Research Article  Open Access
Hoda M. Elqudaby, Hassan A. M. Hendawy, Eglal R. Souaya, Gehad G. Mohamed, Ghada M. G. Eldin, "Utility of Activated Glassy Carbon and Pencil Graphite Electrodes for Voltammetric Determination of Nalbuphine Hydrochloride in Pharmaceutical and Biological Fluids", International Journal of Electrochemistry, vol. 2016, Article ID 8621234, 9 pages, 2016. https://doi.org/10.1155/2016/8621234
Utility of Activated Glassy Carbon and Pencil Graphite Electrodes for Voltammetric Determination of Nalbuphine Hydrochloride in Pharmaceutical and Biological Fluids
Abstract
This work compares voltammetric response of nalbuphine hydrochloride (NP·HCl) at both activated glassy carbon and pencil graphite electrodes. The electrochemical oxidation of the drug was studied using cyclic voltammetry (CV), differential pulse voltammetry (DPV), and square wave voltammetry (SWV) techniques. For analytical purpose a wellresolved irreversible diffusion controlled voltammetric peak was established in BrittonRobinson (BR) buffer solution of pH 6.00 using pencil graphite electrode (PGE). Using activated glassy carbon electrode (GCE) a wellresolved irreversible diffusion controlled voltammetric peak was obtained at pH 7.00 using the same buffer solution. According to the linear relationship between the peak current and NP·HCl concentration, DPV and SWV methods were developed for their quantitative determination in pharmaceutical and human biological fluids. The linear response was obtained in the range from to mol L^{−1} using PGE and from to mol L^{−1} using a GC electrode, respectively. Precision and accuracy of the developed method were checked by recovery studies.
1. Introduction
Nalbuphine hydrochloride (NP·HCl) is a phenanthrene derivative. It is an opioid analgesic where it has mixed opioid agonist and antagonist activity. It is used for the relief of moderate to severe pain and as adjunct to anaesthesia. It is structurally related to naloxone and oxymorphone. Pharmacologically, it is quantitatively similar to pentazocine but it is a more potent antagonist at opioid acceptors. It is reported to produce no significant cardiovascular effect in patient with ischaemic heart disease. It differs from pure Л agonists such as morphine in that it is analgesic sedative and has respiratory depressant actions. Actions are subject to a ceiling effect and may not increase proportionately with dose [1]. Nalbuphine has the IUPAC name (5α,6α)17(cyclobutylmethyl)4,5expoxymorphinan3,6,1 4triol hydrochloride; Ncyclobutylmethyl14hydroxydihydronormorphine (Figure 1) [2].
Very few analytical methods have been established for the determination of NP·HCl in pharmaceuticals, dog, human, and rabbit plasma using highperformance liquid chromatography where either UV or electrochemical detection was used [3–8]. A solid phase extraction procedure was developed for the quantification of NP·HCl in human plasma with subsequent assay by highperformance liquid chromatography and electrochemical detection [9].
NP·HCl was simultaneously determined in human hair by gas chromatography, mass spectrometry [10]. Tranexamic acid derived gold nanoparticles modified glassy carbon electrode was used as a sensor for NP determination where the sensor responded linearly in the range of 0.05–1.25 μg mL^{−1} [11]. NP·HCl was determined spectrophotometrically using Nbromosuccinimide as an oxidant [12] and stability indicating methods [13].
The advantage of PGE over the existing GCE is its high electrochemical reactivity, commercial availability, good mechanical rigidity, and low cost; the behavior of many pharmaceuticals on GCE was discussed in many of our previous researches [14–16]. Although PGE is relatively new type of carbon electrode, it has been successfully applied to the cathodic and anodic voltammetry by virtue of its high electrochemical reactivity, low technology, and ease of modification [17–22]. In the present work we reported the electrochemical behavior of NP·HCl using activated glassy carbon (GCE) and pencil graphite electrode (PGE) in BrittonRobinson buffer of pH 6.00 and 7.00 using pencil graphite electrode (PGE) and activated glassy carbon (GCE) electrode, respectively. Moreover, electroanalytical methods are far less expensive and are more portable than the aforementioned techniques. Specifically, voltammetry is more regularly used in industrial, environmental applications and in the trace drugs detection in their dosage forms and especially in biological samples since it combines excellent sensitivity, selectivity, accuracy, and precision with low cost of instrumentation and maintenance.
Different experimental conditions were studied and then the electrodes were applied successfully for determination of NP·HCl in pure, pharmaceutical, and biological fluids. The results obtained can support the use of this suggested voltammetric method in the routine analysis of the cited drug.
2. Experimental
2.1. Chemicals and Reagents
Nalbuphine hydrochloride and its pharmaceutical dosage form (Nalufin) were kindly provided by Amoun Company, Cairo, Egypt. All chemicals for preparation of buffers and supporting electrolytes were of reagent grade (Merck or Sigma) which are provided from National Organization for Drug Control and Research (NODCAR). Stock solution of NP·HCl ( mol L^{−1}) was prepared in deionized water and kept in the refrigerator. BrittonRobinson buffer (0.04 mol L^{−1}, pH 2.00–10.0) and standard solutions were prepared by serial dilution of the stock solution with selected supporting electrolyte.
2.2. Instrumental and Experimental
Voltammetric measurement was obtained using the electrochemical analyzer computrace system with 797 VA computrace software (1.0) from Metrohm, Switzerland. A threeelectrode cell was employed. The working electrodes were a HB rotring tikky hi polymer pencil graphite electrode with a diameter of 0.7 mm identifiable with S0312690, R505708N and batch number (4006856 505733) and a glassy carbon stationary electrode as a working electrode (mini glassy carbon disk electrode of the active zone: 2.8 mm for ELCD641/656). Electrical contact with the working electrodes was achieved by soldering a copper wire to the metallic part of the apparatus fixing the pencil; Ag/AgCl (3 mol L^{−1} KCl) was used as a reference electrode and platinum wire as a counter electrode. For analytical application, the following parameters were employed: DPVpulse amplitude 50 mV, pulse width 40 ms, and scan rate 100 ; SWVpulse amplitude 20 mV, frequency 50 Hz, potential step 6 mV, and electrochemical analyzer made the background subtraction automatically. For CV, the initial and final potentials were variable, depending on the pH value and the cutoff of the electrolyte. Scan rate measurements in the range of 20–460 mV s^{−1} were carried out. The pH measurements were performed using Jenway 3330 Research pH meter, UK. Ultrasonic Cleaner, United Jewelry Tool Supplies, model UTA60, 6L capacity, Italy, was used: deionized water used throughout the present study was supplied from a HamiltonAquaMetric deionized water system. All the experiments were performed at a temperature of 25°C.
2.3. Area of the Electrode
In order to determine the active area of graphite pencil and glassy carbon electrodes surface was obtained by applying the cyclic voltammetric method using 1.0 mM at different scan rates. For a reversible process, the following RandlesSevcik formula was used:where refers to the anodic peak current, is the number of electrons transferred, is the surface area of the electrode, is the diffusion coefficient, is the scan rate, and is the concentration of . For 1.0 mM in 0.1 M KCL electrolyte, , cm^{2} s^{−1}; then from the slope of the plot of versus , the electroactive area was calculated. In our experiment electroactive area calculated from RandlesSevcik equation was found to be 0.269 and 0.097 cm^{2} for graphite pencil and glassy carbon electrodes, respectively. Electroactive area of PGE has almost doubled active area compared to GCE, so there is a greater response of PGE than GCE on peak current that resulted from NP·HCl drug.
2.4. Experimental Procedure
In the electrochemical measurements, pencil graphite electrode was electrochemically pretreated by scanning the potential between 0.02 and 0.30 V with a scan rate of 20 mV s^{−1} for 100 cycles in 0.04 mol L^{−1} BrittonRobinson buffer. Voltammetric analyses were performed in 10 mL of BR buffer solution pH 6.00 for PGE while they were performed in 20 mL of BR buffer solution at pH 7.00 for GCE. Stock solution of the prepared drug solution containing 3.939 and 7.878 mg mL^{−1} of NP·HCl for PGE and GCE, respectively, was introduced into the electrolytic cell and after a total of 10 mm of pencil graphite was immersed into the supporting electrolyte. The cyclic voltammograms were recorded at a scan rate 60 mV s^{−1}. The calibration curves of NP·HCl using DPV and SWV were established by plotting the peak current (μA) against drug concentration (mol L^{−1}). The analytical parameters such as ruggedness, precision, relative standard deviations, limit of detection, and limit of quantification were calculated to check the accuracy and precision of the proposed method.
2.4.1. Analysis of Pharmaceutical Dosage Form
The PGE and GCE were applied for the determination of nalufin ampoule with a specified content of NP·HCl of 20 mg mL^{−1}. The procedure for sample was 1 mL portion of nalufin ampoule, was pipetted into a 25 mL calibrated flask, and was diluted up to the mark with deionized water. The amount of NP·HCl per ampoule was calculated using the linear regression equation obtained from the calibration curve of pure NP·HCl.
2.4.2. Application to Human Urine
Direct application to human urine and without any sample pretreatment like precipitation was carried out. Urine was supplied from healthy volunteers, allowed to settle for about 30 minutes, and then used for the experiments. A drug solution of NP·HCl dissolved in deionized water to achieve a final concentration of 20 mg mL^{−1} appropriate volumes of this sample was transferred into the voltammetric cell and diluted up to the volume with BrittonRobinson buffer at pH 6.00 and 7.00 for PGE and GCE, respectively, and subsequently analyzed according to the recommendation in the general analytical procedure. An aliquot of human urine sample was collected and analyzed as a sample.
3. Results and Discussion
3.1. Electrooxidation of NP·HCl
The oxidation behavior of NP·HCl was studied over pH range of 2.00–10.0 in various supporting electrolytes. The cyclic voltammogram of NP·HCl in BR buffer at pH 6.00 or pH 7.00 in case of PGE and GCE, respectively, was shown in Figure 2.
(a)
(b)
The electrochemical behavior of the NP·HCl drug at the selected pH endued one main irreversible anodic peak at 472 and 413 mV for both PGE and GCE, respectively. On the reverse scan no corresponding reduction peak was observed, so the behavior of NP·HCl drug undergoes irreversible oxidation process.
3.2. Effect of pH
To study the effectiveness of pH on electrodes reaction and select the suitable pH for oxidation of NP·HCl drug using PGE and GCE, the irreversible oxidation reaction of mol L^{−1} NP·HCl drug was studied over the pH range 2.00 to 10.0 in BR buffer solution by cyclic voltammetry. The solution pH influenced the peak current and peak potential considerably with the increase in pH of the solution where peak potential was shifted to less positive values and obeys the following equations:The slope of this equation is found to be 62.45 and 51.53 mV/pH for PGE and GCE, respectively. This closeness of the slope to the expected theoretical value [23] of 59 mV/pH suggests that the number of the electrons transferred during oxidation process is equal to that of the hydrogen ions taking part in the electrode reaction.
The proposed mechanism of the electrooxidation of NP·HCl can be given as in Scheme 1.
From the plot of versus pH (Figure 3), it is clear that the intensity of the peak current was increased to a high value at pH 6.00 and pH 7.00 for PGE and GCE, respectively. Then the peak intensity decreases because the best result with respect to sensitivity accompanied with sharper response was obtained with these pH values. Therefore, pH 6.00 and pH 7.00 were selected for further experimental studies.
(a)
(b)
3.3. Effect of Scan Rate
The effect of scan rate on the electrooxidation of NP·HCl was examined by cyclic voltammetry (Figure 4). The effect of the square root of the scan rate on the anodic peak current showed a linear relationship between square root of the scan rate and anodic peak current as shown in Figure 4 which was of exemplary diffusion controlled currents [24]. The equation can be expressed as follows: Also there is a linear relationship that was observed between and (Figure 4) which follows the equation:which made it clear that the slope values of 0.419 and 0.576 for PGE and GCE, respectively, were comparable with theoretically expected value of 0.5 for a diffusion controlled process which confirms that the electrooxidation of NP·HCl was diffusion controlled using both PGE and GCE electrodes.
(a)
(b)
From Figure 4, it is noticed that any increase in the scan rate causes shift in the peak potential to a positive value and a linear relationship was observed in the range of 20 to 240 mV s^{−1} scan rate. The equation can be expressed asIn order to calculate the number of electron transfers during oxidation for an irreversible electrode process, according to Laviron [25], is defined by the following equation:where α is the transfer coefficient, is the standard heterogeneous rate constant of the reaction, is number of electrons transferred, is the scan rate, and is the thermal standard redox potential. Thus, the value of can be easily calculated from the slope of versus plot. In this system, the slope was 0.05225 and 0.07028 for PGE and GCE, respectively. Taking K, J K^{−1} mol^{−1}, and C mol^{−1}, the value was calculated to be 1.132 and 0.842 for PGE and GCE, respectively, according to Bard and Faulkner [26], where α can be given aswhere was the potential when the current was at half the peak value. From this, the value of α was calculated to be 0.7 and 0.8 for PGE and GCE, respectively. Then, the number of electrons () transferred in the electrooxidation of NP·HCl was calculated to be 1.2 and 1.0 for PGE and GCE, respectively. The value of can be determined from the intercept of the previous plot if the value of is known. The value of in (6) can be obtained from the intercept of versus curve by extrapolating to the vertical axis at [27]. In the system under study the intercept for versus plot was 0.4873 and 0.3639 for GCE and PGE, respectively, and was found to be 363 and 488 for PGE and GCE, respectively [26, 28].
3.4. Analytical Applications
In order to develop a voltammetric methodology for determination of the drug, we selected the DPV and SWV methods, since the peaks were sharper and better defined at lower concentration of NP·HCl; then those obtained by cyclic and linear sweep voltammetry with a lower background current lead to improvement in resolution. The precision of the method was evaluated by repeating three experiments on the same day and in the same standard condition to maintain the repeatability of the proposed method. For these studies mol L^{−1} of NP·HCl solution was used. The results were given as shown in Tables 1 and 2.


In order to provide DPV and SWV quantitative procedure, the dependence of the peak current on the drug concentration was investigated. Linear calibration curves were obtained for NP concentration in the range from to and to mol L^{−1} for the first and the second peaks, respectively, in case of PGE so NP·HCl has two electroactive sites which are characterized by the high electron density where oxidation is most likely to occur and from to mol L^{−1} in case of GCE (Figure 5). The characterization of these graphs was shown in Tables 1 and 2. The limit of detection (LOD) and the limit of quantification (LOQ) were also shown in Tables 1 and 2.
(a)
(b)
LOD and LOQ were calculated on the peak current using the following equations:where is standard deviation of the peak current five runs and is the slope of the calibration curve [29].
Applicability of the PGE and GCE was investigated for the determination of NP·HCl in a pharmaceutical ampule Nalufin (20 mg mL^{−1}). Differential pulse voltammograms were obtained by adding appropriate standard solution to diluted solution under the optimized conditions described earlier. The results of determination of NP·HCl in ampule dosage forms were shown in Table 3. A recovery of 100.2 and 99.98% with relative standard deviation of 0.8 and 0.94% using PGE and GCE was obtained, respectively.
 
Tabulated value at 95% confidence limit = 2.77, , degree of freedom = 4. Tabulated value at 95% confidence limit = 6.39, . 
The resulting mean values of NP·HCl content in pharmaceutical formulation for PGE and GCE showed good agreement with the declared values of 20 mg/NP ampule. These results indicated that PGE has adequate precision and accuracy for the determination of NP·HCl.
3.5. Detection of NP·HCl in Spiked Human Urine
The applicability of the proposed technique to human urine was investigated. The calibration curve was obtained for spiked samples and represented graphically in Figure 6. The obtained regression equation and related validation parameter are shown in Table 4. To determine NP·HCl drug in spiked urine samples neither time consuming extraction and evaporation steps nor sample pretreatment was required. The proposed method gave reproducible results and was easy to perform and sensitive enough for the determination of NP·HCl drug in human urine sample. The stability of urine sample kept in a refrigerator (±4°C) was tested by performing five consecutive analyses of the samples over a period of approximately 5 h. There were no significant differences in the peak currents and potentials between the first and the last measurements.

(a)
(b)
3.6. Precision (Repeatability and Reproducibility)
The intra and interday precision were evaluated by assaying freshly prepared solutions in triplicate on the same day and on three different days, respectively, using the proposed method. The repeatability (intraday) and reproducibility (interday) of the results obtained by means of the proposed SWV procedure were examined and the results indicated high accuracy and precision of the proposed procedure and proved to be suitable for quality control of NP·HCl (Table 5).
 
Each result is the average of three separate measurements. 
4. Conclusion
In the presented study, an accurate, simple, and sensitive cyclic, DPV, and SWV voltammetric determination of NP·HCl drug was employed in pure and dosage forms using the most popular and simpler working electrodes named graphite pencil electrode (PGE) and activated glassy carbon electrode (GCE) [30] where the electrooxidative behavior of the cited drug was studied. It showed one welldefined irreversible anodic peak. Different parameters were tested to optimize the best condition for determination and the analytical procedure was fully validated regarding linearity precision, accuracy, reproducibility, sensitivity, and selectivity. The method developed was also compared with the reference one [31] and was proved to be a satisfactory alternative for the fast, simple, and clean quantitative determination of NP·HCl.
According to LOD and LOQ electrochemical characterization of both electrodes towards NP·HCl oxidation, it is clear that PGE has the highest electrocatalytic activity followed by a divided GCE. This work will be continued in order to apply this method as recommended routine analysis of the drug under study.
Conflict of Interests
The authors declare that there is no conflict of interests regarding the publication of this paper.
Acknowledgment
The authors would like to express their gratitude to Department of Analytical Chemistry at Faculty of Science, Ain Shams University, Cairo University, and National Organization for Drug Control and Research (NODCAR, Egypt) for providing instruments and the means necessary to accomplish this work.
References
 A. Brayfield, Martindale: “The Complete Drug Reference” Drug Monographs Volume A, Pharmaceutical Press, Gurnee, Ill, USA, 38th edition, 2012.
 M. J. O'Neil, Ed., The Merck Index, RSC Publishing, 15th edition, 2013.
 L.H. Pao, C.H. Hsiong, O. Y.P. Hu, and S.T. Ho, “Highperformance liquid chromatographic method for the simultaneous determination of nalbuphine and its prodrug, sebacoyl dinalbuphine ester, in dog plasma and application to pharmacokinetic studies in dogs,” Journal of Chromatography B: Biomedical Sciences and Applications, vol. 746, no. 2, pp. 241–247, 2000. View at: Publisher Site  Google Scholar
 S.H. Ho, J.J. Wang, O. Y.P. Hu, P.S. Chiang, and S.C. Lee, “Determination of nalbuphine by highperformance liquid chromatography with ultraviolet detection: application to human and rabbit pharmacokinetic studies,” Journal of Chromatography B: Biomedical Sciences and Applications, vol. 678, no. 2, pp. 289–296, 1996. View at: Publisher Site  Google Scholar
 F. de Cazanove, J.M. Kinowski, M. Audran, A. Rochette, and F. Bressolle, “Determination of nalbuphine in human plasma by highperformance liquid chromatography with electrochemical detection. Application to a pharmacokinetic study,” Journal of Chromatography B: Biomedical Applications, vol. 690, no. 12, pp. 203–210, 1997. View at: Publisher Site  Google Scholar
 D. Groenendaal, M. C. M. BlomRoosemalen, M. Danhof, and E. C. M. De Lange, “Highperformance liquid chromatography of nalbuphine, butorphanol and morphine in blood and brain microdialysate samples: application to pharmacokinetic/pharmacodynamic studies in rats,” Journal of Chromatography B, vol. 822, no. 12, pp. 230–237, 2005. View at: Publisher Site  Google Scholar
 L. M. Dubé, N. Beaudoin, M. Lalande, and I. J. McGilveray, “Determination of nalbuphine by highperformance liquid chromatography with electrochemical detection: application to clinical samples from postoperative patients,” Journal of Chromatography B: Biomedical Sciences and Applications, vol. 427, pp. 113–120, 1988. View at: Publisher Site  Google Scholar
 P. Kintz, A. Tracqui, and P. Mangin, “Determination of nalbuphine using highperformance liquid chromatography coupled to photodiodearray detection and gas chromatography coupled to mass spectrometry,” Journal of Chromatography B: Biomedical Sciences and Applications, vol. 579, no. 1, pp. 172–176, 1992. View at: Publisher Site  Google Scholar
 E. Nicolle, S. Veitl, C. Guimier, and G. Bessard, “Modified method of nalbuphine determination in plasma: validation and application to pharmacokinetics of the rectal route,” Journal of Chromatography B: Biomedical Applications, vol. 690, no. 12, pp. 89–97, 1997. View at: Publisher Site  Google Scholar
 J. Young Kim, M. Kyo In, K. Jung Paeng, and B. Chul Chung, “Simultaneous determination of nalbuphine and opiates in human hair by gas chromatographymass spectrometry,” Chromatographia, vol. 59, no. 34, pp. 219–226, 2004. View at: Google Scholar
 T. Shaikh, A. Nafady, F. N. Talpur et al., “Tranexamic acid derived gold nanoparticles modified glassy carbon electrode as sensitive sensor for determination of nalbuphine,” Sensors and Actuators B: Chemical, vol. 211, pp. 359–369, 2015. View at: Publisher Site  Google Scholar
 A. M. ElDidamony, M. Z. Saad, and N. O. Saleem, “Spectrophotometric determination of some analgesic drugs in pharmaceutical formulations using Nbromosuccinimide as an oxidant,” Journal of the Association of Arab Universities for Basic and Applied Sciences, vol. 17, pp. 43–50, 2015. View at: Publisher Site  Google Scholar
 M. M. Fouad, S. A. Abdel Razaq, Z. A. Elsayed, and L. A. Hussin, “Stability indicating methods for determination of nalbuphinehydrochloride,” British Journal of Pharmaceutical Research, vol. 3, no. 2, pp. 259–272, 2013. View at: Publisher Site  Google Scholar
 H. M. Elqudaby, G. G. Mohamed, F. A. Ali, and S. M. Eid, “Validated voltammetric method for the determination of some antiprotozoa drugs based on the reduction at an activated glassy carbon electrode,” Arabian Journal of Chemistry, vol. 6, no. 3, pp. 327–333, 2013. View at: Publisher Site  Google Scholar
 H. M. Elqudaby, G. G. Mohamed, and G. M. G. El Din, “Electrochemical behaviour of trimebutine at activated glassy carbon electrode and its direct determination in urine and pharmaceutics by square wave and differential pulse voltammetry,” International Journal of Electrochemical Science, vol. 9, pp. 856–869, 2014. View at: Google Scholar
 H. M. Elqudaby, H. A. M. Hendawy, and M. A. Zayed, “Microdetermination of entecavir drug in its pharmaceuticals forms and in biological fluids using anodic voltammetry,” World Journal of Pharmaceutical Research, vol. 7, pp. 1115–1120, 2014. View at: Google Scholar
 A. Levent, Y. Yardim, and Z. Senturk, “Voltammetric behavior of nicotine at pencil graphite electrode and its enhancement determination in the presence of anionic surfactant,” Electrochimica Acta, vol. 55, no. 1, pp. 190–195, 2009. View at: Publisher Site  Google Scholar
 W. Gao, J. Song, and N. Wu, “Voltammetric behavior and squarewave voltammetric determination of trepibutone at a pencil graphite electrode,” Journal of Electroanalytical Chemistry, vol. 576, no. 1, pp. 1–7, 2005. View at: Publisher Site  Google Scholar
 D. Demetriades, A. Economou, and A. Voulgaropoulos, “A study of pencillead bismuthfilm electrodes for the determination of trace metals by anodic stripping voltammetry,” Analytica Chimica Acta, vol. 519, no. 2, pp. 167–172, 2004. View at: Publisher Site  Google Scholar
 H. Karadeniz, B. Gulmez, F. Sahinci et al., “Disposable electrochemical biosensor for the detection of the interaction between DNA and lycorine based on guanine and adenine signals,” Journal of Pharmaceutical and Biomedical Analysis, vol. 33, no. 2, pp. 295–302, 2003. View at: Publisher Site  Google Scholar
 A. M. Bond, P. J. Mahon, J. Schiewe, and V. VicenteBeckett, “An inexpensive and renewable pencil electrode for use in fieldbased stripping voltammetry,” Analytical Chemistry Acta, vol. 345, no. 1–3, pp. 67–74, 1997. View at: Publisher Site  Google Scholar
 E. Dede, Ö. Sağlam, and Y. Dilgin, “Sensitive voltammetric determination of niclosamide at a disposable pencil graphite electrode,” Electrochimica Acta, vol. 127, pp. 20–26, 2014. View at: Publisher Site  Google Scholar
 I. Martin, F. C. Gritiani, L. S. Canaes, F. A. de Souza Campos Junior, L. M. da Silva Cruz, and S. Rath, “Determination of parabens in shampoo using high performance liquid chromatography with amperometric detection on a borondoped diamond electrode,” Talanta, vol. 85, no. 1, pp. 1–7, 2011. View at: Publisher Site  Google Scholar
 D. K. Gosser, Cyclic Voltammetry: Simulation and Analysis of Chemical Mechanism, VCH, New York, NY, USA, 1993.
 E. Laviron, “General expression of the linear potential sweep voltammogram in the case of diffusionless electrochemical systems,” Journal of Electroanalytical Chemistry, vol. 101, no. 1, pp. 19–28, 1979. View at: Publisher Site  Google Scholar
 A. J. Bard and L. R. Faulkner, Electrochemical Methods Fundamentals and Applications, Wiley, 2nd edition, 2004.
 Y. Wu, X. Ji, and S. Hu, “Studies on electrochemical oxidation of azithromycin and its interaction with bovine serum albumin,” Bioelectrochemistry, vol. 64, no. 1, pp. 91–97, 2004. View at: Publisher Site  Google Scholar
 M. P. Miranda, R. Del Rio, M. A. Del Valle, M. Faundez, and F. Armijo, “Use of fluorinedoped tin oxide electrodes for lipoic acid determination in dietary supplements,” Journal of Electroanalytical Chemistry, vol. 668, pp. 1–6, 2012. View at: Publisher Site  Google Scholar
 E. Swartz and I. S. Krull, Analytical Method Development and Validation, Marcel Dekker, New York, NY, USA, 1997.
 J. Wang, Analytical Electrochemistry, John Wiley & Sons, 2nd edition, 1948.
 Edition Cantorverlag, Aulendorf, Germany, ECV, p. 1035, 2002.
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Copyright © 2016 Hoda M. Elqudaby et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.