ir.amu.ac.inir.amu.ac.in/7782/1/T 3817.pdfACKNOWLEDGEM:;NT It is with great indebtness and gratitude...
Transcript of ir.amu.ac.inir.amu.ac.in/7782/1/T 3817.pdfACKNOWLEDGEM:;NT It is with great indebtness and gratitude...
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STUDIES ON INORGANIC ION EXCHANGERS AND
CHELATE EXCHANGERS
NEELAM SHARMA DEPARTMENT OF CHEMISTRY A11GARH MUSLIM UNIVERSITY
A11GARH
A THESIS SUBMITTED IN FULFILMENT OF THE REQUIREMENTS FOR THE DEGREE OF DOCTOR OF PHILOSOPHY IN THE
FACULTY OF SCIENCE OF THE ALIGARH MUSLIM UNIVERSITY ALIGARH 1989
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c_7x 9dic h cp. Cf:Za wa t M.Sc., Ph.D,
READER IN CHEMISTRY
CERTIFICATE
Ph. Office : 6515
DEPARTMENT OF CHEMISTRY ALIGARH MUSLIM UNIVERSITY
ALIGARH-202002 INDIA
This is to certify that the work embodied in this thesis
entitled, "Studies on inorganic ion exchangers
and chelate exchangers" is original, carried out by
Ms.Neelam Shilrma under my supervision and is suitable
for submission for the award of Ph.D. degree in Chemistry
of this University.
.i i ( i ~~- I( / I\_
.1
t;'' .. , 1 .. l ~
;(-J.P. RAWAT)
-
M^Ciyi/C/i
c
yoviA/Vi
'V
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ACKNOWLEDGEM:;NT
It is with great indebtness and gratitude that I pay
my thanks to Dr. J.P. Rawat v;ho served as a beacon of light
v>rhile I v;as canoeing in ever increasing and turbulent ocean
of chemical sciences. His timely advice, fatherly interest,
healthy criticism and constant encouragement enabled me to
give the work its present shape„
I am grateful to Professor S.M. Osman, Chairuian,
Department of Chemistry for providing the necessary research
facilities.
I would be failing in my duties if I don't acknowledge
my friends especially Miss. Archana Agarwal and Mrs. Sangeeta
Kumar for their continued help and cooperation. I am thankful
to my lab colleagues for maintairinc a congenial atmosphere.
Mr. Rakesh Kumar, my husk and, deserves to be praised
highly who while cooperating witi me becomes the very source
of strength to me.
I also thank Ui:iiversity Grants Commission for a
research grant.
(NEELAM
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C O N T E N T S
1. List of Publications
2. List of Tables
3. List of Figures
Chapter - I
5. Chapter - II
Chpater - III
Paae r;o,
Introduction
References
Stannic phthalojihosphate a nevi cation exchanger for the removal and recovery of Pb(II)
Introduction 72
Experimental 73
Results 75
Discussion 95
References 99
Ion exchange equilibria of alkaline earth metal ions on stannic phthalophosphate
Introduction lOl
Experimental 102
Results 105
Discussion 137
References 14i
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7. Chpater - IV
8. Chapter - V
Tin thioglycola-::e as a new material for the recovery and removal of mercury
Introduction 14 3
Experimental 14 5
Results 150
Discussion 158
References 161
Ferroin sorbed zinc silicate in the in the deterrnination of cerium in presence of rare earth
Introduction 162
Experimental 163
Results 165
Discussion 168
References 171
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LIST OF PUBLICATI QMS
1. Stannic phthalophosphate a nev; cation exchanger for the
removal and recovery of Pb(Il)
Indian Journal of Chemistry (Communicated).
2. Ion exchange equilibria of alkaline earth metal ions on
stannic phthalophosphate
(Communicated).
3. Tin thioglycolate as a new material for the recovery and
removal of mercury.
(Communicated).
4. Ferroin sorbed zinc silicate as indicator in the determi-
nation of cerium in presence cc rare earth
(Commsunicated) .
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- 1 1
LIST OF TABLES
TABLE 1.1 S y n t h e s i s and I o n - e x c h a n g e p r o p e r t i e s of
M u l t i v a l e n t m e t a l s a l t s
Pane I'vO,
1 n
TABLE 1.2 Some of the important Chelate exchange
resins 39
TABLE 2,1 Conditions of preparations of stannic
phthalophosphate 74
TABLE 2,2 Solubility of stannic phthalophosphate 77
TABLE 2.3 pH titration of stannic phthalophosphate 81
TABLE 2,4 Kd values of different metal ions 85
TABLE 2.5(a) Uptake of Pb(ll) by stiinnic phthalophosphate from solutions of diffs^rent concentrations 85
2,5(b) Uptake of Pb(II) at lover concentration 87
2,5 (c) Uptake of Pb(II) from solutions containing
same amount of Pb(II) c.t various concentra-
tions 87
TABLE 2.6 Rate of Sorption of Pb(II) 8b
TABLE 2,7 Some separations on stannic phthalophosphate
columns 9 0
+ '̂ TABLE 3,1 Ionic fractions of Mg , Selectivity
coefficients and thermodynamic equilibrium + 2 +
constants for Mg -H exchange on stannic
phthalophosphate 105
TABLE 3.2 Ionic fractions of Ca"̂ *", selectivity
coefficients and thermodynamic equilibrium + 2 +
constants for Ca -H exchange on stannic
phthalophosphate 108
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- IIX -
+ 2 TABLE 3,3 Ionic fractions of Sr , selectivity
coefficients and thermc'clynaniic equilibrium + 2 +
constants for Sr -H exchange on stannic
phthalophosphate 111
+ 2 TABLE 3.4 Ionic fractions of Ba , selectivity
coefficients and thermodynamic equilibrium + 2 + constants for Ba -H exchange on stannic
phthalophosphate 114
TABLE 3.5 Thermodynamic parameters for Hydrogen-
Magnesium exchange on stannic phthalo-
phosphate at constant iDnic strength 123
TABLE 3.6 Thermodynamic parameteis for Hydrogen-
calcium exchange on ste::inic phthalophosphate
at constant ionic strer. jth 123
TABLE 3.7 Thermodynamic parameters for Hydrogen-
Strontium exchange on scannic phthalo-
phosphate at constant i Dnic strength 124
TABLE 3.8 Thermodynamic parameter,? for Hydrogen-
Barium exchange on stannic phthalophosphate
at constant ionic strength 124
TABLE 3.9 Equilibrium constants and selectivity + 2 +
coefficients for Mg -H exchange on
stannic phthalophosphate 125
TABLE 3.10 Equilibrium constants and selectivity + 2
coefficients for Ca -H exchange on
stannic phthalophosphat(i 128
TABLE 3.11 Equilibrium constants and selectivity + 2 coefficients for Sr -H exchange on
stannic phthalophosphate 13 1
TABLE 3.12 Equilibrium constants and selectivity + 2 coefficients for Ba -H e;:change on
stannic phthalophosphate; 134
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- IV
TABLE 4.1 Synthesis of Tin thioglycolate under
different conditions 14 6
TABLE 4.2 Uptake of Fig (II) fro.n its solutions of
different concentrations by tin thiogly-
colate 15 3
TABLE 4.3 Rate of sorption of Hg(II) 154
TABLE 4.4 Reduction of As(V) to As(III) 156
TABLE 4.5 Study of Precision for Hg(Il) uptake by
tin thioglycolate 157
TABLE 5.1 Determination of Cerium(IV) 165
TABLE 5.2 Determination of Cerium in presence of
other metal ions 166
TABLE 5.3 Reproducibility of determination of
Cerium 167
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- V
LIST OF FIGURES
Page No.
FIGURE 2.1
FIGURE 2.2
FIGURE 2.3
FIGURE 2.4(a)
FIGURE 2.4(b)
FIGURE 2.5
FIGURE 2.6
FIGURE 2.7
FIGURE 2.8
FIGURE 2.9
FIGURE 2.10
FIGURE 2.11
FIGURE 3.1
FIGURE 3.2
FIGURE 3.3
FIGURE 3.4
FIGURE 3.5
Plot of Ion-exchange capacity against
number of regeneration cycles
Capacity and % weight losses of exchanger
at different temperatures
pH titration curve of stannic phthalo-
phosphate using O.IN NaCl"*" O.IN Na CO
solutions
IR spectrum of phthalic anhydride
IR spectrum of stannic phthalophosphate
exchanger
Rate of Sorption of Pb'.Il)
+ 2 +? Separation of Zn -Pb
+ 2 + • Separation of Sr -Pb
4-2 +.'' Separation of Co -Pb
+ 2 +'' Separation of Ni -Pb
+ 2 +2 Separation of Cu -Pb
+ 2 +'' Separation of Mg -Pb
+ 2 Ion exchange isotherm of Mg ion on
stannic phthalophosphate
+ 2 Ion exchange isotherm of Ca ion on
stannic phthalophosphate
+ 2 Ion exchange isotherm cf Sr ion on
stannic phthalophosphate
Ion exchange isotherm cf Ba ion on
stannic phthalophosphate
Selectivity coefficients Vs equivalent + 2
fractions of Mg ion :.n exchanger phase
76
78
82
84
84
89
92
92
93
93
94
94
106
109
112
115
118
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VI
FIGURE 3.6
FIGURE 3.7
FIGURE 3.8
FIGURE 3.9
FIGURE 3.10
FIGURE 3.12
FIGURE 3.13
FIGURE 4.1
FIGURE 4.2
FIGURE 4.3
Selectivity Coefficients Vs equivalent + 2 .
fractions of Ca ion m exchanger phase
Selectivity Coefficients Vs equivalent + 2
fractions of Sr ion in exchanger phase
Selectivity Coefficients Vs equivalent + 2 fractions of Ba ion in exchanger phase
Plot of In K Vs l/T for alkaline earth
metal ions
Mass action plot for Hydrogen Magnesium
exchange on stannic phthalophosphate
Mass action plot for Hydrogen-strontium
exchange on stannic phthalophosphate
Mass action plot for Hydrogen-Barium
exchange on stannic phthalophosphate
X-ray diffraction c:; Tin thioglycolate
Uptake of Hg(II) from its solution of
different concentra-;ions
Rate of Sorption of Hg(ll)
119
120
121
122
126
132
135
151
152
155
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CHAPTER - I
Introduction
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1 CHAPTER ~ I
I N T R O D U C T I O N
Analytical chemistry deals with the solving of quali-
tative and quantitative problems. Qualitative analysis deals
with the finding what constituent or constituents are in an
analytical sample^ and quantitative analysis deals with the
determination of how much of a given substance is in the
sample. With today's instrumentation and with the large
variety of chemical measurements available, specificity or
sufficient selectivity can often bp. achieved so that a qua-
ntitative measurement serves as a c[ualitatlve measurement.
The development of methods for these analyses is the main
aim of analytical chemistry.
Analytical chemistry, like other areas of chemistry
and of all sciences, has gone thrc-ugh a period of rapid
growth and change. At present, new areas such as chemical
physics, biophysics and molecular biology are rapidly deve-
loping. Many advances in these ar>;'as were made possible by
analytical results.
The importance of analytical chemistry in related
scientific areas can be illustratec by considering its
impact on clinical analysis, in phcrmaceutical research
and quality control, and in envirormental analysis.
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2
In the past, the medical profession used clinical
results qualitatively and many of their diagnosis were
based on symptoms and/or X-ray examinations. The tests
were improved to the point where it became possible to
quantitatively determine these components. Now these
test results play a major role in influencing the diag-
gnosis.
Currently, quite a large number of tests are per-
formed in clinical laboratories. The major portion of
these tests deal with blood and urine samples and include
the determination of glucose, urea nitrogen, protein nit-
rogen, sodium, potassium, calciT-im, UCO^A^J^^s' "^^^^ acid,
and pH, etc.
In the pharroaceutical industry the quality of the
manufactured drugs in tablets, solution and emulsion
forms must be carefully controlled. Slight changes in
composition or in the purity of the drug itself can
affect the therapeutic value. Accurate and sensitive
tests must be developed since the level that are being
determined are often as little .;s 1 nano gram.
Analytical methods providt; the basis for the
studies including the application of science and tech-
nology toward the control and in.provement of environ-
mental quality. The development of analytical methods of
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3
separation, identification, and subsequent determination
have provided information about the presence of dust and
suspended particulate matter in air as lime, limestone,
and cement dust from kilning operations, coke dust and
polycyclic aromatics from coking operations, and fluorides
from metallurgical processes. Other contaminants are fly
ash from coal-fired electrical power plants and wind-blown
slag and insulation from industrial operations. Water is
also as complex a system as air, when it comes to environ-
mental monitoring. As in the study of air, analytical
chemistry has played a major rola in the environmental
science of water.
There are various methods in analytical chemistry
that are employed for separation. Some of them are*chro-
matography, electrophoresis, ion-exchange, solvent extra-
ction, ring oven technique and dialysis. Out of them
ion-exchange has come to be recognised as an extremely
valuable technique. Ion-exchange had a great impact on
analytical chemistry.
Ion-exchange is a reversible, stoichiometric ex-
change between the ions in the mobile liquid phase and
the ions on the exchange sites on the stationary phase.
The major application of ion excJiangers is the separation
of ionic or partially ionic mixtures. But recently, Sepa-
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4
ration of nonionic organic molecules on ion exchangers has
also been reported. The retention of these kinds of mole-
cules on ion exchanger depends upon the highly polar chara-
cter of ion exchanger and the se-.ection of eluting condi-
tions.
Ion exchangers can separate the micro ( < 1 - mg
quantities) as well as the macro (> 1 - g quantities)
samples. Because of the macro application, ion exchangers
can also be used on industrial scale. A wide variety of
very complex mixtures have been separated on ion exchangers.
These includes the separation of rare earths in hitherto
unknown purity (1-7). Ion-exchange chromatography has played
an important role in the isolation and identification for
the concentration and extraction of the most important
metals and of the new transuranium elements (8-13) and has
even been used for enrichment of isotopes (14-19), Organic
substances such as amino acids (20-28), peptides (29,23,30),
proteins (23,31), nucleic acids (32), alcohols (23,33,34),
glycols (33,35,36), carbonyl compounds (23,33,37,38), car-
bohydrates and derivatives (23,39-43), ethers (38,44),
amines (23,44-46), hydrocarbons (38,47) and phenols (38,48)
have also been separated in ion-e:
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r) concerned, organic resins are by far the most important ion
exchangers. The more recent analytical applications of ion
exchange resins include the collection of selenium (IV)(49),
ppb level of aluminium (50), preconcentration of cobalt (51),
trace determination of trimethylselenonium in urine (52),
molybdenum (53) and iron (54), preparative, fractionation
of petroleum heavy ends (55), determination of pt and pd (56),
analysis of metamict mineral containing U, Ti, Nb and rare
earths (57) and the determination of low level bromide in
fresh water (58). Ion exchange has also been used with
success in the food industry (59) and for determining polar
organics in shell process v/ater;; (60).
The water pollution is increasing day by day. However,
the methods based on ion-exchange are becoming of promising
success when applied to this fi:-̂ ld. The use of ion exchangers
on large scale may provide mankind v.'ith pure water and may be
useful for the concentration and extraction of the most
important metals and ra\\' materials v.'hich is becoming more and
more difficult to produce.
The English agriculturist H.S.Thompson(61) was the first
to observe and to publish descriptions of the phenomenon
of ion exchange by the name of base exchange. Thompson
found that the ammonium sulfate absorbed by soils
could not be washed out by water and that much of
the absorbed ammonium sulfate was converted to calcium sulfate,
It v/as VJay (62), who thoroughly explored the phenomenon and
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6
demonstrated the underlying mechanism to be one of base ex-
change involving the complex silicates present in the soil.
Ca - Soil + (NH4)2SO^ = NH^ - Soil + CaSO^
The first attempt to employ ion exchange for commer-
cial purposes was made by Harm in 1896 (63). In his patent.
Harm claimed to have a successful process utilising a natu-
rally occurring cation exchanging silicate for removing
sodium and potassium from sugar beet juice. However, success-
ful large-scale applications of cation exchange were developed
by Cans (64) who synthesized inorganic materials of the type
Na^Al„Si-O^Q in which the Na was exchangeable. He success-
fully applied his inorganic synthetic cation exchanger to
water softening and sugar treatment on a technological scale.
To a large exlent his synthetic exchanger replaced the natu-
rally occuring exchangers or zeolites.
One decided shortcoming of the inorganic exchangers
at that time resided in the fact that they were acid sensi-
tive and did not lend themselves to any exchange reactions
in which hydrogen ions were taking part.
It is only in the past forty years that ion exchange
has reached the point where it should be considered a unit
process at par with tne traditional ones such as distillation,
precipitation, and adsorption. Adams and Holmes (65) in 1935,
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English Chemists discovered and appreciated the potentialities
of the ion exchanging properties of synthetic resins. They
synthesized both anion and cation exchange resins thus making
it possible to deionize water in the cold for the first time.
The really modern era in ion exchange technology began
in 1944 when D'Alelio of the General Electric Company's Pitts-
field laboratories synthesized resins from preformed polyst-
yrene (66), These resins were the forerunners of the currently
available line of polystyrene resins which, compared to
earlier resins, possess greatly improved capacity and chemical
and mechanical stability.
The application of organic ion-exchange resins are
also limited under certain conditions i.e. they are unstable
in aqueous systems at high temperatures and in presence of
the ionizing radiations. For these reasons there has been
a revived interest in inorganic ion-exchangers in recent
decades, as they are unaffected by ionizing radiations and
are also sensitive to higher temperatures. The structure of
these inorganic ion exchangers is stiff; therefore they are
more selective and suitable for the separation of ions on
the basis of their different pore sizes. Being stable towards
ionizing radiations, they can be: used advantageously in
reactor technology. Inorganic ion exchange membranes have
also recently been used preferably over organic ones because
of the ability of inorganic membranes to withstand higher
temperatures and their high selectivity for cetain ions.
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8
Inorganic ion exchangers also find applications in
the analysis of alloys (67,68) and silicate rocks (68,69)
separation of metals from drugs 170,71) and in the detec-
tion of iron and molybdenum (72,•/3).
The selectivity of inorganic ion exchangers has been
utilized for the preparation of ion selective electrodes
(74). The ion selective electrodes have now come to be
recognized as an important tool for solving various analytical
problems (75-77).
In order to understand the applications and in order
to improve upon them, systematic and fundamental studies are
being persued of these materials. This new interest in inor-
ganic ion exchangers may be said to begin in 194 3. It was
shov/n by Boyd (78) that columns containing finely divided
zirconium phosphate supported on silica wool could be used
to separate uranium and plutoniurii from fission products by
ion exchange process. In addition to zirconiiim phosphate
many other similar substances may be prepared by containing
oxides of group IV with more acidic oxides of group V and VI
of the periodic table.
The various inorganic ion exchangers reported upto
1963, have been summarized by Amphlett (79) in his classical
book, "Inorganic Ion-exchanger". The relevant work from 1962
to 1970 has been reviewed by Pekerek (80) and Vesely (81).
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!)
Marinsky has summarised the theoretical aspects of exchange
in inorganic ion exchange materials (82) , The synthesis and
application of inorganic ion exchangers have been reviewed
by Walton (83-88), Recent reviews on the applications of
ion exchange have been edited by Marinsky (89) and Walton
(90), Recent literature on these materials has been covered
by Clearfield in his monograph in 1982 (91). Zirconium
phosphate is a most extensively studied material in this
family and a large number of research papers have been
published on it. The ion-exchange properties of some of the
more important inorganic ion-exchangers of the zirconium
phosphate type have been summai'ised in Table 1.1
-
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?.3
Ion exchangers can be utilized :.n the laboratory in many
other ways:
1) Interfering ions can be removed.
2) Group separations are possible,
3) Samples can be concentrated.
4) Charges on ions can be established.
5) Samples can be purified.
6) Standard solutions can be prepared.
7) Formation constants of complexes can be determined.
8) They can be used as acid and base catalysts.
If v/ater is passed through two columns, the first
containing a cation exchanger in the hydrogen form and the
second an anion exchanger in tt- hydroxide form, deionized
water can be prepared. The reactions, assuming all salts in
the '^ater are univalent cations (M ) and anions (X ) are
Cation exchanger: Resin - SO~H''"+MX ;^=±LResin-S03M"^-fHX.
Anion exchanger : Resin - NR30K'-VHX^=^ Resin-NR3X""+H20
Water purification for the laboratory using this procedure
has two advantages in comparison to distillation.
1) The ion-exchange procedure is faster and cheaper .
2) It easily Satisfies the pui-ity requirements of a
scientific laboratory.
Ion exchangers can be utilized in the preparation
of solutions in several ways, I'or example, ionic salts can
-
C'4
be removed from organic reaction mixtures. This often faci-
litates purification of the organic compounds through crys-
tallization, A solution of a metal chloride or some other
anion can be prepared by passing a metal nitrate solution
through a colum.n of an anion exchanger charged in the
chloride form or anion form of interest. If a vjeiqhed
amount of KCl is passed through a cation exchanger in the
hydrogen form, and the effluent is collected and diluted
to a known volume, a standard solution of HCl is prepared.
This is possible since the exchange of ions is stoichio-
metric. Conversion of salts to an acid (or base if an anion-
exchanger hydroxide form is used) can also be used for
analysis.
The properties of ion exchangers facilitate the
selection of the correct ion exchanger for the particular
problem. The more important properties are colour, density;
mechanical strength; particle size; capacity; selectivity;
amount of crosslinking, swelling; porosity-surface area;
and chemical resistance. The exchange of univalent ions
may be represented by the following equation
(A+)^+ (B-^)^ ^ . ^ (A-*-) 3 . (B-^)^
where R and S refer to the cation being in the resin phase
and solution phase, respectively. Since the reaction
reaches an equilibrium position, an equilibrium expression
-
25
in terms of concentrations can be written as
R _ ^ s ^ ^ R
where the square brackets are for equilibrium concen-
tration .
If the experimental variables are held constant and
the concentrations of A and B are low, K is a constant
and is an indication of the preference the ion exchanger
shov7s for one ion over another.
For a good ion exchanger the rate of exchange should
be rapid. Several properties like particle size, mechanical
strength, crosslinking, swelling and porosity-surface area
influence the exchange rates.
Total capacity of an ion exchanger is a measure of
the total amount of exchangeable ions expressed per unit
weight of dry ion exchanger (mmol/g) or v/ater sv/ollen ion
exchanger (mmol/ml). It is determined by taking a weighed
sample of the ion exchanger, in column and passing a solu-
tion of KCl through the column in large excess. For the
cation exchanger in the H form, the effluent will be acidic
which can be titrated v;ith standard base. For the anion
exchanger, the solution v.-ill be basic, if the exchanger is
in OH form, and the effluent ip titrated with standard acid.
-
25
If the exchanger is in the Cl form/ a KNO solution is used
and the exchanged Cl" is determined by a Ag"̂ titration. From
the titration data and v/eight of the exchanger, the capacity-
can be calculated.
Separations of inorganic mixtures to a more or less
extent are based on one of the three different principles.
1. At low concentration the extent of exchange is directly
proportional to the valency of the exchanging ion.
2. At constant valence the extent of exchange is directly
proportional to the atomic number at lov/ concentration.
3. The extant of exchange highly depends upon the formation
of complexes.
Besides the above three factors some others such as
concentration, pH, temperature may influence the separations.
Distribution coefficient K, may be determined to
calculate the separation factor which may be regarded as a
measure of possible separation.
y _ Amount of ion (A) present in exchanger phase g M Amount of ion TAI present in solution phase ml
The separation between a given pair is possible or
not is predicted by comparing their K. values. It is also
possible to separate a trace quantity of a metal from a macro
amount of another metal ion.
-
27
Organic compounds that have ionic character (acidic
or basic) can be separated on anion and cation ion exchangers.
Many nonionic organic compounds are retained by ion exchangers
through adsorption, salting out, size and other exchanger-
solute interactions. By proper choice of eluting conditions
separations are possible. The total capacity of the exchanger
towards an organic solute may be quite different than found
for the exchange capacity for the exchanger.
Thermodynamics is a very important tool to study the
theory of ion exchange and also for :an insight to the under-
lying mechanisms involved. Two different approaches are usually
applied for this purpose (though ether meritable approaches
exist, these two are most widely accepted).
The first approach is based on the design of more and
more elaborate models. Tnis approach gives a semiquantitative
picture to a practical chemist who is interested in under-
standing the physical causes of the phenomena. Thermodynamics
is the appropriate means of explaining any equilibria.Rigorous
thermodynamics, however, is, inherently abstract. The rigorous
and abstract treatment of thermodynamics is'correct' and
universal, but it yields a minimum of information about the
physical causes of the phenomena to which it is applied.
-
28
In the second approach attempts have been made to
correlate the activities v;ith some measurable quantities with
the thermodynamic equations. Probably the tirst quantitative
formulation of ion exchange equilibria was made by Cans (239)
using the law of mass action in its simplest form. This
concept was extended by Kielland (240). A similar choice of
the general treatment was given by Gaines and Thomas (241).
The most acceptable model, however, is the semiquantitative
one of Gregor which relates selectivity to hydrated ionic
volumes.
The particular use of the thermodynamic equilibrium
constant is made to find out the free energy changes of the
ion exchange process, usually, by the expressions:
A F = - RT In ka
Where Z:̂ F is change in free energy. From the Ka values
at different temperatures, the enthalpy changes in the system
may be evaluated. The enthalpy change is directly related to
the changes in the number and the strength of the bonds
involved in the ion exchange reaction.
The therroodynamic studies cf alkali metal ions on
semicrystalline zirconium phosphate were performed by many
scientists (242-247). The thermodynamics for alkali and
alkaline earth metal cations on ferric antimonate (248-249),
-
?9
and niobium arsenate (250) were made in our laboratories.
The kinetics of simple homogeneous chemical reaction
is governed by their differential rate of the reaction depe-
nding on the concentrations of the reactants.
Ion exchange kinetics involves three types of processes.
1. Interdiffusion of counter ions in the adharent film,
2. Interdiffusion of the counter ions with in the ion
exchanger particles themselves, and
3. Chemical exchange reaction.
It is important to note that of all the studies on
ion exchange kinetics which have appeared in the literature
to date, none of them has been shown by chemical exchange
reactions.
Nachod and Wood (251) made the first serious study on
the kinetics of ion exchange. They studied the reaction rate
with which ions from solution are removed by the solid ion
exchanger or conversely the rate ^t wnich the exchangeable
ions are released from the exchanger, Boyd et al (252) have
later on studied the kinetics of metal ions on resin beads,
and nave given an elaborate understanding about particle and
film diffusion which are governed by ion exchange.
-
30
Costantino et al. (253) have studied the self diffusion
process of Na"̂ and K"*" ions on microcrystals of zr (NaPO^) 2. 3H2O
and Zr(KPO.)^.3H^0 and modified Picks equation to take into
account the non-uniformity of the particle size. The equation
so obtained was employed in tne study of self diffusion rate
of Na^ and K^ ions on the above mentioned exchangers.
Kinetic studies on inorganic ion exchangers were made
in our laboratories and kinetic studies on the exchange ot + 7+ 2+ 2+ 2+ 3+ 4 +
the cation Ag , Mg , Ca , Sr , Ba , Y and Th were
made on tantalum arseiiate (254). Similar studies were also
been made. The distribution of an ion between the exchanger
and solution phases can give a direct measure of their rela-
tive selectivities. Often, the ion exchanger takes up certain
ions in preference to other counter ions present. This sele-
ctivity depends mainly on.
1. The Donnan potential.
2. Sieve action.
3. Complex formation.
An inorganic ion exchanger can be prepared by intro-
ducing triethylamine group into the hydrous oxide of a
trivalent or tetravalent metal ion. The amine group may also
act as a chelating group to certain cations and hence such a
material may be useful in two ways: (1) as anion exchanger
and (ii) a chelating exchanger.
-
Si
Chelating ion exchangers show a definite selectivity
towards certain ions or groups of ions. Thus the chelating
ion exchanger may provide a convenient technique for the
analytical concentrations of many of the more interesting
trace elements from natural waters and collection of toxic
elements from industrial waste waters. The selectivity of
most complexing agents resides predominantly in their ability
to form chelates with certain cations. The maximum efficiency
in the separation can be achieved by variation of the pH.
Therefore the development of complexing ion exchangers have
taken place, where complexatior. equilibria plays an important
role, such studies can be directed to follov/ing three cate-
gories :
(i) An ion exchanger is used in appropriate metal ion form
and the complexing agent is present as a solute in the
liquid phase.
(ii) An exchanger containing e. complexing agent functional
group attached to the matrix, is used and the metal
ion is present in the liquid phase.
iii) The solid phase is a chelating and the liquid phase
also contain a complexinc agent as solute.
Implementation of the fi.rst and second possibilities
will involve directly the metal complex equilibria, but in
heterogeneous phase, whereas the third possibility is
mainly advantageous of chelate exchange systems. In This
-
32
field the succ;essful efforts have been made by Bayer and
Cov/orkers (255-258). Blausius and coworkers (259-268),
Gregor and Cov/orkers (262-267)and many others (269-297).
A complex has been defined as "a species formed by
the association of two or more simpler species each capa-
ble of independent existence"(298). When one of the simpler
species is a metal ion, the resulting entity is known as
metal complex. The metal ion occupies the central position.
When the central metal atom of a complex is bound to
its immediate neighbours by covalent bonds by accepting an
electron pair from each nonmetal atom, the metal ion is
called the acceptor atom and the nonmetal ion, donor atom,
A more generally used convention is to call the non metal
ion which is attached to metal ion, ligand (L) and the
bond between them, metal-ligand bond (M-L) , According to
lewis concept this is regarded as an acid base reaction
where the central metal ion is the lewis acid and the
ligand is the lewis base. -
Some ligands are attached to the metal atom by more
than one donor atom in such a manner as to form a hetero-
cyclic ring. This type of ring has been given a special
name "chelate ring" and the molecule or ion from which it
is formed is known as chelating agent. The process of
-
33
forming a chelate ring is known as chelation. An example of
such a ring is the one formed in fig. 1 by the glycinate ion,
H^C - NH^
C= C - 0
Cu
.NH^ - CH^
0 C=0
The first chelating moleculeswere discovered by
Morgen and Drew (299) with donor atoms and it was the
Caliper like mode of attachment of the molecule to the
metal atom.
Metal chelates may be examined from atleast three
points of view.
1. the central metal ion
2. the chelating molecule.
3. the nature of the bonds linking (l) and (2), and the
influence of each and all of these on the behavior of
the metal chelate as a whole.
If a molecule is to function as a chelating agent/
it must fulfil at least two conditions:
1. It must possess at least two appropriate functional
groups/ the donor atoms of which are capable of combi-
ning with a metal atom by donating a pair of electrons.
These electrons may be contributed by basic coordinating
-
34
groups such as NH_ or acidic groups that have lost a
proton. Some acidic groups that combine with metal
atoms by the replacement of hydrogen are:
- CCOH
- SC3H
OH (enolic and phenolic)
. H
- NCT
- SH
Coordinating groups include:
0
NH^
NH
N=0
—
=
-
_
0 - R
NOH
OH (alcohol ic)
S - ( t h i o e t h e r )
2. These functional groups must be so situated in the
molecule that they permit the formation of a ring
with a metal atom as the closing member.
Sometimes these two conditions are not always suffi-
cient for the formation of chelate ring. Under some condi-
tions, for example, in solutions of sufficiently low pH, a
potential chelating molecule may attach itself to a metal
atom through only one ligand atom (300).
-
35
Accordin(3 to Gregor et al. (273), the following pro-
perties are required for a chelate exchanger.
1. The chelat:.ng agent should yield a resin gel of suffi-
cient stab:Llity.
2. The chelating molecule must possess sufficient chemical
stability. So that during the synthesis of the resin
the functicnal structure is not changed by polymeri-
zation or any other reaction.
3. The steric structure of the chelating molecule should
be compact, so that the formation of the chelate rings
will not b«: hindered by the matrix.
4. Because the agents forming relatively stable complexes
are at least tridentate, it is necessary that the ligand
groups of the chelating molecule be situated appropria-
tely, so that the specific arrangement of the ligand
will be preserved in the resin.
The complex formation in such reactions is based,
mainly on the use of N, S, P, As, 0 as donor atoms. For the
formation of coordination bonding, a donor atom must be an
element of high electronegativity.
So far, only the simplest type of chelating molecule
has been discussed - the type that is attached to metal
-
35
atoms by two donor or ligand atoms. There are, however,
many molecules v/ith three or more donor atoms capable of
combining with metal atoms and forming interlocking or
fused chelate rings. According to the number of donor atoms
capable of combining with a metal atom, these are called
tridentate, quadridentate, quinquedentate, sexadentate
and octadentate chelating molecules respectively. In
forming a metal chelate, a multidentate chelating agent
may not use all its donor atoms.
Chelate exchangers that contain only nitrogen as
ligand atom is comparatively small. Gold and Gregor (269)
have prepared a chelating exchanger that contains aromatic
nitrogen as the only functional chelation proceeds with
eopper(I) and Silver(l).
Chelating ion exchangers with nitrogen and oxygen as
donor atoms have been prepared in large group. Klyachko(3 01).
prepared a material by fixing EDTA as a solid solution within
a phenolformaldehyde condensate. Many workers prepared such
materials by fixing ligands to the benzene nucleus of the
970 crosslinked polystyrene" . Blasius (261) prepared such
materials by the reaction of chloromethylated polystyrene
with various aliphatic amines and stamberg (294,297)
prepared several resins, with vicinal dioxime groups using
-
polystyrene as starting material. Incorporation of thiol
groups has also been applied to prepare such materials
(272/92) with sulphur as the sole donor atom.
The theory of complex formation on chelating exchan-
gers is a field needing further extensive study. The use
of a chelating resins in analytical chemistry appears to
be of advantage either when the separation problem cannot
be solved by simpler means or when time can be saved.
The reagents which form metal chelates are found
important both in qualitative as well as in quantitative
analysis.Dimethylglyoxime, 8-hydroxyquinoline, cupferron,
Fehling solution, 0-phenthroline and aluminon are examples
of substances v;hich are indispensable in analytical separa-
tions and precipitations. In physiological chemistry the
chelate compounds are useful in the biuret reaction, in
the amino acid salts of the heavy metals chlorophyll, blood
pigment, and cytochrome are special chelates v/hich play an
important role in life processes, "Two very important chelate
compounds, the alkali metal salts of ethylenediamine tetra-
acetic acid and the condensed phosphates are used v;here
the removal of metallic ions are required such as the sof-
tening of water, negative catalysis, and clarification of
solutions.
-
s»
The ace:ylacetonates of metals are cyclic complexes
which are widely used in the purification of metals because
of their high volatility and solubility in non-polar sol-
vents. Chelating agents in connection with cation exchange
resins and soi.vent extraction are useful in the separation
of radioactive metals.
Some of the important exchangers have been summarised
in Table 1.2
-
Table "1.2
Some of the Important chalate exchange resins
Si)
S.No. Type of Exchanger Sorption Capacity m mole/g
Selectivity Refs
1. Oxime and diethylamino 2.00 resin
2. 8-hydroxyquinoline and -8-hydroxyquinodine
resin
3. 0-hydroxyoxime resin
4. Thioglycolate resin
5. Aminoacid type resin
6. Phosphate type resin
7. N-Acylphenyl hydro- 0.4 5 xylamines
8. Aluminium oxide
9. Alumina and Silica gel
10. Microreticular resin
11. Cellulosic exchanger
12. Cation exchange resin
13. Sulphonatecfitype resin
14. Carboxylic ion exchanger
15. Chilosan
16. Dithiocarbamate
17. Acrylic resin
18. Semithiocarbazide
Cu(ll)
Cu(Il), Zn(II)
Cu(ll), Mo (VI)
A g d ) , Bi(IIl),Sn(IV) Sb(Ill) , Hg(Il) ,U(VI) from pH = 3.5
U(VI), Cu(II), Ni(II) Fe(lII)
U(VI), Th(IV)
NH4
Ag(l)
Ag(l)
Sb(IIl), CoCll)
Zn(II)
Ni(II)
CoCen)^"^
Cu(II)
Cu(II)
Cu(ll)
Pb(ll), Pt(lV), Rh(III), Ir(III)
302
303
304
305
306
306
307
308
309
310
311
311
312
313
314
315
316
317
-
40
Sorption S.No. Type of Exchanger Capacity Selectivity Refs,
m mole/g
19. Poly(Vinylbezylthio- 819 mg/g Au(III) 318 urea)
20. Poly(hydroxamic acid) - Cu(II), Cd(II), 319 Zn{ll)
21. Chelating resin - Mo(VI), W(VI) 320 U(VI), V(II)
22. Chelating resin 1.9 Cu(II) 324
-
41
The present work was undertaken to synthesize a nev/
ion exchange material/ stannic phthalophosphate, to carry
out experiments for its physical characterization, to study
its ion exchange behaviour with special reference to sele-
ctivity for heavy metal ions and to study the ion exchange
equilibria applying the laws of reversible thermodynamics,
for alkaline earth metal ions. Experiments were also carried
out to determine thermodynamic parameters AH, As & A c .
The work was extended to prepare a new chelate ion
exchanger, tin thioglycolate, to carry out experiments for
its physical characterization and to study the selective
behaviour on the basis of complex formation with mercury(II)
and to study the reproducibility for quantitative separa-
tion.
To study the application of inorganic ion exchanger
the ferroin sorbed zinc silicate was used as an indicator
in the form of. beads for the selective determination of
Ce(lV) in presence of rare-earth metal ions. A study of
reproducibility was also made in order to find the preci-
sion of determinations.
-
42
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