|Home | About | Journals | Submit | Contact Us | Français|
Three simple spectrophotometric and atomic absorption spectrometric methods are developed and validated for the determination of moxifloxacin HCl in pure form and in pharmaceutical formulations. Method (A) is a kinetic method based on the oxidation of moxifloxacin HCl by Fe3+ ion in the presence of 1,10 o-phenanthroline (o-phen). Method (B) describes spectrophotometric procedures for determination of moxifloxacin HCl based on its ability to reduce Fe (III) to Fe (II), which was rapidly converted to the corresponding stable coloured complex after reacting with 2,2′ bipyridyl (bipy). The formation of the tris-complex formed in both methods (A) and (B) were carefully studied and their absorbance were measured at 510 and 520 nm respectively. Method (C) is based on the formation of ion- pair associated between the drug and bismuth (III) tetraiodide in acidic medium to form orange—red ion-pair associates. This associate can be quantitatively determined by three different procedures. The formed precipitate is either filtered off, dissolved in acetone and quantified spectrophotometrically at 462 nm (Procedure 1), or decomposed by hydrochloric acid, and the bismuth content is determined by direct atomic absorption spectrometric (Procedure 2). Also the residual unreacted metal complex in the filtrate is determined through its metal content using indirect atomic absorption spectrometric technique (procedure 3). All the proposed methods were validated according to the International Conference on Harmonization (ICH) guidelines, the three proposed methods permit the determination of moxifloxacin HCl in the range of (0.8–6, 0.8–4) for methods A and B, (16–96, 16–96 and 16–72) for procedures 1–3 in method C. The limits of detection and quantitation were calculated, the precision of the methods were satisfactory; the values of relative standard deviations did not exceed 2%. The proposed methods were successfully applied to determine the drug in its pharmaceutical formulations without interference from the common excipients. The results obtained by the proposed methods were comparable with those obtained by the reference method.
Moxifloxacin [1-Cyclopropyl-b-fluoro-1,4-dihydro-8-methoxy-7-[(4aS,7aS)-octahydro-6H-pyrrolo [3,4–6] pyridine-6-yl]-4-oxo-3-quinoline carboxylic acid]1 is a broad-spectrum antibiotic that is active against both Gram-positive and Gram-negative bacteria. 2 The bactericidal activity of the drug is mediated by the inhibition of DNA gyrase (topoisomerase II) and topoisomerase IV, essential enzymes involved in bacterial DNA replication, transcription, repair and recombination. Moxifloxacin is prescribed for the bacterial infections of the respiratory tract including sinusitis, community acquired pneumonia and acute exacerbations of chronic bronchitis.3
Few methods were reviewed in the literature for the analysis of moxifloxacin HCl. Spectrophotometric,4,5 spectrofluorimetric,6 liquid chromatographic,7–10 TLC,11 HPLC,12–16 Capillary electrophoresis,17,18 polarographic,19 and voltammetric20,21 procedures were applied for its determination.
Still, there is a need for simple methods to compete with the new, advancement and automated ones. Therefore, the present study aims to use spectrophotometric and atomic absorption spectrometric (AAS) techniques for the determination of moxifloxacin HCl in pure form and pharmaceutical formulations. Methods A and B are based on the oxidation of the drug by Fe3+ in the presence of (o-phen) or (bipy) and then the tris-complex formed was measured at 510 and 520 nm respectively. While method C based on the precipitation of the ion pair of the drug with bismuth (III) tetraiodide and quantifying it via the formed precipitate of the metal ion present in the supernatant solution using (AAS). The proposed methods were successfully applied to the determination of moxifloxacin HCl in tablet dosage forms without interference of any additives or excipients.
A Shimadzu recording spectrometer UV-1800 equipped with 10 mm two matched quartz cells was used for spectrophotometric measurements. Atomic absorption measurements were carried out using Shimadzu atomic absorption spectrometric device model AA-640-13 at 223 nm analysis wavelength, lamp current 5 mA, slit width 0.38 nm, burner height 5 mm, burner slot, flame 10 cm air-C2H2, support gas flow 10 I min−1, fuel gas flow 2.6 I min−1 and absorption sensitivity of 0.6 ppm.
All materials used were of analytical reagent grade, water was always doubly distilled. Pure sample moxifloxacin HCl was kindly provided by Sabaa International Company for pharmaceuticals and chemical industries S.A.E.
The Standard stock solution (0.8 mg ml−1) in water were prepared by dissolving 80 mg of pure drug in convenient amount of double distilled water in 100 ml volumetric flask followed by dilution to the mark with the same solvent, it is stable for at least 2 weeks if it was stored in a cool (<25 °C).
Pharmaceutical preparations: Moxifloxacin tablets (400 mg moxifloxacin HCl/tablet) were provided by Sabaa International Company for pharmaceuticals and chemical industries S.A.E. (Batch No. 09002).
Iron (III)-o-phenanthrolin22 was prepared by mixing 0.198 g of 1,10 phenanthroline monohydrate (Aldrich Chem. Co. Miluwakee, USA), 2 ml 1 M HCl and 0.16 g ferric ammonium sulphate dodecahydrate (Aldrich, Germany) before dilution with double distilled water to 100 ml in a calibrated flask. Iron (III) – bipyridyl22 was prepared by mixing 0.16 g of 2,2′ bipyridyl (Sigma Chem. Co. Miluwakee, USA) with 2 ml 1 M HCl and 0.16 g ferric ammonium sulphate dodecahydrate, before dilution with double distilled water to 100 ml in a calibrated flask.
Standard bismuth (III) solution, 0.01 M, was prepared by dissolving 0.1 g of Bi(NO3). 5H2O (Merck) in 2.5 ml of HNO3 and adding double distilled water to 25 ml and standardized complexometrically.23 Potassium iodide solution, 0.5 M, was prepared by dissolving 8.28 g of KI (Merck) in 100 ml of double distilled water. 2% HNO3 solution was prepared in double distilled water. 0.8 × 10−3 M solutions of bismuth (III) nitrate and drug were prepared.
(0.8–6) (0.8–4) μgml−1 aliquots of the standard solutions for methods A and B respectively were transferred to a series of 10 ml calibrated flasks. 4 ml of Fe3+-o-phen (method A) or 3.5 ml of Fe3+-bipy (method B) were added, then heating on a boiling water bath for 35, 30 minutes for methods A and B respectively. Mixture was cooled to room temperature (25 °C ± 1 °C), completed to volume with double distilled water. The coloured complexes formed were measured at 510 and 520 nm against a reagent blank treated similarly according to methods A and B respectively.
Aliquots of (0.8–6 μgml−1) of moxifloxacin HCl were assayed as in the general procedure for method A at different times (10, 25, 40, 60 minutes) in a boiling water bath.
To a series of 10 ml volumetric flasks, 0.7 ml of 0.01 M bismuth (III) nitrate solution was added followed by 0.8 ml of 0.5 M potassium iodide solution with continuous mixing. Accurately measured aliquots of the drug (Table 1) were then added followed by 0.7 ml of 2% HNO3. The solution was shaken to coagulate the precipitate then completed to volume with double distilled water, mixed well, and filtered. The precipitate obtained was washed with 2 ml 2% HNO3, completely dried in a vacuum desiccant, then dissolved quantitatively in acetone and the volume was made up to 10 ml in calibrated flask. The absorbance was measured at 462 nm against an appropriate blank prepared simultaneously.
The precipitate in procedure 1 was quantitatively decomposed into 10 ml volumetric flasks using 1 ml concentrated HCl, the mixture was completed to 10 ml with double distilled water and aspirated directly in the atomic absorption spectrometer, absorption was measured at 2230 A° against an appropriate blank prepared simultaneously. Concentration of the consumed bismuth was calculated from a calibration graph of standard Bi(NO3) solution or using regression equation.
The filtrate of procedure 1 were transferred to 25 ml volumetric flask, diluted to volume with double distilled water, absorbance was then measured using atomic absorption spectrometer at 2230 A° against an appropriate blank prepared simultaneously, excess concentration was then determined from a calibration graph of standard Bi(NO3) solution or using regression equation. The concentration of the drug was then calculated where 15.27 μgml−1 Bi (III) 16 μgml−1 drug.
An accurately weighed quantity of the pulverized tablets equivalent to 80 mg of the studied drug was extracted with double distilled water. Mixture was filtered through a filter paper and washed with water, the filtrate and washing were collected in a 100 ml standard flask and diluted to volume with double distilled water. Aliquots of this solution were transferred in a series of 10 ml volumetric flasks, and the analysis was completed as previously mentioned using methods A, B and C by using standard addition technique.
1,10 (o-phen) and 2,2′(bipy) are common reagents for ferrous ion as their red color chelate [Fe(phen)3]2+, [Fe(bip)3]2+ complexes remained stable for weeks. These methods were based on the reducing properties of the drug, it reduces Fe(III) to Fe(II) which was converted rapidly to the corresponding stable coloured reagent Fe(II) complex. (Fig. 1).
Optimum conditions affecting the reaction were studied:
After diluting the reaction solution mixture, it was found that the absorbance of the chromogen formed in method A and B are remained stable for at least 2 hours. This allowed the processing of large batches of samples, and their comfortable measurements with convenience so the methods will be more applicable for large number of samples, calibration graphs obtained were found to be linear over concentration ranges stated in (Table 1).The linearity was evaluated by the relative standard deviation of the slope,24 standard error, variance, Sandell’s sensitivity were also calculated (Tables 1 and and22).
The rate of the reaction was found to be dependent on the drug concentration, the rate was followed at 100 °C with various concentrations of the studied drug in the range of (0.8–6) μgml−1 (Fig. 4).
It is clear that the rate increases as the studied drug concentration increases, indicating that the reaction rate obeys the following equation:
where K′ is the pseudo-order constant of the reaction and n is the order of the reaction. The rate of the reaction may be estimated by the variable-time method measurement25 as ΔA/Δt, where A is the absorbance and t is the time in seconds. Taking logarithms of rates and concentration (Table 3) equation (1) is transformed into:
Regression of log (rate) versus log (drug) gave the regression equation:
Hence the reaction is first order (n ≈ 1) with respect to drug concentration.
The quantitative of the studied drug under the optimized experimental conditions outlined above, would result in a pseudo-first order reaction with respect to its concentration. However, the rate will be directly proportional to drug concentration in a pseudo-first order rate equation as follows:
where K′ is the pseudo-first order constant. Equation (3) was the basis for several experiments, which were run to obtain drug concentration using the rate data. Rate constant, constant concentration and fixed-time.26,27 The most suitable analytical method was selected taking into account the applicability, the sensitivity, the correlation coefficient (r) and the intercept.
Graphs of log (absorbance) versus time for the studied drug concentrations in the range (1.826 × 10−6 to 1.370 × 10−5 M) was plotted and appeared to be rectilinear. Pseudo-first order rate constants corresponding to different drug concentrations (C) were calculated from the slopes multiplied by −2.303 and are presented in (Table 4), (Fig. 5).
Regression of (C ) versus K′ gave the equation:
The value (r) indicates poor linearity, which is probably due to inconsistency of K′ as a result of slight changes due to the elevated temperature of the reaction.
Reaction rates were determined for different concentrations in the range 1.826 × 10−6 to 1.370 × 10−5 M of moxifloxacin HCl. A pre-selected value of the absorbance was fixed and the time was measured in seconds. The reciprocal of time (ie, 1/t) versus the initial concentration of the studied drug (Table 5) was plotted. The following equations for calibration graphs were worked out by linear regression:
The range of the concentration of the studied drug giving the most acceptable calibration graph with the above equations was very limited, which could be disadvantage.
Reaction rates were determined for different concentration of the studied drug, at a pre-selected fixed time, which was accurately determined, the absorbance was measured. Calibration graph of the absorbance versus initial concentration of the moxifloxacin HCl was obtained at fixed times of 10, 25, 35 and 40 min with the calibration equation shown in (Table 6). It is clear that, the most acceptable values of the correlation coefficient and more reaction products (indicated by higher absorbance readings were obtained for a fixed time of 35 min, which was, therefore chosen as the most suitable time interval for measurements.
After optimizing the reaction conditions, the fixed time method was applied to the determination of moxifloxacin hydrochloride in pure form and in pharmaceutical formulations over the concentration range of (0.8–6 μgml−1). Analysis of the date gives the following regression equation:
Formation of ion- pairs between many nitrogenous drugs and metal complexes found wide applications in the field of drug analysis applying colourimetric and (AAS) methods as well as ion-selective electrodes.28–37 In this work the investigated drug react with bismuth (III) tetraiodide to form stable ion- pair complex, this interaction and subsequent formation of the ion- pair occur in acidic medium via the two centers of tertiary amino group of the drug, one of them was formed due to the addition of acid) and two molecules of bismuth (III) tetraiodide. Being insoluble in aqueous solution, this ion- pair complex might be possibly isolated by direct filtration or extraction into organic solvents and assayed accurately without interference from excess unreacted metal complex.
Bismuth (III) tetraiodide complex was used as a reagent for the determination of some nitrogenous compounds.35–37 On mixing aqueous solutions of bismuth (III) tetraiodide complex and drug in acidic medium, a reddish orange precipitate instantaneously appeared that is attributed to the ion- pair formed in the reaction. This precipitate was filtered off and the residual unreacted bismuth (III) tetraiodide complex in the filtrate was analyzed using atomic absorption spectrometric technique. On the other hand the precipitate could be dissolved in acetone and analyzed spectrophotometrically at its peak absorption maximum at 462 nm (Fig. 6) or dissolved in HCl for atomic absorption spectrometric estimation.
Extraction of the formed ion- pair with different solvents was also studied, low polarity solvents such as chloroform and dichloromethane were inefficient due to insolubility of the ion- pair in such solvents, solvents with increase polarity such as n-butanol, acetone, and isobutyl methyl ketone lacked selectivity and did not differentiate between the ion- pair formed and the residual unreacted bismuth (III) tetraiodide in the aqueous phase, therefore filtration was necessary to separate the formed ion- pair.
Determination of the residual non-consumed bismuth (III) tetraiodide complex in the filtrate had the advantages of being rapid, simpler, precise than the direct dissolution of the isolated ion- pair precipitate owing to possible errors during isolation steps, automation of the methods enhance the overall analytical progress of the proposed procedure, making them more suitable for routine quality control analysis of the studied drug.
The different experimental parameters affecting the formation of the ion- pair complex were studied to determine the optimum conditions for the assay procedure:
Generally the formation of the ion- pair was rapid and the colour production was still stable for more than 24 hour. The more favorable sequence addition is bismuth (III)-KI- drug for the highest and completion- ion- pair formation. The linearity was evaluated by the relative standard deviation of the slope, standard error, variance, Sandell’s sensitivity. (Tables 1 and and77).
The composition of the ion- pair associates was established by molar ratio method.38 using equimolar solutions of the drug and reagent (0.8 × 10−3), the results obtained indicate that the composition of the associates was (1:2) drug to reagent. According to this ratio it was found that 15.27 μgml−1 Bi (III) 16 μgml−1 moxifloxacin HCl.
Under the experimental conditions described above the optical characteristics such as Beer’s law limits, Sandell’s sensitivity and molar absorptivity39 were calculated for the proposed methods and the results are summarized in (Table 1). Regression equations, intercepts, slopes and correlation coefficients for the calibration data are presented also in the same table while standard deviation, relative standard deviation and standard error are summarized in (Tables 2 and and77).
The detection limit (LOD) for the proposed methods were calculated using the following equation according to definition40:
where s is the standard deviation of replicate determination values under the same conditions as the sample in the absence of the analyte, and k is the sensitivity, namely the slope of the calibration graph. The detection limits obtained for the absorbance were found to be 0.0762, 0.21, 1.41, 1.423, 1.436 μg/ml for methods A, B, and C (Procedures 1, 2 and 3), respectively.
The limits of quantitation, LOQ, is defined as;
According to this equation, the LOQs were found to be 0.254, 0.6981, 4.676, 4.744, 4.788 μg/ml for methods A, B, and C (Procedures 1, 2, and 3), respectively.
In order to determine the accuracy and precision of the proposed methods, solutions containing 3 different concentrations of drug were prepared and analyzed in six replicate. The relative standard deviation as precision percentage relative error (Er %) as accuracy of the suggested methods were calculated at 95% confidence levels and can be considered satisfactory. Precision was carried out by six determinations at three different concentrations, the percentage relative error was calculated according to the following equation:
The inter- and intra-day precision and accuracy results are shown in (Table 8). The analytical results for accuracy and precision show that the proposed methods have good repeatability and reproducibility.
Robustness was examined by evaluating the influence of small variation of method variables including, concentration of analytical reagents, reaction time. In these experiments, one parameter was changed where as the others were kept unchanged, It was found that none of these variables significantly affect the method. This provided as indication for the reliability of the proposed method during its routine application for analysis of the investigated drug. Ruggedness was tested by applying the proposed methods to the assay of the drug using the same operational conditions but using two different instruments at two different laboratories and different elapsed time. Results obtained were found to be reproducible, as RSD did not exceed 2% (Table 9).
The % recoveries of the pure drug using the proposed methods were compared with that given by the reference method4 are illustrated in (Table 10). The reference method recomonded is uv-spectrophotometric procedure for determination of moxifloxacin hydrochloride using 0.1 N HCl. The validity of the proposed methods was evaluated by statistical analysis41 between the results obtained and that of reference method. Regarding the calculated student’s, t-test and variance ratio F-test, there is no significant difference between the proposed methods and the reference one.
The proposed methods described in this paper are simple, economic, sensitive, don’t require expensive reagents and sophisticated instruments. These methods are applicable for routine analysis of the studied drug in raw materials and pharmaceutical formulations over wide concentration range without interference from common excipients. The methods can use both spectrophotometric and (AAS) techniques for the final measurement step, moreover, they also have the advantages that no extraction is needed to separate the ion- pair formed and so avoiding the hazards of the organic solvents being simpler and more convenient. The statistical parameters indicate the reproducibility and accuracy of the methods.
Author(s) have provided signed confirmations to the publisher of their compliance with all applicable legal and ethical obligations in respect to declaration of conflicts of interest, funding, authorship and contributorship, and compliance with ethical requirements in respect to treatment of human and animal test subjects. If this article contains identifiable human subject(s) author(s) were required to supply signed patient consent prior to publication. Author(s) have confirmed that the published article is unique and not under consideration nor published by any other publication and that they have consent to reproduce any copyrighted material. The peer reviewers declared no conflicts of interest.