mechanism of the complex formation was studied. the...

Nitrilotriacetic acid behaves as an excellent polydentate ligand like other

amino - poly carboxylic acids. It forms stable complexes with a large

number of metal ions at low pH values (1, 2, 3, 4, 5), acting as tridentate

(6) or Tetradentate (7) ligand depending upto the nature of the metal

ions. The metal complex formation even at considerably high pH values

(8).

The absorption spectrum of the Co (II) nitrilotriacetic acid complex

was studied by Nielsch and Beltz (9). Cheng and Warmuth (10) gave a

method for the determination of cobalt in nickel alloys and steel using

NTA. Study of the asorption spectra of chromium (III) nitrilotriacetic acid

was done by Dan Boef and poeder (II). The complex Cu (II)

nitrilotriacetic acid was studied by Man Mohan et.al (12) and the log 1 =

12.96 was found. Nard (13) determined electrometrically the rate

constants of the conversion of Cu (II) ethyl glyclinate N1 diacetate to Cu

(II) - NTA. Nielsch and Boltz (14) reported the Cu (II) - nitrilotriacetic

acid complex (in slightly acidic medium) has maximum absorbance in the

range of 690-710 nm and in alkaline medium in the range of 640-648

nm. Thermodynamic study of the reaction between various bivalent

cations and NTA as a ligand have been done by Hull and Coworkers (15).

At OºC, and U = 0.1 the heat of formation of the 1:1 complexes of Mn

(II), Co (II), Ni (II), Cu (II), Ca (II) and Sn (II) with NTA were measured

calorimetrically. They also found the existence of 1:2 complex of Cu (II)

NTA.

Qian Gao (16) studied bismuth (III) – NTA complex with help of

polarography. The polarographic behaviour of Bi (III) complex with NTA

including the stability constant, thermodynamic function and the

mechanism of the complex formation was studied. The stability constants

of the B1 complex was determined by suing the equation for shift of half

wave potential of kinetic wave. Kornevet. al (17) have done

spectrophotmetric study of the complexing of Co (II) with NTA. Instability

of CoX– and CoX2

4– are 8.85 x 10-11 at 3 pH 7 - and 4.74 10–15 at pH 7

respectively. Where NTA= H3X.

Elenkova and Tsoneva (18) studied the reaction between As

(III) and nitrilotriacetic acid (NTA) was investigated

polarographically and potentiometricall. As (III), in presence of

NTA gave a diffusion controlled current proportional to the

complex concentration in the pH and variable NTA concentration

were calculated from the change of the limiting currents. The

same conditional constants were determined by potentiometric

measurements to the potential of the redox system As (V) - As

(III) NTA at varied pH.

The complex [As (OH)2 Hx–] in formed under the experimental

conditions, whose overall formation constant is log - 15.33 ± 0.15 at ionic

strength = 0.1M and 25.0 ± 0.2ºC.

Redevich (19) reported the composition of complex compounds of

Cu2+, Ni2+, Zn2+ or Co2+ and Nitrilotriacetic acid (1) in the sepration of Y

and samarium by displacement complexing chromatography on the

exchange resin KV-2 in Cu–, Ni– or Co– cycle respectively depends on the

nature of the returningion. Pitre & Chitale (20) have done a polarographic

study of the complexes of neodymium (III) with glycine. Iminiodiacetic

acid and NTA. The studies were done at 32 ± 0.1ºC and pH 2.75 ± 0.02.

The stability constants increased in the order of glycine Iminodiacetic Acid

nitrilotriacetic Acid.

Sepctrophotometic study of complexes of Zinc (II) and cadmium

(II) with nitrilotriacetic and ethylene diamine tetracetic acids were done

by Kornev et. al (21). The method used was competing reaction method

using Co+2 as indicator ion, Formation constant of complexes was

calculated.

Tannanaeva et. al (22) have studied complex formation of

Europium (III) in aquous solution (pH 5-9) containing sodium salts of

EDTA (H4A) and nitrilotriacetate (H3B) by a high resolution

spectrophotometer. 1:1:1 complex EuAB4- forms in the solution and the

log of its stability constant was 21.66.

Simple and mixed complexes of iron (III) involving NTA

(nitrilotriacetic acid) as primary ligand and a series of oxygen bonding

organic anion as secondary ligands was studied by Ramamoorthy and

manning (23). Equilibrium constants are also reported for the

corresponding simple Mln complexes.

Mananin et. al (24) applied the lrving- Rossotti technique to the

study of formation constant of the reaction (MA) - + L2– --- (MAL)2– where

HL2 = catechol, pyragallol and 2, 3 dihydroxynaphthalene, M = Cu²+, Ni²+

& Cd²+ A = Anion of NTA). A similar equatin with L3- represents co-

ordination of protocatechnic acid. The value of formation constant of

KMAL was found to be less that Kf value i.e. the formation constant value

for KML (Binary complex). This behaviour can be explained by the

difference in electrostatic repulsion experienced by L2–.

Rubin and Martell (25) presented a calculation based upon metal

ligand equilibrium, known environmental concentrations of NTA following

extensive detergent usage, and the presence of competitive metal

binding ligands and trace elements demonstrates that NTA will be present

almost completely as Ca and Mg chelates. As analogous estimation of the

completely of NTA over long periods of time caused reproducible are

without measurable effect.

Isotope exchange reactions between the chlorides of Cerium (3+),

Cobalt (3+), mercury (2+) and Zn (2+) and their complexes with

nitrilotriactic acid were studied by Nicholas et. al (26). The experiments

were performed at different temperature and acidity ranges always

keeping the reacting in solution.

Barbara and Cowarkers (27) studied the nitrilotriacetate complexes

of ion (III) . Cobalt (II), Zinc (II), and Cadmium (11) arising in ion

exchange separation of lanthanides with the use of separation of

lanthanides with the use of separators. (NH4)3 FeL2). NH2O (H3L = NTA)

[Cu (HL)] 2H2O,. H (Cu4L3] H2, M2 [Ml2]. NH2O (M = Co1, Zn1 and H4

[ZnL2]. 4th were isolated from the eluted solution of rare earth elements

in an ion exchange persons involving the non-lanthanide elements as

separators. The complexes were characterized by elements in an ion

exchange. The complexes were characterized by elemental analysis, X-

ray differactometry and electronic spectral methods.

Spectrophtometric studies of various metal nitrilotriacetic acid

complex have been made by different workers. Yoshimura and Tanmura

(28) studied the Cr (VI) - NTA complex in dimethyl furunamide as the

solvent and have there by worked out a photometric determination of the

metal. Longman and coworkers (29) studied five published methods that

describe measures for the removal of interferences. However in non of

these methods interfering metals were displaced completely from their

NTA complexes. This method was quite similar in nature in the reduction

in the colour of the zinc- zircon complex by NTA. Tabatbai et. al (30)

determined the amount of NTA in soils applying the same technique and

also by eliminating metal interferences by ion exchange separation and

using a chelating resin. NTA present in trace in tape water was

determined on the basis of quenching of the fluorescence of the gallium -

8 quinolinal complex (31).

MIXED LIGAND COMPLEXES WITH NTA

Mixed ligand complexes are those in which the donor atoms belong

to different ligand molecules. Mixed ligand complexes are frequently

formed in solution but in comparison to simple complex, these have been

only scantily studied. Knowledge of the stability constants of the

appropriate mixed complex is essential for an understanding of problems

particularly related to analytical and biological chemistry. In the recent

year the work on mixed ligands system (32) receiving considerable

attention, which can be evinced by large number of publication.

Miggal et. al (33) studied mixed complexes of cadmium with

thiourea and halide ions in water alcohol solution. They also calculated

the stability constants at 250C and detected the components of the

complexes. At a give co-ordination no. The Thiourea- bromide complexes

of cadmium are more stable than those of iodide, Which are more stable

than thiourea - cadmium complexes, whose stability in turn is slightly

greater than that of cadmium aqueous complexes. The formation of

mixed complexes does not follow statistical distribution. Studnickova et.al

(34) determined stability of mixed complexes of zinc by the extraction

method. Ternary chelates Zn A2B and Zn AB2 formed during extraction of

a zinc salt with acetylactone (HA) and 2,2' bipyridyl or 1, 10

phenonthroline (B) were studied. They showed that ZnA2B chelate has

the character of an adduct with a higher stability and extra stability than

ZnA2. They also detected the stability constant of the ternary chelates by

graphical analysis of the dependence of the zinc distribution ratio on the

equilibrium concentration of B in the aqueous phase with constant

concentration of A. Kodama and Ebine (35) carried out a

spectrophotometric study of Zn- NTA Eriochrome black T system. Jackob

; and Margerum (36) evaluated the formation constants for the system Ni

(II) - NTA - oxalic acid. Ternary system of type M - NTA - L m = Cu, Ni L

= ligands viz. Thiourea, phenyl thourea, were studied by Chidambaram

and Bhattacharya (37) and Day et. al (38), Ramamoorthy et. al (39, 40)

have examined the complexes of Fe (III) and Cu (II) with NTA as a

primary ligand and as series of oxygen bonding organic anions as

secondary ligands.

Rahmani et. al., (41) prepared compounds viz. TIL5x ( where L=

(phenyl thiourea, X = Cl, Br) and TIL5 Qx. (Where Q = 2, 2' - dipyridine,

1, 10- phenanthroline) TIL' x ( L'= Diphenyl thiourea) TIL' QX1 TIL2 11

and TIL2 Q. These compounds were characterized by IR spectra and

electrical conductance. The thiourea are N- bonded; TIL X1T1 L5I and TIL'

× are 1 : 1 electrolytes whereas in the mixed ligand complexes the halo

group is co - ordinate, giving complexes with co-ordination number of T1

of 4 of 8. Some studied on mixed ligand complexes of cobalit (III), Nickel

(II) and Zinc (II) with hydozine and oxalic acid conducted by Mishra et. al

(42). Co (N2H4)2 Xn H20 (X = SO4, oxalte) NiN2H4) SO4, 2H20 were

prepared and characterized by elemental, analytical, thermal, IR studies

and magnetic measurements. They further showed the Cobalt and Nickel

complexes were octahedral.

Mixed ligand complexes of Cadmium with thiourea and

thiocyanatate ions in aqueous alcohol solutions were studied by

Tsiplyalova and Coworkers (43). A paleographic study is 0 – 93% MeOH

(ETOH) at 250 and ionic strength 0.5 was made by them. Mixed

complexes stabilities increase in the order MeOH E+OH. They also

determined stability constants for mixed complexes and co-operation

constants and compared to statistical stability constants for mixed

complexes.

Sirkar (44) have made electrophoretic studies of Cobalt (II), Zinc

(II), beryllium (II), Uranyl (II) Chromium (III) and thorium (IV) oxalate

nitrilotriacetate complexes in solution. A new method involving the use of

paper electrophoresis (PE), was described for the study of equilibrium in

mixed ligand complex systems in solution. This technique was based

upon the movement of a spot of a metal ion under a potential field, with

the complexants added in the background electrolyte (0.1 M NaCIO4) at

pH 10.0. The concentration of one of ligand was kept constant while that

of second ligands concentration as varied. A graph of log (L) against

mobility was used to obtain information on the formation of the mixed

ligand complex and to calculate the stability constant.

Singh et. al (45) studied the system Cu (II), Zn (II), and Co (II)

glutarate - nitrilotriacetate by paper electrophoresis. Yadava et. al (46)

have done electrophoretic studies of mixed ligand complexes in solution ;

Copper (II), Nickel (II), Uranyl (II) and Thorium (IV) Tartarate

Nitrilotriacetate. Singh et. al (47) have done electrophoretic study of

Nickel (II). Uranyl (IV) and thorium (IV) glutarate nitrilotriacetate

systems.

Sirkar (48) have studied electrophoretically Copper (II) < Nickel

(I), Cobalt (II) and Uranium dioxide (II) citrate-nitrilotriacetate

complexes in solution.

Ionophoretic technique has been applied in the study of mixed

complexes (M - Nitrilotriacetate - Valinate) system by Singh et.al (49).

Gupta et. al (50) have studied the M - Nitrilotriacetate - Prolinate system

by applying ionophoretic study. Number of mixed ligand complexes

invading NTA as primary ligand and amino acids as secondary ligand was

studied by Singh et. al recently. (51, 52, 53, 54, 56, 57, 58, 59, 60).

Tiwari et al. studied mixed complexes of sulphur containing amino acid

and NTA with number of metal ions and determined stability constants(61

- 77).

The present chapter deals with the electrophoretic investigation of

dissociation constant of NTA, binary complexes of M - NTA and ternary

complexes of type M - L -NTA.

EXPERIMENTAL

• Metal ions

5.0 × 10-4M solution of Cu (II), Ni (II), Co (II) and Zn (II)

perchlorates were obtained by suitable dilution of the stock solutions.

• Medium

The medium was of strength 0.1 M. The strength of NTA was kept

at 5 × 10-3 for, binary complexes. For dissociation constant 1 × 10-2 M

NTA has used while studying the mixed complexes concentration of NTA

was used; ranging from a strength of 1 × 10-7 M-5 – 1 × 10-3 M.

PROCEDURE

• Dissociation Constant of NTA

A 10 ml solution was made containing 4 × 10-3 NTA and 0.1

perchloric acid. This was taken in the electrophoretic tube, which was in a

water thermostat (35ºC), 50 volt potential difference was imposed on the

two platinum foil electrodes emerged in cup ends of the tube. After

allowing the electrolysis for 30 minutes the contents of negative

compartment was also washed with water, which was added into the

conical flask. Then 5 ml of Fe (III) solution of appropriate concentration

was added to it. The pH of the solution was adjusted by addition of 2.0 ml

of 50% acetic acid and requisite volume of sodium acetate solution. A

pinch of KI was then added and reaction mixture was allowed to rest for 5

minutes. The liberated iodine in the solution was titrate against 1×10-2M

hypo solution by using starch indicator. These observations were taken at

different pH value of the NTA solution of electrophoretic tube. On

electrolysis the negatively charged anions of the NTA migrate from the

negative compartment towards the positive compartment resulting in the

decrease in anion concentration in the negative compartment. Hence the

decrease in the concentration of the anion in the compartment will give a

measure of speed of the negatively charged anion. The iodometric

titration described above helps in determination of the concentration of

the anion in the negative compartment Ferric ion forms a very stable

complex with anion of NTA which is incapable of liberation iodine from the

potassium iodide. Hence the difference intitre values of the ferric ion in

absence and in presence of NTA anion give the concentration of anion.

Binary complexes of M - NTA - The experimental conditions are the

same as in metal - amino acid system.

Ternary complexes of NTA

For the study of mixed complexes, of metal ions with Serine,

Homo Serine, Proline and Hydroxy Proline as primary ligand and NTA

as secondary ligand, the usual experimental procedure adopted for simple

complexation studies was modified. An appropriate reaction mixture

containing metal ion and Serine, Homo Serine, Proline and Hydroxy

Proline and 0.1 M perchloric acid is adjusted to pH 8 by adding caustic

soda. This is important because stable complexes of 1:1 composition with

all the four ligands begin to form much ahead of this pH and remain

intact even beyond this pH.

To the solution the secondary ligand concentration i.e. of NTA was

increased progressively and the electrophoretic observations were made

at every addition of the secondary ligand. Care was taken always for

maintaining the pH of the solution at pH 8.5. All the observation has been

recorded under the following condition. 10 ml of the solution as

electrolyzed in the tube under the potential difference of 50 Volts, for 30

minutes. The contents of the negative compartment was analysed for

metal ions. These observations were repeated at several concentrations

of NTA.

Experimental observations are described in various sections and

attempts have made to interpret them.

Table - 4.1.1

H+ - NTA SYSTEM

[NTA] = 4 × 10–3

pH Titrant Value pH Titrant Value

0.95 1.95 3.81 0.95

1.16 1.95 4.08 0.95

1.27 1.95 4.51 0.95

1.18 1.80 4.85 0.95

1.69 1.75 5.06 0.95

1.80 1.35 5.31 0.95

2.02 1.30 5.76 0.95

2.21 1.30 6.35 0.95

2.32 1.25 6.81 0.95

2.43 1.25 7.11 0.95

2.54 1.05 7.70 0.95

2.76 0.90 8.34 0.95

3.01 0.95 8.96 0.95

3.21 0.95 9.05 0.95

3.18 0.95 9.43 0.95

3.62 0.95 9.43 0.95

3.62 0.95 9.90 0.95

10.31 0.50

Table - 4.2.1

Cu (II) - NTA SYSTEM

[Cu (II)] = 5 × 10–5 M B.E. = 0.350

[NTA] = 1 × 10–3 M A.E. = 0.270

pH Absorbance DA

1.43 0.270 0.080

1.56 0.275 0.075

1.54 0.280 0.070

1.65 0.290 0.060

1.66 0.295 0.055

1.77 0.300 0.050

1.78 0.310 0.040

1.89 0.315 0.035

1.10 0.325 0.025

1.92 0.330 0.020

1.93 0.335 0.015

2.06 0.345 0.005

2.07 0.355 -0.005

2.18 0.360 -0.010

2.19 0.365 -0.015

2.30 0.370 -0.020

2.37 0.370 -0.020

2.46 0.370 -0.020

2.57 0.370 -0.020

3.63 0.370 -0.020

3.96 0.370 -0.020

4.25 0.375 -0.025

4.53 0.370 -0.020

4.83 0.370 -0.020

5.21 0.370 -0.020

5.62 0.370 -0.020

6.03 0.365 -0.015

6.54 0.370 -0.020

7.05 0.370 -0.020

8.58 0.370 -0.020

9.09 0.370 -0.020

9.56 0.370 -0.020

10.10 0.370 -0.020

11.40 0.370 -0.020

12.50 0.370 -0.020

Table - 4.2.2

Ni (II) - NTA SYSTEM

[Ni (II)] = 5 × 10–5 M B.E. = 0.320

[NTA] = 1 × 10–3 M A.E. = 0.260

pH Absorbance DA

1.55 0.260 0.060

1.62 0.260 0.060

1.63 0.265 0.055

1.75 0.270 0.050

1.74 0.280 0.040

1.86 0.285 0.035

1.87 0.295 0.025

1.90 0.300 0.020

1.96 0.305 0.015

2.01 0.315 0.005

2.02 0.320 0.000

2.11 0.325 0.005

2.12 0.335 0.015

2.23 0.340 -0..020

2.23 0.340 -0.020

2.36 0.340 -0.020

2.57 0.340 -0.020

3.02 0.340 -0.020

3.33 0.340 -0.020

3.65 0.340 -0.020

4.06 0.340 -0.020

6.01 0.340 -0..020

6.32 0.345 -0.025

6.83 0.340 -0.020

7.34 0.335 -0.015

7.75 0.340 -0.020

8.16 0.340 -0.020

8.67 0.340 -0.020

9.08 0.340 -0.020

9.59 0.340 -0.020

10.54 0.340 -0.020

11.06 0.340 -0.020

11.58 0.340 -0.020

12.09 0.340 -0.020

12.50 0.340 -0.020

Table - 4.2.3

Co (II) - NTA SYSTEM [Co (II)] = 5 × 10–5 M B.E. = 0.390

[NTA] = 1 × 10–3 M A.E. = 0.315

pH Absorbance DA

1.50 0.315 0.075

1.52 0.315 0.075

1.82 0.315 0.075

2.53 0.330 0.060

2.54 0.335 0.055

2.66 0.340 0.050

2.68 0.345 0.045

2.71 0.350 0.040

2.72 0.355 0.035

2.84 0.360 0.030

2.85 0.365 0.025

2.96 0.370 0.020

2.92 0.380 0.010

3.18 0.400 -0.010

3.20 0.405 -0.015

3.24 0.410 -0.020

3.52 0.410 -0.020

3.81 0.410 -0.020

4.03 0.410 -0.020

4.22 0.410 -0.020

4.46 0.410 -0.025

4.61 0.410 -0.020

4.81 0.410 -0.020

5.01 0.410 -0.015

5.34 0.410 -0.020

5.63 0.410 -0.020

5.98 0.415 -0.025

6.38 0.410 -0.020

6.61 0.410 -0.020

7.01 0.410 -0.020

7.54 0.410 -0.020

8.03 0,410 -0.015

8.57 0.410 -0.020

9.01 0.410 -0.020

11.57 0.410 -0.020

12.08 0.410 -0.020

Table - 4.2.4

Zn (II) - NTA SYSTEM [Zn (II)] = 5 × 10–5 M B.E. = 0.500

[NTA] = 1 × 10–3 M A.E. = 0.400

pH Absorbance DA

1.53 0.400 0.100

1.62 0.400 0.100

1.75 0.400 0.100

1.86 0.400 0.100

1.87 0.400 0.095

1.98 0.400 0.090

1.92 0.410 0.080

2.03 0.420 0.075

2.01 00425 0.070

2.24 0.430 0.060

2.25 0.440 0.055

2.26 0.445 0.045

2.27 0.455 Q.035

2.34 0.470 0.030

2.38 0.480 0.020

2.49 0.485 0.015

2.40 0.495 0.005

2.51 0.500 0.000

2.73 0.520 -0.020

2.81 0.520 -0.020

3.02 0.520 -0.020

3.26 0.520 -0.020

3.43 0.520 -0.020

3.78 0.520 -0.020

4.31 0.520 -0.020

4.62 0.520 -0.020

4.91 0.520 -0.020

5.34 0.525 -0.025

7.51 0.520 -0.020

8.08 0.520 -0.020

8.57 0.520 -0.020

9.06 0.520 -0.020

9.55 0.520 -0.020

10.03 0.520 -0.020

10.52 0.520 -0.020

12.56 0.520 -0.020

Table - 4.3.1

Cu (II) - SERINE-NTA SYSTEM

[Cu (II)] = 5 × 10–5 M B.E. = 0.350

[Serine] = 1 × 10–3 M A.E. = 0.350

-Log [NTA] Absorbance

DA

7.01 0.000 0.000

6.82 0.000 0.000

6.63 0.000 0.000

6.44 0.000 0.000

6.25 0.000 0.000

6.06 0.000 0.000

5.87 0.000 0.000

5.68 0.000 0.000

5.49 0.000 0.000

5.21 0.000 0.000

5.12 0.000 0.000

5.00 0.355 -0.005

4.90 0.360 -0.010

4.75 0.365 -0.0 15

1.00 0.370 -0.020

4.50 0.375 -0.025

4.33 0.380 -0.030

4.14 0.385 -0.035

4.01 0.385 -0.035

3.80 0.385 -0.035

3.62 0.385 -0.035

3.40 0.390 -0.040

3.22 0.385 -0.035

3.00 0.385 -0.035

2.82 0.385 -0.035

2.60 0.385 -0.035

2.43 0.380 -0.035

2.20 0.385 -0.035

2.03 0.385 -0.035

1.80 0.385 -0.035

1.63 0.385 -0.035

1.40 0.385 -0.035

1.23 0.385 -0.035

1.00 0.385 -0.035

Table - 4.3.2

Ni (II) - SERINE -NTA-SYSTEM

[Ni (II)] = 5 × 10–5 M B.E. = 0.320 [Serine] = 1 × 10–3 M A.E. = 0.320

-Log [NTA] Absorbance DA

7.01 0.320 0.000

6.82 0.320 0.000

6.63 0.320 0.000

6.44 0.320 0.000

6.25 0.320 0.000

6.06 0.320 0.000

5.87 0.320 0.000

5.68 0.320 0.000

5.49 0.320 0.000

5.21 0.320 0.000

5.02 0.320 0.000

4.83 0.320 0.000

4.74 0.325 -0.005

4.65 0.330 -0.010

4.46 0.335 -0.015

4.37 0.340 -0.020

4.28 0.345 -0.025

4.09 0.350 -0.030

3.91 0.350 -0.030

3.72 0.350 -0.030

3.63 0.350 -0.030

3.44 0.350 -0.030

3.25 0.355 -0.035

2.96 0.350 -0.030

2.67 0.350 -0.030

2.38 0.350 -0.030

2.09 0.345 -0.030

1.81 0.350 -0.025

1.62 0.350 -0.030

1.43 0.350 -0.030

1.24 0.350 -0.030

1.01 0.350 -0.030

Table - 4.3.3

Co (II) - SERINE -NTA-SYSTEM

[Co (II)] = 5 × 10–5 M B.E. = 0.390 [Serine] = 1 × 10–3 M

A.E. = 0.390


7.01 0.390 0.000

6.82 0.390 0.000

6.63 0.390 0.000

6.44 0.390 0.000

6.25 0.390 0.000

6.06 0.390 0.000

5.87 0.390 0.000

5.68 0.390 0.000

5.49 0.390 0.000

5.20 0.390 0.000

5.01 0.390 0.000

4.82 0.390 0.000

4.63 0.390 0.000

4.44 0.390 0.000

4.25 0.395 -0.005

4.16 0.400 -0.010

5.97 0.405 -0.015

3.88 0.410 -0.020

3.79 0.415 -0.025

3.50 0.420 -0.030

3.31 0.420 -0.030

3.22 0.420 -0.030

3.03 0.420 -0.030

2.84 0.420 -0.030

2.65 0.420 -0.030

2.46 0.420 -0.035

2.27 0.420 -0.030

2.08 0.420 -0.030

1.09 0.415 -0.025

1.60 0.420 -0.030

1.41 0.420 -0.030

1.22 0.420 -0.030

1.03 0.420 -0.030

Table - 4.3.4

Zn (II) - SERINE -NTA-SYSTEM

[Zn (II)] = 5 × 10–5 M B.E. = 0.500 [Serine] = 1 × 10–3 M A.E. = 0.500


7.01 0.500 0.000

6.82 0.500 0.000

6.63 0.500 0.000

6.44 0.500 0.000

6.25 0.500 0.000

6.06 0.500 0.000

5.87 0.500 0.000

5.68 0.500 0.000

5.49 0.500 0.000

5.20 0.500 0.000

5.02 0.500 0.000

4.84 0.500 0.000

4.66 0.500 0.000

4.48 0.500 0.000

4.22 0.505 -0.005

4.14 0.510 -0.010

4.06 0.515 -0.015

3.88 0.529 -0.020

3.70 0.525 -0.025

3.62 0.530 -0.030

3.44 0.530 -0.030

3.26 0.530 -0.030

3.08 0.530 -0.030

2.81 0.535 -0.035

2.63 0.530 -0.030

2.50 0.530 -0.030

2.35 0.530 -0.030

2.20 0.530 -0.030

1.80 0.525 -0.025

1.80 0.530 -0.030

1.60 0.530 -0.030

1.40 0.530 -0.030

1.20 0.530 -0.030

1.00 0.530 -0.030

Table - 4.4.1

Cu (II) - HOMO SERINE -NTA-SYSTEM

[Cu (II)] = 5 × 10–5 M B.E. = 0.350 [Homo Serine] = 1 × 10–3 M A.E. = 0.350


7.00 0.350 0.000

6.80 0.350 0.000

6.60 0.350 0.000

6.40 0.350 0.000

6.20 0.350 0.000

6.00 0.350 6.000

5.80 0.350 0.000

560 0.350 0.000

5.40 0.350 0.000

5.20 0.350 0.000

5.00 0.350 0.000

4.90 0.355 -0.005

4.75 0.360 -0.010

4.65 0.365 -0.015

4.50 0.370 -0.020

4.35 0.375 -0.025

4.20 0.380 -0.030

4.05 0.385 -0.035

3.90 0.390 -0.040

3.80 0.390 -0.040

3.60 0.390 -0.040

3.40 0.390 -0.040

3.20 0.390 -0.035

3.00 0.390 -0.040

2.80 0.390 -0.040

2.60 0.390 -0.040

2.40 0.390 -0.045

2.20 0.390 -0.040

2.00 0.390 -0.040

1.80 0.390 -0.040

1.60 0.390 -0.040

1.40 0.390 -0.040

1.20 0.390 -0.040

1.00 0.390 -0.040

Table - 4.4.2

Ni (II) - HOMO SERINE -NTA-SYSTEM

[Ni (II)] = 5 × 10–5 M B.E. = 0.320 [Homo Serine] = 1 × 10–3 M A.E. = 0.320


7.00 0.320 0.000

6.80 0.320 0.000

6.60 0.320 0.000

6.40 0.320 0.000

6.20 0.320 0.000

6.00 0.320 0.000

5.80 0.320 0.000

5.60 0.320 0.000

5.40 0.320 0.000

5.20 0.320 0.000

5.00 0.320 0.000

4.80 0.320 0.000

4.05 0.320 0.000

3.95 0.325 -0.005

3.80 0.330 -0.010

3.70 0.335 -0.015

3.55 0.340 -0.020

3.45 0.345 -0.025

3.30 0.350 -0.030

3.20 0.355 -0.035

3.00 0.355 -0.035

2.50 0.355 -0.035

2.50 0.355 -0.035

2.50 0.355 -0.035

2.40 0.360 -0.040

2.30 0.355 -0.035

2.15 0.355 -0.035

2.00 0.355 -0.035

1.80 0.350 -0.030

1.60 0.355 -0.035

1.40 0.355 -0.035

1.20 0.355 -0.035

1.00 0.355 -0.035

Table - 4.4.3

Co (II) - HOMO SERINE-NTA-SYSTEM

[Co (II)] = 5 × 10–5 M B.E. = 0.390 [Homo Serine] = 1 × 10–3 M

A.E. = 0.390


7.00 0.390 0.000

6.80 0.390 0.000

6.60 0.390 0.000

6.40 0.390 0.000

6.20 0.390 0.000

6.00 0.390 0.000

5.80 0.390 0.000

5.60 0.390 0.000

5.40 0.390 0.000

5.20 0.390 0.000

5.00 0.390 0.000

4.80 0.390 0.000

4.60 0.390 0.000

4.40 0.390 0.000

4.25 0.395 -0.005

4.10 0.400 -0.010

5.95 0.405 -0.015

3.80 0.410 -0.020

3.70 0.415 -0.025

3.55 0.420 -0.030

3.35 0.420 -0.035

3.20 0.420 -0.035

3.00 0.420 -0.035

2.80 0.420 -0.035

2.60 0.420 -0.030

2.40 0.425 -0.035

2.20 0.420 -0.035

2.00 0.420 -0.035

1.0O 0.430 -0.040

1.60 0.425 -0.035

1.40 0.425 -0.035

1.20 0.425 -0.035

1.00 0.425 -0.035

Table - 4.4.4

Zn (II) - HOMO SERINE-NTA-SYSTEM

[Zn (II)] = 5 × 10–5 M B.E. = 0.500 [Homo Serine] = 1 × 10–3 M

A.E. = 0.500


7.00 0.500 0.000

6.80 0.500 0.000

6.60 0.500 0.000

6.40 0.500 0.000

6.20 0.500 0.000

6.00 0.500 0.000

5.80 0.500 0.000

5.60 0.500 0.000

5.40 0.500 0.000

5.20 0.500 0.000

5.00 0.500 0.000

4.80 0.500 0.000

4.60 0.500 0.000

4.45 0.500 0.000

4.30 0.505 -0.005

4.20 0.510 -0.010

4.05 0.515 -0.015

3.90 0.520 -0.020

3.75 0.525 -0.025

3.65 0.530 -0.030

3.50 0.530 -0.030

3.30 0.530 -0.030

3.10 0.530 -0.030

2.95 0.535 -0.035

2.80 0.530 -0.030

2.60 0.530 -0.030

2.40 0.530 -0.030

2.20 0.535 -0.025

2.00 0.535 -0.030

1.80 0.535 -0.035

1.60 0.535 -0.035

1.40 0.535 -0.035

1.20 0.535 -0.035

1.00 0.535 -0.035

Table - 4.5.1

Cu (II) - PROLINE-NTA-SYSTEM

[Cu (II)] = 5 × 10–5 M B.E. = 0.350 [Proline] = 1 × 10–3 M A.E. = 0.350


7.00 0.350 0.000

6.80 0.350 0.000

6.60 0.350 0.000

6.40 0.350 0.000

6.20 0.350 0.000

6.00 0.350 0.000

5.80 0.350 0.000

5.60 0.350 0.000

5.40 0.350 0.000

5.20 0.350 0.000

4.00 0.350 0.000

4.90 0.350 0.000

4.75 0.355 -0.005

4.G5 0.360 -0.010

1.50 0.365 -0.015

4.35 0.370 -0.020

4.25 0.375 -0.025

4.15 0.380 -0.030

4.05 O.385 -0.035

3.90 0.385 -0.035

3.70 0.385 -0.035

3.50 0.385 -0.035

3.30 0.390 -0.040

3.10 0.385 -0.035

3.00 0.385 -0.035

2.65 0.385 -0.035

2.75 0.385 -0.035

2.60 0.385 -0.035

2.45 0.385 -0.035

2.35 0.385 -0,035

2.20 0.385 -0,035

1.80 0.385 -0.035

1.40 0.385 -0.035

1.00 0.385 -0.035

Table - 4.5.2

Ni (II) - PROLINE-NTA-SYSTEM

[Ni (II)] = 5 × 10–5 M B.E. = 0.320

[Proline] = 1 × 10–3 M A.E. = 0.320


7.00 0.320 0.000

6.80 0.320 0.000

6.60 0.320 0.000

6.40 0.320 0.000

6.20 0.320 0.000

6.00 0.320 0.000

5.80 0.320 0.000

5.60 0.320 0.000

5.40 0.320 0.000

5.20 0.320 0.000

5.00 0.320 0.000

4.90 0.325 -0.000

4.75 0.330 -0.005

4.65 0.335 -0.010

4.50 0.340 -0.015

4.35 0.345 -0.020

4.20 0.345 -0.025

4.00 0.345 -0.025

3.80 0.345 -0.025

3.50 0.345 -0.025

3.20 0.345 -0.025

2.90 0.350 -0.030

2.60 0.345 -0.025

2.40 0.345 -0.025

2.20 0.345 -0.025

2.00 0.350 -0.030

1.80 0.345 -0.025

1.60 0.345 -0.025

1.40 0.345 -0.025

1.20 0.345 -0.025

1.00 0.345 -0.025

Table - 4.5.3

Co (II) - PROLINE-NTA-SYSTEM

[Co (II)] = 5 × 10–5 M B.E. = 0.390

[Proline] = 1 × 10–3 M A.E. = 0.390


7.00 0.300 0.000

6.80 0.300 0.000

6.60 0.390 0.000

6.40 0.390 0.000

6.20 0.390 0.000

6.00 0.390 0.000

5.80 0.390 0.000

5.60 0.390 0.000

5.40 0.390 0.000

5.20 0.390 0.000

5.00 0.390 0.000

4.80 0.390 0.000

4.70 0.390 0.000

4.50 0.300 0.000

4.30 0.390 0.000

4.15 0.395 -0.005

4.00 0.400 -0.010

3.90 0.405 -0.015

3.75 0.410 -0.020

3.60 0.415 -0.025

3.50 0.420 -0.030

3.35 0.420 -0.030

3.20 0.420 -0.030

3.00 0.415 -0.025

2.80 0.420 -0.030

2.60 0.420 -0.030

2.30 0.425 -0.035

1.90 0.420 -0.030

1.60 0.420 -0.030

1.40 0.420 -0.030

1.20 0.420 -0.030

1.00 0.420 -0.030

Table - 4.5.4

Zn (II) - PROLINE-NTA-SYSTEM

[Zn (II)] = 5 × 10–5 M B.E. = 0.500 [Proline] = 1 × 10–3 M A.E. = 0.500


7.00 0.500 0.000

6.80 0.500 0.000

6.60 0.500 0.000

6.40 0.500 0.000

6.20 0.500 0.000

6.00 0.500 0.000

5.80 0.500 0.000

5.60 0.500 0.000

5.40 0.500 0.000

5.20 0.500 0.000

5.00 0.500 0.000

4.80 0.500 0.000

4.60 0.500 0.000

4.45 0.510 -0.005

4.35 0.515 -0.010

4.20 0.520 -0.015

4.15 0.525 -0.020

4.00 0.525 -0.025

3.85 0.525 -0.025

3.70 0.525 -0.025

3.50 0.525 -0.025

3.30 0.525 -0.025

3.15 0.525 -0.025

3.00 0.530 -0.030

2.85 0.525 -0.025

2.70 0.525 -0.025

2.55 0.525 -0.025

2.40 0.530 -0.030

2.20 0.525 -0.025

2.00 0.525 -0.025

1.80 0.525 -0.025

1.60 0.525 -0.025

1.40 0.525 -0.025

1.20 0.525 -0.025

1.00 0.525 -0.025

Table - 4.6.1

Cu (II) - HYDROXY PROLINE-NTA-SYSTEM

Cu (II)] = 5 × 10–5 M B.E. = 0.350 [Hydroxy Proline] = 1 × 10–3 M A.E. = 0.350


7.00 0.350 0.000

6.80 0.350 0.000

6.60 0.350 0.000

6.40 0.350 0.000

6.20 0.350 0.000

6.00 0.350 6.000

5.80 0.350 0.000

560 0.350 0.000

5.40 0.350 0.000

5.20 0.350 0.000

5.00 0.350 0.000

4.90 0.355 -0.005

4.75 0.360 -0.010

4.65 0.365 -0.015

4.50 0.370 -0.020

4.35 0.375 -0.025

4.20 0.380 -0.030

4.05 0.385 -0.035

3.90 0.390 -0.040

3.80 0.390 -0.040

3.60 0.390 -0.040

3.40 0.390 -0.040

3.20 0.390 -0.035

3.00 0.390 -0.040

2.80 0.390 -0.040

2.60 0.390 -0.040

2.40 0.390 -0.045

2.20 0.390 -0.040

2.00 0.390 -0.040

1.80 0.390 -0.040

1.60 0.390 -0.040

1.40 0.390 -0.040

1.20 0.390 -0.040

1.00 0.390 -0.040

Table - 4.6.2

Ni (II) - HYDROXY PROLINE-NTA-SYSTEM

[Ni (II)] = 5 × 10–5 M B.E. = 0.320 [Hydroxy Proline] = 1 × 10–3 M

A.E. = 0.320


7.00 0.320 0.000

6.80 0.320 0.000

6.60 0.320 0.000

6.40 0.320 0.000

6.20 0.320 0.000

6.00 0.320 0.000

5.80 0.320 0.000

5.60 0.320 0.000

5.40 0.320 0.000

5.20 0.320 0.000

5.00 0.320 0.000

4.85 0.320 0.000

4.75 0.325 -0.005

4.60 0.330 -0.010

4.50 0.335 -0.015

4.35 0.340 -0.020

4.25 0.345 -0.025

4.10 0.350 -0.030

4.00 0.355 -0.035

3.85 0.360 -0.040

3.70 0.360 -0.040

3.50 0.360 -0.040

3.10 0.355 -0.035

2.70 0.360 -0.040

2.40 0.360 -0.040

2.20 0.360 - 0.040

2.00 0.360 -0.040

1.80 0.360 -0.040

1.60 0.360 -0.040

1.40 0.360 -0.040

1.20 0.360 -0.040

1.00 0.360 - 0.040

Table - 4.6.3

Co (II) - HYDROXY PROLINE-NTA-SYSTEM

[Co (II)] = 5 × 10–5 M B.E. = 0.390 [Hydroxy Proline] = 1 × 10–3 M A.E. = 0.390


7.00 0.390 0.000

6.80 0.390 0.000

6.60 0.390 0.000

6.40 0.390 0.000

6.20 0.390 0.000

6.00 0.390 0.000

5.80 0.390 0.000

5.60 0.390 0.000

5.40 0.390 0.000

5.20 0.390 0.000

5.00 0.390 0.000

4.80 0.390 0.000

4.60 0.390 0.000

4.50 0.395 -0.005

4.35 0.400 -0.010

4.20 0.405 -0.015

4.10 0.410 -0.020

3.95 0.415 -0.015

3.80 0.420 -0.020

3.70 0.425 -0.035

3.55 0.425 -0.035

3.40 0.425 -0.035

3.20 0.425 -0.035

3.00 0.425 -0.030

2.80 0.425 -0.035

2.60 0.425 -0.035

2.40 0.425 -0.035

2.20 0.430 -0.040

2.00 0.425 -0.035

1.80 0.425 -0.035

1.60 0.425 -0.035

1.40 0.425 -0.035

1.20 0.425 -0.035

1.00 0.425 -0.035

Table - 4.6.4

Zn (II) - HYDROXY PROLINE-NTA-SYSTEM

[Zn (II)] = 5 × 10–5 M B.E. = 0.500

[Hydroxy Proline] = 1 × 10–3 M A.E. = 0.500


7.00 0.500 0.000

6.80 0.500 0.000

6.60 0.500 0.000

6.40 0.500 0.000

6.20 0.500 0.000

6.00 0.500 0.000

5.80 0.500 0.000

5.60 0.500 0.000

5.40 0.500 0.000

5.20 0.500 0.000

5.00 0.500 0.000

4.80 0.500 0.000

4.60 0.500 0.000

4.45 0.500 0.000

4.30 0.505 -0.005

4.20 0.510 -0.010

4.05 0.515 -0.015

3.90 0.520 -0.020

3.75 0.525 -0.025

3.65 0.530 -0.030

3.50 0.530 -0.030

3.30 0.530 -0.030

3.10 0.530 -0.030

2.95 0.535 -0.035

2.80 0.530 -0.030

2.60 0.530 -0.030

2.40 0.530 -0.030

2.20 0.525 -0.025

2.00 0.530 -0.030

1.80 0.530 -0.030

1.60 0.530 -0.030

1.40 0.530 -0.030

1.20 0.530 -0.030

1.00 0.530 -0.030

LITERATURE CITED

1. Carey, G.H. ;

Baguchi, R.F. &

Martell, A.E.

: Inorg. Chem. 3 1280 (1964).

2. Falascka, H.A. : EDTA, Titration, Pergmon Press,

New York (1964).

3. Sathe, R.M.,

Mahederan, M. and

Shetty, S.Y.

: J. Chem. Soc, 5422 (1964).

4. Hull, J.A. ; Daries,

R.H. & Staveley,

L.A.K.

: J. Chem. Soc, 5422 (1964).

5. Thoron, L.C. and

learasss, Z.A.

: Inorg. Chem. 3, 89. (1963).

6. Vehave, A. ; Kyuna,

E. And Isuchiya, R.

: Bull. Chem. Soc. Japan 40, 2377

(1967).

7. Jorzensen, C.K. : Acta. Chem. Scand. 10, 887.

(1956).

8. Coney, G.H. &

Martell, A.E.

: J. Amer. Chem. Soc. 4699 196

1, 89, 2859, (1967).

9. Nielsch, W. and

Beltz. G.

: Z. Anal. Chem. 142 329. (1964).

10. Cheng, K.L. &

Warmuth

: Chemist Analyst 48 96, (1959).

11. Poeder, B.C. ; Dan

Boef. G.

: Anal. Chim. Acta 30, 261,

(1964).

12. Manmohan, S.E. &

Jawamoto, R.I.

: J. Electronnel. Chem. 14, 213,

(1967).

13. Nard, M. : Acta chem. Scand, 9 401 (1955)

14. Boltz, G. and

Nielsch W.

: Z. anal. Chem. 142 240 (1954)

15. Hull, J.A.; Davies,

R.H. & Staveley

L.A.K.

: J. Chem. Soc. 5422 , (1964).

16. Gao, Qian : Gooding Xuexias theaxan suebao

5 (5) 631-4 (1988).

17. Kornev, V.I.;

Valyaleva, V.A.:

Mukanov, I.P.

Zn. Fiz Khim, 52 (5), 1132-5

(1988)

18. Elenkova, N.G.:

Tsoneva, R.A.

: J. inorg. Nucl. Chem. 35 (3),

841-7. (1993)

19. Redevich, V.S. : Zn. Fiz. Khim. 51 (7), 1760-2

(1977)

20. Pitre K.S. & Chitale

V.K.

: J. Indian Chem. Soc. 58 (1), 82-

3, (9181)

21. Kornev, V.I.;

Valyalem, V.a.;

Zobnin, S.I.

: Zn. Fiz. Khim. 52 (10) 2702

(1978).

22. Tananaeva, N.N.;

Kostromine, S.I.

: Zn. Neogr. Khim.17 (9), 2783-6:

(1972)

23. ramamoorthy, S.;

Manning, P.C.

: J. inorg. Nucl. Chem. 35 (5)

1571-5. (1973).

24. Manani, L.P.

Jujurkar,,

G,R,;Bhattacharya,

P.K.

: Indian J. Chem. 10 (7), 742-3.

(1992).

25. Rubin, Martina;

Martill, A.E.

: Biol. Trace, Elem. Res. 2 (1), 1-

19, 1980.

26. Nicholas, A.; Tifone,

A.; Bllgado, L.N.;

Nassif, S.T.

:

Radiochem. Radioanaly. Lett. 57

(1) 43-54. (1983)

27. Frank, Barbara;

Wysockacisek,

Janina, Soltysiak,

Brazyna Binl, K.

:

Two Mauk. Mat. Fiz, Chem. 25

(1) 37-44, 1983 ( Pub. 1994).

28. Yoshimura, C.&

Tanmura, k.

: Bunseki, Kazaku, 21 929 (1992)

29. Longman, G.F.;

Stiff, M.J. &

Gardiner, D.K.

: Wat. Res. 5 1171 (1991)

30. Tabatabai, M.A.;

Bremmer, J.M. and

Storier, R.R.

: Commum. Soil. Sci. Plant. Anal.

3 57, (1972)

31. Robinson, J.L. &

Lott, P.F.

: J. Microchem. 18, 128, (1973)

32. Nielsch. W. & Beltz;

G.

: Z. Anal. Chem. 14 4401, (1955)

33. P.K. Miggal &

Triplyahova V.A.

: Deposited Doc. 1976 VINITI

3976-76 ; 11 pp

34. Studnickova, M,;

Smela, J. and

Precentel, P.

: Collect, Czech. Chem. Commun.

42 (2), 548-61 (1996)

35. Kodoma, M, &

Ebine, H,

: Bull. Chem. Soc. Japan, 40

1857 (1997).

36. Jackobs, N.E. &

Margerum, D.N.

: Inorg. Chem. 6 2038 (1967).

37. Chidambram, M.V.

and Bhattacharya,

P.K.

: Acta Chim. (Hung), 75, 123

(1973)

38. Bajchi, R. and Dey.

A.K.

: Ind-J. Chem. 15 (3), 831 (1978)

39. Ramamoorthy, S.,

Gurabaschetti, C. &

Fecchio, D.

: J. inorg. Nucl. Chem. 34 1651

(1972)

40. Ramamoorty, S.;

Manning, P.G. &

Gurnaschetti, C.

: J. inorg. Nucl. Chem. 34, 3443.

(1992)

41. Rahmani, R. and

Malik, W.U.

: Proc. Indian Natl. Sci. Acad. Part

A. 46 (6), 572-5, (1980)

42. Mishra, R.K. and

Dey A.K.

: J. Indian. Chem. Soc. 60 (6),

521-3 (1983).

43. Tsiplayakova, V.A.;

Chan Thi Thanh.

perong & Nguyen.

: Zn. Neorg. Khim 27 (7) 1701-6.

(1982)

44. Sirkar, J.K. J. Chem. Eng. Data 29 (2), 141-

3, (1984).

45. Singh, R.K.P.;

Yadava, J.R.;

Yadava, K.L.

: J. Electrochemical. Soc. India 30

(3), 250-2 (1981).

46. Yadava, J.R.;Sirkar

J.K.; Yadava, K.L.

: Electrochim. Acta 26 (3) 391-4,

(1981).

47. Singh, R.K.P.;

Khelawan, R.

Yadava, K.L.

: Natl. Acad.Sci. Lett. (India) 4

(II). 441-51, (1981)

48. Sirkar, J.K. : Z. Phys. Chem. (Leipzig) 268 (1)

156-60. (1987)

49. Singh, S; Rani,

B.R.; Vyas, M.

Yadava, K.L.

: Chem. Ser. 26 (2) 363-6.

(1996)

50. Gupta, Deepa;

Singh, S; Yadava,

K.L.

: Acta Chim. Hung. 120 (1) 47-55

(1995)

51. Singh, S. and

Yadava, K.L.

: J. Chem., Soc. (Pak) 9 (4) 1515

(1987)

52. Singh, S. and

Yadav, K.L.

: Proc. Ind. Nat. Sci. Aca. 53 (A),

421 (1997)

53. Singh, S. and

Yadav, K.L.

: Z. Phys. Chemie 287 903 (1986)

54. Singh, S. and

Yadav, K.L.

: Z. Phys. Chemie. 267 1008

(1986)

55. Singh, S and Yadav,

K.L.

Pol. J. Chem. 59, 1021, (1988).

56. Singh S. and

Yadav, K.L.

: Bull. Soc. Chem. (France) 127,

507 (1990)

57. Singh S. and Yadav,

K.L.

: Nat. Aca. Sci. (latter), 14 (8),

343 (1991)

58. Singh, S and

Tripathi, S.R.

: Proc. Nat Aca.Sci. 62 (A), 393

(1992)

59. Singh, S. and Gaur.

K.

: J. Chemitrack 3, 1 (2001).

60. Singh, S. and Gaur,

K.

: Asian J.Chem. 15 (1), 353

(2003).

61. Tewari B.B. and Yadav,

K.L.

: Trans. SAEST. 25 (4), 124 (1990).


K.L.

: J. Chromatogr. 542 - 537 (1991).


K.L.

: Bull. Soc. Fr. 128, 141 (1991).


K.L.

: J. Chem. Soc. Pak. 13 (4), 244

(1991).


K.L.

: J. Chromatogr. 547 - 554 (1991).


K.L.

: Trans. SAEST. 27 (1), 31 (1992).


K.L.

: Proc. Nat. Acad. Sci. 61 (A), 13

(1992).

68. Tewari B.B., Pandey

A.K. and Singh R.K.P.

: Proc. Nat. Acad. Sci. 65 (A), 35

(1995).


K.L.

: Biomed. Chromatogr. 10 (5), 221

(1996).

70. Tewari B.B. : J. Chromatogr. 910 (1), 181

(2001)

71. Singh, S.S., Singh,

V.K. and Singh, S.

: Pur. Aca. Sci. 12, 346 (2006).

72. Singh, N. and Singh, S. : Pur. Aca. Sci. 12, 261 (2006).

73. Singh, S.S., Singh,

V.K. and Singh, S.

: J. Chemtrack 8, 13 (2006).

74. Mishra and Singh, S. : J. Chemtrack 8, 119 (2006).

75. Pandey, A.K. and

Singh, S.

: J. Chemtrack 8, 133 (2006).

76. Yadav, T.K. and Singh,

S.

: Int. J. Phy. Sci. 19 (1), 117 (2009).

77. Singh, N. and Singh, S. : Int. J. Phy. Sci. 19 (1), 125 (2009).

* * * * * *

mechanism of the complex formation was studied. the...

Documents