# Tin(II) Selective PVC Membrane Electrode Based on Salicylaldehyde Thiosemicarbazone as an Ionophore

Authors: Sulekh Chandra; Kusum Sharma; Adarsh Kumar
Journal: Journal of Chemistry
 (2013)

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## Abstract

A polymeric membrane-based tin selective electrode was developed by using salicylaldehyde thiosemicarbazone (STSC). The best performance was recorded with a membrane composition of PVC : TBP : ionophore : NaTPB as 28 : 59 : 8 : 5 (w/w%). The Nernstian slope calculated from the calibration curve for Sn2+ sensor was 28.8±0.4 mV/decade. The detection limit of the sensor was 2.10×10−8 M, in the linear concentration range of 1.0×10−2−1.1×10−7 M. It was relatively fast response time (<8 s for concentration ≥1.0×10−4 and <12 s for concentration of ≥1.0×10−6 M) and can be used for 9 months without any considerable divergence in potentials. The proposed sensor exhibit relatively good selectivity and high sensitivity for tin(II) as other mono-, di-, and trivalent cations and can be used in a pH range of 2.0–8.5. The analytical usefulness of the proposed electrode has been evaluated by its application in the determination of stannous in artificially made samples.


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## Body

## 1. Introduction

Tin is a natural element in the earth’s crust. Tin metal is used to line cans for food, beverages, and aerosols. It can combine with chemicals like chlorine, sulfur, or oxygen to form inorganic tin compounds. These compounds are used in toothpaste, perfumes, soaps, food additives, and dyes. Tin can also combine with carbon to form organotin compounds which are used to make plastics, food packages, plastic pipes, pesticides, paints, and pest repellents. Inorganic tin compounds are used as pigments in the ceramic and textile industry. In addition, stannous chloride, SnCl2, is widely used in daily human life to conserve soft drinks, in food manufacturing, processing, and packaging, and in biocidal preparations. The available methods for determination of low concentrations of tin ion in solution include spectrophotometry [1, 2], atomic absorption spectrometry [3, 4], atomic emission spectrometry [5, 6], electrochemical methods [7, 8], and spectrofluorimetric methods [9]. These methods are either time consuming, involving multiple sample manipulation, or too expensive for the most analytical laboratories. The potentiometric membrane sensors have shown to be very effective tools for the analysis of a wide variety of metal ions [10, 11]. They are very simple, fast, inexpensive, and capable of providing reliable responses in a broad concentration range.In the present study salicylaldehyde thiosemicarbazone was incorporated as the ionophore. It shows better potentiometric response as compared to the previously reported tin ion selective electrodes [12, 13] based on different ionophores.


## 2. Experimental

### 2.1. Reagents and Apparatus

Reagent-grade salicylaldehyde and thiosemicarbazide were obtained from Sigma-Aldrich (Delhi) used as purchased. DBP (dibutyl phthalate), DOP (dioctyl phthalate),o-NPOE (o-nitrophenyl octyl ether), and TBP (Tri-n-butyl phosphate) were purchased from Merck (Delhi). High-molecular-weight PVC powder, THF, and cation excluder NaTPB (sodium tetraphenyl borate) and metal salts were purchased from Fluka and Sigma-Aldrich. All the reagents were of highest purity grade and used without further purification. Standard solutions were freshly prepared in deionized water.


### 2.2. Physical Measurement

The C, H, and N were analyzed on a carlo-Erba 1106 elemental analysis. Electron impact mass spectra were recorded on JEOL, JMS, DX-303 mass spectrophotometer;1H NMR spectra were recorded on a Hitachi FT-NMR, Model R-600 spectrophotometer using CDCl3 as solvent. IR spectra (KBr) were recorded on a Bruker FT-IR spectrophotometer (Delhi).


### 2.3. Synthesis of Ionophore

The hot ethanolic solutions (20 mL) of salicylaldehyde (1.31 mL 0.01 mmol), thiosemicarbazide (1.14 g 0.01 mmol) with few drops of acetic acid were mixed with constant stirring. This mixture was refluxed at 80 ± 5°C. On cooling a yellowish-coloured compound has separated out. It was filtered, washed several times with cold EtOH and dried in vacuum over P4O10 (see Figure 1).Figure 1
Syntheses of ionophore.


### 2.4. Salicylaldehyde Thiosemicarbazone

Yield (75.0%), M.P.: 184°C. Anal. calc. for (%) = C8H9N3OS: C, 49.21; H, 4.65; N, 21.52; O, 8.19. Found: (%): C, 49.18; H, 4.64; N, 21.54; O, 8.11. Mass. (m/z): 195.05 (M+) amu. FT-IR (KBr): ν(NH2) 3173 (b), ν(NH) 2987 (b), ν(C=N) 1538, ν(C=S) 829.


## 2.1. Reagents and Apparatus

Reagent-grade salicylaldehyde and thiosemicarbazide were obtained from Sigma-Aldrich (Delhi) used as purchased. DBP (dibutyl phthalate), DOP (dioctyl phthalate),o-NPOE (o-nitrophenyl octyl ether), and TBP (Tri-n-butyl phosphate) were purchased from Merck (Delhi). High-molecular-weight PVC powder, THF, and cation excluder NaTPB (sodium tetraphenyl borate) and metal salts were purchased from Fluka and Sigma-Aldrich. All the reagents were of highest purity grade and used without further purification. Standard solutions were freshly prepared in deionized water.


## 2.2. Physical Measurement

The C, H, and N were analyzed on a carlo-Erba 1106 elemental analysis. Electron impact mass spectra were recorded on JEOL, JMS, DX-303 mass spectrophotometer;1H NMR spectra were recorded on a Hitachi FT-NMR, Model R-600 spectrophotometer using CDCl3 as solvent. IR spectra (KBr) were recorded on a Bruker FT-IR spectrophotometer (Delhi).


## 2.3. Synthesis of Ionophore

The hot ethanolic solutions (20 mL) of salicylaldehyde (1.31 mL 0.01 mmol), thiosemicarbazide (1.14 g 0.01 mmol) with few drops of acetic acid were mixed with constant stirring. This mixture was refluxed at 80 ± 5°C. On cooling a yellowish-coloured compound has separated out. It was filtered, washed several times with cold EtOH and dried in vacuum over P4O10 (see Figure 1).Figure 1
Syntheses of ionophore.


## 2.4. Salicylaldehyde Thiosemicarbazone

Yield (75.0%), M.P.: 184°C. Anal. calc. for (%) = C8H9N3OS: C, 49.21; H, 4.65; N, 21.52; O, 8.19. Found: (%): C, 49.18; H, 4.64; N, 21.54; O, 8.11. Mass. (m/z): 195.05 (M+) amu. FT-IR (KBr): ν(NH2) 3173 (b), ν(NH) 2987 (b), ν(C=N) 1538, ν(C=S) 829.


## 3. Potential Measurements

All the membrane electrode potential measurements were performed at constant temperature (25 ± 0.05°C) using digital pH meter and potentiometer (ELICO L1-10, India) in conjugation with saturated calomel electrodes as reference electrodes. The representation of electrochemical cell for the EMF measurements is shown in Table1.Table 1
External reference
Aqueous sample
Ion-selective membrane
Internal filling solution
Internal reference
electrode (SCE)
1.0 × 10−2 M Sn(NO3)2
solution (SCE)


### 3.1. Electrode Preparation

The general procedure was used for the preparation of the PVC membrane. For the preparation of membrane contents’ the fixed mixture of PVC : plasticizer : ionophore : excluder in 28 : 59 : 8.0 : 5.0 (w/w%) was taken as fixed. The mixture was thoroughly dissolved in THF (5 mL). The resulting mixture was poured into a glass dish. The solvent evaporated slowly until a sticky and oily mixture was obtained. A 5 mm diameter Pyrex tube was dipped into this mixture for few seconds and then removed. To obtain a 0.3 mm thick nontransparent membrane, fix one end of the Pyrex tube. It was dried for 5 Hrs. Pyrex tube was then filled with1.0×10-2 M Sn(NO3)2 as an internal filling solution. The electrode was kept as it is and conditioned for 24 hrs by soaking it in Sn(NO3)2 solution. The blank membrane having only PVC as membrane ingredients was also prepared and studied, while membrane having PVC with plasticizer generates small potential with slope of ~8.9 mV/decade.


## 3.1. Electrode Preparation

The general procedure was used for the preparation of the PVC membrane. For the preparation of membrane contents’ the fixed mixture of PVC : plasticizer : ionophore : excluder in 28 : 59 : 8.0 : 5.0 (w/w%) was taken as fixed. The mixture was thoroughly dissolved in THF (5 mL). The resulting mixture was poured into a glass dish. The solvent evaporated slowly until a sticky and oily mixture was obtained. A 5 mm diameter Pyrex tube was dipped into this mixture for few seconds and then removed. To obtain a 0.3 mm thick nontransparent membrane, fix one end of the Pyrex tube. It was dried for 5 Hrs. Pyrex tube was then filled with1.0×10-2 M Sn(NO3)2 as an internal filling solution. The electrode was kept as it is and conditioned for 24 hrs by soaking it in Sn(NO3)2 solution. The blank membrane having only PVC as membrane ingredients was also prepared and studied, while membrane having PVC with plasticizer generates small potential with slope of ~8.9 mV/decade.


## 4. Results and Discussion

### 4.1. Effect of Membrane Composition and Response Characteristics

The response of different metal ions and rare earth ions as plotted as the negative log of concentration and the potential values obtained for different metal ions. Best response and slope were seen for the Sn2+ ion as compared to the other cations as shown Figure 2. The plot between the concentration and EMF in Figure 2 indicates that the best response was obtained for the Sn2+, whereas transition metal ion gave a poor response. The calibration curve slope was found to be 28.8 ± 0.4 mV/decade in the linear range of 1×10-2–1×10-7 M Sn2+ concentration with the detection limit of 2.10×10-8 M. Further result of changes in the membrane composition on the electrode response was studied. It is well known [14, 15] that sensitivity and selectivity obtained for a given ionophore is significantly affected by the membrane composition of an ion sensor membrane. The different membrane ingredients, such as amount of ionophore and nature of the plasticizer and additives, influence the potentiometric response behaviour of the sensor [16, 17]. Best optimized studies membrane for Sn2+ selective electrode are reported in Table 2 sensor 2. The results given in the Table 2 show that the electrode worked well in plasticizer/PVC ratio of nearly 2, which ensures enough mobility of the membrane constituents. The best sensitivity and selectivity was recorded for TBP as plasticizer. Further the amount of ionophore also affected the Nernstian slope value. It has been observed (Table 2) that on increasing the concentration of the ionophore more than 2% (w/w), the slope deteriorated and a narrow linear concentration range was achieved. Hence, a very small amount of ionophore is required for the study. The presence of lipophilic anion excluder in cation sensor based on neutral carrier not only reduces the ohmic resistance but also enhances the response behaviour and selectivity [14]. It also assists in the extraction capability of the carrier in the membrane electrodes study [18, 19]. According to the results in Table 2, most optimum plasticizer used was TBP and the ionic additive NaTPB, and the optimum ratio for further studies was PVC : TBP : ionophore : NaTPB as 28 : 59 : 8 : 5 (w/w%).Table 2
Composition of PVC membrane of (STSC) and performance characteristics of Sn2+ selective sensors based on them.
S. no.
PVC
Plasticizer
Ionophore
Excluder NaTPB
Slope (mv/decade)
Linear range
1
28
67 (TBP)
0
5
8.9
1 × 10−3 to 1 × 10−6
2
28
58 (TBP)
8
5
29.2
1 × 10−2 to 1 × 10−8
3
28
57 (TBP)
5
5
35.7
1 × 10−3 to 1 × 10−7
4
28
59 (TBP)
7
5
22.8
1 × 10−2 to 1 × 10−5
6
28
57 (DOP)
5
5
18.3
1 × 10−3 to 1 × 10−5
7
28
58 (DOP)
4
5
33.4
1 × 10−2 to 1 × 10−4
8
28
59 (DOP)
3
5
25.7
1 × 10−2 to 1 × 10−5Figure 2
Potential response of various ion-selective electrodes based on STSC.


### 4.2. pH and Nonaqueous Effect

The pH dependence of the electrode potential was tested over the range 0.5–14.0 for Sn2+ in concentration 1.0×10-3 as shown in Figure 3. The pH of the solutions was adjusted by the addition of dilute hydrochloric acid or sodium hydroxide. It is clear from Figure 3 that the useful pH range is 2.0–8.5, as the potentials remain constant in this range. The sharp change in potentials at higher pH values may be due to the hydrolysis of Sn2+, while at lower pH values H+ ions start contributing to the charge transport process of the membrane, thereby, causing interference.Figure 3
The effect of pH of test solution on the response of the Sn2+ ion-selective electrode.


### 4.3. Response and Lifetime

Response time is critically reviewed when it comes to analytical application of the sensor [20]. The static response time of the membrane sensor thus obtained was <8 s, for concentration ≥1.0×10-4 and <12 s for concentration of ≥10−6 (Figure 4). It should be noted that the equilibrium potential remains constant for more than 8 min.Figure 4
The effect of the time on potentiometric response of Sn2+ electrode.The lifetime of the membrane sensor was about 9 months, during which it could be used without any measurable divergence. The time of contact and concentration of the equilibrium solution was also optimized so that the stable sensor generated and reproducible potentials at relatively short response time obtained. It was found that an equilibrating solution of1.0×10-2 M and contact time of 24 Hrs was appropriate for smooth functioning of the electrode. Membranes were stored in 1.0×10-2 M Sn(NO3)2 solution when not in used.


### 4.4. Potentiometric Selectivity

The selectivity is the most important characteristic, as it determines the extent of utility of a sensor in real sample measurement. The selectivity coefficient values were determined by fixed interference method (FIM) [20, 21]. The selectivity coefficient values KA,Bpot indicate that the electrode is moderately selective to Sn2+ over a number of other cation (Table 3). The potential of a cell comprising an ion-selective electrode [22] and a reference electrode is measured with solutions of constant level of interference, aB, and varying activity of the primary ion, aA. The potential values obtained are plotted against the activity of the primary ion. The intersection of the extrapolation of the linear portions of this curve will give the value of aA which is to be used to calculate KA,Bpot from the equation:
(1)KA,Bpot=(aAaB)ZA/ZB,
where both ZA and ZB have the same signs, positive or negative. Value of selectivity coefficient equal to 1.0 indicates that the sensor responds equally to primary as well as interfering ions. However, values smaller than 1.0 indicate that membrane sensor is responding more to primary ion than to interfering ions and in such a cases the sensor is said to be selective to primary ion over interfering ion. Further, the smaller the selectivity coefficient is, the higher the selectivity order is. A perusal of Table 4 shows that selectivity coefficient values for the present sensor are much smaller than 1.0 over a number of studied mono-, di-, and trivalent cations. Hence, the sensor is sufficiently selective over these ions and can therefore be used to estimate tin in the presence of these ions by direct potentiometry.Table 3
Selectivity coefficient valuesKA,Bpot for Sn2+ selective sensor by fixed interference method.
S. no.
Interfering ion (B)
Selectivity coefficients
1
K+
6.01 × 10−4
2
N
H
4
+
4.03 × 10−3
3
Cd2+
6.44 × 10−4
5
Cu2+
4.03 × 10−2
6
Ni2+
8.11 × 10−2
7
Zn2+
5.12 × 10−3
8
Co2+
2.01 × 10−2
9
Mn2+
3.11 × 10−3
10
Ni2+
3.11 × 10−3
11
Ag+
2.51 × 10−4
12
Hg2+
2.51 × 10−3
13
Ca2+
1.06 × 10−2
14
Sr2+
3.01 × 10−2
15
Cr3+
1.01 × 10−4
16
Al3+
6.01 × 10−4
17
Ti+
2.1 × 10−3
18
Cs+
2.06 × 10−3
19
Na+
3.01 × 10−3
20
Pb2+
1.01 × 10−3Table 4
Determination of Sn2+ concentrations in different artificially made samples.
Artificially made samples
Sn2+ sensor (Found)
By Titration method
S-1 (25 ppm), 4.8 mg
4.7 mg  ± 0.05
4.6 mg ± 0.08
S-2 (50 ppm), 9.6 mg
9.5 mg ± 0.04
9.7 mg ± 0.05
S-3 (75 ppm), 14.4 mg
14.8 mg ± 0.01
14.3 mg ± 0.07
S-4 (100 ppm), 19.2 mg
19.0 mg ± 0.09
19.1 mg ± 0.02
S-5 (125 ppm), 24.0 mg
24.1 mg ± 0.01
24.2 mg ± 0.04
S-6 (250 ppm), 48.0 mg
48.1 mg ± 0.08
48.5 mg ± 0.06
S-7 (500 ppm), 96.03 mg
96.2 mg ± 0.04
96.1 mg ± 0.08
S-8 (1000 ppm), 192.06 mg
192.1 mg ± 0.05
192.1 mg ± 0.04


### 4.5. Analytical Applications

The analytical application of proposed work (sensor no. 2) is evaluated by estimation of Sn2+ concentrations in different artificially made samples with simple starch-iodine-based titration. To prepare the sample of different concentration’s samples 4.8 mg (25 ppm), 9.6 mg (50 ppm) 14.4 mg (75 ppm), 19.2 mg (100 ppm), 24 mg (125 ppm), 48 mg (250 ppm), 96.03 mg (500 ppm), and 192.06 mg (1000 ppm) of SnCl2 · 2H2O accurately weighed, add to a 100 mL volumetric flask, dissolve in 25 mL of hydrochloric acid, dilute to volume with water, and mix well. Transfer 50 mL of this solution to a 500 mL conical flask, and add 5 g of potassium sodium tartrate, and then a cold saturated solution of sodium bicarbonate until the solution is alkaline to litmus paper. Titrate at once with 0.1 N iodine using starch TS as the indicator. The obtained results were comparatively compiled with sensor no. 2 in Table 4. Each mL of 0.1 N iodine consumed is equivalent to 11.28 mg of SnCl2 · 2H2O.


## 4.1. Effect of Membrane Composition and Response Characteristics

The response of different metal ions and rare earth ions as plotted as the negative log of concentration and the potential values obtained for different metal ions. Best response and slope were seen for the Sn2+ ion as compared to the other cations as shown Figure 2. The plot between the concentration and EMF in Figure 2 indicates that the best response was obtained for the Sn2+, whereas transition metal ion gave a poor response. The calibration curve slope was found to be 28.8 ± 0.4 mV/decade in the linear range of 1×10-2–1×10-7 M Sn2+ concentration with the detection limit of 2.10×10-8 M. Further result of changes in the membrane composition on the electrode response was studied. It is well known [14, 15] that sensitivity and selectivity obtained for a given ionophore is significantly affected by the membrane composition of an ion sensor membrane. The different membrane ingredients, such as amount of ionophore and nature of the plasticizer and additives, influence the potentiometric response behaviour of the sensor [16, 17]. Best optimized studies membrane for Sn2+ selective electrode are reported in Table 2 sensor 2. The results given in the Table 2 show that the electrode worked well in plasticizer/PVC ratio of nearly 2, which ensures enough mobility of the membrane constituents. The best sensitivity and selectivity was recorded for TBP as plasticizer. Further the amount of ionophore also affected the Nernstian slope value. It has been observed (Table 2) that on increasing the concentration of the ionophore more than 2% (w/w), the slope deteriorated and a narrow linear concentration range was achieved. Hence, a very small amount of ionophore is required for the study. The presence of lipophilic anion excluder in cation sensor based on neutral carrier not only reduces the ohmic resistance but also enhances the response behaviour and selectivity [14]. It also assists in the extraction capability of the carrier in the membrane electrodes study [18, 19]. According to the results in Table 2, most optimum plasticizer used was TBP and the ionic additive NaTPB, and the optimum ratio for further studies was PVC : TBP : ionophore : NaTPB as 28 : 59 : 8 : 5 (w/w%).Table 2
Composition of PVC membrane of (STSC) and performance characteristics of Sn2+ selective sensors based on them.
S. no.
PVC
Plasticizer
Ionophore
Excluder NaTPB
Slope (mv/decade)
Linear range
1
28
67 (TBP)
0
5
8.9
1 × 10−3 to 1 × 10−6
2
28
58 (TBP)
8
5
29.2
1 × 10−2 to 1 × 10−8
3
28
57 (TBP)
5
5
35.7
1 × 10−3 to 1 × 10−7
4
28
59 (TBP)
7
5
22.8
1 × 10−2 to 1 × 10−5
6
28
57 (DOP)
5
5
18.3
1 × 10−3 to 1 × 10−5
7
28
58 (DOP)
4
5
33.4
1 × 10−2 to 1 × 10−4
8
28
59 (DOP)
3
5
25.7
1 × 10−2 to 1 × 10−5Figure 2
Potential response of various ion-selective electrodes based on STSC.


## 4.2. pH and Nonaqueous Effect

The pH dependence of the electrode potential was tested over the range 0.5–14.0 for Sn2+ in concentration 1.0×10-3 as shown in Figure 3. The pH of the solutions was adjusted by the addition of dilute hydrochloric acid or sodium hydroxide. It is clear from Figure 3 that the useful pH range is 2.0–8.5, as the potentials remain constant in this range. The sharp change in potentials at higher pH values may be due to the hydrolysis of Sn2+, while at lower pH values H+ ions start contributing to the charge transport process of the membrane, thereby, causing interference.Figure 3
The effect of pH of test solution on the response of the Sn2+ ion-selective electrode.


## 4.3. Response and Lifetime

Response time is critically reviewed when it comes to analytical application of the sensor [20]. The static response time of the membrane sensor thus obtained was <8 s, for concentration ≥1.0×10-4 and <12 s for concentration of ≥10−6 (Figure 4). It should be noted that the equilibrium potential remains constant for more than 8 min.Figure 4
The effect of the time on potentiometric response of Sn2+ electrode.The lifetime of the membrane sensor was about 9 months, during which it could be used without any measurable divergence. The time of contact and concentration of the equilibrium solution was also optimized so that the stable sensor generated and reproducible potentials at relatively short response time obtained. It was found that an equilibrating solution of1.0×10-2 M and contact time of 24 Hrs was appropriate for smooth functioning of the electrode. Membranes were stored in 1.0×10-2 M Sn(NO3)2 solution when not in used.


## 4.4. Potentiometric Selectivity

The selectivity is the most important characteristic, as it determines the extent of utility of a sensor in real sample measurement. The selectivity coefficient values were determined by fixed interference method (FIM) [20, 21]. The selectivity coefficient values KA,Bpot indicate that the electrode is moderately selective to Sn2+ over a number of other cation (Table 3). The potential of a cell comprising an ion-selective electrode [22] and a reference electrode is measured with solutions of constant level of interference, aB, and varying activity of the primary ion, aA. The potential values obtained are plotted against the activity of the primary ion. The intersection of the extrapolation of the linear portions of this curve will give the value of aA which is to be used to calculate KA,Bpot from the equation:
(1)KA,Bpot=(aAaB)ZA/ZB,
where both ZA and ZB have the same signs, positive or negative. Value of selectivity coefficient equal to 1.0 indicates that the sensor responds equally to primary as well as interfering ions. However, values smaller than 1.0 indicate that membrane sensor is responding more to primary ion than to interfering ions and in such a cases the sensor is said to be selective to primary ion over interfering ion. Further, the smaller the selectivity coefficient is, the higher the selectivity order is. A perusal of Table 4 shows that selectivity coefficient values for the present sensor are much smaller than 1.0 over a number of studied mono-, di-, and trivalent cations. Hence, the sensor is sufficiently selective over these ions and can therefore be used to estimate tin in the presence of these ions by direct potentiometry.Table 3
Selectivity coefficient valuesKA,Bpot for Sn2+ selective sensor by fixed interference method.
S. no.
Interfering ion (B)
Selectivity coefficients
1
K+
6.01 × 10−4
2
N
H
4
+
4.03 × 10−3
3
Cd2+
6.44 × 10−4
5
Cu2+
4.03 × 10−2
6
Ni2+
8.11 × 10−2
7
Zn2+
5.12 × 10−3
8
Co2+
2.01 × 10−2
9
Mn2+
3.11 × 10−3
10
Ni2+
3.11 × 10−3
11
Ag+
2.51 × 10−4
12
Hg2+
2.51 × 10−3
13
Ca2+
1.06 × 10−2
14
Sr2+
3.01 × 10−2
15
Cr3+
1.01 × 10−4
16
Al3+
6.01 × 10−4
17
Ti+
2.1 × 10−3
18
Cs+
2.06 × 10−3
19
Na+
3.01 × 10−3
20
Pb2+
1.01 × 10−3Table 4
Determination of Sn2+ concentrations in different artificially made samples.
Artificially made samples
Sn2+ sensor (Found)
By Titration method
S-1 (25 ppm), 4.8 mg
4.7 mg  ± 0.05
4.6 mg ± 0.08
S-2 (50 ppm), 9.6 mg
9.5 mg ± 0.04
9.7 mg ± 0.05
S-3 (75 ppm), 14.4 mg
14.8 mg ± 0.01
14.3 mg ± 0.07
S-4 (100 ppm), 19.2 mg
19.0 mg ± 0.09
19.1 mg ± 0.02
S-5 (125 ppm), 24.0 mg
24.1 mg ± 0.01
24.2 mg ± 0.04
S-6 (250 ppm), 48.0 mg
48.1 mg ± 0.08
48.5 mg ± 0.06
S-7 (500 ppm), 96.03 mg
96.2 mg ± 0.04
96.1 mg ± 0.08
S-8 (1000 ppm), 192.06 mg
192.1 mg ± 0.05
192.1 mg ± 0.04


## 4.5. Analytical Applications

The analytical application of proposed work (sensor no. 2) is evaluated by estimation of Sn2+ concentrations in different artificially made samples with simple starch-iodine-based titration. To prepare the sample of different concentration’s samples 4.8 mg (25 ppm), 9.6 mg (50 ppm) 14.4 mg (75 ppm), 19.2 mg (100 ppm), 24 mg (125 ppm), 48 mg (250 ppm), 96.03 mg (500 ppm), and 192.06 mg (1000 ppm) of SnCl2 · 2H2O accurately weighed, add to a 100 mL volumetric flask, dissolve in 25 mL of hydrochloric acid, dilute to volume with water, and mix well. Transfer 50 mL of this solution to a 500 mL conical flask, and add 5 g of potassium sodium tartrate, and then a cold saturated solution of sodium bicarbonate until the solution is alkaline to litmus paper. Titrate at once with 0.1 N iodine using starch TS as the indicator. The obtained results were comparatively compiled with sensor no. 2 in Table 4. Each mL of 0.1 N iodine consumed is equivalent to 11.28 mg of SnCl2 · 2H2O.


## 5. Conclusions

In this work, the first Sn(II) electrochemical sensor was introduced based on of salicylaldehyde thiosemicarbazone (STSC) as a sensing material. The proposed electrochemical sensor with a membrane composition containing 28% poly(vinyl chloride) (PVC), 59% tri-n-butyl phosphate (TBP) as solvent mediator, 5% sodium tetraphenylborate (NaTPB) as cation excluder, and 8% STSC worked as an ionophore. The electrochemical sensor exhibits a nice Nernstian response of 28.8 ± 0.4 mV per decade of tin activity and a wide dynamic working range1.0×10-2–1.1×10-7 M. The detection limit of the sensor is 2.10×10-8 M and can be used in the pH range of 2.0–8.5. The electrochemical sensor has fast response time and relatively long lifetime (more than 9 months).



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*Source: 130372-2012-08-14.xml*