# Surface-Enhanced Oxidation and Determination of Isothipendyl Hydrochloride at an Electrochemical Sensing Film Constructed  by Multiwalled Carbon Nanotubes

Authors: S. N. Prashanth; Shankara S. Kalanur; Nagappa L. Teradal; J. Seetharamappa
Journal: International Journal of Electrochemistry
 (2012)

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## Abstract

The electrochemical behavior of isothipendyl hydrochloride (IPH) was investigated at bare and multiwalled-carbon-nanotube modified glassy carbon electrode (MWCNT-GCE). IPH (55μM) showed two oxidation peaks in Britton-Robinson (BR) buffer of pH 7.0. The oxidation process of IPH was observed to be irreversible over the pH range of 2.5–9.0. The influence of pH, scan rate, and concentration of the drug on anodic peak was studied. A differential pulse voltammetric method with good precision and accuracy was developed for the determination of IPH in pure and biological fluids. The peak current was found to be linearly dependent on the concentration of IPH in the range of 1.25–55 μM. The values of limit of detection and limit of quantification were noticed to be 0.284 and 0.949 μM, respectively.


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## Body

## 1. Introduction

Since the discovery by Iijima [1], carbon nanotube (CNT) including single-walled carbon nanotube (SWCNT) and multiwalled carbon nanotube (MWCNT), has attracted much attention due to its unique structure and extraordinary properties [2]. CNT possesses subtle electronic properties, huge surface area, efficient catalytic activity, and strong adsorption ability, high chemical and thermal stability, high elasticity, high tensile strength, and in some instances metallic conductivity [3, 4]. The modification of electrode surfaces with MWCNT for use in analytical sensing is well documented. It has demonstrated the ability to promote the electron-transfer reactions of electroactive biomolecules [5–7]. These excellent properties suggest that CNT is a fascinating electrode material, and now, it is widely used in electrochemistry and electroanalytical chemistry [8–10].Isothipendyl hydrochloride (Figure1) is a phenothiazine-related drug and has a broad range of clinical applications as antipruritic for local and generalized allergic reactions and radiation sickness [11]. It reduces vascular permeability and significantly reduces secretory activities. Large doses may cause drowsiness, nausea, and vomiting.Figure 1
Structure of IPH.Several methods have been reported for the determination of IPH in forensic samples, pharmaceutical formulations and body fluids [12–15]. Because of its pharmacological importance and lack of reports on its electrochemical behavior and analysis by voltammetry, we thought of investigating the electrochemical behavior of IPH at bare glassy carbon electrode (GCE) and over multiwalled carbon-nanotube modified glassy carbon electrode (MWCNT-GCE) in detail. Further, we have developed a differential pulse voltammetric method for the determination of IPH in pure and biological samples.


## 2. Experimental

### 2.1. Apparatus

Electrochemical studies were carried out on a CHI-1103A electrochemical analyzer (CH Instruments Ltd. Co., USA, version 9.03). A conventional three-electrode system consisting of a GCE (3 mm diameter) or MWCNT-GCE as the working electrode, a platinum wire as a counter electrode, and an Ag/AgCl (3 M KCl) as reference electrode was employed. For reproducible results, improved sensitivity and resolution of voltammetric peaks, the working electrode was polished with 0.05 micron alumina powder on a polishing cloth. Then, it was thoroughly rinsed with milli-pore water. All the reported potentials are against Ag/AgCl (3 M KCl).


### 2.2. Reagents

MWCNTs were obtained from Sigma-Aldrich (>99%, 10–20 nm in diameter). Pure IPH was obtained from German Remedies Ltd. A stock solution of IPH (2.5 mM) was prepared in millipore water and stored in a refrigerator at 4°C. In the present study, BR buffer (pH 2.5–10.6) was used as supporting electrolyte. All the solutions were prepared in milli-pore water, and all other chemicals used were of analytical reagent grade.


### 2.3. Preparation of MWCNT-Modified GCE

MWCNTs were refluxed in concentrated nitric acid for about 5 h, filtered, and washed with milli-pore water till the filtrate became neutral and finally dried [16]. The MWCNTs suspension was prepared by dispersing 2 mg of MWCNTs in 10 mL acetonitrile using ultrasonic agitation to obtain a relatively stable suspension. Before modification, the GCE was carefully polished with 1.0, 0.3, and 0.05 μm α-alumina on a smooth polishing cloth and then washed in methanol and water. The cleaned GCE was coated by casting 20 μL of the black suspension of MWCNTs and dried in air. After modification, the electrode was rinsed with water for about 5 min to remove the loosely adsorbed nanotubes, if any.


### 2.4. Working Procedure

The MWCNT-GCE was first activated in BR buffer of pH 7.0 by cyclic voltammetric sweeps between 0 and 1.4 V till stable cyclic voltammograms were obtained. The modified electrode was then transferred into 10 mL BR buffer (pH 7.0.) containing IPH (55μM), and an accumulation time of 240 s was given. After this accumulation time, the electrode was used to record the cyclic voltammogram/differential pulse voltammogram.Working solutions were prepared by diluting the stock solution as required with BR buffer (0.04 M) of required pH. For DPV, the following parameters were maintained: sweep rate 20 mV s−1, pulse amplitude 50 mV, pulse width 30 ms, and pulse period 500 ms. For analytical applications, oxidation peak a1 was selected. All electrochemical experiments were carried out at 25°C. After every measurement, new MWCNT-GCE was prepared.


### 2.5. Determination of IPH in Human Urine and Plasma Samples

Spiked urine samples were obtained by treating 0.9 mL aliquots of urine with 100μL IPH standard solution (2.5 mM) to obtain 250 μM IPH. A suitable aliquot of spiked urine was diluted with BR buffer, without any pretreatment, to prepare appropriate sample solution, and differential pulse voltammogram was recorded under optimized conditions.Spiked serum samples were prepared by following the procedure reported earlier [17]. Serum samples, obtained from healthy individuals (after having obtained their written consent), were stored frozen until assay. For the determination of IPH in plasma, 500 μL of IPH (2.5 mM) was added to 500 μL of untreated plasma. The mixture was vortexed for 30 s. In order to precipitate the plasma proteins, the plasma samples were treated with 250 μL perchloric acid (15%). After that, the mixture was vortexed for further 30 s and then centrifuged at 5000 rpm for 5 min. An appropriate volume of supernatant liquor was transferred in the voltammetric cell containing BR buffer of pH 7.0, and voltammograms were recorded. The voltammogram of sample without IPH did not show any signal that can interfere with the direct determination. The content of the drug in plasma was determined referring to the calibration graph or regression equation.


## 2.1. Apparatus

Electrochemical studies were carried out on a CHI-1103A electrochemical analyzer (CH Instruments Ltd. Co., USA, version 9.03). A conventional three-electrode system consisting of a GCE (3 mm diameter) or MWCNT-GCE as the working electrode, a platinum wire as a counter electrode, and an Ag/AgCl (3 M KCl) as reference electrode was employed. For reproducible results, improved sensitivity and resolution of voltammetric peaks, the working electrode was polished with 0.05 micron alumina powder on a polishing cloth. Then, it was thoroughly rinsed with milli-pore water. All the reported potentials are against Ag/AgCl (3 M KCl).


## 2.2. Reagents

MWCNTs were obtained from Sigma-Aldrich (>99%, 10–20 nm in diameter). Pure IPH was obtained from German Remedies Ltd. A stock solution of IPH (2.5 mM) was prepared in millipore water and stored in a refrigerator at 4°C. In the present study, BR buffer (pH 2.5–10.6) was used as supporting electrolyte. All the solutions were prepared in milli-pore water, and all other chemicals used were of analytical reagent grade.


## 2.3. Preparation of MWCNT-Modified GCE

MWCNTs were refluxed in concentrated nitric acid for about 5 h, filtered, and washed with milli-pore water till the filtrate became neutral and finally dried [16]. The MWCNTs suspension was prepared by dispersing 2 mg of MWCNTs in 10 mL acetonitrile using ultrasonic agitation to obtain a relatively stable suspension. Before modification, the GCE was carefully polished with 1.0, 0.3, and 0.05 μm α-alumina on a smooth polishing cloth and then washed in methanol and water. The cleaned GCE was coated by casting 20 μL of the black suspension of MWCNTs and dried in air. After modification, the electrode was rinsed with water for about 5 min to remove the loosely adsorbed nanotubes, if any.


## 2.4. Working Procedure

The MWCNT-GCE was first activated in BR buffer of pH 7.0 by cyclic voltammetric sweeps between 0 and 1.4 V till stable cyclic voltammograms were obtained. The modified electrode was then transferred into 10 mL BR buffer (pH 7.0.) containing IPH (55μM), and an accumulation time of 240 s was given. After this accumulation time, the electrode was used to record the cyclic voltammogram/differential pulse voltammogram.Working solutions were prepared by diluting the stock solution as required with BR buffer (0.04 M) of required pH. For DPV, the following parameters were maintained: sweep rate 20 mV s−1, pulse amplitude 50 mV, pulse width 30 ms, and pulse period 500 ms. For analytical applications, oxidation peak a1 was selected. All electrochemical experiments were carried out at 25°C. After every measurement, new MWCNT-GCE was prepared.


## 2.5. Determination of IPH in Human Urine and Plasma Samples

Spiked urine samples were obtained by treating 0.9 mL aliquots of urine with 100μL IPH standard solution (2.5 mM) to obtain 250 μM IPH. A suitable aliquot of spiked urine was diluted with BR buffer, without any pretreatment, to prepare appropriate sample solution, and differential pulse voltammogram was recorded under optimized conditions.Spiked serum samples were prepared by following the procedure reported earlier [17]. Serum samples, obtained from healthy individuals (after having obtained their written consent), were stored frozen until assay. For the determination of IPH in plasma, 500 μL of IPH (2.5 mM) was added to 500 μL of untreated plasma. The mixture was vortexed for 30 s. In order to precipitate the plasma proteins, the plasma samples were treated with 250 μL perchloric acid (15%). After that, the mixture was vortexed for further 30 s and then centrifuged at 5000 rpm for 5 min. An appropriate volume of supernatant liquor was transferred in the voltammetric cell containing BR buffer of pH 7.0, and voltammograms were recorded. The voltammogram of sample without IPH did not show any signal that can interfere with the direct determination. The content of the drug in plasma was determined referring to the calibration graph or regression equation.


## 3. Results and Discussion

### 3.1. Cyclic Voltammogram of IPH at MWCNT-GCE

The cyclic voltammograms of 55μM IPH at bare GCE and MWCNT-GCE in BR buffer of pH 7.0 along with that of blank are shown in Figure 2. IPH showed two oxidation peaks at 0.721 V (a1) and 0.958 V (a2) at bare GCE (Figure 2). No reduction peak was observed in the reverse scan suggesting that the electrochemical oxidation of IPH was an irreversible process. At MWCNT-GCE, these oxidation peaks appeared at 0.696 V and 0.912 V, respectively, with a considerable enhancement in the peak current. Thus, the negative shifts in peak potentials were observed to be 25 mV and 46 mV for peak a1 and a2, respectively, suggesting that MWCNT exhibited catalytic effect towards electrooxidation of IPH [8, 18].Figure 2
Voltammograms of blank buffer (1); 55μM IPH on bare GCE (2) and on MWCNT-GCE (3) in BR buffer of pH 7.0 at a scan rate of 50 mV s−1.Successive cyclic voltammograms were recorded to check the adsorption of the oxidation product of IPH on MWCNT-GCE. The oxidation peak currents of IPH were found to be decreased during the successive scans and finally remained unchanged. This was attributed to the adsorption of oxidative product of IPH on the modified electrode surface.


### 3.2. Influence of Amount of MWCNT Suspension

The amount of MWCNT on GCE may influence the electrooxidation of IPH. With increase in the volume of MWCNT suspension from 0 to 20μL, the oxidation peak current of IPH was observed to be increased remarkably (Figure not shown). The oxidation peak currents considerably increased as the surface concentration of IPH at MWCNT-GCE increased. With further increase in the volume, the oxidation peak current remained almost constant. Considering the peak current as well as the time needed for evaporation of acetonitrile, 20 μL of MWCNT suspension was used to modify the GCE surface.


### 3.3. Effect of Accumulation Time

Since the oxidation current is strongly dependent on the accumulation time, we have examined the influence of accumulation time on oxidation peak currents of IPH at the MWCNT-GCE. Accumulation of drug on the electrode surface was done under open circuit potential for different time intervals, and then cyclic voltammograms were recorded at a scan rate of 50 mV s−1. While maintaining the accumulation time of 0 to 240 s, the oxidation peak currents increased remarkably (figure not shown). However, the oxidation peak currents decreased slightly with further increase in the accumulation time suggesting that the amount of IPH tends to a limiting value at the MWCNT film. Considering the sensitivity and working efficiency, an accumulation time of 240 s was maintained throughout.


### 3.4. Effect of pH

The electrochemical behavior of IPH in BR buffer of different pH values was studied. At pH 3.5, the voltammogram of IPH was almost similar to that of promethazine (PMZ) owing to the close similarity in structure [19]. IPH is different from PMZ only in one benzene ring, which is replaced by pyridine ring in IPH. Two oxidation waves were seen on the initial scan, and no reduction peak was observed. Like in the case of another phenothiazine derivative, ethopropazine, the peak potential of a1 (of IPH) was pH dependent indicating the involvement of proton in the oxidation process [20]. With increase in pH from 2.5 to 7.0, the oxidation peak currents of a1 and a2 gradually increased at MWCNT-GCE (Figure 3). Furthermore, increasing pH to 9.0, the oxidation peak currents of a1 gradually decreased with broader and ill-defined peaks. Apparently, the oxidation signals of IPH seemed to be sensitive in the buffer of pH 7.0.Figure 3
Plot ofIpa versus pH for the electrooxidation of IPH on MWCNT-GCE in BR buffer at a scan rate of 50 mV s−1.We have also investigated the effect of pH on the oxidation peak potential. With an increase in pH from 2.5 to 7.0, the oxidation peak potential gradually shifted to negative potential suggesting that the protons were involved in the oxidation of IPH. The plot of peak potential of a1 versus pH showed a linear segment at pH 8.0. This intersection point of the curve was found to be close to the pKa value of IPH (8.6) [21]. This could be attributed to changes in protonation of acid-base properties of the molecule. The slope was found to be 29.6 mV/pH, which is close to the reported value for PMZ [22, 23] and the theoretical value for a two-electron and one-proton transfer reaction. Thus, it could be concluded that the electrode reaction mechanisms of IPH and PMZ are identical at least over the pH range of 2.5–7.0.


### 3.5. Effect of Scan Rate

Useful information on electrochemical mechanism can be acquired from the relationship between peak current and scan rate. Therefore, the electrochemical behavior of IPH in BR buffer of pH 7.0 at different scan rates was studied and the results are shown in Figure4.Figure 4
Voltammograms of 55μM IPH in Britton-Robinson buffer of pH 7.0 on MWCNT-GCE at different scan rates: (1) 10, (2) 20, (3) 30, (4) 40, (5) 60, (6) 80, and (7) 100 mV s−1.The peak current was observed to be proportional to the scan rate indicating that the electrode process was adsorption controlled [24]. A linear relationship was observed between logIpa and logυ as per (1) shown below:(1)log⁡⁡Ipa(μA)=0.8255log⁡⁡υ-3.5906.
The slope of 0.83 (obtained from the plot of logIpa versus logυ) was noticed to be close to the theoretical value of 1.0 for an adsorption-controlled process [25, 26]. The Epa of the oxidation peak was also noticed to be dependent on the scan rate. Further, the peak potential was shifted to more positive values with increase in the scan rates. Linear relationship was observed between Epa and scan rate indicating the irreversibility of the oxidation process with a correlation coefficient of 0.9883 according to (2) shown below:(2)Epa(V)=0.0011ν+0.6517.


## 3.1. Cyclic Voltammogram of IPH at MWCNT-GCE

The cyclic voltammograms of 55μM IPH at bare GCE and MWCNT-GCE in BR buffer of pH 7.0 along with that of blank are shown in Figure 2. IPH showed two oxidation peaks at 0.721 V (a1) and 0.958 V (a2) at bare GCE (Figure 2). No reduction peak was observed in the reverse scan suggesting that the electrochemical oxidation of IPH was an irreversible process. At MWCNT-GCE, these oxidation peaks appeared at 0.696 V and 0.912 V, respectively, with a considerable enhancement in the peak current. Thus, the negative shifts in peak potentials were observed to be 25 mV and 46 mV for peak a1 and a2, respectively, suggesting that MWCNT exhibited catalytic effect towards electrooxidation of IPH [8, 18].Figure 2
Voltammograms of blank buffer (1); 55μM IPH on bare GCE (2) and on MWCNT-GCE (3) in BR buffer of pH 7.0 at a scan rate of 50 mV s−1.Successive cyclic voltammograms were recorded to check the adsorption of the oxidation product of IPH on MWCNT-GCE. The oxidation peak currents of IPH were found to be decreased during the successive scans and finally remained unchanged. This was attributed to the adsorption of oxidative product of IPH on the modified electrode surface.


## 3.2. Influence of Amount of MWCNT Suspension

The amount of MWCNT on GCE may influence the electrooxidation of IPH. With increase in the volume of MWCNT suspension from 0 to 20μL, the oxidation peak current of IPH was observed to be increased remarkably (Figure not shown). The oxidation peak currents considerably increased as the surface concentration of IPH at MWCNT-GCE increased. With further increase in the volume, the oxidation peak current remained almost constant. Considering the peak current as well as the time needed for evaporation of acetonitrile, 20 μL of MWCNT suspension was used to modify the GCE surface.


## 3.3. Effect of Accumulation Time

Since the oxidation current is strongly dependent on the accumulation time, we have examined the influence of accumulation time on oxidation peak currents of IPH at the MWCNT-GCE. Accumulation of drug on the electrode surface was done under open circuit potential for different time intervals, and then cyclic voltammograms were recorded at a scan rate of 50 mV s−1. While maintaining the accumulation time of 0 to 240 s, the oxidation peak currents increased remarkably (figure not shown). However, the oxidation peak currents decreased slightly with further increase in the accumulation time suggesting that the amount of IPH tends to a limiting value at the MWCNT film. Considering the sensitivity and working efficiency, an accumulation time of 240 s was maintained throughout.


## 3.4. Effect of pH

The electrochemical behavior of IPH in BR buffer of different pH values was studied. At pH 3.5, the voltammogram of IPH was almost similar to that of promethazine (PMZ) owing to the close similarity in structure [19]. IPH is different from PMZ only in one benzene ring, which is replaced by pyridine ring in IPH. Two oxidation waves were seen on the initial scan, and no reduction peak was observed. Like in the case of another phenothiazine derivative, ethopropazine, the peak potential of a1 (of IPH) was pH dependent indicating the involvement of proton in the oxidation process [20]. With increase in pH from 2.5 to 7.0, the oxidation peak currents of a1 and a2 gradually increased at MWCNT-GCE (Figure 3). Furthermore, increasing pH to 9.0, the oxidation peak currents of a1 gradually decreased with broader and ill-defined peaks. Apparently, the oxidation signals of IPH seemed to be sensitive in the buffer of pH 7.0.Figure 3
Plot ofIpa versus pH for the electrooxidation of IPH on MWCNT-GCE in BR buffer at a scan rate of 50 mV s−1.We have also investigated the effect of pH on the oxidation peak potential. With an increase in pH from 2.5 to 7.0, the oxidation peak potential gradually shifted to negative potential suggesting that the protons were involved in the oxidation of IPH. The plot of peak potential of a1 versus pH showed a linear segment at pH 8.0. This intersection point of the curve was found to be close to the pKa value of IPH (8.6) [21]. This could be attributed to changes in protonation of acid-base properties of the molecule. The slope was found to be 29.6 mV/pH, which is close to the reported value for PMZ [22, 23] and the theoretical value for a two-electron and one-proton transfer reaction. Thus, it could be concluded that the electrode reaction mechanisms of IPH and PMZ are identical at least over the pH range of 2.5–7.0.


## 3.5. Effect of Scan Rate

Useful information on electrochemical mechanism can be acquired from the relationship between peak current and scan rate. Therefore, the electrochemical behavior of IPH in BR buffer of pH 7.0 at different scan rates was studied and the results are shown in Figure4.Figure 4
Voltammograms of 55μM IPH in Britton-Robinson buffer of pH 7.0 on MWCNT-GCE at different scan rates: (1) 10, (2) 20, (3) 30, (4) 40, (5) 60, (6) 80, and (7) 100 mV s−1.The peak current was observed to be proportional to the scan rate indicating that the electrode process was adsorption controlled [24]. A linear relationship was observed between logIpa and logυ as per (1) shown below:(1)log⁡⁡Ipa(μA)=0.8255log⁡⁡υ-3.5906.
The slope of 0.83 (obtained from the plot of logIpa versus logυ) was noticed to be close to the theoretical value of 1.0 for an adsorption-controlled process [25, 26]. The Epa of the oxidation peak was also noticed to be dependent on the scan rate. Further, the peak potential was shifted to more positive values with increase in the scan rates. Linear relationship was observed between Epa and scan rate indicating the irreversibility of the oxidation process with a correlation coefficient of 0.9883 according to (2) shown below:(2)Epa(V)=0.0011ν+0.6517.


## 4. Analytical Applications

### 4.1. Curve of Calibration

Differential pulse voltammetry was used for the determination of IPH because of its higher sensitivity compared to cyclic voltammetry. Sharper and well-resolved curves were obtained in BR buffer of pH 7.0. Under the optimized conditions (sweep rate 20 mV s−1, pulse amplitude 50 mV, pulse width 30 ms, pulse period 500 ms), a linear relation between the peak current and concentration of drug was observed in the range of 1.25–55 μM IPH (Figure 6). Beyond the IPH concentration of 55 μM, the linearity was lost. The differential pulse voltammograms of different concentrations of IPH are shown in Figure 5.Figure 5
Differential pulse voltammograms of IPH at different concentrations: (1) 1.25, (2) 2.5, (3) 5, (4) 10, (5) 18.8, (6) 25, (7) 35, (8) 45, and (9) 55μM.Figure 6
Relation betweenIpa and concentration of IPH on MWCNT-GCE at a scan rate of 50 mV s−1.The plot ofIpa versus the concentration of IPH showed linearity over the concentration range of 1.25–55 μM IPH with the correlation coefficient of 0.9931. The corresponding linear relation expressing the dependence of Ipa on concentration is shown below:(3)Ipa(μA)=0.1053C+3.1423,
where C is in μM L−1. Characteristics of the calibration graph are recorded in Table 1.Table 1
Characteristics of calibration plot of IPH.
DPVLinearity range [μM]1.25–55LOD [μM]0.28LOQ [μM]0.94Interday assay RSD [%]1.41Intraday assay RSD [%]1.21The limit of detection (LOD) and limit of quantification (LOQ) were calculated based on the peak current using (4) and (5) [27, 28]:(4)LOD=3sm,(5)LOQ=10sm,
where s is the standard deviation of the intercept (n=5) of calibration plot and m is the slope of the calibration curve. The LOD and LOQ values were found to be 0.28 μM and 0.94 μM, respectively. The interday reproducibility of the method was examined by recording voltammograms of 5 replicates of 5 μM, 20 μM and 50 μM IPH. These yielded the RSD values of 1.28, 1.42, and 1.53%, respectively. Further, the RSD values for intraday assay reproducibility at 5 μM, 20 μM, and 50 μM solutions (n=5) were found to be respectively, 1.12, 1.36, and 1.15%. The corresponding results are shown in Table 1. Low values of both LOD and LOQ confirmed the sensitivity of the proposed method. Further, the low values of RSD revealed the good precision of the proposed method for the assay of IPH.


### 4.2. Effects of Interferents

The selectivity of the proposed method was examined by studying the effects of interferents, namely, glucose, sucrose, starch, acacia powder, ascorbic acid, and talc. For this, we have recorded differential pulse voltammograms of 2.5μM IPH in the presence of different concentrations of interferents. The results of effects of interferents on the peak current of IPH are shown in Table 2.Table 2
Effects of interferents in the determination of 2.5μM IPH at MWCNT-GCE.
InterferentConcentration [μM]Current [μA]Signal change [μA]RSD [%]IPH only2.53.510——Ascorbic acid303.6500.1402.41Glucose803.5180.0081.63Sucrose803.5200.0101.55Talc503.5250.0151.68Acacia powder503.5860.0761.87Starch503.6210.1112.05It was noticed that the ascorbic acid did not interfere with the peak current of IPH up to 12-fold excess while the acacia powder, talc, and starch showed no effect on the peak current up to 20-fold excess. Further, glucose and sucrose did not exhibit any interference up to 32-fold excess. These results indicated that the proposed method is selective for the determination of IPH. Hence, IPH could be easily determined in the presence of above interferents.


### 4.3. Determination of IPH in Urine and Plasma Samples

The practical analytical application of the method was further established by determining IPH in human urine samples without any preliminary treatment. The recoveries from urine samples were examined by spiking drug free urine with known amounts of IPH and by recording the differential pulse voltammograms. The calibration graph was used to determine the concentration of IPH in urine samples. The results of analysis are listed in Table3. Higher average recovery (99.37–100.07%) and lower RSD values (less than 1.51%) highlighted good recovery and reproducibility of the results.Table 3
Results of analysis of IPH in spiked urine and serum samples at MWCNT-GCE.
Urine samplesIPH added [μM]nAmount found [μM]Average recovery [%]RSD [%]241.9999.371.511049.9599.460.9225425.02100.070.2335434.9999.980.16Serum samples241.9396.42.201049.7397.31.2925424.2897.11.9835434.9496.81.02The applicability of the proposed method was also examined by analyzing IPH in plasma samples. Suitable amounts of IPH spiked serum samples were diluted with supporting electrolyte and differential pulse voltammograms were recorded. The amount of IPH in serum samples was then determined by referring to the calibration plot. The results incorporated in Table3 indicated good recovery of IPH. The proposed method is simple, easy to perform, and sensitive enough for the assay of IPH in human serum samples.


## 4.1. Curve of Calibration

Differential pulse voltammetry was used for the determination of IPH because of its higher sensitivity compared to cyclic voltammetry. Sharper and well-resolved curves were obtained in BR buffer of pH 7.0. Under the optimized conditions (sweep rate 20 mV s−1, pulse amplitude 50 mV, pulse width 30 ms, pulse period 500 ms), a linear relation between the peak current and concentration of drug was observed in the range of 1.25–55 μM IPH (Figure 6). Beyond the IPH concentration of 55 μM, the linearity was lost. The differential pulse voltammograms of different concentrations of IPH are shown in Figure 5.Figure 5
Differential pulse voltammograms of IPH at different concentrations: (1) 1.25, (2) 2.5, (3) 5, (4) 10, (5) 18.8, (6) 25, (7) 35, (8) 45, and (9) 55μM.Figure 6
Relation betweenIpa and concentration of IPH on MWCNT-GCE at a scan rate of 50 mV s−1.The plot ofIpa versus the concentration of IPH showed linearity over the concentration range of 1.25–55 μM IPH with the correlation coefficient of 0.9931. The corresponding linear relation expressing the dependence of Ipa on concentration is shown below:(3)Ipa(μA)=0.1053C+3.1423,
where C is in μM L−1. Characteristics of the calibration graph are recorded in Table 1.Table 1
Characteristics of calibration plot of IPH.
DPVLinearity range [μM]1.25–55LOD [μM]0.28LOQ [μM]0.94Interday assay RSD [%]1.41Intraday assay RSD [%]1.21The limit of detection (LOD) and limit of quantification (LOQ) were calculated based on the peak current using (4) and (5) [27, 28]:(4)LOD=3sm,(5)LOQ=10sm,
where s is the standard deviation of the intercept (n=5) of calibration plot and m is the slope of the calibration curve. The LOD and LOQ values were found to be 0.28 μM and 0.94 μM, respectively. The interday reproducibility of the method was examined by recording voltammograms of 5 replicates of 5 μM, 20 μM and 50 μM IPH. These yielded the RSD values of 1.28, 1.42, and 1.53%, respectively. Further, the RSD values for intraday assay reproducibility at 5 μM, 20 μM, and 50 μM solutions (n=5) were found to be respectively, 1.12, 1.36, and 1.15%. The corresponding results are shown in Table 1. Low values of both LOD and LOQ confirmed the sensitivity of the proposed method. Further, the low values of RSD revealed the good precision of the proposed method for the assay of IPH.


## 4.2. Effects of Interferents

The selectivity of the proposed method was examined by studying the effects of interferents, namely, glucose, sucrose, starch, acacia powder, ascorbic acid, and talc. For this, we have recorded differential pulse voltammograms of 2.5μM IPH in the presence of different concentrations of interferents. The results of effects of interferents on the peak current of IPH are shown in Table 2.Table 2
Effects of interferents in the determination of 2.5μM IPH at MWCNT-GCE.
InterferentConcentration [μM]Current [μA]Signal change [μA]RSD [%]IPH only2.53.510——Ascorbic acid303.6500.1402.41Glucose803.5180.0081.63Sucrose803.5200.0101.55Talc503.5250.0151.68Acacia powder503.5860.0761.87Starch503.6210.1112.05It was noticed that the ascorbic acid did not interfere with the peak current of IPH up to 12-fold excess while the acacia powder, talc, and starch showed no effect on the peak current up to 20-fold excess. Further, glucose and sucrose did not exhibit any interference up to 32-fold excess. These results indicated that the proposed method is selective for the determination of IPH. Hence, IPH could be easily determined in the presence of above interferents.


## 4.3. Determination of IPH in Urine and Plasma Samples

The practical analytical application of the method was further established by determining IPH in human urine samples without any preliminary treatment. The recoveries from urine samples were examined by spiking drug free urine with known amounts of IPH and by recording the differential pulse voltammograms. The calibration graph was used to determine the concentration of IPH in urine samples. The results of analysis are listed in Table3. Higher average recovery (99.37–100.07%) and lower RSD values (less than 1.51%) highlighted good recovery and reproducibility of the results.Table 3
Results of analysis of IPH in spiked urine and serum samples at MWCNT-GCE.
Urine samplesIPH added [μM]nAmount found [μM]Average recovery [%]RSD [%]241.9999.371.511049.9599.460.9225425.02100.070.2335434.9999.980.16Serum samples241.9396.42.201049.7397.31.2925424.2897.11.9835434.9496.81.02The applicability of the proposed method was also examined by analyzing IPH in plasma samples. Suitable amounts of IPH spiked serum samples were diluted with supporting electrolyte and differential pulse voltammograms were recorded. The amount of IPH in serum samples was then determined by referring to the calibration plot. The results incorporated in Table3 indicated good recovery of IPH. The proposed method is simple, easy to perform, and sensitive enough for the assay of IPH in human serum samples.


## 5. Conclusions

Multiwalled carbon-nanotube-modified glassy carbon electrode was developed as an electrochemical sensor for the assay of IPH based on the enhanced peak current responses of oxidation of IPH. This novel sensing system for IPH was found to be convenient and showed excellent analytical characteristics such as significant lowering of the detection limit, higher sensitivity, and better selectivity. The method provides a simple approach for the determination of IPH in spiked human urine and serum samples without any pretreatment. The principal advantage of the proposed method is its freedom from the interference by excipients.



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*Source: 875631-2012-01-29.xml*