlled oven. The plates were cooled to room temperature in a closed chamtjer and then used as such.

2.5 Solvent Systems Used

Aqueous FA(10"^ 10-^ 0.1. 1.0, 5.0. 10.0, and 20.0 M) Aqueous SF (10"^, 10-^ 0.1, 1.0, 2.0, 5.0 M) Mixtures of 1.0 M aq. FA and 1.0 M aq. SF (8:2, 6:4, 1:1, 4:6. and 2:8 ratio)

(0 (ii) (iii)

2.6 Procedure

The sample solution (3-5 MO was loaded on plain or TBA impregnated SG chromatoplates with the help of micropi-pettes. The spots were dried at room temperature t)efore development. The glass jars containing mobile phase were covered with lids and left for 10 minutes before introducing tfie plates for development. The plates were developed in the chosen mobile phase by the ascending technique with a solvent run to 10 cm in all cases, unless othenwise stated. After

development, the plates were air dried and the cations were detected by spraying appropnate coloring reagents The R, values were calculated from the values of R, (ft. ot leading front) and fly {Rt of trailing front).

3 Results and Discussion

The results of this study are summarized in Figures 1-4 and

Tables 1-6.

Table 1

Binary separations achieved on silica gel layers impregnated with 40% TBA in different solvent systems.

Solvent system Separations achieved {R^ - Rj)

1.0 M FA V(y-(0.3-0.15)-Ti'''(0.0-0.0) or Ap-(0.8-0.7) V(y*(0.3-0.15)-W*-(0.0-0.0) or Np-(1.0-0.8) AP'(0.6-0.5)-Ti*-(0.0-0.0) Fe'-(0.7-0.5)-Ti'-(0.0-0.0) Ti'*(0.0-0.0)-Ni^-(0.9-0.7) UOi*{0.8-0.6)-Ti"(0.0-0.0) or VO'*(0.35-0.2) Fe^*(0.0-0.0)-mixtures of Ni^'. Co'' Mn'-(1.0-0.8)-Cu="(0.3-0.2) or Fe'-(0.1-0.0) Mn^'(1.0-0.8y-Bi''(0.1-0.0) or Zn'-(0 05-0.0) UOf(0.25-0.22)-Co'-(0.8-0.7) Ap-(0.2-0.1)-Cu'-(0.3-0.26) or Cd'-(0.8-0.7) Ap-(0.2-0.1 )-Ni'-{ 1.0-0.9) Zn'*(0.28-0.17)-Cd'-(0.8-0.66) UO|-(0.36-0.33)-Zr^-(0.0-0.0) Ti''*(0.0-0.0)-Ap-(0.42-0.2) or Ta**(0.45-0.3) Se'-(1.0-0.9)-Pb'* or Bi '(O.O-O.O) Se'-(1.0-0.9)-Ti**(0.0-0.0) or Fe"(0.25-0.0) Se'-(1.0-0.9)-Zn''(0.25-0.1) U'*(0.75-0.6)-Zr'-(0.0-0.0) VO^*(0.3-0.0)-Zn^-(0.6-0.45) or Cd'-(0.6-0.4)

1.0 M S F

M .0 M SF + 1.0 M FA (8:2)

1 . 0 M S F +

1.0 M FA (4; 6) 1.0 M S F + 1.0 M FA (6:4)

Tr(0.66-0.52)-Tp-(0.0-0.0) Cr^*(0.53-0.45)-Ni^-(1.0-0.9) Se'*(0.68-0.50)-Bi'l0.08-0.0) or Pb'-(O.O-O.O) Zn'*(0.83-0.7)-Ni^-(1.0-0.9) Cd^'(0.7-0.5)-Nl'*(1.0-0.8) Fe''(0.75-0.4)-Ni^* + Co"(1.0-0.8)

Reversed phase chromatography on SG impregnated with TBA gave excellent results. The thin layers were of good quality. However, the plates prepared by direct impregnation proved superior to those obtained by indirect impregnation. The time of development ranged from 1-2 h depending upon the mobile phase composition. The spots were compact and well formed in all solvent systems and at ail percent impregnations (10-70%) of TBA. However. Cd^*. Ag*, Hg2**, and Hg^* showed some tailing («L -RJ > 0.3) in some solvent systems. The R, values of metal ions were found to depend upon the time and temperature of drying of the impregnated SG plates. The plates were quite stable in acidic developers and also in 1.0 M SF but at a higher pH of mobile phase the plates were deformed on drying. Specifically, the plates developed in 5.0 M aqueous SF (pH - 7.75) were deformed

Journal of Planar Chromatography VOL. I.JUNE 1988 1 2 9

RP-TLC of Heavy Metal Ions

Table 2

Binary separations obtained on silica gel layers impregnated with 60% and 20% TBA using different solvent systems.

% Impreg- Solvent system Separations achieved (ft, - R,) nation with TBA

Table 4

Quarternary separations achieved on silica gel layers impregnated with 40% TBA by using solvent system containing 1.0 M SF and 1.0 M FA In an 8:2 ratio (ascent 12 cm).

Separations achieved (R^ - R,)

60 1.0 M FA

60 60

20

1.0 M S F

1.0MSF + 1.0 M FA (8:2)

1.0MSF + 1.0 M FA (8:2)

AP*(0.55-0.45)-Ni'*(0.8-0.7) Ti'*(0.0-0.0)-Np-(1-0-0.7) Ti'*(0.0-0.0)-Ta'*(0.95-0.45) Zn'*(0.0-0.0)-Ta'*(0.9-0.4) Zr^*(0.0-0.0)-Th**(0.8-0.45) Ti**(0.0-0.0)-Th'*(0.85-0.5) Mn^*(0.7-0.55)-BP'(D.D-0.0) VO^*(0.6-0.5)-T1^*(0.05-0.0) VO^*(0.6-0.5)-2r'*(0.05-0.0) VO^*(0.05-0.4)-W**(0.04-0.0) VCy *(0.45-0.3)-Cu'*(1.0-0.9) Vcy *(0.55-0.35)-Cu'*(1.0-0.9) Zn'*(0.1 -0.0)-Crf*(1.0-0.75) Zn'*(0.3-0.2)-Hg'*(0.04-0.0) Hg2*(0.35-0.25)-Ptf'(0.1-0.0) CU^*(0 .3-0 .2) -NP*(1 .0-0.9)

Cd='*(0.9-0.7)-Ag*(0.O-0.0) V(y*(0.2-0.0)-CkJ^*(0.9-0.7) VO^*(0.2-0.0)-Fe'*(0.63-0.45)

AI^*(0.2-0.17)-Cu^*(0.3-0.28)-NI^*(0.9-0.6)-Ti''-(0.0-0.0) AP* (0 .2 -0 . 15)-Cd='*(0.8-0.7)-Ni^*(0.9-0.8)-Ti*-(0.0-0.0)

Ti'*(0.0-0.0)-UO^*(0.46-0.44)-Co'*(1.0-0.9)-Ap-(0.15-0.14) Ti'*(0.0-0.0)-Zn^*(0.4-0.36)-Cd^*(0.9-0.75)-Ni^-(1.0-0.9) Ti**(0.0-0.0)-Co^*(1.0-0.8)-Cf^*(0.2-0.15)-Cd^*(0.63-0.52) Cr^'(0.07-0.0)-Bi^*(0.45-0.37)-Crf*(1.0-0.8)-Co^*(0.8-0.7) Cr'*(0.17-0.16)-Ag'(0.0-0.0)-Cd'*(0.85-0.73)

Table 5

TLC data for some metal ions on SG layers impregnated with 40% TBA using 1.0 M SF + 1.0 M FA (8:2) as solvent system.

Metal Ions/Metal salts

Cu^Vcopper chloride Ni^Vnickel sulfate Co^Vcobalt chloride Zn^Vzinc chloride Cd^Vcadmium nitrate

Concentration range loaded (pg)

1.0-400 0.5-400

10.0-600 0.5-400

10.0-200

Range of R, obtained

0.3 -0.37 0.94-1.0 0.9 -1.0 0.33-0.41 0.72-0.85

Lower detectability level (pg)

1.0 0.5

10.0 0.3 1.0

Table 3

Ternary separations achieved on silica gel layers impregnated with variable concentrations of TBA in different solvent systems.

% Impregnation with TBA Solvent system Separations achieved (ft^ - Ftr)

20

40

40

40

60 60

1.0MFA + 1 . 0 M S F ( 8 : 2 )

1.0 M FA + 1 . 0 M S F ( 8 : 2 )

1.0 M FA + 1 . 0 M S F ( 4 : 6 )

1.0 M FA + 1 . 0 M S F ( 6 : 4 )

1.0 M FA 1.0 M FA + 1 . 0 M S F ( 8 : 2 )

70 1.0 M S F +

1.0 M FA (8:2)

Zn'*(0.65-0.1)-Cd^*(0.9-0.7)-TI'*(0.0-0.0)

Ti**(0.0-0.0)-UO|*(0.36-0.33)-Ni^*(1.0-0.7) Ti**(0.0-0.0)-Zn'*(0.4-0.3)-Co'*(0.95-0.9) Ti**(0.0-0.0)-UOf(0.36-0.33)-NP*(1.0-0.87) Ti**(0.0-0.0)-UOf(0.36-0.33)-Co^*(1.0-0.85) VO^'(0.20-0.0)-UOr(0.48-0.4)-Ti'*(0.0-0.0) AP*(0.26-0.25)-Ti**(0.0-0.0)-Cd^'(0.55-0.5) AI'*(0.12-0.10)-Nl'*(1.0-0.9)-Ti**(0.0-0.0)

Co^*(0.85-0.7)-Ti**(0.0-0.0)-AP*(0.55-0.45) Cu'*(0.35-0.20)-Cd'*(1.0-0.8)-Pb^*(0.0-0.0) Zn='*(0.23-0.20)-Cd^*(0.95-0.8)-Pb'*(0.0-0.0) Zn'*(0.27-0.25)-Cd^*(0.95-0.8)-Hg|*(0.0-0.0) UO|*(0.27-0.25)-Fe"(0.1 -O.0)-Co='*(1.0-0.9) VO^*(0.1 -0.0)-Fe'*(0.35-0.3)-Co^*(1.0-0.9) Cu'*(0.3-0.2)-Ni^*(1.0-0.92)-Ag-(0.0-0.0) Cu'*(0.3-0.25)-Cd='*(0.97-0.8)-Bi^*(0.06-0.0) TP(0.23-0.2)-Cd^*(1.0-O.8)-Agl0.O-0.0) TI'*(0.23-0.2)-Hg='-(0.0-0.0)-Cd^*(1.0-0.8) TI'*(0.38-0.35)-Pb^*(0.1 -0.0)-Cd'*(1.0-0.95) TP*(0.27-0.25)-TI*(0.0-0.0)-Ni^-(1.0-0.95) Zn'*(0.22-0.15)-Cd^*(0.88-0.77)-Ti'-(0.0-0.0) Tt*(0.75-0.65)-Zn^-(0.3-0.18)-Bi'*(0.0-0.0) Zn^*(0.1 -0.05)-Tr(0.65-0.5)-Pb'-(0.0-0.0) UO|*(0.28-0.24)-Zr'*(0.0-0.0)-Co^-(0.95-0.8) Cu'*(0.3-0.25)-Co^*(1.0-0.9)-Ti*'(0.0-0.0) Cu^*(0.3-0.25)-Co^*(1.0-0.85)-Zr'*(0.0-0.0)

130 VOL. I.JUNE 1988 Journal ot Planar Ctirotnatography


Table 6

TLC parameters for the separation of Zn'* from Cd '

and Co'* with 1.0 M SF + 1.0 M FA (8:2) solvent system.

Ni '

% Impregnation with TBA

40

60

70

Separating cation pair

Zn-Cd Zn-Ni Zn-Co Zn-Cd Zn-Ni Zn-Co Zn-Cd Zn-Ni Zn-Co

TLC Afl,

0.52 0.52 0.48 0.65 0.71 0.69 0.73 0.78 0.72

Darameters a

10.1 16.3 11.98 25.69 60.76 45.14 48.8 86.6 39.6

Rs

5.3 4.38 5.3 4.66 7.00 7.00 5.33 9.62 6.27

on drying. The effects of various factors on the chromatographic behavior of metal ions are given below .

3.1 Effect of Aqueous SF Concentration on the Mobility of Metal Ions

On the basis of their chromatographic behavior on SG layers impregnated with 40% TBA in varying concentrations of SF (0.001 to 5.0 M), metal ions can be classified into the following groups:

(0 Metal ions such as U0|*, Fe^*, AP*, Ag*. Pb^*, B\^\ 1\^\ and Ti** showed no mobility over the entire range of SF concentrations. The low R, value for these metal ions may be attributed to the formation of anionic/neutral complexes with SF similar to those reported by Oureshi et a/. [27] for rew cations. HgJ* and Hg^* produced tailed spots starting from the point of application.

(iO Ni^* and Co^* moved with the solvent front giving high R, (= 0.9) over the whole concentration range. The absence of sorption in these cases may be attributed to the lack of formation of anionic metal formate complexes.

(iii) Metal ions like Tl* and Cd^* showed an increase in mobility with the increase in SF concentration giving fl, equal to 0.9 in 5 M SF. The increase in R, value with the increase in SF concentration is probably due to increased complexation at higher pH.

(Iv) Cu^* and Zn^* did not move in solvents containing up to 1.0 M SF. However, a sudden increase in their R, values was observed in 2.0 M and 5.0 M SF.

All the melal ions were detected satisfactorily at all SF concentrations (0.001-5.0 M). The development time increases with the ncrease in molar concentration of SF until it reaches to 2 h in 5.0 M SF.

3.2 Effect of FA Concentration on the Mobility of Metal Ions

The study of chromatographic behavior of metal ions on 40% TBA impregnated SG plates in acidic developers containing

varying molar concentrations of aqueous FA (0.001-20.0 M) gave some interesting results. The main points emerging from this study are as follows:

(i) HgJ'' formed elongated spots at all FA concentrations while Bi^* and Cd^* produced tailed spots (starting from the origin) in 5-20 M and 0.001 M - 0.1 M FA, respectively.

(ii) Ag*, Pb^*, and Ti"* remained at the point of application at all FA concentrations used. Conversely, Ni^* and Co^* moved with the solvent front, probably due to the solvation of these ions/complexes by the mobile phase.

(iii) UOl\ Fe^\ A!'*, Bi^\ Zn^\ Cr^*, Cu^\ and Cd^* did not move in mobile phases containing up to 0.1 M FA. On further increase in acid concentrations, these metal ions show significant mobility giving ft, 0.7-0.9 in 1.0 M FA. The R, values reach a maximum (R, = 1.0) at higher FA concentrations {i.e. 5-20 M). The higher FA concentration was found unsuitable because of (i) spreading of spots, C") longer development time (iii), less sharp detection of most of the metal ions.

The increase in W, with increasing molar concentration of FA is attributed to the increase in the number of H* ions competing with the cations or cationic complexes for the exchange sites.

3.3 Effect of TBA Impregnation on the Mobility of Metal Ions

Figure 1 shows that TBA impregnated SG layers are more strongly sorbing than unimpregnated or plain SG layers for

l.OMSF • l-OMSF + IOM FA (1:1)

+0.8

.•0-6

I •0-6 ARf

• 0-2

00

-0.2

catlons Figure 1

Comparison of s«lectjvjtles of TBA-impregnated and unimpregnated silica get layers in different solvent systems.

Journal o( Pla«Br Ciiromalogtnphv VOL I.JUNE 1988 1 3 1


most of the metal ions, as indicated by positive values of AWf. Here Afl( is the measure for the difference in the fl( values of metal ions on unimpregnated and impregnated SG layers, i.e. Afl, = fl, on unimpregnated SG layers - R, on impregnated SG layers. Thus, TBA impregnation enhances the selectivity of the plain SG layers.

Figure 2 shows the effect of the degree of impregnation of TBA on the R, values of metal ions in 1.0 M FA and in 1.0 M FA + 1.0 M SF (2:8) solvent systems. The R, values for only those cations which gave compact spots were taken for plotting the figures. It is evident from Figure 2 that, in 1.0 M FA, the R, values generally decrease with increasing degree of impregnation. However, Cd^* and Bi^* showed constancy of R, values at ail degrees of impregnation. Zn^* showed significant tailing (R, = 0.0-0.6) over 10-20% impregnation.

In solvent system containing a mixture of 1.0 M FA and 1.0 M SF in a ratio of 2:8, the plots (Figure 2) showed frequent fluctuations over the entire range of TBA impregnation. Interestingly, a few cations showed stronger sorption at 30% TBA impregnation. Detection of all metal ions was very clean and sharp at all degrees of impregnation but the spots were more compact at higher degrees. The shapes of these curves can be tentatively explained on the basis of the existence of a neutral, positive, or negative species as well as the possibie formation of less strongly adsorbed higher charged negative

complexes. Some other phenomena, such as the adsorption in the network of the support, precipitation in the network of the support, precipitation, hydrolysis, and solvent-solvent interactions, may play an important role affecting the sorption behavior of metal ions on impregnated SG layers.

3.4 Effect of Mixed Solvent Systems Containing Mixture of 1.0 M FA and 1.0 M SF on the Mobility of Metal Ions

It is clear from Figure 3a that 1.0 M SF is the best solvent for the separation of Zn^* from Cd^*, Ni^* and Co^* on 60% TBA impregnated SG layers. However, the separation of Cd^* from Zn^* in this solvent is also possible on 40% impregnated plates but the greater tailing of Cd^* decreases the resolution of its separation from Zn^* (Figure 3b). It is obvious from Figure 3b that 1.0 M SF behaves differently from 1.0 M FA as a mobile phase. Most of the cations move faster in FA and produce more compact spots compared to SF. Ni^* and Co^* show identical tjehavior in both the solvent systems and move with the solvent front. Figures 3c-d, summarize the chromatographic behavior of metal ions in solvent systems containing mixtures of 1.0 M FA and 1.0 M SF in different molar ratios. Evidently, most of the metal ions show relatively greater mobility and higher compactness in solvents containing tiigher percentages of FA.

_ j I 1 i _

r -o--

10 20 30 iO SO 60 70 V. impr«gr\Qtior\ w i t h T8A

10 20 JO 40 50 SO 70 ' / . . r r p r t g n o l i o n w i t h TBA

Rf 0

0

0

Rf 0

0

0.

s

c

4

2 -

0

-g,-- ' - g . - . ^ - . ^ : ^ ^

1 0

0 8

0-6

Rf 0 4

0 2

0 0

1*

- S - - 0 - - 0 -

" • - - o o — o I ^ t Ô-

~-c>-,o_ - 0 - - 0 - - —

- - 0 - -

Tl

"^^^"^Q—^ --f—9 ^ -

Hg

10 20 30 4 0 50 60 70

V , imprtgnot ion wi th TBA 10 20 30 60 50 60 70

V . imprtgnotion with TBA

Figure 2

Plot of R, Vs percentage impregnation of TBA in t)€n7ene. - ® ® - 1.0 M FA; - i ' »•>- 1.0 M FA + 1.0 M SF (2:8) .

132 V O L 1, J U N E 1988 Journ.'^l of PInnnr Chfnrn.'i'' / j i .K'f ' .


1 OM SF

A-IOM SF»1 0MFA(«:2) B-IOM SF + 10MFA(2:8) C-)OM SF • )0M FA(1:))

A-VOMSF«).OH FA(S:4) B-lOM SF + 10MFA(4:6)

4 > O b . | Z o Z < - > N -Utlons

Figures

Pkrt of R| n metal lone in different eoivent systems, a - 60% TBA impregnated SO layers. b ,cd • 40% TBA impregnated SG layers. • — • Compact spots; A — A TaBed spots virfth SL - n , > 0.4; O — O T a i M spots with R - RT < 0.4.

3.5 Effect of pH of Metal Solutions on the Separation ofZn^* from Ni**, Co**, and Cd**

Rgure 4 shows that the R, values of Zn^*, Ni^*, Co^\ and Cd * are independent of the pH of the sample solution in the pH range of 1-5. Thus a good separation of Zn^* from these metal ions can be obtained on 60% TBA impregnated SG

10

oe I 0 6(-

Rf0 4

0 2 •

00

Cd^ Ni *on4 Co?* - • m • •

2 3 t fH of fflttal tolution*

Figure 4

Plot of pH o< metal solutions M . R, on silica gel layers impregnated with 60% TBA In solvwil syslMn containtng l A i t SF and 1 . 0 M FA In an 8:2 ratio.

layers in mobile phase containing a mixture of 1,0 M SF and 1.0 M FA in 8:2 by using unbuffered sample solutions without adhering to the close control of the sample pH.

Enhancement of the selectivity of SG layers by impregnation with TBA provides an opportunity to achieve many analytically important separations. Many such separations have actually t>een realized and are tabulated in Tables 1-4. Separations such as Zn^*-Cd^\ AP*-CU^*, VCP*-TP*, VCP*-W*\

Th''*-Zr*\ Fe3*-TP^ AP^-Cu^^-Ni^^-Ti"*, Cr^^-BJ^*-Cd^^-Co^*, Zn^^-Cd^^-Pb^* and Zn^-'-Tr-Pb^* are worth mentioning.

Table 5 summarizes the results of the effect of loading on the fl( values and the lowest possible detectable amount of metal ions on the chromatoplates. TBA impregnated SG layers gave highly compact spots over a wide range of loading of the nrretal ions. 0.5 pg of Ni * gave R, equal to 0.94 while it is 1.0for400Mgof Ni *.

In order to present a clearer picture regarding the separation of Zn^* from Cd^*, Ni^*, and Co^*, someTLC parameters such as Afl, (ft, of separating metal ion - Rf of Zn^*), separation factor (a) and resolution (f?J have been calculated. These data are shown in Table 6. The values for a and Rg have t)een calculated by using the following relationships

(i) a

K' 1- f l ,

(M = separating metal)

where K' is a capacity factor which measures the degree of retention of a solute compared to the solvent.

fls M

1/2 (d, + dz)

where AX is the distance between the centers of spots and di, d2 are their respective diameters. Two solutes are just separated if R, is equal to 1. It is clear from Table 6 that a good separation of Zn^* from Gd^*, Ni *, and Go * can be carried out by the proposed method. The Afl| value is always greater than 0.5. A high value of separation factor and well resolved spots with H. > 5 are the added advantages of this study.

The proposed method, consisting in the use of 40-60% TBA impregnated SG layers and a mixture of 1.0 M SF and 1.0 M FA in a 8:2 ratio as developer is very reliable and reproduc-'Me for achieving the separation of a particular cation from others in general. It is especially useful if one needs sharper aix) clearer ternary and quartemary separations. The spots are so well formed and compact that good quartemary separations are always possible. It is a very reliable method for separating Zn^* from Cd^* over a reasonable pH range of sample solutions.

Journal cil Plan.ir Chromatopfaphy vol I .11 INF 19R8 133


Acknowledgment

The authors thank Prof A. U. Malik. Chairman, Department of Applied Chemistry, for providing facilities and the University Grants Commission (India) for financial assistance to N. Fatima.

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[26] M. Oureshi, K. G. Varshney, and R. P. S. Rajput, Anal. Chem. 47 (1975) 1520.

[27] M. Oureshi, K. G. Varshney, and ft C. Kaushik, Anal. Chem. 45 (1973) 2433.

Ms received: November 10, 1987 Accepted by SN: January 5, 1988

134 VOL. I.JUNE 1988 Journal of Planar Chromatograptiy

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CORE – Aggregating the world’s open access research papers · Dr. Mohammad Ajmal Environmental Research Lab. Deptt. of Applied Chemistry Z.U. College of Engg.&Tech. Aligarh Muslim