Beirut Arab University, Faculty of Pharmacy, Department of Pharmaceutical Technology
Email: marwa.jamal@bau.edu.lb
Received: 26 Sep 2019, Revised and Accepted: 15 Jan 2020
ABSTRAC
Objective: Development and validation of a sensitive, indirect spectrophotometric kinetic method, based on oxidationreduction reaction, using potassium permanganate, for the quantitative assay of pitavastatin calcium, a cardiovascular drug used for the treatment of hyperlipidemia.
Methods: The developed spectrophotometric kinetic method is based on the ability of potassium permanganate to oxidize Pitavastatin, where, the drug solution is treated with a fixed concentration of permanganate in acidic medium, and after a specified time, the unreacted permanganate is measured at 525 nm. All variables affecting the color development have been investigated and the conditions were optimized. Different kinetic methods, including initial rate, rate constant, fixed time and fixed concentration, were applied for the determination Pitavastatin.
Results: During the course of the reaction, the absorbance values, at 525 nm, related to KMnO_{4,} decreased linearly with increasing the concentration of the drug. The reaction rate obeyed was found to be pseudofirstorder and the kinetic method used was the fixedtime method. The assay of PITA in the concentration range of 1680 μg/ml, using the fixed time method was successfully determined with a correlation coefficient value of 0.9999. The applicability of the developed method was also demonstrated by the determination of pitavastatin in its pure form and in its pharmaceutical formulation, where, the effect of excipients has also been studied and found to have no effect.
Conclusion: The developed indirect spectrophotometric kinetic method, using the fixed time method, was used for the determination of Pitavastatin in pharmaceutical tablets. This method was simple, accurate and easy to apply for routine assay and in quality control laboratories.
Keywords: Pitavastatin Calcium, Potassium Permanganate, Oxidation, Kinetic methods and Spectrophotometry
© 2020 The Authors. Published by Innovare Academic Sciences Pvt Ltd. This is an open access article under the CC BY license (http://creativecommons.org/licenses/by/4.0/)
DOI: http://dx.doi.org/10.22159/ijpps.2020v12i3.35888. Journal homepage: https://innovareacademics.in/journals/index.php/ijpps
INTRODUCTION
The kinetic spectrophotometric method is an analytical method in which the rate of a reaction is measured and utilized to determine the concentration of drugs [1]. The application of kinetic methods of chemical analysis has gained increasing importance because of their high selectivity and sensitivity. In order to determine the amount of substance being analyzed in solution, it is necessary to measure the rate of decrease of increase of substance concentration. By applying the isolation method, the concentration of one of the substances (indicator substance) changes in the course of the reaction, and the concentration of the remaining substances either do not change or its change is negligible [2]. Various kinetic methods have been applied for the determination of many pharmaceutical formulations [3–7]. Potassium permanganate, a strong oxidizing agent, has been used in an oxidimetric analytical method for the determination of many compounds [8–13].
Pitavastatin Calcium (PIT), chemically known as (3R,5S,6E)7[2cyclopropyl4(4fluorophenyl) quinolin3yl]3,5dihydroxyhept6enoic acid (fig. 1), is a coenzyme A (HMGCoA) reductase inhibitors (statins) that inhibits the synthesis of mevalonate, a ratelimiting step in cholesterol level. Competitive inhibition of HMGCoA reductase by the statins decreases hepatocyte cholesterol synthesis, which results in increase extraction of LDLC from the blood and decreases circulating LDLC concentrations [14].
Fig. 1: Pitavastatin calcium
PIT has been determined in its pharmaceutical dosage form by simple spectrophotometric analysis [15–18], titrimetric analysis [19] and liquid chromatographic analysis [20–22]. Degradation pathway for PIT has been developed using LC/MS method [23], or UPLC method [24], also photostability of PIT has been studied [25], In many biological fluids, PIT has been assayed by LC/MS in human plasma [26], urine [27].
Screening the literature, no kinetic method has been reported for the determination of PITA in pharmaceutical preparations. In the present work, a simple and reliable kinetically based spectrophotometric method is proposed for the determination of PITA in its pharmaceutical dosage form Livazo^{®}. The proposed method depends on the oxidation of the drug with potassium permanganate, where the A value of the excess unused permanganate is measured at 525 nm. The applied kinetic methods were validated according to ICH guidelines [28]. The results obtained were compared with those obtained by the RPHPLC method [29], using the ttest and Ftest [30].
MATERIALS AND METHODS
Apparatus
Spectrophotometer
The spectrophotometric measurements were carried out on a Jasco V530 double beam UVVis Spectrophotometer connected to a computer loaded with Jasco UVPC software and an HP Deskjet 5652 printer. The absorption spectra were measured using 1 cm quartz cells. The absorption spectra were recorded on the same spectrophotometer, with 1 cm quartz cells and supported with Jasco Spectra Manager software for GULLIVER Ver. 1.53, and the same printer.
Chemicals
PIT supplied by AlgorithmLebanon was used as a working standard. An acetic acid solution obtained from SIGMAALDRICH was used as solvents for the preparation of the standard solutions. KMnO_{4} was supplied by Fluka. The pharmaceutical preparation Livazo^{®} was obtained from AlgorithmLebanon.
Preparation of standard solutions
Standard stock solutions
PIT standard stock solution (0.16 mg/ml) was prepared by accurately transferring 16 mg into the 100ml volumetric flask using 3:2, v/v acetic acid as solvent.
KMnO_{4} standard solution (0.01 mole/l) was prepared by accurately transferring 158 mg into a 100ml volumetric flask. The powdered was dissolved and diluted to the mark with distilled water.
Calibration graph
Accurate volumes of PIT standard stock solution were transferred into five separate 10ml volumetric flasks. To each flask, 0.5 ml KMnO_{4} were added, the flasks were diluted to the mark with water to obtain a calibration set in the range of 1680 µg/ml. The prepared flasks were kept aside at room temperature, for 30 min. The absorbance values were measured at 525 nm using blank solutions prepared simultaneously. The corresponding regression equation, relating final concentration versus corresponding absorbance values was derived.
Tablet assay
Accurately ten tablets of Livazo 4 mg ^{®} were separately weighed and powdered. Accurate weight equivalent to 16 mg PIT of the finely powdered tablets, were transferred into the 100ml calibrated flask, 50 ml 3:2, v/v acetic acid was added and the flask was shaken for 15 min, filtered and completed to volume with 3:2, v/v acetic acid. 2ml of the prepared solution were transferred into 10ml calibrated flask, 0.5 ml, 0.01 mol/l KMnO_{4} was added and the resulting solution was mixed and diluted to volume with water. The prepared tablet solution containing 32 μg/ml PIT was put aside for 30 min to allow enough time for the oxidation reaction to occur and the absorbance value was measured at 525 nm against a blank solution prepared similarly.
RESULTS AND DISCUSSION
The absorption spectrum of aqueous potassium permanganate solution in acidic medium exhibited an absorption band at 525 nm. The addition of the studied drug, PIT, to this solution produces a decrease in the intensity of this absorption band (fig. 2). This decrease in the absorption intensity is due to the oxidation of the drug by potassium permanganate in acidic medium, where potassium permanganate is consumed by the drug and is transformed into colorless manganese ions. Since the intensity of permanganate pink color decreases with time; therefore a kinetically based method was developed for the determination of PIT in its pharmaceutical formulation.
Conditions optimization
The various experimental factors affecting the development and stability of the reaction product were studied and optimized. Such factors that were changed individually, include the concentration of the reagents (KMnO4 and acetic acid), temperature and time.
Effect of KMnO_{4} concentration
Potassium permanganate oxidizes PIT in the presence of acetic acid, where it is reduced into colorless manganese ions. Preliminary experiments were performed to determine the optimal KMnO_{4} concentration, it was found that the use of 5x10^{4} mol/l gave optimum absorbance values at 525 nm. Thus, when permanganate was reacted with increasing concentrations of PIT in acetic acid medium, there occurred a concomitant fall in the concentration of permanganate as is shown by the decreasing absorbance values (fig. 2). This decrease was proportional to the concentrations of PIT in the calibration graphs.
Fig. 2: Absorption spectrum of 5x10^{4} mol/l KMnO_{4}, 1680 μg/mlof PIT with 5x10^{4} mol/lKMnO_{4}, at room T, for 30 min
Fig. 3: Effect of volume of 3:2, v/v acetic acid on the absorbance of the reaction product of 32 μg/ml of PIT with 0.5 ml, 0.01 mol/l KMnO_{4} at 525 nm
Fig. 3: Absorbancetime curve for the reaction of PIT (1680 μg/ml) with KMnO_{4} in acidic medium
Effect of acetic acid concentration
To investigate the effect of acetic acid concentration on the reaction, 1.06.0 ml of 3:2, v/v acetic acid were added to a fixed concentration of PIT (32 μg/ml) and KMnO_{4} (5x10^{4} mol/l). After 30 min, it was observed that constant absorbance readings were obtained when different volumes of 3:2, v/v acetic acid was used (fig. 3). Hence, acetic acid concentration does not have any effect on the reaction pathway and its volume was maintained constant in all the flasks of the calibration graphs.
Effect of time
The effect of time was also studied, where the reaction was found to be complete and quantitative when the mixture was allowed to stand for 30 min, beyond this standing time and up to 40 min, the absorbance values remained constant (fig. 3).
Effect of temperature
The effect of temperature was also studied and it was found that providing heat to the mixture resulted in the loss of the pink color of permanganate where manganese dioxide brown precipitate appeared. Thus, room T has been chosen as the optimal temperature for the assay of PIT.
Evaluation of the kinetic methods
The quantitative determination of PIT under the optimized experimental conditions outlined above would result in a pseudofirstorder reaction with respect to PIT concentration where the rate will be directly proportional to drug concentration in a pseudofirstorder rate equation as follows:
Rate = Kˊ [C]^{n}………… (eq. 1)
Where Kˊ is the rate constant and n is the order of reaction
Eq. (1) was the basis for several experiments, which were carried out to obtain drug concentration. The rate constant, fixedconcentration, and fixed time methods [2], were tried and the most suitable analytical method was selected taking into account the applicability, the sensitivity, the correlation coefficient (r), and the intercept.
Taking logarithms of rates and concentrations, the above equation becomes:
Log (rate) = log = log kˊ+n log [C]………. (eq. 2)
Where A is the absorbance, t is the time in seconds and K is the pseudofirstorder rate constant.
From the absorbancetime plot, for different PIT concentration (fig. 3), the reaction rate may be estimated by the variabletime method, measured as , where A is the absorbance and t is the time in seconds. Regression of log (rate) versus log [C] gave the regression equations:
Log (rate) =2.46+1.10 log C (fig. 4)
With a correlation coefficient (r) = 0.990 and with, kˊ = 3.46 x10^{3} s^{1} and the order of reaction is first order (n ~1).
It can be concluded that the quantitative determination of PIT under the optimized experimental conditions outlined above would result in a pseudofirstorder reaction with respect to PIT concentration where the rate will be directly proportional to drug concentration in a pseudofirstorder rate equation (fig. 4).
Fig. 4: Log rate versus log C of PIT
Rateconstant method
Graphs of Log (Absorbance) versus time, over the concentration range of (1.65 x10^{5}8.24 x10^{5} mole/l/) (fig. 5), were plotted and all appeared to be rectilinear. The obtained graphs were used to calculate the firstorder rate constants corresponding to different PIT concentrations. These constants were calculated from the slopes multiplied by (2.303) and are presented in table 1.
Regression of [C] versus kˊ gave the equation:
kˊ=0.056+118.86 C r = 0.835
The value of the correlation coefficient (r) indicates poor linearity, which is probably due to changes in the rate constant (kˊ)
Initial rate method
The initial rate of the reaction was determined from the absorbancetime plots (fig. 3), by measuring the slopes of the initial tangents to the absorbancetime curves at different concentrations of the investigated drugs. The values of the calculated slopes are summarized in table 2.
Regression of the initial rate between two and ten minutes versus [C] gave the equations:
υ = ΔA/Δt =0.00017+101.7 C, r = 0.995 for PIT, kˊ= 101.7 min^{1}
The values of the correlation coefficients (r) indicate poor linearity, the high wale of the rate constant Kˊ indicates that the first step is too fast and not rate determining.
Fig. 5: Values of kˊ, calculated from the slopes of log A versus time graphs multiplied by (2.303), four different concentrations of PIT
Table 1: These constants were calculated from the slopes multiplied by (2.303) and are presented
Drug  Kˊ(s^{1)}  C, [mol/l] 
PIT  0.0562  1.647 x10^{5} 
0.0488  3.294 x10^{5}  
0.0491  4.941 x10^{5}  
0.0477  6.588 x10^{5}  
0.0470  8.235x10^{5} 
Table 2: Values of slopes calculated for different concentrations of PIT at room T with 0.5 ml 0.01 mol/l potassium permanganate
Drug  C, mol/l  Slope, s^{1} 
PIT  1.647 x10^{5}  0.00579 
3.294 x10^{5}  0.00853  
4.941 x10^{5}  0.01177  
6.588 x10^{5}  0.01487  
8.235x10^{5}  0.01760 
Fixed concentration method
The kinetic study of PIT was followed up at different concentration levels by recording the time in seconds required for the absorbance to reach a preselected value. This preselected value was chosen as it gave the widest calibration range. The reciprocals of time (1/Δt) were plotted versus the initial concentration of the PIT and the equations of calibration graphs are given in table 3. The values of the correlation coefficients indicate poor linearity, which is considered a disadvantage.
Table 3: Value of (1/Δt) taken at fixed absorbance^{*} for different concentrations of PIT at room T with 0.5 ml, 0.01 mol/l potassium permanganate
Drug  Δt (min)  1/Δt(s^{1})  C, mol/l  Regression equation  Regression coefficient (r) 
PIT  15.00  0.00111  1.647 x10^{5}  1/Δt = 0.000751+11.79 C  r = 0.960 
13.30  0.00125  3.294 x10^{5}  
12.00  0.00139  4.941 x10^{5}  
10.90  0.0153  6.588 x10^{5}  
10.00  0.0167  8.235x10^{5} 
*The preselected absorbance values for PIT is 0.2
Fixed time method
Reaction rates were determined for different concentrations of PIT at a preselected fixedtime. Calibration graphs of absorbance versus concentration of PIT were established at fixed times of 15, 20, 30 and 40 min in the concentration range of 1.647 x10^{5}8.235x10^{5} mol/l (1680 μg/ml). The calculated regression equations are assembled at table 4. It is clear at 15 min the value of the correlation coefficient is poor and that indicates that the kinetic reaction did not reach stability. However, at 20 min the slopes increase with time and the most suitable values for the correlation coefficient (r) and the intercept (a) were obtained for a fixedtimes of 30 min (table 4). This was therefore chosen as the most suitable time interval for measurement.
Table 4: Regression equations at different fixed times for PIT at 15, 20, 30 and 40 min in the concentration range of 1.647 x10^{5}8.235x10^{5} mol/l (1680 μg/ml)
Drug  Time (min)  Regression equation^{*}  Correlation coefficient (r) 
PIT  15  A= 0.0372+0.00681 C  0.9940 
20  A= 0.0682+0.00798 C  0.9997  
30  A= 0.00818+0.00818 C  0.9999  
40  A= 0.09225+0.00824 C  0.9997 
*Regression equation calculated using concentrations in μg/ml.
Method validation
Statistical evaluation of the regression line (table 5) gave small values for the standard deviation of residuals (S_{y/x}), the standard deviation of the slope S_{b}. These small values reflect the high reproducibility of the proposed method. The limit of detection LOD and quantitation LOQ were calculated using the statistical treatment of calibration data. These statistical data challenged for the robustness of the fixedtime method under the optimum reaction condition for carrying it in the assay of PIT.
Table 5: Analytical parameters for the determination of PIT using the fixedtime method
Parameters  PIT 
λ _{nm}  525 
Linearity range (µg/ml)  1680^{*} 
a (intercept)  0.08495 
b (slope)  0.008175 
r (correlation coefficient)  0.9999 
S_{a}  0.00346 
a/S_{a}  24.54 
S_{b}^{2}  4.25 x10^{9} 
S_{b}  6.52 x10^{5} 
F  15714 
Sig F  1.119 x10^{6} 
S_{y/x}  3.26 x10^{5} 
LOD (µg/ml)  1.26 
LOQ (µg/ml)  4.23 
^{*}5 points, at 16µg/ml intervals
Pharmaceutical application
Assay of PIT in its pharmaceutical formulation Liv`azo® 4 mg using the developed method was successfully applied without interference from the excipients. Excellent percent recovery and RSD demonstrated the applicability of the method. ttest and Ftest values were also calculated using a standard reference method [29]. The student ttest and variance ratioFtest values at 95% confidence level did not exceed the theoretical values [30], indicating no significant difference in accuracy and precision of the proposed kinetic spectrophotometric method and the RPHPLCmethod [29].
Table 6: Determination of PIT in pharmaceutical preparations using the fixedtime method and RPHPLC method
Drug  Pharmaceutical preparation  Mean recovery±SD^{a} RSD %^{b} Er %^{c} 

Fixedtime method  RPHPLC method  
PIT  Livazo^{®}4 mg  100.32±0.552 0.744 1.59 
101.08±0.996 0.985 1.08 
t** = 1.49 F** = 3.25 
^{a}mean±SD for the five determinations, ^{b}% Relative standard deviation, ^{c}% Relative error, ^{**}Theoretical values of tand Fat P = 0.05 are 2.13 and 6.93, respectively.
CONCLUSION
The low cost of the kinetic spectrophotometric technique makes it highly desirable for the determination of Pitavastatin in pharmaceutical formulations. Although the poor selectivity of the proposed methods, yet it is more simple, timesaving and more economic compared with HPLC and other sophisticated chemometric methods. These facts encourage to apply such methods in drug quality control laboratories.
ACKNOWLEDGMENT
The Author is thankful to Prof. Azza A. GazyDepartment of pharmaceutical technologyPharmaceutical analytical chemistry and drug quality controlBeirut Arab University, for her continuous guidance and support
FUNDING
Nil
AUTHORS CONTRIBUTIONS
Marwa k. Al Jamal designed, planned, and performed the experiments and the measurements. She processed the experimental data along with the calculations, drafted the manuscript, designed the fig. and interpreted the results.
Declared none
REFERENCES
Iatsimirskii KBK. No Title. Metody Analiza Moscow; 1963.
Yatsimirsku KB. Kinetic methods of analysis international series of monographs in analytical chemistry. 1st Editio. Oxford: Pergamon Press; 1966. p. 3554.
Anastasia CZ, Constantine GP. Simultaneous determination of iron(II) and iron(III) oxides in geological materials by ion chromatography. Analyst 1990;115:80912.
Salinas FL, Berzes Nevado JJ, Espinosa M. The solubility of alkalimetal fluorides in nonaqueous solvents with and without crown ethers, as determined by flame emission spectrometry. Talanta 1984;31:325–30.
Sanchiez CP, Albero MI, Garcia SM. Kinetic determination of Hg(II) in different materials, based on its inhibitory effect on a catalysed process. Talanta 1988;35:397–400.
Shantier SW, Gadkarien EA, Ibrahim K, Hagga ME. Kinetic determination of tobramycin in drug formulations. Res J Pharm Biol Chem Sci 2012;3:566–73.
Darwish I, MAS, ALArfaj H. Novel selective kinetic spectrophotometric method for determination of norfloxacin in its pharmaceutical formulations. Talanta 2009;78:1383–8.
Rizk M, Belal F, Ibrahim F, Ahmed SM, ElEnany NM. A simple kinetic spectrophotometric method for the determination of oxamniquine in formulations and spiked biological fluids. J Pharm Biomed Anal 2000;23:50313.
AOM, AAO, ZAT. Kinetic spectrophotometric determination of certain cephalosporins in pharmaceutical formulations. Int J Anal Chem 2009. Doi:10.1155/2009/596379
NR, AKN, HASN. Kinetic spectrophotometric method for the determination of silymarin in pharmaceutical formulations using potassium permanganate as oxidant. Pharmazie 2004;59:1126.
Niranjani S, Venkatachalam K. Simple titrimetric, spectrophotometric and gravimetric methods for the assay of pitavastatin calcium in a green manner. J Pharm Sci Res 2019;11:1766–74.
Kumar JVS, Prasanthi S, Guravaiah M, Sekaran C bala. Application of potassium permanganate to the spectrophotometric determination of oseltamivir phosphate in bulk and capsules. Asian J Pharm Clin Res 2012;5:18–22.
Yulianita R, Sopyan I, Muchtaridi M. Forced degradation study of statins: a review. Int J Appl Pharm 2018;10:38–42.
O’Neil M, Smith A, Heckelman P. The merck index merck research laboratories. Thirteenth; 2001.
Virupaxappa BS, Shivaprasad KH, Latha MS. Novel spectrophotometric method for the assay of pitavastatin calcium in pharmaceutical formulations. Chem Sin 2011;2:1–5.
M. K. NRP, S. M, S. J. S. B, D. S, R. and Srinivas M. Spectrophotometric determination of 3hydroxy3methylglutaryl coenzymeA reductase inhibitors in pharmaceutical preparations. Biomed Chromatogr 2006;20:282–93.
Virupaxappa BS, Shivaprasad KH, Latha MS. Novel spectrophotometric method for the assay of pitavastatin calcium in pharmaceutical formulations. Der Chem Sinica 2011;2:1–5.
Yunoos M, Sowjanya M, Sushma B, Kumar KP. A validated simple UV spectrophotometric method for the estimation of pitavastatin in bulk and pharmaceutical dosage form. Asian J Res Chem 2014;7:393–6.
Janagiraman S, Raju T, Giribabu K. Simple titrimetric analysis for determination of pitavastatin calcium in bulk and formulation dosage. Int J Modern Chem 2014;6:18–27.
Sujatha K, Rao JVLNS. A new validated stabilityindicating RPHPLC method for the estimation of pitavastatin in tablet dosage forms. Int J Pharm Pharm Res 2014;3:67–74.
Neelima B, Kumar PR, Bindu VH, Prasad YR. A validated stabilityindicating RPHPLC method for estimation of pitavastatin in bulk and pharmaceutical dosage form. Int J Pharm Sci 2013;3:309–15.
Kumar NS, Nisha N, Nirmal J, Sonali N, Bagyalakshmi J. Pharmaceutical determination of pitavastatin calcium in pharmaceutical dosage forms. Pharm Anal Acta 2011;2:2–5.
Goud ES, Reddy VK, Reddy MNC. Development and validation of a reversephase liquid chromatographic method for the determination of related substances of pitavastatin for 2 and 4 mg tablets. Int J Pharm Pharm Sci 2014;6:95–100.
Antony Raj Gomas, Pannala Raghu Ram, Nimmakayala Srinivas, Jadi Sriramulu. Degradation pathway for pitavastatin calcium by validated stability indicating UPLC method. Am J Anal Chem 2010;2:83–90.
Grobelny P, Viola G, Vedaldi D, Dall'Acqua F, Gliszczynska Swigło A, Mielcarek J. Photostability of pitavastatina novel HMGCoA reductase inhibitor. J Pharm Biomed Anal 2009;50:597–601.
Ashwini Ojha, Swati Guttikar, Chintan Vayeda, Harish Padh. Determination of pitavastatin from human plasma using highperformance liquid chromatography with fluorescence detection. Chin J Chromatography 2007;25:715–8.
Tian L, Huang Y, Jia Y, Hua L, Li Y. Development and validation of a liquid chromatographytandem mass spectrometric assay for pitavastatin and its lactone in human plasma and urine. J Chromatography B 2008;865:127–32.
ICH Harmonized Tripartite guideline, Validation of analytical procedures text and methodology Q2 (R1) Currant step 4 version, Parent guideline dated 27 November (Complementary guideline on Methodology dated 6 incorporated Geneva; 1996. p. 113.
Tirumala K, Gautam CHVS, Gangadhar J, Jayajeevitha M, Prakash KV. RPHPLC assay for estimation of pitavastatin in bulk and pharmaceutical dosage forms. Int J Pharm Sci Nanotechnol 2014;7:2346–9.
JN, Mileer JCM. Statistics and chemometrics for analytical chemistry. 5th ed. London, Pearson Prentice Hall; 2005.