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ISRN Analytical Chemistry
Volume 2013 (2013), Article ID 861851, 7 pages
http://dx.doi.org/10.1155/2013/861851
Research Article

Spectrophotometric Determination of Bromhexine HCl in Pure and Pharmaceutical Forms

1Department of Chemistry, Jawaharlal Nehru Technology University, Hyderabad 500085, India
2Department of Chemistry, Nizam College, Hyderabad 500001, India

Received 8 June 2013; Accepted 3 July 2013

Academic Editors: E. Billiot, S. Göktürk, and D. Patra

Copyright © 2013 K. Susmitha 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.

Abstract

Five spectrophotometric methods for determination of bromhexine HCl have been developed, validated, and applied for the assay of the drug in pharmaceuticals. Methods A, B, and C are based on ion-pair complexation of drug, in acidic buffers, with triphenylmethane dyes, namely, bromothymol blue (BTB), bromophenol blue (BPB), and bromocresol green (BCG). The complexes are extracted into chloroform, and absorbance is measured at around 415 nm as function of concentration of the drug. The stoichiometry of the complex is found to be 1 : 1 in each case. Method D depends upon charge-transfer complexation of neutralized drug with iodine which produces iodide ion whose absorbance at 366 nm is measured as function of concentration of the drug. This complex too has 1 : 1 composition as determined by Job’s method. Method E is developed on the basis of oxidation of the drug with alkaline KMnO4 which generates green-colored manganate ion with 610 nm. As the intensity of green color increased with increasing time kinetics of the reaction is followed, and calibration curves are constructed by using initial rate and fixed time methods. Excellent recovery studies with high accuracy and precision indicate that the methods can be successfully used in industries for the assay of drug in pure form and pharmaceuticals.

1. Introduction

Bromhexine HCl (BRH), chemically named 2-amino-3,5-dibromo-N-cyclohexyl-N-methyl benzenemethanamine hydrochloride, is a mucolytic agent used in the treatment of respiratory disorders associated with viscid or excessive mucus [1, 2]. The drug is official in IP [3] and BP [4]. Because of its physiological importance, the drug has been quantified by exploiting its chemical [5, 6] and physical properties [725]. The different analytical methods used to quantify the drug as a single active pharmaceutical ingredient include flow injection analysis with ion-selective electrodes [7], inductively coupled plasma mass spectrometry [8], electrokinetic chromatography [9], electrochemical oxidation at the glassy carbon electrode [10], liquid chromatography [11], liquid gas chromatography [12], GC with mass detection [13], and voltammetry [14]. The drug has also been quantified in its combined formulations using HPLC [1518], direct and derivative UV spectrophotometry [1923]. These methods involve scarcely available costly equipment and tedious experimentation. Simple, accurate, and precise methods using spectrophotometry have also been developed based on the production of chromophore by the interaction of the drug with an analytical reagent, as chromogen [2426]. Availability of vast number of analytical reagents to serve as chromogens always leaves a lot of scope for pharmaceutical analysis. Thorough survey of the literature showed that the quantification methods of our interest are not reported yet, and hence in the present communication we report five quantification methods, namely, A, B, C, D, and E, that have been developed and validated for quantification of bromhexine HCl both in pure and pharmaceutical forms.

2. Experiment

2.1. Instruments

The UV-Visible spectra of the samples were recorded on SHIMADZU 140 double beam, Thermo Nicolet 1000 and ELICO 159 UV-Visible single beam spectrophotometers using quartz cells of 10 mm path length. An Elico model Li-120 pH meter was used for pH measurement.

2.2. Materials

HPLC grade chloroform, 1,2 Dichloroethane (DCE), Analytical grade (AR) HCl, Sodium acetate, KMnO4, Sodium hydroxide and dyes viz., (a) BTB (b) BPB (c) BCG supplied by Sd Fine Chemicals, Mumbai, were used in the study. Iodine (BDH, Poole, UK) was twice sublimed and preserved in vacuum desiccator (mp 113.6–3°C). Iodine in 1,2-dichloroethane (DCE) was freshly prepared (daily) by dissolving 254 mg solute in 50 mL of solvent (4.0 × 10−3 M). The drug was procured from Aurobindo Pharmaceuticals, Hyderabad, as a gift sample.

2.3. Methods A, B, and C

The methods A, B, and C are based on the interaction of the drug with bromothymol blue (BTB), bromophenol blue (BPB), and bromocresol green (BCG), respectively, to form chloroform-extractable ion pair complexes (Scheme 1) which absorb around 415 nm (Figure 1). The absorbance of this band increases with increasing the concentration of the drug and formed a basis for the quantification of the drug. The dyestuffs were used as 0.025% solutions in doubly distilled water. Sodium acetate hydrochloric acid buffers of pH 2.8, 2.5, and 3.5 were prepared by mixing 50 mL of 1.0 M sodium acetate solution with 49.50 mL, 50.50 mL, and 46.25 mL of 1.0 M HCl solution, respectively, and diluted to 250 mL with doubly distilled water. The pH of each solution was adjusted to an appropriate value with the aid of a pH meter.

861851.sch.001
Scheme 1: Bromhexine HC1-dye complex.
861851.fig.001
Figure 1: Absorption spectra of bromhexine hydrochloride-dye complex extracted into 10 mL chloroform: (a) drug = 10 μg mL−1 + 5 mL of 0.025% BTB + 5 mL of pH2.8 buffer, (b) drug = 9 μg mL−1 + 5 mL of 0.025% BPB + 5 mL of pH2.5 buffer, and (c) drug = 9.5 μg mL−1 + 5 mL of 0.025% BCG + 5 mL of pH3.5 buffer.
2.4. Method D Interaction of Iodine with Drug

The method depends upon the interaction of neutralized drug with iodine that generates iodide ion having an absorption band at 366 nm (Figure 2). The absorbance of this band increases with increasing the concentration of the drug and formed a basis for the quantification of the drug. Mixing the solution of iodine prepared in DCE with BRH resulted in a change of violet color of iodine into light brown to pale yellow color, and as a consequence, absorption spectra exhibited a new band of 366 nm. This is attributed due to ion formed by the interaction of iodine with drug (Scheme 2).

861851.sch.002
Scheme 2
861851.fig.002
Figure 2: Absorption spectra of (a) reaction product of 12.5 μg mL−1 bromhexine hydrochloride with iodine in 1,2-dichloroethane and (b) iodine.
2.5. Method E: Kinetic Method

The method depends on the oxidation of the drug with alkaline KMnO4 (1 × 1−2 M) to produce manganate ion which absorbs at 610 nm (Figure 3) and formed a basis for quantification of drug. A solution of 0.45 M NaOH is used to produce required alkalinity. Mixing the solutions of permanganate and the drug slowly developed green colour, and hence kinetics of the reaction was followed spectrophotometrically with a view to develop a method for the quantitative determination of the drug spectrophotometrically. The initial rate and fixed time methods are followed for the determination of BRH.

861851.fig.003
Figure 3: Absorption spectra of (a) drug (b) KMnO4 (), and (c) reaction product of 15 μg mL−1 bromhexine hydrochloride with alkaline KMnO4.
2.6. Calibration Curves for Methods A, B, and C

Different aliquots of drug solution were transferred into 125 mL separating funnel. To this 5 mL of buffer, 5 mL of dye was added, and total volume was made up to 20 mL with water. 10 mL of chloroform was added, and the contents were shaken for 5 min. The two layers were allowed to separate for 5 min. The organic layer was separated, and absorbance of yellow-colored solution which is stable at least for 3 hrs is measured at 415 nm against blank similarly prepared. The same procedure of analysis is followed either for assay of pure drug or for dosage form. The calibration graphs are linear for the drug analysed using these dyes (Figure 4).

861851.fig.004
Figure 4: Calibration curves.
2.7. Calibration Curve for Method D

Into separate 10 mL volumetric flasks different aliquots of BRH solution was transferred followed by the addition of 1 mL of iodine solution. The volume was completed using the same solvent and the absorbance was measured against reagent blank at 366 nm.

2.8. Calibration Curve for Method E
2.8.1. Initial Rate Method

Aliquots of 1 to 8 mL of bromhexine HCl solution containing 2.5 mg mL−1 of drug were pipetted into a series of 10 mL standard flasks. To each flask, 1.0 mL of 0.45 M NaOH and 1 mL of potassium permanganate were added successively and then diluted with distilled water at . The contents of each flask were mixed well, and the increase in absorbance as a function of time was measured at 610 nm. The initial rate of the reaction () at different concentrations was evaluated by measuring the slope of the tangent to the absorbance-time plot. The calibration graphs were obtained by plotting the initial rate of reaction () versus concentration of bromhexine HCl.

2.8.2. Fixed Time Method

A fixed time of 20 min was selected for the fixed time method. At this time the absorbance of reaction mixture measured against a reagent blank prepared similarly. The calibration curve was obtained by plotting the absorbance against the initial concentration of bromhexine HCl. Table 1 summarizes the limits of Beer’s law, Limit of Detection (LOD), Limit of quantification (LOQ), molar absorptivity, regression equation, correlation coefficients and relative standard deviations.

tab1
Table 1: Optical characteristics, precision, and accuracy data.
2.9. Assay of Drug in Pharmaceuticals
2.9.1. Procedure for the Assay of Pure Drug

Five different solutions of pure drug in the range of calibration curve were selected, and the recovery experiments were performed. The recoveries and their relative standard deviation are tabulated in (Table 2).

tab2
Table 2: Application of proposed methods for the determination of BRH in pure form.
2.9.2. Procedure for the Assay of Dosage Forms

Ten tablets of bromhexine 8 mg are powdered and dissolved in doubly distilled water and stirred thoroughly and then filtered through a Whatman number 42 filter paper. This solution was transferred into 100 mL standard volumetric flask and diluted with doubly distilled water as required. Different solutions of drug in the range of calibration curve were chosen, and the assay was estimated using the calibration curve and the results of the recovery studies are tabulated in (Table 3).

tab3
Table 3: Application of proposed methods for the determination of BRH in pharmaceutical preparation.

3. Results and Discussion

3.1. Methods A, B, and C

BRH forms ion-pair complexes in acidic buffer with dyestuffs viz., BTB, BPB and BCG. These complexes are quantitatively extracted into chloroform. The ion-pair complexes with BTB, BPB and BCG absorbed maximally at 415 nm (Figure 1). The reagent blank under similar conditions showed no absorption. BRH contains aromatic amine group which is protonated in acidic medium, while sulphonic acid group is present in BTB: that is the only group undergoing dissociation in the PH range 1–5. BPB and BCG are examples of sulphonepthalein type of dye. The colour of such dyes is due to the opening of lactoid ring and subsequent formation of quinoid group. It is supposed that the two tautomers are present in equilibrium but due to strong acidic nature of the sulphonic acid group, the quinoid body must predominate. Finally the protonated BRH forms ion-pairs with the dyestuffs which are quantitatively extracted into chloroform.

3.2. Stoichiometry

In order to establish molar ratio between BRH and dyestuffs used, Job’s method of continuous variation (Figure 5) has been applied [28]. In this method, solutions of drug and dyestuff with identical molar concentrations () were mixed in varying volume ratios in such a way that the total volume of each mixture was the same. The absorbance of each solution was measured and plotted against the mole fraction of the drug, .

861851.fig.005
Figure 5: Jobs plots.

This measurement showed that 1 : 1 complex was formed. Job’s method of stoichiometry is also applied for iodine with BRH which indicated that the charge-transfer complex formed is of 1 : 1 composition.

The stoichiometric ratio between bromhexine HCl and potassium permanganate was evaluated by limiting logarithmic method [29]. In this method two sets of experiments were performed. In the first set the concentration of BRH was varied keeping a constant concentration of KMnO4, while in the second set the concentration of BRH was kept constant and the KMnO4 concentration was varied. Log absorbance versus log[BRH] or [KMnO4] was plotted to evaluate the slopes of the respective lines. From evaluation of slopes molar combining ratio is 5 : 2 between bromhexine HCl and potassium permanganate. The literature survey reveals that bromhexine HCl undergoes oxidation and gives rise to 2-amino-3, 5-dibromobenzaldehyde and N-methyl cyclohexanamine [14] (Figure 6).

861851.fig.006
Figure 6: Oxidation of bromhexine HCl with alkaline KMnO4.
3.3. Formation Constants

The formation constants for method A, B and C are estimated from Job’s plot by the following method described by Likussar and Boltz [30] and Momoki et al. [31]. The method involves drawing the tangents at the origin of Job’s plot from both sides, and the absorbance at intersection point is taken for 100% complexation. The absorbance at peak height of Job’s plot is taken for ()%, where is the % degree of dissociation of the complex. The instability constant, , is calculated, where is the concentration of drug used for Job’s method. The reciprocal of is the required stability constant .

3.4. Formation Constant for Method D

Formation constant () has been evaluated by using Benesi-Hildebrand equation [32]: where is absorbance, is molar absorptivity, and and are initial concentrations of acceptor and donor [drug], respectively. A plot of versus yields a straight line whose slope and intercept give the value of .

3.5. Optimization of the Factors Affecting the Absorbance

The factors effecting the absorbance of ion-pair complexes like pH and volume of the dye, in methods A, B, and C, have been optimized. 1.8 mL of BTB and buffer of pH 2.8, 1.6 mL of BPB and buffer of pH 2.5, and 2.0 mL of BCG and buffer of pH 3.5 are found to be optimal for methods A, B, and C, respectively. However 5 mL of each dye is used, at optimal pH, in the study to ensure complete extraction of the drug. Similarly the 1 mL of iodine for method D and 1 mL of KMnO4, 1 mL of 0.45 NaOH for method E are found to be optimal and hence are used in the study.

3.6. Validation of the Proposed Methods

The proposed methods have been validated in terms of guidelines proposed by ICH [33], namely, selectivity, specificity, accuracy, precision, limits of calibration curve, LOD, LOQ, robustness, ruggedness, and regression equation. Student’s -test and variance -test have been performed in comparison with a reference method. To test the reproducibility of the proposed methods, five replicate determinations of 15.0 µg mL of BRH were made. The coefficient of variation was found to be less than 1.2% for all the procedures.

The proposed methods have been successfully applied to the determination of BRH in pharmaceutical preparations. The results obtained and shown in Table 1 were compared to those obtained by a reference method [14] by means of -test at 95% confidence level. In all cases, the average results obtained by proposed methods and reference method were statistically identical, as the difference between the average values had no significance at 95% confidence level.

4. Conclusions

The proposed spectrophotometric methods present selective and simple, specific, and inexpensive analytical procedures for determination of BRH, in pure or in tablet dosage forms without interference from common excipients. Moreover, the developed methods are time saving and do not require elaborate treatments associated with chromatographic methods. These attributes make them suitable for routine analysis in quality control laboratories.

Acknowledgments

The authors are grateful to the Head, Department of Chemistry, and Principal, Nizam College, for providing facilities. The support rendered by Department of Chemistry, Jawaharlal Nehru Technology University, is duly acknowledged.

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