# Electrochemical Oxidation of an Immunosuppressant, Mycophenolate Mofetil, and Its Assay in Pharmaceutical Formulations

Authors: S. N. Prashanth; K. C. Ramesh; J. Seetharamappa
Journal: International Journal of Electrochemistry
 (2011)

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## Abstract

Electrochemical oxidation of mycophenolate mofetil (MMF) has been studied at a glassy carbon electrode in aqueous solution over a wide pH range. MMF was oxidized on glassy carbon electrode (GCE) by an irreversible process that was controlled mainly by diffusion. The irreversibility of the electrode process was verified by different criteria. A probable mechanism for electrochemical oxidation of MMF was proposed. Differential-pulse voltammogram of the drug showed two oxidation peaks at 0.631 V and at 0.921 V (verses SCE) in phosphate buffer of pH 6.0. This process could be used to determine MMF in the concentration range of5.0×10−7 to 7.5×10−4 M with a limit of detection of 1.48×10−7 M. The method was successfully applied for the analysis of MMF in pure and dosage forms and in biological fluids.


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## Body

## 1. Introduction

Mycophenolate mofetil (MMF), chemically known as (Z)-2-morpholinoethyl6-(4-hydroxy-6-methoxy-7-methyl-3-oxo-1,3-dihydroisobenzofuran-5-yl)-4-methylhex-4-enoate, is rapidly absorbed following oral administration and hydrolyzed to its active metabolite, mycophenolic acid (MPA).  It is a reversible inhibitor of inosine monophosphate dehydrogenase (IMPDH) and thus inhibits purine synthesis [1], with potent cytostatic effects on both T and B lymphocytes.  The plasma halflife of MPA is approximately 16 h.  It is used for the prophylaxis of graft rejection in kidney [2], heart [3], and liver transplantation [4], and it has also been used after transplantation of the lung [5], pancreas [6], and intestines [7].  It has also been tried for the prophylaxis of graft-versus-host disease after bone marrow transplantation [8].  Due to the clinical advantages of MMF, there has been an increase in the number of MMF formulations in the market in recent years [9].A few analytical methods namely, HPLC [10–14], LC-MS [14], spectrophotometric [15], and micellar electrokinetic chromatographic [16] have been reported for the determination of MMF in bulk, pharmaceutical formulations, and biological samples. The reported chromatographic and spectroscopic methods were found to be time consuming. This prompted us to develop a simple, rapid, and cost-effective analytical method for routine analysis.  Literature survey revealed that no electrochemical method was reported to date for the estimation of MMF in bulk drug and formulations.  In the present study, we report a simple, precise, accurate, and economically viable electrochemical method for the estimation of MMF in bulk and pharmaceutical formulations, and in biological fluids.  Statistical tests were performed for validation of data.


## 2. Experimental

### 2.1. Apparatus

Electrochemical studies were carried out on a CHI-1103a electrochemical analyzer (CH Instruments Ltd., Co., USA, version 9.03) electrode system involving a GCE (3 mm diameter) as the working electrode, a platinum wire as a counter electrode, and a saturated calomel electrode (SCE) as reference electrode.


### 2.2. Reagents

Pure MMF was obtained as a gift sample from Dr. Reddy’s Laboratories, India.  Tablets were obtained from local sources commercially. A stock solution of MMF (2.5 mM) was prepared in a mixture containing water and methanol (50 : 50) and stored in a refrigerator at 4°C.  In the present study, phosphate buffer (pH = 3.0–10.4) were used.  Millipore water was used throughout.


### 2.3. Working Procedure

For reproducible results, improved sensitivity, and good resolution of voltammetric peaks, the working electrode was polished carefully with 1.0, 0.3, and 0.05μm α-alumina on a smooth polishing cloth, and then washed in methanol.  Then, it was thoroughly rinsed with water. All the reported potentials are against saturated calomel electrode (SCE).Working solutions were prepared by diluting the stock solution as required with relevant buffer of required pH.  For DPV, the following parameters were maintained: sweep rate, 20 mV s−1, pulse amplitude, 50 mV, pulse width, 60 ms, and pulse period, 200 ms.  For analytical applications, oxidation peak a1 was selected.  All experiments were carried out at 25 ± 1°C.


### 2.4. Analysis of Tablets

Ten tablets of MMF were powdered in a mortar. A portion of the powder equivalent to 2.5 mM MMF was transferred into a 100 mL volumetric flask and completed to volume with methanol and water mixture (50 : 50). The contents of the flask were sonicated for 10 min to affect complete dissolution. Appropriate solutions were prepared by taking suitable aliquots of the clear supernatant liquid and diluting them with supporting electrolyte.  To study the accuracy of the proposed method and to check the interferences from excipients used in the dosage form, recovery experiments were carried out. The content of the drug in the tablet was determined from the calibration graph or regression equation.


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

Spiked urine samples were obtained by treating 0.9 mL aliquots of urine with 100μL MMF standard solution (2.5 mM) to obtain 250 μM MMF. A suitable amount of aliquot of spiked urine was diluted with phosphate buffer (without any pretreatment) to prepare appropriate sample solutions and differential pulse voltammograms were as recorded under optimized conditions.Serum samples, obtained from healthy individuals (after having obtained their written consent), were stored frozen until assay.  For the determination of MMF in plasma, 500μL MMF solutions (2.5 mM) were 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.  Appropriate volume of supernatant liquor was transferred in the voltammetric cell containing phosphate buffer of pH 6.0 and voltammograms were recorded.  The voltammograms of samples without MMF did not show any signal that can interfere with the direct determination.  The content of the drug in plasma/spiked urine sample 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) electrode system involving a GCE (3 mm diameter) as the working electrode, a platinum wire as a counter electrode, and a saturated calomel electrode (SCE) as reference electrode.


## 2.2. Reagents

Pure MMF was obtained as a gift sample from Dr. Reddy’s Laboratories, India.  Tablets were obtained from local sources commercially. A stock solution of MMF (2.5 mM) was prepared in a mixture containing water and methanol (50 : 50) and stored in a refrigerator at 4°C.  In the present study, phosphate buffer (pH = 3.0–10.4) were used.  Millipore water was used throughout.


## 2.3. Working Procedure

For reproducible results, improved sensitivity, and good resolution of voltammetric peaks, the working electrode was polished carefully with 1.0, 0.3, and 0.05μm α-alumina on a smooth polishing cloth, and then washed in methanol.  Then, it was thoroughly rinsed with water. All the reported potentials are against saturated calomel electrode (SCE).Working solutions were prepared by diluting the stock solution as required with relevant buffer of required pH.  For DPV, the following parameters were maintained: sweep rate, 20 mV s−1, pulse amplitude, 50 mV, pulse width, 60 ms, and pulse period, 200 ms.  For analytical applications, oxidation peak a1 was selected.  All experiments were carried out at 25 ± 1°C.


## 2.4. Analysis of Tablets

Ten tablets of MMF were powdered in a mortar. A portion of the powder equivalent to 2.5 mM MMF was transferred into a 100 mL volumetric flask and completed to volume with methanol and water mixture (50 : 50). The contents of the flask were sonicated for 10 min to affect complete dissolution. Appropriate solutions were prepared by taking suitable aliquots of the clear supernatant liquid and diluting them with supporting electrolyte.  To study the accuracy of the proposed method and to check the interferences from excipients used in the dosage form, recovery experiments were carried out. The content of the drug in the tablet was determined from the calibration graph or regression equation.


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

Spiked urine samples were obtained by treating 0.9 mL aliquots of urine with 100μL MMF standard solution (2.5 mM) to obtain 250 μM MMF. A suitable amount of aliquot of spiked urine was diluted with phosphate buffer (without any pretreatment) to prepare appropriate sample solutions and differential pulse voltammograms were as recorded under optimized conditions.Serum samples, obtained from healthy individuals (after having obtained their written consent), were stored frozen until assay.  For the determination of MMF in plasma, 500μL MMF solutions (2.5 mM) were 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.  Appropriate volume of supernatant liquor was transferred in the voltammetric cell containing phosphate buffer of pH 6.0 and voltammograms were recorded.  The voltammograms of samples without MMF did not show any signal that can interfere with the direct determination.  The content of the drug in plasma/spiked urine sample was determined referring to the calibration graph or regression equation.


## 3. Results and Discussion

### 3.1. Electro-Oxidation of MMF

The structure of MMF is shown in Figure1. Cyclic voltammogram of 1.25 × 10−4 M MMF in phosphate buffer of pH 6.0 at a sweep rate of 100 mV s−1 exhibited two anodic peaks at 0.631 V with a peak current of 7.868 μA and at 0.921 V with a peak current of 7.292 μA, respectively.  No peak was observed in the reverse scan suggesting that the oxidation process was irreversible in nature.  The multisweep cyclic voltammograms of MMF in phosphate buffer of pH 6.0 at the scan rate of 100 mV s−1 are shown in Figure 2. The significant decrease in peak current was noticed upon successive cyclic voltammetric sweeps.  This phenomenon might be attributed to the fouling of the electrode surface due to adsorption of MMF or its oxidation product on the electrode surface [17]. To check the adsorption characteristics and to examine the reversibility of the first peak, another experiment was carried out by reversing the cycle in the potential range of 0.2–0.8 V. But, we did not notice any peak in the reverse scan indicating the irreversibility of the first peak. Further, the peak currents were found to decrease in successive cycles thereby revealing the adsorption of the oxidized product on the electrode surface.  Therefore, the voltammograms corresponding to the first cycle were considered. Among two anodic peaks a1 and a2, peak a1 was considered for further investigation as it was sharper and well defined with higher peak current.Figure 1
Structure of MMF.Figure 2
Multisweep cyclic voltammograms of 1.25 × 10−4 M MMF in phosphate buffer of 6.0 pH at a scan rate 100 mV s−1.


### 3.2. Effect of pH

Electro oxidation of 1.25 × 10−4 M MMF was studied in phosphate buffer in the pH range of 3.0–10.0 by cyclic voltammetry (Figure 3). The potential of peak a1 was noticed to be shifted to less positive values up to pH 7.0 and then became almost pH independent (Figure 3) with weak and ill-defined peaks, beyond pH 7.0. Basically, two linear regions were obtained; one in the pH range of 3.0–7.0 with a slope of 56 mV/pH suggesting the number of electrons to be equal to that of protons taking part in the electrode reaction [18] and another one in the pH range of 7.0–10.0 with a slope of 8.1 mV/pH. The intersection of these lines was located around pH 8 which is close to the pKa value of 8.5 for phenolic moiety of MMF [19]. The first trend noticed could be due to the oxidation of deprotonated form of MMF. A prewave was observed on more basic pH. This was attributed to formation of aldehyde from alcohol side chain [20] which in turn was formed due to the cleavage of the lactone ring.  Further, highest peak intensity (for peak a1) was noticed at pH 6.0 and then decreased continuously with further increase in pH. Hence, phosphate buffer of pH 6.0 was selected as the supporting electrolyte for further studies.Figure 3
Cyclic voltammograms of 1.25 × 10−4 M MMF in phosphate buffers of different pH at a scan rate of 100 mV s−1.


### 3.3. Effect of Scan Rate

The effect of scan rate on electrooxidation of 1.25 × 10−4 M MMF in the range of 10–800 mV s−1was examined in phosphate buffer of pH 6.0 by cyclic voltammetry (Figure 4).  The plot of the peak current versusvalues of square root of scan rate (10–350 mV s−1) revealed a linear relationship (r2 = 0.9912) indicating  the electrooxidation to be a diffusion-controlled process [21] and the same can be represented using the equation shown below:(1)ipa(μA)=0.548ν1/2(mVs-1)-0.431.
Therefore, we propose that the electrooxidation of MMF is solution process in the scan rate range of 10–350 mV s−1 while it is surface process in the scan rate range of 400–800 mV s−1.Figure 4
Cyclic voltammograms of 1.25 × 10−4 M MMF in phosphate buffer of pH 6.0 on GCE at different scan rates: (1) 10, (2) 20, (3) 40, (4) 60, (5) 80, (6) 100, (7) 200, (8) 300, (9) 400, (10) 500, (11) 600, (12) 700, and (13) 800 mV s−1. Insert: peak current versus square root of scan rate in the scan rate range 10–350 mV s−1.The peak potential was found to be linearly shifted to more positive values with increase in scan rate.  A linear Randles-Seveik plot (ip versus ν) was obtained (figure not shown) in the scan rate of 400–800 mV s−1 (r2 = 0.9904) according to the equation: (2)ipa(μA)=0.021ν(mVs-1)+2.706,
indicating that the electrochemical behaviour of MMF on GCE seems limited by adsorption [22].  Linear relationship was observed between Epa and scan rate was observed with a correlation coefficient of 0.9887 according to the equation shown below: (3)Epa(mV)=0.091ν(mVs-1)+620.310.


### 3.4. Electrochemical Oxidation Mechanism

The first oxidation peak noticed in MMF could be attributed to oxidation occurring at phenolic –OH which is similar to that observed in vanillylmandelic acid [23] and salbutamol [24] followed by a nucleophilic attack at the para position to OH group by either water molecule or methanol.  The second oxidation peak observed was attributed to oxidation of enolic –OH group. The above mechanism was proposed based on the plot of Ep versus pH which gave a slope of 56 mV/pH indicating the participation of equal number of electrons and protons in electrooxidation process [18]. A probable reaction mechanism for the oxidation of MMF is shown in Scheme 1.  In order to confirm this, bulk electrolysis was performed using working electrode of high surface area for 6 h at a fixed potential of 1.2 V. For this, an initial overall concentration of 1 mM MMF was maintained in 40 mL of phosphate buffer solution. The charge passed was 1.150 × 10−1C, and the end current was −1.004 × 10−5 A.  The products were isolated and subjected to mass spectral analysis which showed three peaks at m/z values of 334, 320, and 302, respectively, corresponding to the fragmentation peaks of oxidation products of MMF  namely, a, b, and c, respectively (Scheme 1).Scheme 1
Probable oxidation pathway for the electrochemical oxidation of MMF.


### 3.5. Analytical Features

Differential pulse voltammetric technique provides higher sensitivity and better peak resolution compared to cyclic voltammetry for studying the electrochemical behavior of electroactive compounds. Therefore, we used this technique for the determination of MMF. The differential pulse voltammogram of MMF at different concentrations in phosphate buffer of pH 6.0 at GCE are shown in Figure5. Under the optimized conditions, the calibration graph for MMF showed the linearity in the concentration range of 1.5 × 10−7–7.5 × 10−4 M.  The characteristics of calibration graph are recorded in Table 1. Validation of the procedure for quantitative determination of MMF was examined via evaluation of the limit of detection (LOD) and limit of quantification (LOQ). The LOD and LOQ values were calculated using the equations shown below:(4)LOD=3sm,LOQ=10sm,
where s is the standard deviation of the peak currents (five runs) and m is the slope of the calibration curve [25].  LOD and LOQ were found to be 1.48 × 10−7 and 4.94 × 10−7 M, respectively.  The repeatability of the current measurement was calculated from five independent runs of 1.25 × 10−4 M MMF solution. The RSD values for Interday assay and intraday assay were calculated.  The corresponding values shown in Table 1 indicated good reproducibility of the results.Table 1
Characteristics of calibration plot of MMF.
DPVLinearity range (μM)0.5–750LOD (μM)0.148LOQ (μM)0.494Interday assay RSD* (%)1.51Intraday assay RSD* (%)1.24*Average of 5 determinations.Figure 5
Differential pulse voltammogram of MMF at different concentrations:  (1) 0.5, (2) 2.5, (3) 10, (4) 25, (5) 50, (6) 100, (7) 150, (8) 300, (9) 400, (10) 500, (11) 600, and (12) 750μM. Insert: calibration plot for the determination of MMF.


### 3.6. Effects of Interferents

The selectivity of the proposed method was investigated by studying the effects of interferents, namely, glucose, magnesium stearate, starch, acacia powder, ascorbic acid, and talc on electrochemical determination of MMF.  For this, we have recorded differential pulse voltammogram of 20 μM MMF in presence of different concentrations of interferents. The results of effects of interferents on peak current of MMF are shown in Table 2.  It was noticed that the ascorbic acid, magnesium stearate, and starch did not interfere up to 10-fold excess while glucose, talc, and acacia powder exerted no effect up to 20-fold excess. Therefore, the proposed method offers good selectivity for the determination of MMF.Table 2
Effects of interferents on differential pulse voltammetric response of 20μM MMF at GCE.
InterferentConcentration (μM)Current (μA)Signal change (μA)RSD* (%)MMF                   (no interferent)200.610——Ascorbic acid2000.596−0.0141.91Glucose4000.618+0.0081.57Magnesium stearate2000.619+0.0091.55Talc4000.605−0.0051.46Acacia powder4000.607−0.0032.05Starch2000.603−0.0071.65*Average of 5 determinations.


### 3.7. Pharmaceutical Applications (Tablet Analysis)

The developed DPV method was applied successfully for the assay of MMF in tablets.  The results of analysis of MMF recorded in Table3 were found to be satisfactory.  Further, recovery studies were carried out by standard addition method.  For this, known quantities of pure MMF were mixed with definite amounts of preanalyzed formulations and the mixtures were analyzed as before.  The total amount of the drug was then determined, and the amount of the added drug was calculated by difference.  The average percent recoveries obtained were found to be quantitative indicating good recovery of the drug (Table 3).Table 3
Results of analysis of MMF in pharmaceutical samples.
TabletBaxmuneaMyceptbLabeled claim (mg)500500Amount found (mg)494490Recovery (%)98.898.0RSDc (%)1.741.89Pure MMF added to tablet solution (mg)2020Amount found (mg)19.7520.20Recovery (%)98.75101.0RSDc (%)1.321.29aMarketed by Ranbaxy laboratories.bMarketed by Panacea biotec.cAverage of 6 determinations.


### 3.8. Determination of MMF in Urine and Plasma Samples

The practical analytical application of the method was further established by determining MMF in human urine samples without any preliminary treatment.  The recoveries from urine samples were examined by spiking drug-free urine with known amounts of MMF.  The calibration graph was used to determine the concentration of MMF in urine samples.  The results of analysis are listed in   Table4.  The average recovery was observed to be higher than 99.5% and the RSD values were less than 2.1%.  These values indicated good recovery and reproducibility of the results.Table 4
Results of analysis of MMF in spiked urine and serum samples.
MMF added (μM)nAmount found (μM)Average recovery (%)RSD (%)Urine samples544.9899.601.681049.9599.501.2220420.04100.021.8340439.9099.752.13Serum samples544.9398.602.201049.6896.802.2920419.2896.402.9840439.0997.722.08The applicability of the proposed method was further examined by analyzing MMF in plasma samples employing GCE.  Serum samples were spiked with known amounts of MMF and further diluted with supporting electrolyte.  The amount of MMF in serum samples was determined by referring to the calibration plot.  The results incorporated in Table4 indicated good recovery of MMF.


## 3.1. Electro-Oxidation of MMF

The structure of MMF is shown in Figure1. Cyclic voltammogram of 1.25 × 10−4 M MMF in phosphate buffer of pH 6.0 at a sweep rate of 100 mV s−1 exhibited two anodic peaks at 0.631 V with a peak current of 7.868 μA and at 0.921 V with a peak current of 7.292 μA, respectively.  No peak was observed in the reverse scan suggesting that the oxidation process was irreversible in nature.  The multisweep cyclic voltammograms of MMF in phosphate buffer of pH 6.0 at the scan rate of 100 mV s−1 are shown in Figure 2. The significant decrease in peak current was noticed upon successive cyclic voltammetric sweeps.  This phenomenon might be attributed to the fouling of the electrode surface due to adsorption of MMF or its oxidation product on the electrode surface [17]. To check the adsorption characteristics and to examine the reversibility of the first peak, another experiment was carried out by reversing the cycle in the potential range of 0.2–0.8 V. But, we did not notice any peak in the reverse scan indicating the irreversibility of the first peak. Further, the peak currents were found to decrease in successive cycles thereby revealing the adsorption of the oxidized product on the electrode surface.  Therefore, the voltammograms corresponding to the first cycle were considered. Among two anodic peaks a1 and a2, peak a1 was considered for further investigation as it was sharper and well defined with higher peak current.Figure 1
Structure of MMF.Figure 2
Multisweep cyclic voltammograms of 1.25 × 10−4 M MMF in phosphate buffer of 6.0 pH at a scan rate 100 mV s−1.


## 3.2. Effect of pH

Electro oxidation of 1.25 × 10−4 M MMF was studied in phosphate buffer in the pH range of 3.0–10.0 by cyclic voltammetry (Figure 3). The potential of peak a1 was noticed to be shifted to less positive values up to pH 7.0 and then became almost pH independent (Figure 3) with weak and ill-defined peaks, beyond pH 7.0. Basically, two linear regions were obtained; one in the pH range of 3.0–7.0 with a slope of 56 mV/pH suggesting the number of electrons to be equal to that of protons taking part in the electrode reaction [18] and another one in the pH range of 7.0–10.0 with a slope of 8.1 mV/pH. The intersection of these lines was located around pH 8 which is close to the pKa value of 8.5 for phenolic moiety of MMF [19]. The first trend noticed could be due to the oxidation of deprotonated form of MMF. A prewave was observed on more basic pH. This was attributed to formation of aldehyde from alcohol side chain [20] which in turn was formed due to the cleavage of the lactone ring.  Further, highest peak intensity (for peak a1) was noticed at pH 6.0 and then decreased continuously with further increase in pH. Hence, phosphate buffer of pH 6.0 was selected as the supporting electrolyte for further studies.Figure 3
Cyclic voltammograms of 1.25 × 10−4 M MMF in phosphate buffers of different pH at a scan rate of 100 mV s−1.


## 3.3. Effect of Scan Rate

The effect of scan rate on electrooxidation of 1.25 × 10−4 M MMF in the range of 10–800 mV s−1was examined in phosphate buffer of pH 6.0 by cyclic voltammetry (Figure 4).  The plot of the peak current versusvalues of square root of scan rate (10–350 mV s−1) revealed a linear relationship (r2 = 0.9912) indicating  the electrooxidation to be a diffusion-controlled process [21] and the same can be represented using the equation shown below:(1)ipa(μA)=0.548ν1/2(mVs-1)-0.431.
Therefore, we propose that the electrooxidation of MMF is solution process in the scan rate range of 10–350 mV s−1 while it is surface process in the scan rate range of 400–800 mV s−1.Figure 4
Cyclic voltammograms of 1.25 × 10−4 M MMF in phosphate buffer of pH 6.0 on GCE at different scan rates: (1) 10, (2) 20, (3) 40, (4) 60, (5) 80, (6) 100, (7) 200, (8) 300, (9) 400, (10) 500, (11) 600, (12) 700, and (13) 800 mV s−1. Insert: peak current versus square root of scan rate in the scan rate range 10–350 mV s−1.The peak potential was found to be linearly shifted to more positive values with increase in scan rate.  A linear Randles-Seveik plot (ip versus ν) was obtained (figure not shown) in the scan rate of 400–800 mV s−1 (r2 = 0.9904) according to the equation: (2)ipa(μA)=0.021ν(mVs-1)+2.706,
indicating that the electrochemical behaviour of MMF on GCE seems limited by adsorption [22].  Linear relationship was observed between Epa and scan rate was observed with a correlation coefficient of 0.9887 according to the equation shown below: (3)Epa(mV)=0.091ν(mVs-1)+620.310.


## 3.4. Electrochemical Oxidation Mechanism

The first oxidation peak noticed in MMF could be attributed to oxidation occurring at phenolic –OH which is similar to that observed in vanillylmandelic acid [23] and salbutamol [24] followed by a nucleophilic attack at the para position to OH group by either water molecule or methanol.  The second oxidation peak observed was attributed to oxidation of enolic –OH group. The above mechanism was proposed based on the plot of Ep versus pH which gave a slope of 56 mV/pH indicating the participation of equal number of electrons and protons in electrooxidation process [18]. A probable reaction mechanism for the oxidation of MMF is shown in Scheme 1.  In order to confirm this, bulk electrolysis was performed using working electrode of high surface area for 6 h at a fixed potential of 1.2 V. For this, an initial overall concentration of 1 mM MMF was maintained in 40 mL of phosphate buffer solution. The charge passed was 1.150 × 10−1C, and the end current was −1.004 × 10−5 A.  The products were isolated and subjected to mass spectral analysis which showed three peaks at m/z values of 334, 320, and 302, respectively, corresponding to the fragmentation peaks of oxidation products of MMF  namely, a, b, and c, respectively (Scheme 1).Scheme 1
Probable oxidation pathway for the electrochemical oxidation of MMF.


## 3.5. Analytical Features

Differential pulse voltammetric technique provides higher sensitivity and better peak resolution compared to cyclic voltammetry for studying the electrochemical behavior of electroactive compounds. Therefore, we used this technique for the determination of MMF. The differential pulse voltammogram of MMF at different concentrations in phosphate buffer of pH 6.0 at GCE are shown in Figure5. Under the optimized conditions, the calibration graph for MMF showed the linearity in the concentration range of 1.5 × 10−7–7.5 × 10−4 M.  The characteristics of calibration graph are recorded in Table 1. Validation of the procedure for quantitative determination of MMF was examined via evaluation of the limit of detection (LOD) and limit of quantification (LOQ). The LOD and LOQ values were calculated using the equations shown below:(4)LOD=3sm,LOQ=10sm,
where s is the standard deviation of the peak currents (five runs) and m is the slope of the calibration curve [25].  LOD and LOQ were found to be 1.48 × 10−7 and 4.94 × 10−7 M, respectively.  The repeatability of the current measurement was calculated from five independent runs of 1.25 × 10−4 M MMF solution. The RSD values for Interday assay and intraday assay were calculated.  The corresponding values shown in Table 1 indicated good reproducibility of the results.Table 1
Characteristics of calibration plot of MMF.
DPVLinearity range (μM)0.5–750LOD (μM)0.148LOQ (μM)0.494Interday assay RSD* (%)1.51Intraday assay RSD* (%)1.24*Average of 5 determinations.Figure 5
Differential pulse voltammogram of MMF at different concentrations:  (1) 0.5, (2) 2.5, (3) 10, (4) 25, (5) 50, (6) 100, (7) 150, (8) 300, (9) 400, (10) 500, (11) 600, and (12) 750μM. Insert: calibration plot for the determination of MMF.


## 3.6. Effects of Interferents

The selectivity of the proposed method was investigated by studying the effects of interferents, namely, glucose, magnesium stearate, starch, acacia powder, ascorbic acid, and talc on electrochemical determination of MMF.  For this, we have recorded differential pulse voltammogram of 20 μM MMF in presence of different concentrations of interferents. The results of effects of interferents on peak current of MMF are shown in Table 2.  It was noticed that the ascorbic acid, magnesium stearate, and starch did not interfere up to 10-fold excess while glucose, talc, and acacia powder exerted no effect up to 20-fold excess. Therefore, the proposed method offers good selectivity for the determination of MMF.Table 2
Effects of interferents on differential pulse voltammetric response of 20μM MMF at GCE.
InterferentConcentration (μM)Current (μA)Signal change (μA)RSD* (%)MMF                   (no interferent)200.610——Ascorbic acid2000.596−0.0141.91Glucose4000.618+0.0081.57Magnesium stearate2000.619+0.0091.55Talc4000.605−0.0051.46Acacia powder4000.607−0.0032.05Starch2000.603−0.0071.65*Average of 5 determinations.


## 3.7. Pharmaceutical Applications (Tablet Analysis)

The developed DPV method was applied successfully for the assay of MMF in tablets.  The results of analysis of MMF recorded in Table3 were found to be satisfactory.  Further, recovery studies were carried out by standard addition method.  For this, known quantities of pure MMF were mixed with definite amounts of preanalyzed formulations and the mixtures were analyzed as before.  The total amount of the drug was then determined, and the amount of the added drug was calculated by difference.  The average percent recoveries obtained were found to be quantitative indicating good recovery of the drug (Table 3).Table 3
Results of analysis of MMF in pharmaceutical samples.
TabletBaxmuneaMyceptbLabeled claim (mg)500500Amount found (mg)494490Recovery (%)98.898.0RSDc (%)1.741.89Pure MMF added to tablet solution (mg)2020Amount found (mg)19.7520.20Recovery (%)98.75101.0RSDc (%)1.321.29aMarketed by Ranbaxy laboratories.bMarketed by Panacea biotec.cAverage of 6 determinations.


## 3.8. Determination of MMF in Urine and Plasma Samples

The practical analytical application of the method was further established by determining MMF in human urine samples without any preliminary treatment.  The recoveries from urine samples were examined by spiking drug-free urine with known amounts of MMF.  The calibration graph was used to determine the concentration of MMF in urine samples.  The results of analysis are listed in   Table4.  The average recovery was observed to be higher than 99.5% and the RSD values were less than 2.1%.  These values indicated good recovery and reproducibility of the results.Table 4
Results of analysis of MMF in spiked urine and serum samples.
MMF added (μM)nAmount found (μM)Average recovery (%)RSD (%)Urine samples544.9899.601.681049.9599.501.2220420.04100.021.8340439.9099.752.13Serum samples544.9398.602.201049.6896.802.2920419.2896.402.9840439.0997.722.08The applicability of the proposed method was further examined by analyzing MMF in plasma samples employing GCE.  Serum samples were spiked with known amounts of MMF and further diluted with supporting electrolyte.  The amount of MMF in serum samples was determined by referring to the calibration plot.  The results incorporated in Table4 indicated good recovery of MMF.


## 4. Conclusions

The electrochemical behavior of MMF at GCE was investigated for the first time. MMF was found to undergo oxidation irreversibly in phosphate buffer of pH 6.0. The proposed differential pulse voltammetric procedure was employed successfully to determine MMF in tablets and biological samples. Since, the method is simple, fast, and inexpensive, it could be readily adopted in clinical and quality control laboratories.



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*Source: 193041-2011-10-10.xml*