# Ion Dynamics Study of Potato Starch + Sodium Salts Electrolyte System

Authors: Tuhina Tiwari; Neelam Srivastava; P. C. Srivastava
Journal: International Journal of Electrochemistry
 (2013)

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## Abstract

The effect of different anions, namely,SCN−, I−, and ClO4−, on the electrical properties of starch-based polymer electrolytes has been studied. Anion size and conductivity are having an inverse trend indicating systems to be predominantly anionic conductor. Impact of anion size and multiplet forming tendency is reflected in number of charge carriers and mobility, respectively. Ion dynamics study reveals the presence of different mechanisms in different frequency ranges. Interestingly, superlinear power law (SLPL) is found to be present at <5 MHz frequency, which is further confirmed by dielectric data.


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## Body

## 1. Introduction

Potentiality of polymer electrolytes was first recognized by Armand et al. [1]. Since then, extensive work has been carried out in the field resulting in further subdivision of field into different branches, such as gelled polymer electrolyte, polymer-salt complex electrolyte, and composite polymer electrolyte. Biopolymer-based polymer-salt complex electrolytes are relatively new class of material and serving as environment friendly alternates to their synthetic counter parts [2, 3]. Among the biopolymers-based polymer-salt complexes, starch-based materials are gaining much recognition. Many leading groups [4–8] are working in the field. A review of natural polysaccharides as electroactive polymers by Finkenstadt summarizes the basics and importance of starch-based electrolytes [4]. Conductivity up to 10−1.6 S/cm is reported by Ning et al. using ionic liquid as a plasticizer in starch-based polymer electrolytes [8].Most of the reports on the starch-based electrolytes deals only with the electrical properties of system. This motivated us to understand the ion dynamics in these systems. Earlier we have studied potato starch-based electrolyte systems having iodide anion for two different cations [9, 10] which exhibited good electrolytic nature. Now, we extended our study to comprehend the effect of different anion in starch-based polymer-salt complexes. ClO4-, I-, and SCN- anions are known for making polymer-salt complexes with synthetic polymers. Hence, in present paper, we are reporting starch-based electrolyte systems prepared by doping starch with sodium salt of these anions.Prepared system’s electrical behavior is analyzed using Impedance spectroscopy and by representing the impedance data in different formalism, namely, dielectric, modulus and conductivity. The use of conductivity formalism to investigate the dynamics of charge carrier is quite admired because of its simplicity. In 1977, Jonscher proposed “Universal dielectric response” to deal with dielectric properties of materials [11]. Later in 1978 he proposed conductivity power law σ=σ0+Aωn [12], which is followed by all kind of disordered materials and hence, termed as “Universal dynamic response” which has been further elaborated by Almond et al. in 1983 [13]. In original work of Jonscher, exponent “n” was restricted to be <1 (now known as sublinear power law or Jonscher Power law). With the progress of time it has been recognized that if temperature and frequency range is wider then “n” may also have values >1 (known as superlinear power law) [14–18]. Though superlinear power law is proposed to exist at very high frequency but in the present system this is found even in MHz frequency range. Similar behavior is noted by other workers as well [14]. In the present work, a detail investigation is carried out to separate sublinear power law and superlinear power law regions. Number of charge carrier and mobility are estimated from dielectric data, to understand the effect of anion size.


## 2. Experimental Details

### 2.1. Material Preparation

Potato starch (PS)(C6H10O5)n, NaI, NaSCN, NaClO4, Glutaraldehyde (GA) (C5H8O2), and Polyethylene glycol 300 (PEG), all from Loba Chemie, were used to prepare material with distilled water as solvent. Three series of samples (i.e., with three different salts) were prepared using solution cast technique at 30°C. For 1 gm of starch ~10% of PEG (0.17 gm or 5 drops), sodium salt (5 to 50% of PS), and 2 mL GA were taken together in distilled water. Mixtures were stirred at 30°C on magnetic stirrer for one hour and heated till it dry. Samples were in film form which was cut in to pieces for study.


### 2.2. Devices and Technique

AC conductivity is measured by computer controlled HIOKI HiTester LCR meter (3532-50) in the range 42 Hz to5×106 Hz. Ionic transference number of the material is estimated by dc polarization method using Keithley DMM 2100. Silver foils are used as electrode. Dielectric and Modulus data are estimated from the impedance spectra.


## 2.1. Material Preparation

Potato starch (PS)(C6H10O5)n, NaI, NaSCN, NaClO4, Glutaraldehyde (GA) (C5H8O2), and Polyethylene glycol 300 (PEG), all from Loba Chemie, were used to prepare material with distilled water as solvent. Three series of samples (i.e., with three different salts) were prepared using solution cast technique at 30°C. For 1 gm of starch ~10% of PEG (0.17 gm or 5 drops), sodium salt (5 to 50% of PS), and 2 mL GA were taken together in distilled water. Mixtures were stirred at 30°C on magnetic stirrer for one hour and heated till it dry. Samples were in film form which was cut in to pieces for study.


## 2.2. Devices and Technique

AC conductivity is measured by computer controlled HIOKI HiTester LCR meter (3532-50) in the range 42 Hz to5×106 Hz. Ionic transference number of the material is estimated by dc polarization method using Keithley DMM 2100. Silver foils are used as electrode. Dielectric and Modulus data are estimated from the impedance spectra.


## 3. Results and Discussion

### 3.1. Transference Number and Electrical Conductivity

The simplest method to establish electrochemical nature is the measurement of ionic transference number (tion). It represents the fractional contribution of ionic charge carrier to the total electrical conductivity. In the present case, this parameter is estimated by dc polarization method [19]. In the procedure, 0.2 V potential was applied across the Ag/electrolyte/Ag and current was monitored as a function of time. On the application of voltage, current decreased with time and after some time it became constant as the electrolyte was depleted of charge carrier. tion is estimated using following formula:
(1)tion=iinitial-ifinaliinitial,whereiinitial is the initial current flown and ifinal is the value of final saturated current. This tion gives the total ionic contribution to conductivity. For all the three systems tion has value ~0.99 which indicates the electrolytic nature of prepared materials. To separate cationic/anionic transference number, combined a.c./d.c. method [20] was used. The method is similar to that described above with the only difference that the blocking electrodes were replaced by nonblocking one. tcation can be estimated from the cole-cole plot and polarization curve. In the present case, anticipating the movement of both the ions (sodium/iodide) Na-Hg amalgam was used as a nonblocking electrode to separate the tNa+. The success was not achieved in present case since water absorbed in the starch matrix started reacting with the amalgam and the experiment failed. But as water is available in starch matrix, the effect of proton and hydroxyl ions on the conductivity of the system cannot be fully ruled out.Conductivity (σ) has been calculated using sample dimension “L” and electrode area “A” with the help of formula
(2)σ=1Z′LA,whereZ′ is intercept on real axis of Z′′ versus Z′ plots obtained in frequency range 42 Hz to 5 MHz.In polymer-salt composites, conductivity varies with addition of salt and passes through maxima and minima. Therefore, it indicates that in polymer-salt systems, dissociation of salt and the number of available charge carrier are not directly related to the amount of salt added. Instead, columbic interaction among them together with their interaction with the matrix plays an important role.Figure1 shows the conductivity (σ) versus wt% of salt curves for all the three systems. The variation for all the three systems were following the similar trends as reported for other polymer-salt complex systems. The NaSCN doped system exhibit maximum conductivity (1.12×10-4 S/cm) whereas NaClO4 system exhibited the lowest one (7.19×10-6 S/cm). It indicates that the conductivity is following a trend given as follows:
(3)σSCN->σI->σClO4-.Variation of conductivity and dielectric parameter with wt% of added salt (a) NaClO4 Salt, (b) NaI salt, and (c) NaSCN salt.
(a)
(b)
(c)Table1 shows anion size and corresponding highest conductivity values of different salt mixed systems. Conductivity is inversely following anion size indicating dominance of anions as charge carriers in the systems.Table 1
Values of conductivity and dielectric parameters for different salt (NaClO4, NaI, NaSCN) containing systems along with the salt anion size.
Anion
Size (pm)
σ
max (S/cm)
ε
′
ε
′
′
ClO
4
-
250
7.19
×
10
-
6
19.8
5.97
I
-
220
1.22
×
10
-
5
31.8
11.3
SCN
-
213
1.12
×
10
-
4
45.2
63.5Systems are further analyzed in terms of number of mobile charge carrier “N” and mobility “μ”. Conductivity can be represented as
(4)σ=Nqμ,whereN is number of mobile charge carrier, q is charge on carrier and μ is the mobility of the system. Mobility of any system can be given as
(5)μ=qL24MτepkT,whereq is charge on carrier, L is sample thickness, M is defined as the ratio of the sample thickness to twice the Debye length, τep is relaxation time in presence of polarization [21].M and τep are correlated with tanδ as per following equation:
(6)tanδ=ωτep1+ω2(τep2/M).This formula is best applicable [21] to the systems having conductivity <10−3 S/cm and τep<1, thus it can be used in present system. Values of M, τep can be found by fitting the tanδ versus ω curve for above equation. Fitting parameters are estimated using “Origin” software. Figure 2 shows tanδ versus ω curve for the three systems having 50% salt. It can be seen that the curve for NaI system has a broad nature. This can be interpreted as distribution in iodide ion’s state, that is, indicating the presence of different multiplet of iodide ions, resulting in distributed relaxation time. Iodide ion has a well-known multiplet forming tendency especially in starch; hence, this is an expected behavior.Figure 2
tan
δ versus ω curve for the three systems (i.e., NaClO4, NaI, and NaSCN containing systems) having 50% salt.Table2 summarizes the values of mobility “μ” and number of charge carriers “N” for all the three systems having 50% salt. It indicates that NaSCN containing system possesses greater μ and N in comparison to other systems that means the anion size not only controls the mobility of the system but at the same time it affects the salt dissociation as well. However, the mobility trend between NaI and NaClO4 is reversed. Though the single ClO4- ion has greater anion size than the other two ions (SCN- and I-) hence should have lowest mobility but possibly the greater size of I- multiplet are responsible for reduced mobility in NaI system.Table 2
Values ofτep, M, µ, and N for different salt (NaClO4, NaI, and NaSCN) containing systems.
Salt
τ
ep (sec)
M
μ (cm2V−1s−1)
N (cm−3)
NaSCN
2.43
×
10
-
4
3.81
×
10
+
3
4.76
×
10
-
7
1.47
×
10
+
21
NaI
5.17
×
10
-
3
9.65
×
10
+
2
7.95
×
10
-
8
4.89
×
10
+
20
NaClO4
2.58
×
10
-
3
4.16
×
10
+
2
2.12
×
10
-
7
6.88
×
10
+
19


### 3.2. Frequency Dependence of Conductivity

Impedance data presented in Conductivity formalism (σ=σ0+Aωn) is a well-accepted technique to understand the ion dynamics in disordered systems. The value of exponent “n” represents different types of ion motion dominating in the system [22]. For a very long period, Universal Power Law [12, 13, 23] has been followed as thumb rule according to which exponent “n” can have values <1 and preferably ≃0.5–0.65 for conducting systems. This law was followed by almost all disordered materials, such as glasses, conducting polymers, and composites [22]. Recently, many experimental data reported in the literature have n=1 or >1 and are known as Nearly Constant Loss (NCL) and Super Linear Power Law (SLPL), respectively. Though theories predicted these phenomena to occur in GHz range but experimentally exponent “n” were reported to have ≥1 even in MHz range [14], theories for explaining such behavior are still in their infancy [14–18, 22]. Exponent depends upon frequency and it designates the ion dynamics prevailing in that frequency range. DC conductivity and ion hopping occur at comparatively larger time scale (low frequency) whereas NCL/SLPL is a lower time scale (higher frequency) phenomena [24], and are represented by n<1 and n≥1, respectively. All these are time dependence and hence the ion movements are statistical in nature, with particular phenomenon dominating in specific frequency region and resulting in corresponding value of “n” in that frequency region.Theoretically, frequency dependence of conductivity will follow a trend [15, 22] given below from lower to higher frequency (up to GHz frequency):
(7)polarization⟶dcconductivity(n~0)⟶ionhopping(n~0.5)⟶NCL(n=1)⟶SLPL(n>1).The literature shows that moving beyond the SLPL region, conductivity achieves a plateau followed by dispersion in frequency > GHz [22], which is not discussed here as it is beyond the scope of present work. When studies have been carried out in wider frequency and temperature range, universality of σ=σ0+Aωn extend to nearly constant loss type of behavior [14, 15, 25]. But SLPL is reported only in few systems. Different theoretical models are being devised to explain NCL/SLPL which are applicable to all material [14–18] but with limited success. In a recent communication, Tiwari and his co-worker [26], referring ADWP model, reported that the NCL/SLPL phenomena can exist even at low frequency decided by glass transition temperature and working temperature together. In the present system, Tg is found to be ~80°C [27]; hence, according to  Tiwari and Shahi [26], at low temperature the power law exponent (n=1+T/Tg) comes out to be ~1.8 which did not exactly match with experimental values but confirmed the SLPL type phenomenon in present system. A detail discussion of conductivity power law in present system is given below.Figure3 shows logσ versus logω curve for present systems. As discussed above, the value of exponent “n” will have different value, varying from 0 to 2, in different frequency region. As indicated by arrow in Figure 3 the polarization is present up to quite high frequency.Conductivity variations with frequency for different system (a) NaClO4 Salt, (b) NaI salt, and (c) NaSCN salt.
(a)
(b)
(c)Figure4(a) shows the fitting curve for σ=σ0+Aωn along with the experimental points in complete frequency range, excluding the polarization region. The curve does not exactly fit according to the equation, indicating the existence of different ion dynamics. Curve starts deviating at certain frequency (as marked by arrow in present case), indicating existence of different fitting parameters above and below this frequency. When the fitting was carried out separately in two different frequency ranges, it was quite good as shown in Figures 4(b) and 4(c). This resulted in two sets of fitting parameter in two different regions.(a) A typical fitting curve forσ=σ0+Aωn along with the experimental points in complete frequency range. (b) Fitting for the same curve in the higher frequency range above the arrow marked in (a). (c) Fitting for the same curve in the lower frequency range below the arrow marked in (a).
(a)
(b)
(c)Table3 shows the values of exponent “n” in different frequency ranges for the three salt systems. We are getting two different regions: higher frequency region with n>1 indicating SLPL phenomenon; mid frequency region with n≃0.5 representing ion hopping. There are many theoretical attempts [14–18] to provide an explanation to the behavior but none is completely successful.Table 3
Values of exponent “n” in different frequencies (Ion hopping and SLPL) range for (a) NaClO4, (b) NaI, and (c) NaSCN containing systems.
(a)
NaClO4
wt% of Salt
Value of exponent “n”
Higher frequency range
Lower frequency range
5
1.77
0.53
10
1.61
0.49
15
1.53
0.53
20
1.51
0.51
25
1.51
0.52
30
1.39
0.52
35
1.47
0.47
40
1.37
0.54
45
1.46
0.36
50
1.39
0.51
(b)
NaI
wt% of Salt
Value of exponent “n”
Higher frequency range
Lower frequency range
5
1.76
0.60
10
1.68
0.68
15
1.50
0.65
20
1.47
0.58
25
1.31
0.62
30
1.40
0.62
35
1.35
0.65
40
1.50
0.41
45
1.36
0.41
50
1.38
0.57
(c)
NaSCN
wt% of Salt
Value of exponent “n”
Higher frequency range
Lower frequency range
5
1.46
0.52
10
1.44
0.63
15
1.41
0.56
20
1.46
0.54
25
1.36
0.46
30
1.35
0.30
35
1.47
0.36
40
1.40
0.48
45
1.68
0.54
50
1.48
0.25


### 3.3. Frequency Dependence of Dielectric and Modulus Values

Dielectric parameters estimated at frequency 5 MHz for the three different salts are listed in Table1. The anion size effect could also be seen in these data. The values are maximum for SCN- and minimum for ClO4-. The variation of dielectric parameters follows the trend of conductivity variation with salt concentration as shown in Figure 1.Superlinear power law is characterized by presence of a shallow to deep minima in dielectric loss spectra depending upon the strength of SLPL behavior. Hence, for a crosscheck of the SLPL region, discussed in Section3.2, dielectric loss variations with frequency have been studied. Figures 5(a) and 5(b) represent the variation of ε′, ε′′ with frequency for one salt (NaI). These curves represent the typical polymer electrolyte type of nature. Curves in Figure 5(c) indicate towards presence of a shallow minimum at high frequency when plotted in extended view for sodium iodide. Similar curves are, also, found for other two systems. This confirms our conclusion regarding the ion dynamics discussed in Section 3.2.Variation of (a) real part and (b) imaginary part of dielectric parameter with frequency. (c) Extended view of (b) at higher frequency for NaI.
(a)
(b)
(c)The impedance data is further analyzed in terms of electrical modulus as depicted in Figures6(a) and 6(b). Values of Electrical modulus have been calculated using following formulas:
(8)M′=ε′(ε′′2+ε′2),M′′=ε′′(ε′′2+ε′2).Variation of (a) real part (b) imaginary part of electric modulus variation with frequency for NaI.
(a)
(b)Relaxation peaks observed inM′′ versus logω curves are summarized in Table 4. Peaks shift with salt concentration in the similar fashion as conductivity variation.Table 4
Values of relaxation peak frequency in imaginary part of Modulus versus frequency curve.
wt% of Salt
Peak frequency (Hz) inM′′
NaSCN
NaI
NaClO4
5
1945000
1945000
2462000
10
1213000
756200
1536000
15
1536000
2462000
2462000
20
1213000
1078000
1945000
25
1213000
2462000
1213000
30
2771000
1945000
2462000
35
1078000
2462000
2462000
40
1365000
3118000
1365000
45
419100
2462000
2462000
50
Out of range
2462000
1078000


## 3.1. Transference Number and Electrical Conductivity

The simplest method to establish electrochemical nature is the measurement of ionic transference number (tion). It represents the fractional contribution of ionic charge carrier to the total electrical conductivity. In the present case, this parameter is estimated by dc polarization method [19]. In the procedure, 0.2 V potential was applied across the Ag/electrolyte/Ag and current was monitored as a function of time. On the application of voltage, current decreased with time and after some time it became constant as the electrolyte was depleted of charge carrier. tion is estimated using following formula:
(1)tion=iinitial-ifinaliinitial,whereiinitial is the initial current flown and ifinal is the value of final saturated current. This tion gives the total ionic contribution to conductivity. For all the three systems tion has value ~0.99 which indicates the electrolytic nature of prepared materials. To separate cationic/anionic transference number, combined a.c./d.c. method [20] was used. The method is similar to that described above with the only difference that the blocking electrodes were replaced by nonblocking one. tcation can be estimated from the cole-cole plot and polarization curve. In the present case, anticipating the movement of both the ions (sodium/iodide) Na-Hg amalgam was used as a nonblocking electrode to separate the tNa+. The success was not achieved in present case since water absorbed in the starch matrix started reacting with the amalgam and the experiment failed. But as water is available in starch matrix, the effect of proton and hydroxyl ions on the conductivity of the system cannot be fully ruled out.Conductivity (σ) has been calculated using sample dimension “L” and electrode area “A” with the help of formula
(2)σ=1Z′LA,whereZ′ is intercept on real axis of Z′′ versus Z′ plots obtained in frequency range 42 Hz to 5 MHz.In polymer-salt composites, conductivity varies with addition of salt and passes through maxima and minima. Therefore, it indicates that in polymer-salt systems, dissociation of salt and the number of available charge carrier are not directly related to the amount of salt added. Instead, columbic interaction among them together with their interaction with the matrix plays an important role.Figure1 shows the conductivity (σ) versus wt% of salt curves for all the three systems. The variation for all the three systems were following the similar trends as reported for other polymer-salt complex systems. The NaSCN doped system exhibit maximum conductivity (1.12×10-4 S/cm) whereas NaClO4 system exhibited the lowest one (7.19×10-6 S/cm). It indicates that the conductivity is following a trend given as follows:
(3)σSCN->σI->σClO4-.Variation of conductivity and dielectric parameter with wt% of added salt (a) NaClO4 Salt, (b) NaI salt, and (c) NaSCN salt.
(a)
(b)
(c)Table1 shows anion size and corresponding highest conductivity values of different salt mixed systems. Conductivity is inversely following anion size indicating dominance of anions as charge carriers in the systems.Table 1
Values of conductivity and dielectric parameters for different salt (NaClO4, NaI, NaSCN) containing systems along with the salt anion size.
Anion
Size (pm)
σ
max (S/cm)
ε
′
ε
′
′
ClO
4
-
250
7.19
×
10
-
6
19.8
5.97
I
-
220
1.22
×
10
-
5
31.8
11.3
SCN
-
213
1.12
×
10
-
4
45.2
63.5Systems are further analyzed in terms of number of mobile charge carrier “N” and mobility “μ”. Conductivity can be represented as
(4)σ=Nqμ,whereN is number of mobile charge carrier, q is charge on carrier and μ is the mobility of the system. Mobility of any system can be given as
(5)μ=qL24MτepkT,whereq is charge on carrier, L is sample thickness, M is defined as the ratio of the sample thickness to twice the Debye length, τep is relaxation time in presence of polarization [21].M and τep are correlated with tanδ as per following equation:
(6)tanδ=ωτep1+ω2(τep2/M).This formula is best applicable [21] to the systems having conductivity <10−3 S/cm and τep<1, thus it can be used in present system. Values of M, τep can be found by fitting the tanδ versus ω curve for above equation. Fitting parameters are estimated using “Origin” software. Figure 2 shows tanδ versus ω curve for the three systems having 50% salt. It can be seen that the curve for NaI system has a broad nature. This can be interpreted as distribution in iodide ion’s state, that is, indicating the presence of different multiplet of iodide ions, resulting in distributed relaxation time. Iodide ion has a well-known multiplet forming tendency especially in starch; hence, this is an expected behavior.Figure 2
tan
δ versus ω curve for the three systems (i.e., NaClO4, NaI, and NaSCN containing systems) having 50% salt.Table2 summarizes the values of mobility “μ” and number of charge carriers “N” for all the three systems having 50% salt. It indicates that NaSCN containing system possesses greater μ and N in comparison to other systems that means the anion size not only controls the mobility of the system but at the same time it affects the salt dissociation as well. However, the mobility trend between NaI and NaClO4 is reversed. Though the single ClO4- ion has greater anion size than the other two ions (SCN- and I-) hence should have lowest mobility but possibly the greater size of I- multiplet are responsible for reduced mobility in NaI system.Table 2
Values ofτep, M, µ, and N for different salt (NaClO4, NaI, and NaSCN) containing systems.
Salt
τ
ep (sec)
M
μ (cm2V−1s−1)
N (cm−3)
NaSCN
2.43
×
10
-
4
3.81
×
10
+
3
4.76
×
10
-
7
1.47
×
10
+
21
NaI
5.17
×
10
-
3
9.65
×
10
+
2
7.95
×
10
-
8
4.89
×
10
+
20
NaClO4
2.58
×
10
-
3
4.16
×
10
+
2
2.12
×
10
-
7
6.88
×
10
+
19


## 3.2. Frequency Dependence of Conductivity

Impedance data presented in Conductivity formalism (σ=σ0+Aωn) is a well-accepted technique to understand the ion dynamics in disordered systems. The value of exponent “n” represents different types of ion motion dominating in the system [22]. For a very long period, Universal Power Law [12, 13, 23] has been followed as thumb rule according to which exponent “n” can have values <1 and preferably ≃0.5–0.65 for conducting systems. This law was followed by almost all disordered materials, such as glasses, conducting polymers, and composites [22]. Recently, many experimental data reported in the literature have n=1 or >1 and are known as Nearly Constant Loss (NCL) and Super Linear Power Law (SLPL), respectively. Though theories predicted these phenomena to occur in GHz range but experimentally exponent “n” were reported to have ≥1 even in MHz range [14], theories for explaining such behavior are still in their infancy [14–18, 22]. Exponent depends upon frequency and it designates the ion dynamics prevailing in that frequency range. DC conductivity and ion hopping occur at comparatively larger time scale (low frequency) whereas NCL/SLPL is a lower time scale (higher frequency) phenomena [24], and are represented by n<1 and n≥1, respectively. All these are time dependence and hence the ion movements are statistical in nature, with particular phenomenon dominating in specific frequency region and resulting in corresponding value of “n” in that frequency region.Theoretically, frequency dependence of conductivity will follow a trend [15, 22] given below from lower to higher frequency (up to GHz frequency):
(7)polarization⟶dcconductivity(n~0)⟶ionhopping(n~0.5)⟶NCL(n=1)⟶SLPL(n>1).The literature shows that moving beyond the SLPL region, conductivity achieves a plateau followed by dispersion in frequency > GHz [22], which is not discussed here as it is beyond the scope of present work. When studies have been carried out in wider frequency and temperature range, universality of σ=σ0+Aωn extend to nearly constant loss type of behavior [14, 15, 25]. But SLPL is reported only in few systems. Different theoretical models are being devised to explain NCL/SLPL which are applicable to all material [14–18] but with limited success. In a recent communication, Tiwari and his co-worker [26], referring ADWP model, reported that the NCL/SLPL phenomena can exist even at low frequency decided by glass transition temperature and working temperature together. In the present system, Tg is found to be ~80°C [27]; hence, according to  Tiwari and Shahi [26], at low temperature the power law exponent (n=1+T/Tg) comes out to be ~1.8 which did not exactly match with experimental values but confirmed the SLPL type phenomenon in present system. A detail discussion of conductivity power law in present system is given below.Figure3 shows logσ versus logω curve for present systems. As discussed above, the value of exponent “n” will have different value, varying from 0 to 2, in different frequency region. As indicated by arrow in Figure 3 the polarization is present up to quite high frequency.Conductivity variations with frequency for different system (a) NaClO4 Salt, (b) NaI salt, and (c) NaSCN salt.
(a)
(b)
(c)Figure4(a) shows the fitting curve for σ=σ0+Aωn along with the experimental points in complete frequency range, excluding the polarization region. The curve does not exactly fit according to the equation, indicating the existence of different ion dynamics. Curve starts deviating at certain frequency (as marked by arrow in present case), indicating existence of different fitting parameters above and below this frequency. When the fitting was carried out separately in two different frequency ranges, it was quite good as shown in Figures 4(b) and 4(c). This resulted in two sets of fitting parameter in two different regions.(a) A typical fitting curve forσ=σ0+Aωn along with the experimental points in complete frequency range. (b) Fitting for the same curve in the higher frequency range above the arrow marked in (a). (c) Fitting for the same curve in the lower frequency range below the arrow marked in (a).
(a)
(b)
(c)Table3 shows the values of exponent “n” in different frequency ranges for the three salt systems. We are getting two different regions: higher frequency region with n>1 indicating SLPL phenomenon; mid frequency region with n≃0.5 representing ion hopping. There are many theoretical attempts [14–18] to provide an explanation to the behavior but none is completely successful.Table 3
Values of exponent “n” in different frequencies (Ion hopping and SLPL) range for (a) NaClO4, (b) NaI, and (c) NaSCN containing systems.
(a)
NaClO4
wt% of Salt
Value of exponent “n”
Higher frequency range
Lower frequency range
5
1.77
0.53
10
1.61
0.49
15
1.53
0.53
20
1.51
0.51
25
1.51
0.52
30
1.39
0.52
35
1.47
0.47
40
1.37
0.54
45
1.46
0.36
50
1.39
0.51
(b)
NaI
wt% of Salt
Value of exponent “n”
Higher frequency range
Lower frequency range
5
1.76
0.60
10
1.68
0.68
15
1.50
0.65
20
1.47
0.58
25
1.31
0.62
30
1.40
0.62
35
1.35
0.65
40
1.50
0.41
45
1.36
0.41
50
1.38
0.57
(c)
NaSCN
wt% of Salt
Value of exponent “n”
Higher frequency range
Lower frequency range
5
1.46
0.52
10
1.44
0.63
15
1.41
0.56
20
1.46
0.54
25
1.36
0.46
30
1.35
0.30
35
1.47
0.36
40
1.40
0.48
45
1.68
0.54
50
1.48
0.25


## 3.3. Frequency Dependence of Dielectric and Modulus Values

Dielectric parameters estimated at frequency 5 MHz for the three different salts are listed in Table1. The anion size effect could also be seen in these data. The values are maximum for SCN- and minimum for ClO4-. The variation of dielectric parameters follows the trend of conductivity variation with salt concentration as shown in Figure 1.Superlinear power law is characterized by presence of a shallow to deep minima in dielectric loss spectra depending upon the strength of SLPL behavior. Hence, for a crosscheck of the SLPL region, discussed in Section3.2, dielectric loss variations with frequency have been studied. Figures 5(a) and 5(b) represent the variation of ε′, ε′′ with frequency for one salt (NaI). These curves represent the typical polymer electrolyte type of nature. Curves in Figure 5(c) indicate towards presence of a shallow minimum at high frequency when plotted in extended view for sodium iodide. Similar curves are, also, found for other two systems. This confirms our conclusion regarding the ion dynamics discussed in Section 3.2.Variation of (a) real part and (b) imaginary part of dielectric parameter with frequency. (c) Extended view of (b) at higher frequency for NaI.
(a)
(b)
(c)The impedance data is further analyzed in terms of electrical modulus as depicted in Figures6(a) and 6(b). Values of Electrical modulus have been calculated using following formulas:
(8)M′=ε′(ε′′2+ε′2),M′′=ε′′(ε′′2+ε′2).Variation of (a) real part (b) imaginary part of electric modulus variation with frequency for NaI.
(a)
(b)Relaxation peaks observed inM′′ versus logω curves are summarized in Table 4. Peaks shift with salt concentration in the similar fashion as conductivity variation.Table 4
Values of relaxation peak frequency in imaginary part of Modulus versus frequency curve.
wt% of Salt
Peak frequency (Hz) inM′′
NaSCN
NaI
NaClO4
5
1945000
1945000
2462000
10
1213000
756200
1536000
15
1536000
2462000
2462000
20
1213000
1078000
1945000
25
1213000
2462000
1213000
30
2771000
1945000
2462000
35
1078000
2462000
2462000
40
1365000
3118000
1365000
45
419100
2462000
2462000
50
Out of range
2462000
1078000


## 4. Conclusion

Potato starch-based electrolyte systems doped with sodium salts of three different anion, namely,ClO4-, I-, and SCN-, have been successfully prepared. Anion size and conductivity follow an inverse trend indicating systems to be predominantly anionic conductor. Anion size has an inverse effect on number of charge carriers. All of the prepared materials have tion>0.99 confirming their electrolytic nature. Multiplet formation tendency of iodide ion affected the mobility trend. SLPL is observed in studied frequency range at room temperature. Anion size has affected the range of its dominance, which has been further confirmed by dielectric loss parameter variation with frequency.



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*Source: 670914-2013-12-11.xml*