# Studies on Ion-Exchange Properties of Polyaniline Zr(IV) Tungstoiodophosphate Nanocomposite Ion Exchanger

Authors: K. Jacinth Mispa; P. Subramaniam; R. Murugesan
Journal: Journal of Polymers
 (2013)

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## Abstract

Organic-inorganic hybrid materials prepared by sol-gel approach have attracted a great deal of attention in material science. Organic polymeric part of the composite provides mechanical and chemical stability whereas the inorganic part supports the ion-exchange behaviour and thermal stability and also increases the electrical conductivity. Such modified composite materials can be applied as an electrochemically switchable ion exchanger for water treatment, especially water softening. Polyaniline zirconium(IV) tungstoiodophosphate nanocomposite ion exchanger is prepared by sol-gel method. Polyaniline zirconium(IV) tungstoiodophosphate nanocomposite ion exchanger is synthesized and characterized by Fourier transform-infrared spectra, ultraviolet-visible spectra, X-ray diffraction, scanning electron microscopy, thermogravimetric analysis, ion exchange, conductivity, and antimicrobial studies. A mechanism for the formation of the polyaniline zirconium(IV) tungstoiodophosphate nanocomposite ion exchanger was discussed. The route reported here may be used for the preparation of other nanocomposite ion exchangers.


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## Body

## 1. Introduction

Organic-inorganic hybrid materials prepared by sol-gel approach have attracted a great deal of attention in material science. Organic polymeric part of the composite provides mechanical and chemical stability whereas the inorganic part supports the ion-exchange behaviour, thermal stability and also increases the electrical conductivity. Such modified composite materials can be applied as electrochemically switchable ion exchanger [1, 2] for water treatment, especially water softening. The synthesis of hybrid ion exchangers with controlled functionality and hydrophobicity could open new avenues for organometallic chemistry, catalysis, organic host-guest chemistry, analytical chemistry [3–5], hydrometallurgy, antibiotic purification, separation of radioactive isotopes and large scale application in water treatment and pollution control [6, 7]. Thus, organic-inorganic hybrid materials are expected to provide many possibilities as new composite materials. Accordingly, the hybrid can be used to modify organic polymer materials or to modify inorganic glassy materials. In addition to these characteristics, the hybrid materials can be considered as new composite materials that exhibit very different properties from their original components, that is, organic polymer and inorganic materials especially in the case of molecular level hybrids. Thus, the synthesis of polymeric/inorganic composites has received a great deal of attention because it provided new materials with special mechanical, chemical, electrochemical, and optical as well as magnetic properties [8–11].A few such excellent ion exchange materials have been developed and are successfully being used in chromatographic techniques [12–14]. An inorganic ion exchanger based on organic polymeric matrix is an interesting material, as it possesses the mechanical stability due to the presence of organic species and the basic characteristics of an inorganic ion exchanger regarding its selectivity for some particular metal ions [15–17]. It was therefore considered to synthesize such hybrid ion exchangers with a good ion exchange capacity, high stability, reproducibility, and selectivity for heavy metal ions, indicating that they are useful in environmental applications. Synthetic ion exchangers based on tetravalent metals have been the objects of considerable study in recent years because of their selectivity and intercalation properties. Zirconium based ion exchangers have received attention because of their excellent ion-exchange behaviour and some important chemical applications in the field of ion exchange, ion-exchange membrane, and solid state electrochemistry [18]. Goward et al. [19] have reported that polyaniline Zr(IV) tungstophosphate nanocomposite ion exchanger was used for the selective separation of La3+ and UO22+. The literature reveals that several three-component ion exchangers, that is, zirconium(IV) iodooxalate, zirconium(IV) phosphosilicate, zirconium(IV) phosphoborate, and zirconium(IV) tungstophosphate [20], behaviour studied for their synthesis, ion-exchange behavior, and analytical applications. This work deals with the synthesis, characterization, and the study of ion-exchange properties of polyaniline Zr(IV) tungstoiodophosphate as a new ion exchanger.


## 2. Materials and Methods

### 2.1. Synthesis of Zirconium(IV) Tungstoiodophosphate

Zirconium(IV) tungstoiodophosphate ion exchanger was prepared by mixing 1.61 g of zirconium oxychloride octahydrate (0.1 M) in 50 mL of 4 N hydrochloric acid solution. This was added to a solution containing 5.4 g of potassium iodate (0.5 M) and 8.3 g of sodium tungstate (0.5 M) in 100 mL of water at the flow rate of 0.5 mL min−1. To the resulting mixture, 50 mL of 1 M orthophosphoric acid was added by maintaining the pH as 1 with constant stirring using a magnetic stirrer at room temperature. The white gel obtained was filtered off, washed thoroughly with distilled water to remove excess acid and was dried in an air oven at 60°C.


### 2.2. Preparation of Polyaniline-Cl−

Polyaniline was prepared from aniline byin situ chemical oxidative polymerization technique using potassium perdisulphate (KPS) as an oxidant. Polymerization was effected at room temperature by drop-wise addition of the oxidant (0.1 M) in water to the continuously stirred solution of aniline (0.1 M) in hydrochloric acid for an hour. After the addition of the oxidant, polymerization was allowed to proceed further for 24 hours in a refrigerator. The formed precipitate was filtered, washed with distilled water, methanol, and acetone repeatedly until the filtrate became colourless, and was dried in an air oven at 60°C. The dried greenish black powder of polyaniline-Cl− was ground into a fine powder.


### 2.3. Preparation of Polyaniline Zirconium(IV) Tungstoiodophosphate

The composite ion exchanger was prepared by the sol-gel mixing of polyaniline, an organic conducting polymer with the inorganic precipitate of zirconium(IV) tungstoiodophosphate [21–23]. In this process, in situ polymerization of aniline (0.1 M) in the presence of 100 mg of zirconium(IV) tungstoiodophosphate was carried out using 0.1 M KPS as oxidant. Polymerization was effected by drop-wise addition of 5.7 g of the oxidant in 100 mL of water to the continuously stirred solution of aniline and zirconium(IV) tungstoiodophosphate in 1 N hydrochloric acid for an hour. After addition of all potassium perdisulphate, polymerization was allowed to proceed further for 24 hours in a refrigerator. The resultant mixture was turned slowly into greenish black coloured slurry. The polyaniline composite gels were filtered off and washed thoroughly with distilled water to remove the excess acid and any adhering trace of potassium perdisulphate. The product was dried in air oven at 60°C. The dried gel was put into the distilled water to obtain granules of uniform size. The washed gels were dried at 60°C in an air oven. The dried granules were converted into the H+ form by keeping them immersed in 1 M nitric acid for 24 hours with occasional shaking and intermittently replacing the supernatant liquid with fresh acid. The material thus obtained was then washed with distilled water to remove the excess acid before drying finally at 60°C.


### 2.4. Characterisation

Polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger and H+ form of conducting polymeric-inorganic hybrid ion exchanger were characterized by FT-IR spectra, UV-visible spectra, X-ray diffraction, SEM, TGA, and conductivity studies. AC electrical conductivity measurement was done on the pelletized samples by using Digital LCR meter (Pacific, Model: PLCR 8C) at different temperatures. UV-visible spectra of the synthesized samples were recorded at room temperature in different solvents, namely, NMP, chloroform, o-cresol, and DMSO in 300–900 nm range with Elico model SL-164 Double Beam UV-visible spectrophotometer. FT-IR spectra of conducting organic polymer, inorganic ion exchanger, and conducting polymer-inorganic hybrid ion exchanger were taken by KBr disc method at room temperature performed on NEXUS-670 FT-IR spectrophotometer. The powder X-ray diffraction technique has been employed to identify the crystalline phases of the samples using monochromatized Cu-K∝ (λ=1.5056 Å) on X-ray diffractometer (Model: PW3040/60 X’pert PRO) at a 0.2° scan rate (in 2θ). SEM was performed on ground materials by an electron microscope JEOL Model JSM-6390LV at various magnifications (5x to 300,000x). TGA studies of the conducting polymeric composite materials in the original form were carried out by an automatic thermobalance on heating the material from 30°C to 1000°C at a constant rate of 10°C min−1 in the nitrogen atmosphere with Perkin Elmer, Diamond Thermogravimetric Analyzer.


## 2.1. Synthesis of Zirconium(IV) Tungstoiodophosphate

Zirconium(IV) tungstoiodophosphate ion exchanger was prepared by mixing 1.61 g of zirconium oxychloride octahydrate (0.1 M) in 50 mL of 4 N hydrochloric acid solution. This was added to a solution containing 5.4 g of potassium iodate (0.5 M) and 8.3 g of sodium tungstate (0.5 M) in 100 mL of water at the flow rate of 0.5 mL min−1. To the resulting mixture, 50 mL of 1 M orthophosphoric acid was added by maintaining the pH as 1 with constant stirring using a magnetic stirrer at room temperature. The white gel obtained was filtered off, washed thoroughly with distilled water to remove excess acid and was dried in an air oven at 60°C.


## 2.2. Preparation of Polyaniline-Cl−

Polyaniline was prepared from aniline byin situ chemical oxidative polymerization technique using potassium perdisulphate (KPS) as an oxidant. Polymerization was effected at room temperature by drop-wise addition of the oxidant (0.1 M) in water to the continuously stirred solution of aniline (0.1 M) in hydrochloric acid for an hour. After the addition of the oxidant, polymerization was allowed to proceed further for 24 hours in a refrigerator. The formed precipitate was filtered, washed with distilled water, methanol, and acetone repeatedly until the filtrate became colourless, and was dried in an air oven at 60°C. The dried greenish black powder of polyaniline-Cl− was ground into a fine powder.


## 2.3. Preparation of Polyaniline Zirconium(IV) Tungstoiodophosphate

The composite ion exchanger was prepared by the sol-gel mixing of polyaniline, an organic conducting polymer with the inorganic precipitate of zirconium(IV) tungstoiodophosphate [21–23]. In this process, in situ polymerization of aniline (0.1 M) in the presence of 100 mg of zirconium(IV) tungstoiodophosphate was carried out using 0.1 M KPS as oxidant. Polymerization was effected by drop-wise addition of 5.7 g of the oxidant in 100 mL of water to the continuously stirred solution of aniline and zirconium(IV) tungstoiodophosphate in 1 N hydrochloric acid for an hour. After addition of all potassium perdisulphate, polymerization was allowed to proceed further for 24 hours in a refrigerator. The resultant mixture was turned slowly into greenish black coloured slurry. The polyaniline composite gels were filtered off and washed thoroughly with distilled water to remove the excess acid and any adhering trace of potassium perdisulphate. The product was dried in air oven at 60°C. The dried gel was put into the distilled water to obtain granules of uniform size. The washed gels were dried at 60°C in an air oven. The dried granules were converted into the H+ form by keeping them immersed in 1 M nitric acid for 24 hours with occasional shaking and intermittently replacing the supernatant liquid with fresh acid. The material thus obtained was then washed with distilled water to remove the excess acid before drying finally at 60°C.


## 2.4. Characterisation

Polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger and H+ form of conducting polymeric-inorganic hybrid ion exchanger were characterized by FT-IR spectra, UV-visible spectra, X-ray diffraction, SEM, TGA, and conductivity studies. AC electrical conductivity measurement was done on the pelletized samples by using Digital LCR meter (Pacific, Model: PLCR 8C) at different temperatures. UV-visible spectra of the synthesized samples were recorded at room temperature in different solvents, namely, NMP, chloroform, o-cresol, and DMSO in 300–900 nm range with Elico model SL-164 Double Beam UV-visible spectrophotometer. FT-IR spectra of conducting organic polymer, inorganic ion exchanger, and conducting polymer-inorganic hybrid ion exchanger were taken by KBr disc method at room temperature performed on NEXUS-670 FT-IR spectrophotometer. The powder X-ray diffraction technique has been employed to identify the crystalline phases of the samples using monochromatized Cu-K∝ (λ=1.5056 Å) on X-ray diffractometer (Model: PW3040/60 X’pert PRO) at a 0.2° scan rate (in 2θ). SEM was performed on ground materials by an electron microscope JEOL Model JSM-6390LV at various magnifications (5x to 300,000x). TGA studies of the conducting polymeric composite materials in the original form were carried out by an automatic thermobalance on heating the material from 30°C to 1000°C at a constant rate of 10°C min−1 in the nitrogen atmosphere with Perkin Elmer, Diamond Thermogravimetric Analyzer.


## 3. Studies of Ion-Exchange Properties of PANI Zirconium(IV) Tungstoiodophosphate

### 3.1. Ion Exchange Capacity (IEC)

For the determination of ion-exchange capacity, one gram of the dry cation exchanger in H+ form was taken into a glass column. The bed length was approximately 1.5 cm long. 1 M alkali metal chlorides (LiCl, NaCl, and KCl) were used to elute the H+ ions completely from the cation exchange columns maintaining a very slow flow rate of ~0.5 mL min−1. The effluents were titrated against standard 0.1 M NaOH solution for the total ions liberated in the solutions using phenolphthalein indicator.


### 3.2. Effect of Eluent Concentration on IEC

To find out the optimum concentration of eluent for complete elution of H+ ions, a fixed volume (250 mL) of LiCl, NaCl, and KCl solutions of varying concentrations (0.2–1.8 M) was passed through a column containing 1 g of the exchanger in H+ form with a flow rate of ~0.5 mL min−1. The effluent was titrated against standard alkali solution of 0.1 M NaOH for the H+ ions eluted out for the determination of eluent concentration using phenolphthalein as an indicator.


### 3.3. Elution Behavior

A column containing 1 g of the exchanger in H+ form was eluted with 1.4 M of LiCl, 1.4 M of NaCl and 1.2 M of KCl solutions of different 10 mL fractions with minimum flow rate of 0.5 mL min−1. Each fraction of 10 mL effluent was titrated against standard NaOH (0.1 M) solution to determine the strength of H+ ions eluted out.


### 3.4. Effect of Time on IEC

The optimum shaking time of ion exchanger with LiCl, NaCl, and KCl solutions for complete elution of H+ ions was also determined. 0.25 g of the ion exchanger was shaken with 25 mL of alkali metal chloride solutions (LiCl, NaCl, and KCl), and the amount of liberated H+ ions was titrated against the standard NaOH solution after every half an hour interval.


### 3.5. pH Titration

The pH titration studies of PANI Zr(IV) tungstoiodophosphate was performed by the method of Topp and Pepper [24]. A total of 200 mg portions of the cation exchanger in the H+ form were placed in each of the several 250 mL conical flasks followed by the addition of equimolar solutions of alkali metal chlorides (LiCl, NaCl, and KCl) and their hydroxides (LiOH, NaOH, and KOH) in different volume ratios; the final volume was kept as 50 mL to maintain the ionic strength constant. The pH of the solution was recorded every 24 hours until equilibrium was attained which needed 5 days.


### 3.6. Selectivity (Sorption) Studies

The distribution behaviour of metal ions plays an important role in the determination of the selectivity of the material. The distribution coefficient (Kd values) of various metal ions on cation exchangers can be determined as follows. 200 mg of the composite cation exchanger beads in the H+ form was taken with 20 mL (0.005 M) of different metal nitrate solutions, PbNO3, Co(NO3)2, and Cu(NO3)2 and kept for 24 hours with continuous shaking for 6 hours in a shaker at 25±2°C to attain equilibrium. The metal ions in the solution before and after equilibrium were determined by titrating against standard 0.005 M solutions of EDTA [25]. The distribution coefficient is the measure of a fractional uptake of metal ions competing for H+ ions form a solution by an ion-exchange material and mathematically calculated using the formula
(1)Kd=(I-F)F×Vm,
where I and F are the initial and final amounts of metal ion in aqueous phase (M), V is the volume of the solution (mL), and m is the amount of cation exchanger (g).


## 3.1. Ion Exchange Capacity (IEC)

For the determination of ion-exchange capacity, one gram of the dry cation exchanger in H+ form was taken into a glass column. The bed length was approximately 1.5 cm long. 1 M alkali metal chlorides (LiCl, NaCl, and KCl) were used to elute the H+ ions completely from the cation exchange columns maintaining a very slow flow rate of ~0.5 mL min−1. The effluents were titrated against standard 0.1 M NaOH solution for the total ions liberated in the solutions using phenolphthalein indicator.


## 3.2. Effect of Eluent Concentration on IEC

To find out the optimum concentration of eluent for complete elution of H+ ions, a fixed volume (250 mL) of LiCl, NaCl, and KCl solutions of varying concentrations (0.2–1.8 M) was passed through a column containing 1 g of the exchanger in H+ form with a flow rate of ~0.5 mL min−1. The effluent was titrated against standard alkali solution of 0.1 M NaOH for the H+ ions eluted out for the determination of eluent concentration using phenolphthalein as an indicator.


## 3.3. Elution Behavior

A column containing 1 g of the exchanger in H+ form was eluted with 1.4 M of LiCl, 1.4 M of NaCl and 1.2 M of KCl solutions of different 10 mL fractions with minimum flow rate of 0.5 mL min−1. Each fraction of 10 mL effluent was titrated against standard NaOH (0.1 M) solution to determine the strength of H+ ions eluted out.


## 3.4. Effect of Time on IEC

The optimum shaking time of ion exchanger with LiCl, NaCl, and KCl solutions for complete elution of H+ ions was also determined. 0.25 g of the ion exchanger was shaken with 25 mL of alkali metal chloride solutions (LiCl, NaCl, and KCl), and the amount of liberated H+ ions was titrated against the standard NaOH solution after every half an hour interval.


## 3.5. pH Titration

The pH titration studies of PANI Zr(IV) tungstoiodophosphate was performed by the method of Topp and Pepper [24]. A total of 200 mg portions of the cation exchanger in the H+ form were placed in each of the several 250 mL conical flasks followed by the addition of equimolar solutions of alkali metal chlorides (LiCl, NaCl, and KCl) and their hydroxides (LiOH, NaOH, and KOH) in different volume ratios; the final volume was kept as 50 mL to maintain the ionic strength constant. The pH of the solution was recorded every 24 hours until equilibrium was attained which needed 5 days.


## 3.6. Selectivity (Sorption) Studies

The distribution behaviour of metal ions plays an important role in the determination of the selectivity of the material. The distribution coefficient (Kd values) of various metal ions on cation exchangers can be determined as follows. 200 mg of the composite cation exchanger beads in the H+ form was taken with 20 mL (0.005 M) of different metal nitrate solutions, PbNO3, Co(NO3)2, and Cu(NO3)2 and kept for 24 hours with continuous shaking for 6 hours in a shaker at 25±2°C to attain equilibrium. The metal ions in the solution before and after equilibrium were determined by titrating against standard 0.005 M solutions of EDTA [25]. The distribution coefficient is the measure of a fractional uptake of metal ions competing for H+ ions form a solution by an ion-exchange material and mathematically calculated using the formula
(1)Kd=(I-F)F×Vm,
where I and F are the initial and final amounts of metal ion in aqueous phase (M), V is the volume of the solution (mL), and m is the amount of cation exchanger (g).


## 4. Results and Discussion

In the present study, new and novel organic-inorganic electrically conducting nanocomposite cation exchanger was chemically prepared by sol-gel mixing of organic conducting polymer, polymer (polyaniline) into the matrix of inorganic ion exchanger, Zr(IV) tungstoiodophosphate. The different steps involved in the mechanism for the formation of conducting polymeric-inorganic nanocomposite ion exchanger are shown in Scheme1. Polyaniline gel was prepared by oxidation coupling of monomers using K2S2O8 in acidic medium. The binding of polyaniline into the matrix of Zr(IV) tungstoiodophosphate is possible due to ionic interaction between the radical cation of polyaniline and an ionic group, Zr(IV) tungstoiodophosphate.Scheme 1
Polymerisation reaction with the ion exchanger as the dopant.


### 4.1. Electrical Conductivity Studies

From the capacitance obtained from the instrument and thickness as well as the diameter of the pellet, the AC electrical conductivity of the polyaniline Zr(IV) tungstoiodophosphate sample was calculated using the following equation:(2)Co=Aε0dεr=CCoσ=2πfε0εrtanδ,
where σac is the AC electrical conductivity (S/cm−1); f the frequency (Hz); ε0 the permittivity in free space (8.85×10-12 f/m); εr the relative permittivity (f/m); tanδ the tangent loss (or) dielectric loss; C the capacitance at particular temperature (Faradays); C0 the capacitance at absolute temperature (Faradays); A the area of the sample (m2); d the thickness of the sample (m); r the radius of the sample (m).The capacitance and conductance of the material over a range of temperature and frequency are then calculated from the relationship between the applied voltage and measured current and are related to relative permittivity (εr) and the dielectric loss factor (tanδ), respectively. Dielectric loss or tangent loss (dissipation factor) is the tangent of the loss angle when a dielectric is subject to a sinusoidally varying applied electric field. Since tanδ is equal to the ratio of the imaginary loss to the real (storage) relative permittivity, it is also the ratio of the energy dissipated to the energy stored for each cycle. tanδ is high frequency and temperature dependent, and reaching a maximum value as a dielectric relaxation is passed. Dielectric permittivity is a measure of the energy stored in a material subjected to electrical, stress that is, the ability of an insulator or semiconductor to resist the passage of alternating current or serve as a capacitor.


### 4.2. Charge Transport Properties of PANI and Polyaniline Zr(IV) Tungstoiodophosphate

The conductivity of chemically synthesized PANI and its samples presented in Table1, depends on a number of parameters such as temperature, protonation, and oxidation state [26–32]. The emeraldine salt form of PANI has the electrical conductivity 5.893 × 10−3 Scm−1, which is having high electrical conductivity when compared with that of emeraldine base form of PANI which has 5.528 × 10−7 Scm−1. The incorporation of Zr(IV) tungstoiodophosphate into the matrix of conducting organic polymer leads to an increase in conductivity (8.471 × 10−3 Scm−1) of this ion exchanger as compared to PANI emeraldine salt.Table 1
AC conductivity of various polyaniline samples at room temperature.
Sample
C (nano-or-pico Faradays)
D or tan δ
r (mm)
d (mm)
σ
ac (Scm−1)
PANI salt
15.30 (n.f)
4.90
6.69
1.78
5.893
×
10
-
3
Dedoped PANI
9.2 (p.f)
0.96
6.73
1.42
5.528
×
10
-
7
PANI ZrTIP
16.10 (n.f)
4.40
6.67
2.66
8.471
×
10
-
3
Dedoped PANI ZTIP
8.9 (p.f)
0.57
6.67
0.84
1.916
×
10
-
7
H+ form  of PANI ZTIP
17.16 (n.f)
4.74
6.66
1.53
5.561
×
10
-
3The conductivity for this organic-inorganic hybrid ion exchanger shows semiconductor behaviour. The linear portion of the graphlogσ versus 1/T fits to Arrhenius type equation (3) for this ion exchanger. Figure 1 is a representive of such plot:
(3)σ(T)=σ0exp(-Eg/2KT),
where Eg is the activation energy of conductivity which is obtained from the slope. K is the Boltzmann’s constant, and σ0 represents the value of σ at 1/T=0. The variation of conductivity (σ) as a function of 1/T at constant frequency is shown in Figure 1. The temperature dependence of conductivity is described in Table 2.  The follow up Arrehenius behaviour is regarded as a good approximation to band theory. Further, the temperature dependence of conductivity and the follow up arrehenius behaviour indicate that the conduction in polyaniline hybrid ion exchanger is predominantly performed by variable range hopping process. An increase in the values of the electrical conductivity is driven by an increase in mobility of free charges (i.e., polarons and free ions).Table 2
Conductivity of polyaniline Zr(IV) tungstoiodophosphate ion exchanger at different temperatures.
Temp. (°C)
D
C
σ
ac (Scm−1)
1000/T (K)
ln
σ
ac
100
0.95
41.9
4.76
2.681
−5.3475
95
0.68
35.2
2.86
2.717
−5.8569
90
0.54
30.9
2.00
2.755
−6.2146
85
0.49
28.0
1.64
2.793
−6.4131
80
0.45
25.1
1.32
2.833
−6.6301
75
0.44
18.9
1.02
2.874
−6.8879
70
0.41
16.3
0.80
2.916
−7.1309
65
0.37
14.5
0.64
2.959
−7.354
60
0.33
12.1
0.49
3.003
−7.6211
55
0.29
10.8
0.37
3.049
−7.9020
50
0.26
9.2
0.29
3.096
−8.1456
45
0.21
7.1
0.18
3.145
−8.6226
40
0.18
5.3
0.11
3.195
−9.1150
35
0.16
4.4
0.08
3.247
−9.4335Figure 1
Arrhenius plot for polyaniline Zr(IV) tungstoiodophosphate ion exchanger.In order to determine the conductivity parameters, the temperature dependence of conductivity (linear portion) is fit to the following equation:(4)σ(T)=σ0exp-(T0T)1/2.The activation energy of conductivity for this hybrid ion exchanger was found to be 0.086 eV. Actually, the mobility of charge carriers under the influence of an external field up to 100°C increases with doping level. The value of activation energy is indicating that the charge carrier has to overcome the same energy barrier while conducting. Thus, the polarons act as charge carrier hopping from state in all the polymer samples.


### 4.3. FT-IR Spectra

FT-IR spectra are used as a tool to characterize the molecular structures of organic-inorganic hybrid ion exchanger. The FT-IR spectrum of PANI-Cl− (a), polyaniline Zr(IV) tungstoiodophosphate ion exchanger (b), and H+ form of polyaniline Zr(IV) tungstoiodophosphate ion exchanger (c) are given in Figure 2.Figure 2The peaks at 1565 cm−1 and 1495 cm−1 are attributed to C=N and C=C stretching modes for the quinoid and benzenoid rings, the peaks at about 1300 cm−1 and 1231 cm−1 are attributed to C–N stretching mode for benzenoid ring, and the peak at 1121 cm−1 is assigned to the plane bending vibration of C–H (modes of N=Q=N, Q=NH+–B, and B–NH+–B), and out-plane bending vibrations of PANI are reported to occur at about 801 cm−1.In the present study also, all the peaks represented above are observed in PANI ZTIP nanocomposite ion exchanger (Table3), but they are modified in both intensity and peak position when the polymer is incorporated into the inorganic matrix of Zr(IV) tungstoiodophosphate. An assembly of three peaks in the 500–1000 cm−1 region showed that ionic phosphate groups as well as metal-oxygen bonds are present in the material [33]. It is also an evidence for the formation of PANI ZTIP nanocomposite ion exchanger.Table 3
FT-IR spectral data of the polymer samples.
Characterisation
PANI-Cl− (cm−1)
PANI ZTIP (cm−1)
H+ form of PANI ZTIP (cm−1)
C=N and C=C stretching modes for the quinoid and benzenoid rings
1565, 1495
1595, 1493
1560, 1472
C–N stretching mode for benzenoid ring
1300, 1231
1309, 1216
1383, 1240
In-plane C–H bending mode
1121
1152
1117
Out of  plane C–H bending mode
801
811
798
Due toPO43-, HPO42-, and H2PO42-
1010
1000
M–O bond and presence of iodate
523, 450
590, 506


### 4.4. UV-Visible Spectroscopy

UV-visible spectra of all the polyaniline samples were recorded at room temperature in solvents like N-methyl pyrrolidone, chloroform, and m-cresol and the peak positions are given in Table4. The samples exhibit two or three peaks in these solvents. From the UV-visible spectra of the polymer samples in NMP, it is evident that NMP is of a coordinating nature and the polymer samples get coordinated in the protonated N-site after displacing dopant ions and thereby convert salt into base. This observation is also in good agreement with previous reports. The UV-visible spectrum of PANI samples in chloroform has three absorption peaks (<300 nm, ~400 nm, and ~550 nm). From the UV-visible spectra in chloroform and m-cresol, it is clear that polymer chains have different electronic structures in chloroform and m-cresol. This difference in electronic structures can be attributed only to their difference in conformational structures. Specifically, polymer chains of PANI have a more extended conformation and hence a longer conjugation length in m-cresol than in chloroform. The three absortion peaks of polymer samples in chloroform can be assigned as the transition from π band to π* band, from polaron band to π* band, and π band to polaron band, respectively.Table 4
UV-visible absorption data of polyaniline samples in different solvents.
Sample
Peak position (nm)
NMP
CHCl3
m-Cresol
PANI-HCl
312, 575, 620
224, 428, 651
314, 556
PANI ZTIP
308, 558
226, 326, 554
312, 534
H+ form of PANI ZTIP
319, 617
243, 328, 554
330, 366, 963In m-cresol, the polymer chains of PANI have an extended conformation in which the twist defects between aromatic rings are removed, and hence the interaction between the adjacent polarons becomes stronger. The absorption peak at 550 nm is associated with the replacement of random coil conformation by intraband transitions within the half filled polaron band. At the same time, betweenπ band to π* band (<300 nm) become very weak since the band gap between π band and the polaron band has been eliminated. In all solvents, the difference in the peak position is observed when the polymer is incorporated into the inorganic guest matrix.


### 4.5. X-Ray Diffraction Study

The powder X-ray diffraction technique has been employed to identify the crystalline phases of the samples using monochromatized Cu-K∝ (1.5056 Å). The average crystallite size was measured from X-ray broadening by employing the well-known Scherrer equation, D=0.96λ/βCosθ and the value obtained for different PANI samples are given in Table 5. The XRD pattern for PANI-Cl− (a), H+ form of polyaniline Zr(IV) tungstoiodophosphate ion exchanger (b), and polyaniline Zr(IV) tungstoiodophosphate ion exchanger (c) is given in Figure 3.Table 5
Average crystallite size of polymer samples.
Sample
Crystallite size (nm)
PANI emeraldine salt
64
H+ form of PANI ZTIP
78
PANI ZTIP
75Figure 3


### 4.6. Scanning Electron Microscopy Studies

Scanning electron microscopy was performed on ground materials at various magnifications. SEM images for the polyaniline Zr(IV) tungstoiodophosphate ion exchanger at various magnifications are shown in Figure4.Figure 4It has been revealed that, after binding of polyaniline with Zr(IV) tungstoiodophosphate, the morphology has been changed, and the average crystallite size of the composite material was found to be ~75 nm. The X-ray powder diffraction pattern of this ion exchanger suggests an amorphous nature of the composite material. Thus, it was confirmed from both XRD and SEM that the crystallite size shows the nanorange.


### 4.7. Thermal (TGA) Studies

TGA and DTG (first derivative of TGA) curves for polyaniline emeraldine salt (a) and polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger (b) in nitrogen atmosphere are shown in Figure5. The results reveal a typical three-step weight loss behaviour. For polyaniline, in the first step, 7.0% weight loss is seen up to 130°C. This is attributed to the loss of water molecules from the polymer samples. The second weight loss starts at around 120°C and ends at around 560°C. This is attributed to possibly coevolution of acid, as well as the low molecular weight fragments of the polymer. The third step, starting from 560°C onwards, represents degradation of the polymer, and this also indicates the decomposition of the backbone of polyaniline. A large weight loss above 560°C and up to 1000°C was found to be 58.0% and leaving a marked amount of residue (42.0% wt) due to carbonization in nitrogen atmosphere [34].Figure 5TGA studies of the composite cation exchange material in the original form were carried out by an automatic thermobalance on heating the material from 40°C to 1000°C at a constant rate of 10°C min−1 in the nitrogen atmosphere. The thermogravimetric analysis curves, TGA and DTG, reveal a considerable weight loss of about 15.8% from 40°C to 120°C in polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger, and this can be explained due to the removal of external water molecules. Slow weight loss of the material from 120°C to about 440°C may be due to the removal of dopant as well as conversion of phosphate group to pyrophosphate group [35]. A weight loss of mass observed after 440°C is due to decomposition of the organic part of polyaniline. The steep decrease in weight loss in the temperature region 440–700°C can be explained as the removal of pyrophosphate group besides thermal decomposition of polyaniline chain. At 900°C, the decomposition of the polymer has been completed and after 900°C the plateau represents the completion of degradation. The residue obtained after 900°C (24.0%) may be due to carbonization of polyaniline and the formation of metal oxide.


### 4.8. Ion-Exchange Properties

#### 4.8.1. Ion-Exchange Capacity (IEC)

The ion-exchange capacity of the hybrid ion exchanger for alkali metal ions increases according to the decrease in the hydrated ionic radii [36–38] as evident from Table 6. Nachod and Wood have also given the similar observations for the exchanged alkali metal ions on carbonaceous zeolite [39]. The maximum ion-exchange capacity sequence for alkali metal ions is K+> Na+> Li+. The size of exchanging ion affects IEC of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger.Table 6
IEC of various ions on polyaniline Zr(IV) tungstoiodophosphate ion exchanger.
Exchanging ions
pH of the metal solution
Ionic radii (Å)
Hydrated ionic radii (Å)
Ion-exchange capacity (meq·dry g−1)
Li+
3.3
0.68
3.40
4.2
Na+
5.0
0.97
2.76
5.3
K+
6.8
1.33
2.32
5.9


#### 4.8.2. Effect of Eluent Concentration on IEC

Effect of alkali metal chloride concentration on ion exchange capacity of PANI ZTIP nanocomposite ion exchanger is presented in Figure6 and Table 7. The data revealed that the rate of elution increased with the eluent concentration. The highest rate of elution was observed with 1.4 M, 1.4 M, and 1.2 M LiCl, NaCl, and KCl eluent, respectively, for maximum release of H+ ions from polyaniline Zr(IV) tungstoiodophosphate ion exchanger by using 1 g of the cation exchanger.Table 7
Effect of  the concentration of eluent on IEC.
Concentration of eluent (M)
Ion-exchange capacity (meq·dry/g)
Li+ion
Na+ion
K+ ion
0.2
2.5
2.9
3.5
0.4
2.7
3.2
3.9
0.6
3.0
3.6
4.3
0.8
3.3
4.1
4.8
1.0
3.7
4.4
5.1
1.2
3.9
4.8
5.9
1.4
4.2
5.3
5.9
1.6
4.2
5.3
5.9
1.8
4.2
5.3
5.9Figure 6
Effect of concentration of eluent on IEC.


#### 4.8.3. Elution Behaviour

The elution behaviour (Figure7) indicated that the exchange is quite fast because only 170 mL of LiCl solution (1.4 M), 150 mL of NaCl solution (1.4 M), and 140 mL of KCl solution (1.2 M) are enough to release the total H+ from 1 g of PANI ZrTIP cation-exchange material (Table 8).Table 8
Elution behavior of polyaniline Zr(IV) tungstoiodophosphate ion exchanger.
Volume of eluent (mL)
Strength of H+ released (M)
LiCl
NaCl
KCl
10
0.0650
0.0740
0.0830
20
0.0450
0.0470
0.0440
30
0.0380
0.0422
0.0395
40
0.0370
0.0390
0.0392
50
0.0340
0.0370
0.0228
60
0.0330
0.0292
0.0197
70
0.0320
0.0289
0.0186
80
0.0290
0.0267
0.0175
90
0.0290
0.0250
0.0173
100
0.0280
0.0240
0.0160
110
0.0250
0.0200
0.0150
120
0.0240
0.0160
0.0149
130
0.0200
0.0156
0.0145
140
0.0200
0.0153
0.0140
150
0.0180
0.015
0.0140
160
0.0170
0.015
0.0140
170
0.0150
0.015
0.0140
180
0.0150
0.015
0.0140
190
0.0150
0.015
0.0140
200
0.0150
0.015
0.0140Figure 7
Elution behavior of polyaniline Zr(IV) tungstoiodophosphate ion exchanger.


#### 4.8.4. Effect of Time on IEC

The effect of elution time on IEC of the hybrid exchanger is shown in Table9. The effect of equilibration time on exchange capacity of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger using LiCl, NaCl, and KCl eluents shows that constant capacity occurs after 3.5, 3.0, and 2.5 hours respectively, and is shown in Figure 8.Table 9
Effect of elution time on IEC of polyaniline  Zr(IV) tungstoiodophosphate ion exchanger using LiCl, NaCl, and KCl eluents.
Equilibrium time (Hours)
Ion-exchange capacity of ion exchanger (meq·dry g−1)
Li+ion
Na+ion
K+ ion
0
1.28
2.12
3.92
0.5
1.92
3.40
5.60
1.0
2.00
4.00
6.30
1.5
2.14
5.40
7.80
2.0
4.12
6.20
9.60
2.5
5.32
7.00
15.20
3.0
5.80
7.40
15.20
3.5
6.32
7.40
15.20
4.0
6.32
7.40
15.20
4.5
6.32
7.40
15.20
5.0
6.32
7.40
15.20Figure 8
Effect of elution time on IEC of polyaniline Zr(IV) tungstoiodophosphate ion exchanger using (a) LiCl (b) NaCl (c) KCl eluents.


#### 4.8.5. pH Titration

The pH titration curves for polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger were obtained under equilibrium conditions with LiOH/LiCl, NaOH/NaCl, and KOH/KCl systems indicating bifunctional behaviour of the material as shown in Figure9.Figure 9
pH value of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger with various alkali metal hydroxides.At low pH, the weak acidic groups remain undissociated. The addition of LiOH, NaOH, and KOH neutralized the solution, and the weak acidic group dissociates; thus, the ion exchange starts toward completion. The pH titration curves showed a gradual rise in pH initially and a steep rise at the end because strong acidic groups were completely exchanged with Li+, Na+ and K+ ions at the end. The rate of H+-K+ exchange was faster than those of H+-Na+, and H+-Li+ exchanges.


#### 4.8.6. Selectivity (Sorption) Studies

In order to find out the potentiality of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger in the separation of metal ions, distribution studies for three metal ions were performed in four solvent systems. The results of distribution studies (Table10) show that Kd value varies with the nature and composition of contacting solvents. It was also observed from the sorption studies (Kd values) that the composite has a maximum selectivity towards Pb2+ than other metal ions like Cu2+ and Co2+.Table 10
Distribution coefficient values of some metal ions on polyaniline Zr(IV) tungstoiodophosphate in different solvent systems.
Metal ions
K
d values in different solvent systems
DMW
10% ethanol
10% acetone
1 M H2SO4
Pb2+
265
172
251
51
Cu2+
96
115
122
13
Co2+
59
86
37
90


#### 4.8.7. Studies of Antimicrobial Activity

The antimicrobial activity studies of the PANI and polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger were carried out using the Kirby-Bauer antimicrobial susceptibility test procedure [40] against two bacteria, namely, E. coli and Proteus vulgaris (Figure 10). The test solutions of these two samples were prepared in NMP solvent. The antimicrobial activity study results are summarized in the Table 11.Table 11
Antimicrobial activity studies of polymer samples.
Organisms
Media
Zone of  inhibition in (mm)
Control
PANI
Polyaniline Zr(IV) tungstoiodophosphate ion exchanger
Escherichia coli
Muller
18
15
20
Proteus vulgaris
Histon Agar
20
20
16Zone formation against (a)E. coli and (b) Proteus vulgaris.
(a)
(b)From the table, polymer and the conducting polymeric-inorganic nanocomposite ion exchanger showed higher antimicrobial activity againstE. coli and Proteus vulgaris, and inhibition zones were formed due to their antimicrobial activity.


## 4.1. Electrical Conductivity Studies

From the capacitance obtained from the instrument and thickness as well as the diameter of the pellet, the AC electrical conductivity of the polyaniline Zr(IV) tungstoiodophosphate sample was calculated using the following equation:(2)Co=Aε0dεr=CCoσ=2πfε0εrtanδ,
where σac is the AC electrical conductivity (S/cm−1); f the frequency (Hz); ε0 the permittivity in free space (8.85×10-12 f/m); εr the relative permittivity (f/m); tanδ the tangent loss (or) dielectric loss; C the capacitance at particular temperature (Faradays); C0 the capacitance at absolute temperature (Faradays); A the area of the sample (m2); d the thickness of the sample (m); r the radius of the sample (m).The capacitance and conductance of the material over a range of temperature and frequency are then calculated from the relationship between the applied voltage and measured current and are related to relative permittivity (εr) and the dielectric loss factor (tanδ), respectively. Dielectric loss or tangent loss (dissipation factor) is the tangent of the loss angle when a dielectric is subject to a sinusoidally varying applied electric field. Since tanδ is equal to the ratio of the imaginary loss to the real (storage) relative permittivity, it is also the ratio of the energy dissipated to the energy stored for each cycle. tanδ is high frequency and temperature dependent, and reaching a maximum value as a dielectric relaxation is passed. Dielectric permittivity is a measure of the energy stored in a material subjected to electrical, stress that is, the ability of an insulator or semiconductor to resist the passage of alternating current or serve as a capacitor.


## 4.2. Charge Transport Properties of PANI and Polyaniline Zr(IV) Tungstoiodophosphate

The conductivity of chemically synthesized PANI and its samples presented in Table1, depends on a number of parameters such as temperature, protonation, and oxidation state [26–32]. The emeraldine salt form of PANI has the electrical conductivity 5.893 × 10−3 Scm−1, which is having high electrical conductivity when compared with that of emeraldine base form of PANI which has 5.528 × 10−7 Scm−1. The incorporation of Zr(IV) tungstoiodophosphate into the matrix of conducting organic polymer leads to an increase in conductivity (8.471 × 10−3 Scm−1) of this ion exchanger as compared to PANI emeraldine salt.Table 1
AC conductivity of various polyaniline samples at room temperature.
Sample
C (nano-or-pico Faradays)
D or tan δ
r (mm)
d (mm)
σ
ac (Scm−1)
PANI salt
15.30 (n.f)
4.90
6.69
1.78
5.893
×
10
-
3
Dedoped PANI
9.2 (p.f)
0.96
6.73
1.42
5.528
×
10
-
7
PANI ZrTIP
16.10 (n.f)
4.40
6.67
2.66
8.471
×
10
-
3
Dedoped PANI ZTIP
8.9 (p.f)
0.57
6.67
0.84
1.916
×
10
-
7
H+ form  of PANI ZTIP
17.16 (n.f)
4.74
6.66
1.53
5.561
×
10
-
3The conductivity for this organic-inorganic hybrid ion exchanger shows semiconductor behaviour. The linear portion of the graphlogσ versus 1/T fits to Arrhenius type equation (3) for this ion exchanger. Figure 1 is a representive of such plot:
(3)σ(T)=σ0exp(-Eg/2KT),
where Eg is the activation energy of conductivity which is obtained from the slope. K is the Boltzmann’s constant, and σ0 represents the value of σ at 1/T=0. The variation of conductivity (σ) as a function of 1/T at constant frequency is shown in Figure 1. The temperature dependence of conductivity is described in Table 2.  The follow up Arrehenius behaviour is regarded as a good approximation to band theory. Further, the temperature dependence of conductivity and the follow up arrehenius behaviour indicate that the conduction in polyaniline hybrid ion exchanger is predominantly performed by variable range hopping process. An increase in the values of the electrical conductivity is driven by an increase in mobility of free charges (i.e., polarons and free ions).Table 2
Conductivity of polyaniline Zr(IV) tungstoiodophosphate ion exchanger at different temperatures.
Temp. (°C)
D
C
σ
ac (Scm−1)
1000/T (K)
ln
σ
ac
100
0.95
41.9
4.76
2.681
−5.3475
95
0.68
35.2
2.86
2.717
−5.8569
90
0.54
30.9
2.00
2.755
−6.2146
85
0.49
28.0
1.64
2.793
−6.4131
80
0.45
25.1
1.32
2.833
−6.6301
75
0.44
18.9
1.02
2.874
−6.8879
70
0.41
16.3
0.80
2.916
−7.1309
65
0.37
14.5
0.64
2.959
−7.354
60
0.33
12.1
0.49
3.003
−7.6211
55
0.29
10.8
0.37
3.049
−7.9020
50
0.26
9.2
0.29
3.096
−8.1456
45
0.21
7.1
0.18
3.145
−8.6226
40
0.18
5.3
0.11
3.195
−9.1150
35
0.16
4.4
0.08
3.247
−9.4335Figure 1
Arrhenius plot for polyaniline Zr(IV) tungstoiodophosphate ion exchanger.In order to determine the conductivity parameters, the temperature dependence of conductivity (linear portion) is fit to the following equation:(4)σ(T)=σ0exp-(T0T)1/2.The activation energy of conductivity for this hybrid ion exchanger was found to be 0.086 eV. Actually, the mobility of charge carriers under the influence of an external field up to 100°C increases with doping level. The value of activation energy is indicating that the charge carrier has to overcome the same energy barrier while conducting. Thus, the polarons act as charge carrier hopping from state in all the polymer samples.


## 4.3. FT-IR Spectra

FT-IR spectra are used as a tool to characterize the molecular structures of organic-inorganic hybrid ion exchanger. The FT-IR spectrum of PANI-Cl− (a), polyaniline Zr(IV) tungstoiodophosphate ion exchanger (b), and H+ form of polyaniline Zr(IV) tungstoiodophosphate ion exchanger (c) are given in Figure 2.Figure 2The peaks at 1565 cm−1 and 1495 cm−1 are attributed to C=N and C=C stretching modes for the quinoid and benzenoid rings, the peaks at about 1300 cm−1 and 1231 cm−1 are attributed to C–N stretching mode for benzenoid ring, and the peak at 1121 cm−1 is assigned to the plane bending vibration of C–H (modes of N=Q=N, Q=NH+–B, and B–NH+–B), and out-plane bending vibrations of PANI are reported to occur at about 801 cm−1.In the present study also, all the peaks represented above are observed in PANI ZTIP nanocomposite ion exchanger (Table3), but they are modified in both intensity and peak position when the polymer is incorporated into the inorganic matrix of Zr(IV) tungstoiodophosphate. An assembly of three peaks in the 500–1000 cm−1 region showed that ionic phosphate groups as well as metal-oxygen bonds are present in the material [33]. It is also an evidence for the formation of PANI ZTIP nanocomposite ion exchanger.Table 3
FT-IR spectral data of the polymer samples.
Characterisation
PANI-Cl− (cm−1)
PANI ZTIP (cm−1)
H+ form of PANI ZTIP (cm−1)
C=N and C=C stretching modes for the quinoid and benzenoid rings
1565, 1495
1595, 1493
1560, 1472
C–N stretching mode for benzenoid ring
1300, 1231
1309, 1216
1383, 1240
In-plane C–H bending mode
1121
1152
1117
Out of  plane C–H bending mode
801
811
798
Due toPO43-, HPO42-, and H2PO42-
1010
1000
M–O bond and presence of iodate
523, 450
590, 506


## 4.4. UV-Visible Spectroscopy

UV-visible spectra of all the polyaniline samples were recorded at room temperature in solvents like N-methyl pyrrolidone, chloroform, and m-cresol and the peak positions are given in Table4. The samples exhibit two or three peaks in these solvents. From the UV-visible spectra of the polymer samples in NMP, it is evident that NMP is of a coordinating nature and the polymer samples get coordinated in the protonated N-site after displacing dopant ions and thereby convert salt into base. This observation is also in good agreement with previous reports. The UV-visible spectrum of PANI samples in chloroform has three absorption peaks (<300 nm, ~400 nm, and ~550 nm). From the UV-visible spectra in chloroform and m-cresol, it is clear that polymer chains have different electronic structures in chloroform and m-cresol. This difference in electronic structures can be attributed only to their difference in conformational structures. Specifically, polymer chains of PANI have a more extended conformation and hence a longer conjugation length in m-cresol than in chloroform. The three absortion peaks of polymer samples in chloroform can be assigned as the transition from π band to π* band, from polaron band to π* band, and π band to polaron band, respectively.Table 4
UV-visible absorption data of polyaniline samples in different solvents.
Sample
Peak position (nm)
NMP
CHCl3
m-Cresol
PANI-HCl
312, 575, 620
224, 428, 651
314, 556
PANI ZTIP
308, 558
226, 326, 554
312, 534
H+ form of PANI ZTIP
319, 617
243, 328, 554
330, 366, 963In m-cresol, the polymer chains of PANI have an extended conformation in which the twist defects between aromatic rings are removed, and hence the interaction between the adjacent polarons becomes stronger. The absorption peak at 550 nm is associated with the replacement of random coil conformation by intraband transitions within the half filled polaron band. At the same time, betweenπ band to π* band (<300 nm) become very weak since the band gap between π band and the polaron band has been eliminated. In all solvents, the difference in the peak position is observed when the polymer is incorporated into the inorganic guest matrix.


## 4.5. X-Ray Diffraction Study

The powder X-ray diffraction technique has been employed to identify the crystalline phases of the samples using monochromatized Cu-K∝ (1.5056 Å). The average crystallite size was measured from X-ray broadening by employing the well-known Scherrer equation, D=0.96λ/βCosθ and the value obtained for different PANI samples are given in Table 5. The XRD pattern for PANI-Cl− (a), H+ form of polyaniline Zr(IV) tungstoiodophosphate ion exchanger (b), and polyaniline Zr(IV) tungstoiodophosphate ion exchanger (c) is given in Figure 3.Table 5
Average crystallite size of polymer samples.
Sample
Crystallite size (nm)
PANI emeraldine salt
64
H+ form of PANI ZTIP
78
PANI ZTIP
75Figure 3


## 4.6. Scanning Electron Microscopy Studies

Scanning electron microscopy was performed on ground materials at various magnifications. SEM images for the polyaniline Zr(IV) tungstoiodophosphate ion exchanger at various magnifications are shown in Figure4.Figure 4It has been revealed that, after binding of polyaniline with Zr(IV) tungstoiodophosphate, the morphology has been changed, and the average crystallite size of the composite material was found to be ~75 nm. The X-ray powder diffraction pattern of this ion exchanger suggests an amorphous nature of the composite material. Thus, it was confirmed from both XRD and SEM that the crystallite size shows the nanorange.


## 4.7. Thermal (TGA) Studies

TGA and DTG (first derivative of TGA) curves for polyaniline emeraldine salt (a) and polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger (b) in nitrogen atmosphere are shown in Figure5. The results reveal a typical three-step weight loss behaviour. For polyaniline, in the first step, 7.0% weight loss is seen up to 130°C. This is attributed to the loss of water molecules from the polymer samples. The second weight loss starts at around 120°C and ends at around 560°C. This is attributed to possibly coevolution of acid, as well as the low molecular weight fragments of the polymer. The third step, starting from 560°C onwards, represents degradation of the polymer, and this also indicates the decomposition of the backbone of polyaniline. A large weight loss above 560°C and up to 1000°C was found to be 58.0% and leaving a marked amount of residue (42.0% wt) due to carbonization in nitrogen atmosphere [34].Figure 5TGA studies of the composite cation exchange material in the original form were carried out by an automatic thermobalance on heating the material from 40°C to 1000°C at a constant rate of 10°C min−1 in the nitrogen atmosphere. The thermogravimetric analysis curves, TGA and DTG, reveal a considerable weight loss of about 15.8% from 40°C to 120°C in polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger, and this can be explained due to the removal of external water molecules. Slow weight loss of the material from 120°C to about 440°C may be due to the removal of dopant as well as conversion of phosphate group to pyrophosphate group [35]. A weight loss of mass observed after 440°C is due to decomposition of the organic part of polyaniline. The steep decrease in weight loss in the temperature region 440–700°C can be explained as the removal of pyrophosphate group besides thermal decomposition of polyaniline chain. At 900°C, the decomposition of the polymer has been completed and after 900°C the plateau represents the completion of degradation. The residue obtained after 900°C (24.0%) may be due to carbonization of polyaniline and the formation of metal oxide.


## 4.8. Ion-Exchange Properties

### 4.8.1. Ion-Exchange Capacity (IEC)

The ion-exchange capacity of the hybrid ion exchanger for alkali metal ions increases according to the decrease in the hydrated ionic radii [36–38] as evident from Table 6. Nachod and Wood have also given the similar observations for the exchanged alkali metal ions on carbonaceous zeolite [39]. The maximum ion-exchange capacity sequence for alkali metal ions is K+> Na+> Li+. The size of exchanging ion affects IEC of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger.Table 6
IEC of various ions on polyaniline Zr(IV) tungstoiodophosphate ion exchanger.
Exchanging ions
pH of the metal solution
Ionic radii (Å)
Hydrated ionic radii (Å)
Ion-exchange capacity (meq·dry g−1)
Li+
3.3
0.68
3.40
4.2
Na+
5.0
0.97
2.76
5.3
K+
6.8
1.33
2.32
5.9


### 4.8.2. Effect of Eluent Concentration on IEC

Effect of alkali metal chloride concentration on ion exchange capacity of PANI ZTIP nanocomposite ion exchanger is presented in Figure6 and Table 7. The data revealed that the rate of elution increased with the eluent concentration. The highest rate of elution was observed with 1.4 M, 1.4 M, and 1.2 M LiCl, NaCl, and KCl eluent, respectively, for maximum release of H+ ions from polyaniline Zr(IV) tungstoiodophosphate ion exchanger by using 1 g of the cation exchanger.Table 7
Effect of  the concentration of eluent on IEC.
Concentration of eluent (M)
Ion-exchange capacity (meq·dry/g)
Li+ion
Na+ion
K+ ion
0.2
2.5
2.9
3.5
0.4
2.7
3.2
3.9
0.6
3.0
3.6
4.3
0.8
3.3
4.1
4.8
1.0
3.7
4.4
5.1
1.2
3.9
4.8
5.9
1.4
4.2
5.3
5.9
1.6
4.2
5.3
5.9
1.8
4.2
5.3
5.9Figure 6
Effect of concentration of eluent on IEC.


### 4.8.3. Elution Behaviour

The elution behaviour (Figure7) indicated that the exchange is quite fast because only 170 mL of LiCl solution (1.4 M), 150 mL of NaCl solution (1.4 M), and 140 mL of KCl solution (1.2 M) are enough to release the total H+ from 1 g of PANI ZrTIP cation-exchange material (Table 8).Table 8
Elution behavior of polyaniline Zr(IV) tungstoiodophosphate ion exchanger.
Volume of eluent (mL)
Strength of H+ released (M)
LiCl
NaCl
KCl
10
0.0650
0.0740
0.0830
20
0.0450
0.0470
0.0440
30
0.0380
0.0422
0.0395
40
0.0370
0.0390
0.0392
50
0.0340
0.0370
0.0228
60
0.0330
0.0292
0.0197
70
0.0320
0.0289
0.0186
80
0.0290
0.0267
0.0175
90
0.0290
0.0250
0.0173
100
0.0280
0.0240
0.0160
110
0.0250
0.0200
0.0150
120
0.0240
0.0160
0.0149
130
0.0200
0.0156
0.0145
140
0.0200
0.0153
0.0140
150
0.0180
0.015
0.0140
160
0.0170
0.015
0.0140
170
0.0150
0.015
0.0140
180
0.0150
0.015
0.0140
190
0.0150
0.015
0.0140
200
0.0150
0.015
0.0140Figure 7
Elution behavior of polyaniline Zr(IV) tungstoiodophosphate ion exchanger.


### 4.8.4. Effect of Time on IEC

The effect of elution time on IEC of the hybrid exchanger is shown in Table9. The effect of equilibration time on exchange capacity of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger using LiCl, NaCl, and KCl eluents shows that constant capacity occurs after 3.5, 3.0, and 2.5 hours respectively, and is shown in Figure 8.Table 9
Effect of elution time on IEC of polyaniline  Zr(IV) tungstoiodophosphate ion exchanger using LiCl, NaCl, and KCl eluents.
Equilibrium time (Hours)
Ion-exchange capacity of ion exchanger (meq·dry g−1)
Li+ion
Na+ion
K+ ion
0
1.28
2.12
3.92
0.5
1.92
3.40
5.60
1.0
2.00
4.00
6.30
1.5
2.14
5.40
7.80
2.0
4.12
6.20
9.60
2.5
5.32
7.00
15.20
3.0
5.80
7.40
15.20
3.5
6.32
7.40
15.20
4.0
6.32
7.40
15.20
4.5
6.32
7.40
15.20
5.0
6.32
7.40
15.20Figure 8
Effect of elution time on IEC of polyaniline Zr(IV) tungstoiodophosphate ion exchanger using (a) LiCl (b) NaCl (c) KCl eluents.


### 4.8.5. pH Titration

The pH titration curves for polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger were obtained under equilibrium conditions with LiOH/LiCl, NaOH/NaCl, and KOH/KCl systems indicating bifunctional behaviour of the material as shown in Figure9.Figure 9
pH value of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger with various alkali metal hydroxides.At low pH, the weak acidic groups remain undissociated. The addition of LiOH, NaOH, and KOH neutralized the solution, and the weak acidic group dissociates; thus, the ion exchange starts toward completion. The pH titration curves showed a gradual rise in pH initially and a steep rise at the end because strong acidic groups were completely exchanged with Li+, Na+ and K+ ions at the end. The rate of H+-K+ exchange was faster than those of H+-Na+, and H+-Li+ exchanges.


### 4.8.6. Selectivity (Sorption) Studies

In order to find out the potentiality of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger in the separation of metal ions, distribution studies for three metal ions were performed in four solvent systems. The results of distribution studies (Table10) show that Kd value varies with the nature and composition of contacting solvents. It was also observed from the sorption studies (Kd values) that the composite has a maximum selectivity towards Pb2+ than other metal ions like Cu2+ and Co2+.Table 10
Distribution coefficient values of some metal ions on polyaniline Zr(IV) tungstoiodophosphate in different solvent systems.
Metal ions
K
d values in different solvent systems
DMW
10% ethanol
10% acetone
1 M H2SO4
Pb2+
265
172
251
51
Cu2+
96
115
122
13
Co2+
59
86
37
90


### 4.8.7. Studies of Antimicrobial Activity

The antimicrobial activity studies of the PANI and polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger were carried out using the Kirby-Bauer antimicrobial susceptibility test procedure [40] against two bacteria, namely, E. coli and Proteus vulgaris (Figure 10). The test solutions of these two samples were prepared in NMP solvent. The antimicrobial activity study results are summarized in the Table 11.Table 11
Antimicrobial activity studies of polymer samples.
Organisms
Media
Zone of  inhibition in (mm)
Control
PANI
Polyaniline Zr(IV) tungstoiodophosphate ion exchanger
Escherichia coli
Muller
18
15
20
Proteus vulgaris
Histon Agar
20
20
16Zone formation against (a)E. coli and (b) Proteus vulgaris.
(a)
(b)From the table, polymer and the conducting polymeric-inorganic nanocomposite ion exchanger showed higher antimicrobial activity againstE. coli and Proteus vulgaris, and inhibition zones were formed due to their antimicrobial activity.


## 4.8.1. Ion-Exchange Capacity (IEC)

The ion-exchange capacity of the hybrid ion exchanger for alkali metal ions increases according to the decrease in the hydrated ionic radii [36–38] as evident from Table 6. Nachod and Wood have also given the similar observations for the exchanged alkali metal ions on carbonaceous zeolite [39]. The maximum ion-exchange capacity sequence for alkali metal ions is K+> Na+> Li+. The size of exchanging ion affects IEC of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger.Table 6
IEC of various ions on polyaniline Zr(IV) tungstoiodophosphate ion exchanger.
Exchanging ions
pH of the metal solution
Ionic radii (Å)
Hydrated ionic radii (Å)
Ion-exchange capacity (meq·dry g−1)
Li+
3.3
0.68
3.40
4.2
Na+
5.0
0.97
2.76
5.3
K+
6.8
1.33
2.32
5.9


## 4.8.2. Effect of Eluent Concentration on IEC

Effect of alkali metal chloride concentration on ion exchange capacity of PANI ZTIP nanocomposite ion exchanger is presented in Figure6 and Table 7. The data revealed that the rate of elution increased with the eluent concentration. The highest rate of elution was observed with 1.4 M, 1.4 M, and 1.2 M LiCl, NaCl, and KCl eluent, respectively, for maximum release of H+ ions from polyaniline Zr(IV) tungstoiodophosphate ion exchanger by using 1 g of the cation exchanger.Table 7
Effect of  the concentration of eluent on IEC.
Concentration of eluent (M)
Ion-exchange capacity (meq·dry/g)
Li+ion
Na+ion
K+ ion
0.2
2.5
2.9
3.5
0.4
2.7
3.2
3.9
0.6
3.0
3.6
4.3
0.8
3.3
4.1
4.8
1.0
3.7
4.4
5.1
1.2
3.9
4.8
5.9
1.4
4.2
5.3
5.9
1.6
4.2
5.3
5.9
1.8
4.2
5.3
5.9Figure 6
Effect of concentration of eluent on IEC.


## 4.8.3. Elution Behaviour

The elution behaviour (Figure7) indicated that the exchange is quite fast because only 170 mL of LiCl solution (1.4 M), 150 mL of NaCl solution (1.4 M), and 140 mL of KCl solution (1.2 M) are enough to release the total H+ from 1 g of PANI ZrTIP cation-exchange material (Table 8).Table 8
Elution behavior of polyaniline Zr(IV) tungstoiodophosphate ion exchanger.
Volume of eluent (mL)
Strength of H+ released (M)
LiCl
NaCl
KCl
10
0.0650
0.0740
0.0830
20
0.0450
0.0470
0.0440
30
0.0380
0.0422
0.0395
40
0.0370
0.0390
0.0392
50
0.0340
0.0370
0.0228
60
0.0330
0.0292
0.0197
70
0.0320
0.0289
0.0186
80
0.0290
0.0267
0.0175
90
0.0290
0.0250
0.0173
100
0.0280
0.0240
0.0160
110
0.0250
0.0200
0.0150
120
0.0240
0.0160
0.0149
130
0.0200
0.0156
0.0145
140
0.0200
0.0153
0.0140
150
0.0180
0.015
0.0140
160
0.0170
0.015
0.0140
170
0.0150
0.015
0.0140
180
0.0150
0.015
0.0140
190
0.0150
0.015
0.0140
200
0.0150
0.015
0.0140Figure 7
Elution behavior of polyaniline Zr(IV) tungstoiodophosphate ion exchanger.


## 4.8.4. Effect of Time on IEC

The effect of elution time on IEC of the hybrid exchanger is shown in Table9. The effect of equilibration time on exchange capacity of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger using LiCl, NaCl, and KCl eluents shows that constant capacity occurs after 3.5, 3.0, and 2.5 hours respectively, and is shown in Figure 8.Table 9
Effect of elution time on IEC of polyaniline  Zr(IV) tungstoiodophosphate ion exchanger using LiCl, NaCl, and KCl eluents.
Equilibrium time (Hours)
Ion-exchange capacity of ion exchanger (meq·dry g−1)
Li+ion
Na+ion
K+ ion
0
1.28
2.12
3.92
0.5
1.92
3.40
5.60
1.0
2.00
4.00
6.30
1.5
2.14
5.40
7.80
2.0
4.12
6.20
9.60
2.5
5.32
7.00
15.20
3.0
5.80
7.40
15.20
3.5
6.32
7.40
15.20
4.0
6.32
7.40
15.20
4.5
6.32
7.40
15.20
5.0
6.32
7.40
15.20Figure 8
Effect of elution time on IEC of polyaniline Zr(IV) tungstoiodophosphate ion exchanger using (a) LiCl (b) NaCl (c) KCl eluents.


## 4.8.5. pH Titration

The pH titration curves for polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger were obtained under equilibrium conditions with LiOH/LiCl, NaOH/NaCl, and KOH/KCl systems indicating bifunctional behaviour of the material as shown in Figure9.Figure 9
pH value of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger with various alkali metal hydroxides.At low pH, the weak acidic groups remain undissociated. The addition of LiOH, NaOH, and KOH neutralized the solution, and the weak acidic group dissociates; thus, the ion exchange starts toward completion. The pH titration curves showed a gradual rise in pH initially and a steep rise at the end because strong acidic groups were completely exchanged with Li+, Na+ and K+ ions at the end. The rate of H+-K+ exchange was faster than those of H+-Na+, and H+-Li+ exchanges.


## 4.8.6. Selectivity (Sorption) Studies

In order to find out the potentiality of polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger in the separation of metal ions, distribution studies for three metal ions were performed in four solvent systems. The results of distribution studies (Table10) show that Kd value varies with the nature and composition of contacting solvents. It was also observed from the sorption studies (Kd values) that the composite has a maximum selectivity towards Pb2+ than other metal ions like Cu2+ and Co2+.Table 10
Distribution coefficient values of some metal ions on polyaniline Zr(IV) tungstoiodophosphate in different solvent systems.
Metal ions
K
d values in different solvent systems
DMW
10% ethanol
10% acetone
1 M H2SO4
Pb2+
265
172
251
51
Cu2+
96
115
122
13
Co2+
59
86
37
90


## 4.8.7. Studies of Antimicrobial Activity

The antimicrobial activity studies of the PANI and polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger were carried out using the Kirby-Bauer antimicrobial susceptibility test procedure [40] against two bacteria, namely, E. coli and Proteus vulgaris (Figure 10). The test solutions of these two samples were prepared in NMP solvent. The antimicrobial activity study results are summarized in the Table 11.Table 11
Antimicrobial activity studies of polymer samples.
Organisms
Media
Zone of  inhibition in (mm)
Control
PANI
Polyaniline Zr(IV) tungstoiodophosphate ion exchanger
Escherichia coli
Muller
18
15
20
Proteus vulgaris
Histon Agar
20
20
16Zone formation against (a)E. coli and (b) Proteus vulgaris.
(a)
(b)From the table, polymer and the conducting polymeric-inorganic nanocomposite ion exchanger showed higher antimicrobial activity againstE. coli and Proteus vulgaris, and inhibition zones were formed due to their antimicrobial activity.


## 5. Conclusions

The characterization of polyaniline Zr(IV) tungstoiodophosphate ion exchanger is justified on the basis of FT-IR, UV-visible, XRD, SEM, and TGA. The principle characteristic peaks of quinoid-benzenoid N-moieties, C–N stretching, and C–H aromatic in-plane and out-plane bending vibrations of PANI are reported to occur at about 1600, 1500, 1350, 1130, and 820 cm−1, respectively. In the present study also all the peaks are observed in prepared polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger using potassium perdisulphate as the oxidant, but they are modified both in intensity and peak position when the ion exchanger is incorporated into the conducting polymeric matrix PANI. XRD pattern of this cation exchanger shows that the composite material is in a semicrystalline form. The SEM images and XRD studies show that the average crystallite size of the H+ form of composite material was found to be 78 nm. The thermal analysis points out the inference that prepared polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger is thermally stable. The three different absorption peaks are observed in the UV-visible spectra of the polymer samples due to the transition from π band to π* band, from polaron band to π* band, and from π band to polaran band. This indicates that polarons act as charge carriers in all the polymer samples. From the electrical conductivity studies, it is quite clear that organic-inorganic nanocomposite ion exchanger is having good electrical conductivity compared to those of its corresponding organic polymers. The conducting polymeric-inorganic nanocomposite ion exchanger, polyaniline Zr(IV) tungstoiodophosphate prepared by the sol-gel mixing, has good ion-exchange capacity compared to that of the individual ion exchanger like Zr(IV) tungstoiodophosphate, which has the ion-exchange capacity of 2.2 m.eq.dry/g. Polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger has good ion-exchange capacity towards different metal ions like Li+, Na+, and K+ to the extent of 4.2, 5.3, and 5.9 meq.dry g−1, respectively. The distribution coefficient values from sorption studies show that polyaniline Zr(IV) tungstoiodophosphate nanocomposite ion exchanger has a higher selectivity towards Pb2+ than towards Cu2+ and Co2+; that is, Pb2+ is highly adsorbed in all solvents while Cu2+ and Co2+ ions are poorly adsorbed. Antimicrobial activity study shows that the organic polymer and nanocomposite ion exchanger are effective against Escherichia coliandProteius vulgaris.The intrinsic multifunctional character of organic/inorganic hybrid materials makes them potentially useful in multiple fields. Illustrative examples of this versatility are their high added value applications as coating for corrosion production and abrasion resistance, artificial membranes for ultra- and nanofiltration adsorbents for toxic compounds, and so forth. Most of the organic/inorganic hybrid materials are nanocomposite materials in which the inorganic part and the organic entities interact at the molecular level in the nanoscopic domain. The most obvious advantage of organic and inorganic hybrids is that they have good ion-exchange properties, high stability, reproducibility, and selectivity for heavy toxic metal ions. In the present work, polyaniline Zr(IV) tungstoiodophosphate is a newly synthesised organic-inorganic nanocomposite ion exchanger, which possess all such characteristics and is highly selective for lead, a hazardous toxic metal in the environment. Thus, the material can be used in making Pb(II) ion selective membrane electrode.



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*Source: 356058-2013-10-07.xml*