# Determination of Fluoroquinolones in Pharmaceutical Formulations by Extractive Spectrophotometric Methods Using Ion-Pair Complex Formation with Bromothymol Blue

Authors: Trung Dung Nguyen; Hoc Bau Le; Thi Oanh Dong; Tien Duc Pham
Journal: Journal of Analytical Methods in Chemistry
 (2018)

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## Abstract

In this paper, we reported a new, simple, accurate, and precise extractive spectrophotometric method for the determination of fluoroquinolones (FQs) including ciprofloxacin (CFX), levofloxacin (LFX), and ofloxacin (OFX) in pharmaceutical formulations. The proposed method is based on the ion-pair formation complexes between FQs and an anionic dye, bromothymol blue (BTB), in acidic medium. The yellow-colored complexes which were extracted into chloroform were measured at the wavelengths of 420, 415, and 418 nm for CFX, LFX, and OFX, respectively. Some effective conditions such as pH, dye concentration, shaking time, and organic solvents were also systematically studied. Very good limit of detection (LOD) of 0.084µg/mL, 0.101 µg/mL, and 0.105 µg/mL were found for CFX, LFX, and OFX, respectively. The stoichiometry of the complexes formed between FQs and BTB determined by Job’s method of continuous variation was 1 : 1. No interference was observed from common excipients occurred in pharmaceutical formulations. The proposed method has been successfully applied to determine the FQs in some pharmaceutical products. A good agreement between extractive spectrophotometric method with high-performance liquid chromatography mass spectrometry (HPLC-MS) for the determination of FQs in some real samples demonstrates that the proposed method is suitable to quantify FQs in pharmaceutical formulations.


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## Body

## 1. Introduction

Fluoroquinolones (FQs) are the important antibiotics used for the treatment of Gram-negative bacterial infections in both human and veterinary medicine. They are derivatives of 4-quinolone, which have unsubstituted or substituted piperazine ring attached at the 7-position to the central ring system of quinoline as well as fluorine atom at the 6-position. The FQs are useful to treat a variety of infections, including soft-tissue infections, respiratory infections, urinary tract infections, bone-joint infections, typhoid fever, prostatitis, sexually transmitted diseases, acute bronchitis, community-acquired pneumonia, and sinusitis [1–3].Ciprofloxacin (CFX), which is one of the second-generated groups of synthetic FQs, can exhibit greater intrinsic antibacterial activity and make a broader antibacterial spectrum. Ofloxacin (OFX) is a chiral compound that is widely used to treat above infections. Levofloxacin (LFX) is the pure (–)-(S)-enantiomer of the racemic drug substance ofloxacin. Figures1(a)–1(c) show the chemical structures of CFX, LFX, and OFX, respectively.Figure 1
Chemical structures of ciprofloxacin (a), levofloxacin (b), ofloxacin (OFX) (c), and bromothymol blue (d).
(a)
(b)
(c)
(d)Several techniques like voltammetry [4], flow injection electrogenerated chemiluminescence [5], spectrofluorometry [6, 7], spectrophotometry [8, 9], high-performance liquid chromatography [10, 11], and liquid chromatography tandem mass spectrometry [12, 13] have been used for the determination of fluoroquinolones in pharmaceutical and biological products. Among them, spectrophotometric method has several advantages such as simplicity, fast, and low cost. Spectrophotometry was successfully used for pharmaceutical analysis, involving quality control of commercialized product and pharmacodynamic studies. Spectrophotometric methods for the determination of fluoroquinolones could be classified according to the different reactions: (i) charge-transfer complexation based on the reaction of FQs as electron donors with p-acceptors such as 2,3-dichloro-5,6-dicyano-q-benzoquinone, 7,7,8,8-tetracyanoquinodimethane, q-chloranil, q-nitrophenol, and tetracyanoethylene [7, 14–16]; (ii) oxidative coupling reaction using oxidative coupling with 3-methyl-2-benzothiazolinonehydrazone hydrochloride and cerium (IV) ammonium sulfate, Fe(III)-MBTH, tris(o-phenanthroline) iron(II), and tris (bipyridyl) iron(II) [17, 18]; (iii) ion-pair complex formation with acid-dye reagents such as Sudan III, methyl orange, supracene violet 3B, tropaeolin 000, bromophenol blue, bromothymol blue, bromocresol green, and bromocresol purple [8, 14, 19, 20]. These methods were related with some major drawbacks such as having narrow linearity range, requiring heating and close pH control, long time for the reaction to complete, and low stability of the colored product formed.Bromothymol blue (BTB) (Figure1(d)) is an anionic dye and that can be protonated or deprotonated to form yellow or blue, respectively. The BTB was used to make ion-pair complex, which was applied to determine many pharmaceutical compounds by extractive spectrophotometric methods [21–30]. However, the ion-pair complex between BTB and FQs has not been studied. The method based on ion-pair complexes between analytes and BTB into a suitable organic solvent is also simple, fast, and cheap.In the previous study, we used sulphonphthalein acid including bromophenol blue, bromocresol green, and bromothymol blue to determine ciprofloxacin pharmaceutical formulations and achieved good results [31].In this paper, for the first time, we investigated extractive spectrophotometric method based on the formation of ion-pair complexes between ciprofloxacin, levofloxacin, and ofloxacin with BTB subsequent extraction into chloroform. Some effective conditions on the formation of complexes such as pH, shaking time, organic solvent, and the concentration of dye were systematically studied. The present method was also applied to determine FQs in some pharmaceutical formulations including tablets and infusions.


## 2. Experimental

### 2.1. Apparatus

A double beam UV-visible spectrophotometer (SP-60, Biochrom Ltd., UK) with 1.0 cm of path length quartz cells was used to measure all sample absorbances. Inolab pH-meter instrument (Germany) was used to monitor the pH of solutions. Three standard buffers were used to calibrate the electrode before measuring pH of solutions. All measurements were conducted at 25± 2°C controlled by air conditional laboratory.


### 2.2. Materials and Reagents

All chemicals used were of analytical grade and double-distilled water was used to prepare all solutions in the present study.FQs were purchased from Sigma (Germany, with purity >99.0%), whereas bromothymol blue (BTB) was supplied by Maya-R, China, with purity >99%. The organic solvents including chloroform, dichloromethane, carbon tetrachloride, dichloroethane, benzene, toluene, and other chemicals are analytical reagents (Merck, Germany).The following dosage forms containing FQs were purchased from local pharmacy market and employed in the study: Hasancip and Kacipro tablets equivalent to 500 mg ciprofloxacin (Hasan-Dermapharm and Dong Nam manufacturing-Trading pharmaceutical Co., Ltd, Vietnam). Ciprofloxacin infusion equivalent to 200 mg ciprofloxacin/100 ml solution for infusion (Hebei Tiancheng Pharmaceutical Co., Ltd and Shandong Hualu Pharmaceutical Co., Ltd, China). Stada and DHG tablets equivalent to 500 mg levofloxacin (Stada-VN J.V.Company and DHG pharmaceutical joint–stock company, Vietnam). Ofloxacin (200 mg/tablet) was provided by the Mekophar Chemical Pharmaceutical Company (Vietnam).


### 2.3. Solution Preparation

A stock solution of FQs (1 mg/mL) in double-distilled water. The working standard solution of FQs containing 100µg/mL was prepared by appropriate dilution. The stock solution of BTB (0.025%) was prepared in double-distilled water. All stock solutions were kept in dark bottle, stored in 4°C and could be used within one week.


### 2.4. Construction of Calibration Curves

A series of 125 mL separating funnel, the volumes of working solutions of the drugs in different concentration ranges (CFX (1–35µg/mL), LFX (0.5–25 µg/mL), and OFX (0.5–25 µg/mL) were transferred. Then, 4.0 mL of 0.025% BTB solution was added before thoroughly mixing. After that, a 10 mL of chloroform was added to each of the separating funnel. The contents were shaken for 2 min and allowed to separate the two layers. The yellow-colored chloroform layer containing the ion-pair complexes was measured at 420 nm for CFX, 415 nm for LFX, and 418 nm for OFX against the reagent blanks. At each concentration, the experiment was repeated 6 times. The colored chromogen complexes are stable for 24 h.


### 2.5. Sample Preparation

Weigh and mix the contents of twenty tablets of each drug (CFX, LFX, and OFX), an accurately weighed amount of powder equivalent to 0.1 g of drugs transferred into a 100-mL beaker. A magnetic stirrer was used to completely disintegrate the powder in doubly distilled water. Then, filter through a Whatman paper (No 40) and fill up to 100 mL with doubly distilled water in a volumetric flask. The working solution of the drugs containing 100µg/mL was prepared by dilution and determined under optimum conditions.


### 2.6. Validation with High-Performance Liquid Chromatography-Mass Spectrometry (HPLC-MS)

Some real samples of three FQs were determined by HPLC-MS using HPLC 20 AXL (Shimadzu, Japan) coupled with electrospray ionisation tandem mass spectrometric detection, ABI 5500 QQQ (Applied BioSystem). The chromatographic conditions are including column C18 MRC-ODS (150 mm × 2.1 mm × 3.5µm), mobile phase containing acetonitrile (ACN) with formic acid (0.1%) in water under a flow rate of 0.5 ml/min, and gradient elution. The inject volume is 10 µL.


## 2.1. Apparatus

A double beam UV-visible spectrophotometer (SP-60, Biochrom Ltd., UK) with 1.0 cm of path length quartz cells was used to measure all sample absorbances. Inolab pH-meter instrument (Germany) was used to monitor the pH of solutions. Three standard buffers were used to calibrate the electrode before measuring pH of solutions. All measurements were conducted at 25± 2°C controlled by air conditional laboratory.


## 2.2. Materials and Reagents

All chemicals used were of analytical grade and double-distilled water was used to prepare all solutions in the present study.FQs were purchased from Sigma (Germany, with purity >99.0%), whereas bromothymol blue (BTB) was supplied by Maya-R, China, with purity >99%. The organic solvents including chloroform, dichloromethane, carbon tetrachloride, dichloroethane, benzene, toluene, and other chemicals are analytical reagents (Merck, Germany).The following dosage forms containing FQs were purchased from local pharmacy market and employed in the study: Hasancip and Kacipro tablets equivalent to 500 mg ciprofloxacin (Hasan-Dermapharm and Dong Nam manufacturing-Trading pharmaceutical Co., Ltd, Vietnam). Ciprofloxacin infusion equivalent to 200 mg ciprofloxacin/100 ml solution for infusion (Hebei Tiancheng Pharmaceutical Co., Ltd and Shandong Hualu Pharmaceutical Co., Ltd, China). Stada and DHG tablets equivalent to 500 mg levofloxacin (Stada-VN J.V.Company and DHG pharmaceutical joint–stock company, Vietnam). Ofloxacin (200 mg/tablet) was provided by the Mekophar Chemical Pharmaceutical Company (Vietnam).


## 2.3. Solution Preparation

A stock solution of FQs (1 mg/mL) in double-distilled water. The working standard solution of FQs containing 100µg/mL was prepared by appropriate dilution. The stock solution of BTB (0.025%) was prepared in double-distilled water. All stock solutions were kept in dark bottle, stored in 4°C and could be used within one week.


## 2.4. Construction of Calibration Curves

A series of 125 mL separating funnel, the volumes of working solutions of the drugs in different concentration ranges (CFX (1–35µg/mL), LFX (0.5–25 µg/mL), and OFX (0.5–25 µg/mL) were transferred. Then, 4.0 mL of 0.025% BTB solution was added before thoroughly mixing. After that, a 10 mL of chloroform was added to each of the separating funnel. The contents were shaken for 2 min and allowed to separate the two layers. The yellow-colored chloroform layer containing the ion-pair complexes was measured at 420 nm for CFX, 415 nm for LFX, and 418 nm for OFX against the reagent blanks. At each concentration, the experiment was repeated 6 times. The colored chromogen complexes are stable for 24 h.


## 2.5. Sample Preparation

Weigh and mix the contents of twenty tablets of each drug (CFX, LFX, and OFX), an accurately weighed amount of powder equivalent to 0.1 g of drugs transferred into a 100-mL beaker. A magnetic stirrer was used to completely disintegrate the powder in doubly distilled water. Then, filter through a Whatman paper (No 40) and fill up to 100 mL with doubly distilled water in a volumetric flask. The working solution of the drugs containing 100µg/mL was prepared by dilution and determined under optimum conditions.


## 2.6. Validation with High-Performance Liquid Chromatography-Mass Spectrometry (HPLC-MS)

Some real samples of three FQs were determined by HPLC-MS using HPLC 20 AXL (Shimadzu, Japan) coupled with electrospray ionisation tandem mass spectrometric detection, ABI 5500 QQQ (Applied BioSystem). The chromatographic conditions are including column C18 MRC-ODS (150 mm × 2.1 mm × 3.5µm), mobile phase containing acetonitrile (ACN) with formic acid (0.1%) in water under a flow rate of 0.5 ml/min, and gradient elution. The inject volume is 10 µL.


## 3. Results and Discussion

### 3.1. Optimum Reaction Conditions

#### 3.1.1. Effect of Extracting Solvent

Six organic solvents including chloroform, carbon tetrachloride, dichloromethane, dichloroethane, benzene, and toluene were used to study the effect of solvent to ion-pair formation between FQs and BTB. Figure2 shows that chloroform is the most suitable solvent for the extraction of three FQs with low blank absorbance, highest absorbances, and lowest standard deviations. It implies that chloroform is the best extracting solvent to achieve a good recovery of the complexes with the shortest time to reach the equilibrium processes.Figure 2
The effect of solvent on the ion-pair complex formation (10µg/mL of fluoroquinolones (FQs) with bromothymol blue (BTB)).


#### 3.1.2. Effect of pH

The pH of solution plays an important role in the complex formations. The effect of pH on the formation of ion pairs was examined by varying the pH from 2.0 to 6.0 by adjusting 1 M HCl and 1 M NaOH. The maximum absorbances were observed at pH 3.3, 3.4, and 3.5 for the complexes of BTB and OFX, CFX, and LFX, respectively (Figure3). These pH values correspond to the initial pH of the examined drug and the dye. Therefore, it is not necessary to adjust the pH before extraction.Figure 3
Effect of pH on the absorbances of 10μg/mL of OFX, LFX, and CFX.


#### 3.1.3. Effect of Dye Concentration

The effect of dye concentrations was studied by adding different volumes of 0.025% BTB from 1.0 to 6.0 mL with a fixed concentration of FQs (10μg/mL) (Figure 4). Figure 4 shows that the maximum absorbance of the complex was achieved with 4.0 mL of 0.025% of BTB in each case and excess dye did not affect the absorbance of the complex. Therefore, 4.0 mL of 0.025% of BTB is optimum dye volume and it is kept as constant for further studies.Figure 4
Effect of the volume of 0.025% BTB on the absorbance of 10μg/mL of OFX, LFX, and CFX.


#### 3.1.4. Effect of Shaking Time

The effect of shaking time on the formation and stability of the ion-pair complex was investigated by measuring the absorbance of the extracted ion associates with increasing time from 0 to 4.0 min. Figure5 shows that the ion-pair complexes were formed instantaneously with 2.0 min shaking time. Thus, 2.0 min is the optimum shaking time and it is fixed for further studies.Figure 5
Effect of shaking time on the ion-pair complexes.


#### 3.1.5. Stoichiometry of Ion-Pair Complexes

Job’s method of continuous variation of equimolar solutions was employed to evaluate stoichiometry of the complex. A 3.0 × 10−4 M standard solution of three FQs and 3.0 × 10−4 M solution of BTB were used. A series of the solutions were prepared in which the total volume of drug and reagent was kept in 10 mL, whereas the absorbances were measured at 420, 415, and 418 nm, for CFX, LFX, and OFX, respectively. The absorbances were plotted against the mole fraction of the drugs. The stoichiometry for each drug-dye ion-pair complex was found to be 1 : 1 (Figure 6).Figure 6
Job’s method of continuous variation graph for the reaction of drug with acid dyes BTB, [drug] = [dye] = 3.0 × 10−4 M.


#### 3.1.6. Mechanism of Reaction and Absorption Spectra

Fluoroquinolones can contain a secondary amino group (CFX) and a tertiary amino group (LFX and OFX) that can be easily protonated under acidic conditions. On the one hand, the sulphonic acid group in BTB, that is, the only group undergoing dissociation in the pH range 1–5. The colour of BTB is on the basis of lactoid ring and subsequent formation of quinoid group. It is suggested that the two tautomers are plausible in equilibrium due to strong acidic nature of the sulphonic acid group. Thus, the quinoid body must predominate. Finally, the protonated fluoroquinolones form ion pairs with BTB dye that could be quantitatively extracted into chloroform. The possible reaction mechanisms are proposed and given in a scheme in Figure7.Figure 7
Proposal mechanism for the reaction between levofloxacin, ofloxacin, and bromothymol blue.The absorption spectra of the ion-pair complexes, which were formed between FQs and BTB, were measured in the wavelength range 350–500 nm against the blank solution and shown in Figure8.Figure 8
Absorption spectrum of ion-associate complexes of fluoroquinolones (10µg/mL) with BTB against reagent blank.Figure8 shows that absorption maxima for CFX-BTB, LFX-BTB, and OFX-BTB in chloroform were observed at 420, 415, and 418 nm, respectively. The reagent blanks under similar conditions have insignificant absorbances. At wavelengths 420, 415, and 418 nm, absorption spectrum of BTB does not affect the absorption spectrum of ion-associate complexes of FQs. Therefore, the selectivity of the proposed method for the determination of FQs is guaranteed.


#### 3.1.7. Association Constants of Ion-Pair Complexes

The equation of association constant of ion-pair complex is(1)A/Am1−A/Amn+2CMnn,where A and Am are the observed absorbance and the maximum absorbance value when all the drug present is associated, respectively. CM is the molar concentration of the drugs at the maximum absorbance and n is the stoichiometry in which BTB ion associates with drugs. The conditional stability constants (Kf) of the ion-pair complexes according to Britton [32] for the cases of FQs were calculated from the continuous variation data using the following equation:(2)Kf=A/Am1−A/Amn+2CMnn.The conditional stability constants (Kf) of the ion-pair complexes for FQs are indicated in Table 1.Table 1
The conditional stability constants (Kf) of the ion-pair complexes for FQs.
Sample
V
drug (mL)
V
BTB (mL)
A
n
n
⋀
n
1
−
A
/
A
m
n
+
2
K
f
logKf
Mean
Ofloxacin
1
0.25
2.25
0.202
0.1111
0.7834
0.3116
50204.7802
4.7007
6.08
2
0.5
2
0.272
0.2500
0.7071
0.1486
157048.9127
5.1960
3
0.75
1.75
0.336
0.4286
0.6955
0.0512
572507.7789
5.7578
4
1
1.5
0.419
0.6667
0.7631
0.0035
9562329.8320
6.9806
5
1.25
1.25
0.476
1.0000
1.0000
0.0000
_
_
6
1.5
1
0.432
1.5000
1.8371
0.0002
59414177.6247
7.7739
7
1.75
0.75
0.356
2.3333
7.2213
0.0026
1172246.1806
6.0690
Levofloxacin
1
0.25
2.25
0.137
0.1111
0.7834
0.5749
14789.8587
4.1700
6.04
2
0.5
2
0.313
0.2500
0.7071
0.1856
115961.3839
5.0643
3
0.75
1.75
0.432
0.4286
0.6955
0.0426
708574.1920
5.8504
4
1
1.5
0.559
0.6667
0.7631
0.0005
67745245.6475
7.8309
5
1.25
1.25
0.594
1.0000
1.0000
0.0000
_
_
6
1.5
1
0.53
1.5000
1.8371
0.0004
34165312.8945
7.5336
7
1.75
0.75
0.426
2.3333
7.2213
0.0042
682897.0665
5.8344
Ciprofloxacin
1
0.25
2.25
0.392
0.1111
0.7834
0.2112
83530.0520
4.9218
5.91
2
0.5
2
0.452
0.2500
0.7071
0.1265
178145.0100
5.2508
3
0.75
1.75
0.564
0.4286
0.6955
0.0345
828480.0305
5.9183
4
1
1.5
0.661
0.6667
0.7631
0.0036
8522213.4055
6.9306
5
1.25
1.25
0.752
1.0000
1.0000
0.0000
_
_
6
1.5
1
0.615
1.5000
1.8371
0.0026
4572267.1248
6.6601
7
1.75
0.75
0.538
2.3333
7.2213
0.0043
608798.6008
5.7845
—, not determined.Table1 shows that the log Kf values of ion-pair associates for OFX-BTB, LFX-BTB, and CFX-BTB were 6.08 ± 0.46, 6.04 ± 0.58, and 5.91 ± 0.32, respectively (numbers of replicated experiments, n=6). The obtained results confirmed that the ion-pair formation complexes are of high stability.


### 3.2. Validation of the Present Method

The proposed methods are validated according to ICH recommendations Q2(R1) [33]. The parameters that have been investigated are indicated below.


#### 3.2.1. Linearity, Sensitivity, and Limits of Detection and Quantification

A linear relationship between the measured absorbance and the concentration range studied for each drug as shown in Figure9 and the correlation coefficient (R) of at least 0.997 were achieved. The limit of detection (LOD) and quantification (LOQ) of the method are determined by 3.3SD/b and 10SD/b, respectively, where SD is the standard deviation of blank absorbance values and b is the slope of the calibration curve equation.Figure 9
Calibration curves for OFX, LFX, and CFX at 418, 415, and 420 nm, respectively.The LOD and LOQ values, slope, and intercept of linear graphs for all the drugs and analytical parameters are indicated in Table2. The molar absorptivities and Sandell’s sensitivity of each methods were calculated and these values showed that the molar absorptivity of ion-pair complexes was in the order CFX-BTB > LFX-BTB > OFX-BTB.Table 2
Analytical characteristics of the proposed methods (n=6).
Parameters
Proposed methods
Ofloxacin
Levofloxacin
Ciprofloxacin
Colour
Yellow
Yellow
Yellow
Wavelengthsλmax (nm)
418
415
420
pH
3.3
3.5
3.4
Stability (h)
24
24
24
Shaking time (min)
2
2
2
Stoichiometric ratio
1 : 1
1 : 1
1 : 1
Beer’s law range (µg/mL)
1–35
0.5–25
0.5–25
Limit of detection, LOD (µg/mL)
0.105
0.101
0.084
Limit of quantitation, LOQ (µg/mL)
0.315
0.303
0.252
Molar absorptivity (L/mol.cm)
1.44 × 104
2.07 × 104
2.09 × 104
Sandell’s sensitivity (µg/cm2)
0.068
0.048
0.046
Regression equation (Y = bx + a), where Y is the absorbance, a is the intercept, b is the slope, and x is the concentration in μg/mL
Slope (b)
0.040
0.057
0.061
Intercept (a)
0.0165
0.072
0.089
Correlation coefficient (R)
0.998
0.997
0.998


#### 3.2.2. Accuracy and Precision

The accuracy and precision of the methods were determined by preparing solutions of three different concentrations of drug and analyzing them in six replicates. The precision of the proposed methods was evaluated as percentage relative standard deviation (RSD%) and accuracy as percentage relative error (RE%). The percentage relative error was calculated using the following equation:(3)RE%=founded–addedadded×100.The accuracy and precision were summarized in Table3. The low values of the RSD and RE confirm the high precision and the good accuracy of the present method.Table 3
Evaluation of accuracy and precision of the proposed methods (n=6).
Method
Additive concentration (μg/mL)
Found concentration (μg/mL)
Recovery (%)
RSD (%)
RE (%)
Ofloxacin
5.00
5.11
102.19
2.31
2.2
10.00
10.26
102.64
1.34
2.6
15.00
14.89
99.25
0.88
−0.73
Levofloxacin
5.00
5.16
102.70
2.03
2.8
10.00
10.16
101.56
1.10
1.6
15.00
14.82
98.80
0.50
−1.2
Ciprofloxacin
5.00
5.13
102.71
1.92
2.6
10.00
9.74
97.41
0.52
−2.6
15.00
14.60
97.33
0.57
−2.7


#### 3.2.3. Robustness and Ruggedness

For the evaluation of the method robustness, some parameters were interchanged: pH, dye concentration, wavelength range, and shaking time. The capacity remains unaffected by small deliberate variations. Method ruggedness was expressed as RSD% of the same procedure applied by two analysts and using different instruments on different days. The results showed no statistical differences between different analysts and instruments, suggesting that the developed methods were robust and rugged (Table4).Table 4
The results of analysis of pharmaceutical preparation and standard of fluoroquinolones by two different analysts and instruments (n=6).
Method
Different instruments
Different analysts
X
±SD
RSD (%)
X
±SD
RSD (%)
Ofloxacin-BTB pure ofloxacin (10µg·mL−1) Mekopharm (200 mg ofloxacin per tablet)
10.21
0.19
1.86
9.93
0.24
2.42
199
0.57
0.29
196
0.76
0.39
Levofloxacin-BTB pure levofloxacin (10µg·mL−1) Stada (500 mg levofloxacin per tablet)
10.16
0.15
1.48
10.19
0.21
2.06
498
0.61
0.12
501
0.85
0.17
Ciprofloxacin-BTB pure ciprofloxacin (10µg·mL−1) Hasancip (500 mg ciprofloxacin per tablet)
9.85
0.18
1.83
10.12
0.25
2.47
502
0.64
0.13
497
0.92
0.19


#### 3.2.4. Selectivity and Effect of Interferences

The effect of commonly utilized excipients in drug formulation was studied. The investigated FQs were studied with various excipients such as magnesium stearate, glucose, lactose, starch, and sodium chloride which were prepared in the proportion corresponding to their amounts in the real drugs with a final dosage of 10µg/mL FQ. The effect of excipients on the determination of FQs was evaluated by recovery when determining FQs analyzed with the proposed method in the presence of excipient (Table 5).Table 5
The effect of excipients on the determination of fluoroquinolones (10µg/mL).
Recovery (%) ± SD
Excipients
Amount of excipient added (μg/mL)
Ofloxacin
Levofloxacin
Ciprofloxacin
Magnesium stearate
500
102.04 ± 0.12
101.23 ± 0.089
98.53 ± 0.91
Glucose
250
100.17 ± 0.16
99.04 ± 0.14
99.08 ± 0.062
Lactose
500
99.92 ± 0.21
100.20 ± 0.12
99.73 ± 0.21
Starch
200
100.96 ± 0.24
98.89 ± 0.13
101.31 ± 0.17
Sodium chloride
500
100.13 ± 0.24
100.15 ± 0.11
99.75 ± 0.16The results in Table5 show that the recoveries are in the range of 98.53–102.04, demonstrating that there is no interference of excipients when FQs in drugs are quantified by extractive spectrophotometric using ion-pair formation with BTB. In other words, the present method has a high selectivity for determining FQs in its dosage forms.


### 3.3. Comparison with Other Spectrophotometric Methods

The proposed method compares with other reported methods. It has been observed that the extractive spectrophotometric method with BTB in the present study is of high sensitivity than other ones (Table6). It also does not need heating, the product is stable for a longer time, and the interferences are minimum.Table 6
The comparison of present study with other spectrophotometric methods.
Drug
Reagent
λ
max (nm)
Range of determination (μg/mL)
Molar absorptivity (L/mol⋅cm)
Remarks
Reference
Ciprofloxacin
Co (II) tetrathiocyanate
623
20–240
8.38 × 102
Less sensitive
[34]
Supracene violet 3
575
2.5–30
8.62 × 103
Less sensitive
[35]
Eosin Y
547
2–8
3.56 × 104
Less stable colour
[36]
Merbromin
545
2–15
1.23 × 104
Addition of CN–to inhibit Hg+2 ions
Ce(IV)- MBTH
630
10–50
—
Involves shaking time
[17]
Tris(o-phenanthroline) iron(II)
510
0.04–7.2
3.4 × 104
Involves shaking time and heating
[18]
Tris (bipyridyl) iron(II)
522
0.05–9
2.95 × 104
Involves shaking time and heating
CL
520
16–96
—
Involves shaking time and heating
[16]
TCNE
335
0.25–15
—
Involves shaking time and heating
Sudan II
550
0.8–7.1
5.3 × 104
Narrow linear range
[8]
Congo red
517
0.5–6.0
2.83 × 104
Gentian violet
585
0.5–10
2.21 × 104
Brilliant blue G
610
0.5–6.0
2.86 × 104
Narrow linear range and required pH adjustment
[37]
Bromocresol green
412
1–20
2.28 × 104
Required pH adjustment
[14]
BTB
420
0.5–25
2.09 × 104
Highly sensitive with wide linear dynamic ranges, no heating, and no pH adjustment
This study
Levofloxacin
Chloranilic acid
521
15–250
1.2 × 103
Less sensitive
[14]
Bromocresol green
411
1–20
2.16 × 104
Required pH adjustment
Eosin Y
547
2–8
4.83 × 104
Less stable colour
[36]
Merbromin
545
2–15
1.58 × 104
Addition of CN–to inhibit Hg+2 ions
Cobalt (II) tetrathiocyanate
623
20–240
—
Less sensitive
[34]
Bromophenol blue
424
1.85–31.5
1.98 × 104
Required pH adjustment
[19]
Bromocresol green
428
1.85–25
1.82 × 104
BTB
415
0.5–25
2.07 × 104
Highly sensitive with wide linear dynamic ranges, no heating, and no pH-adjustment
This study
Ofloxacin
Supracene violet 3
575
2.5–25
1.09 × 104
Less sensitive
[35]
Tropaeolin 000
485
2.5–30
8.23 × 102
Less sensitive
Sudan II
560
0.8–8.4
2.97 × 104
Narrow linear range
[8]
Congo red
530
0.5–5.5
3.29 × 104
Gentian violet
575
0.8–11
2.51 × 104
Bromocresol purple
400
1.0–16.0
2. 4 × 104
Required pH adjustment
[38]
Bromocresol green
410
1.0–16.0
1.96 × 104
Required pH adjustment
Bromophenol blue
410
5–25
1.03 × 104
Required close pH control and involved extraction steps
[20]
Bromothymol blue
415
2–15
2.01 × 104
Bromocresol purple
410
2–20
1.64 × 104
Bromothymol blue
415
1–35
1.44 × 104
Highly sensitive with wide linear dynamic ranges, no heating, and no pH-adjustment
This study


### 3.4. Analysis of Pharmaceutical Formulations

The proposed method was applied successfully for the determination of studied drugs in the pharmaceutical formulations (tablets and infusion) and the results are presented in Table7. Six replicated determinations were measured. Table 7 shows that satisfactory recovery data were obtained and the recovery efficiency varies from 97.41% to 101.20%, indicating high accuracy of the present method in determining real pharmaceutical samples.Table 7
Determination of the studied drugs in their pharmaceutical preparations using the proposed method (n=6).
Pharmaceutical preparation
Hasancip tablet
Kacipro tablet
Shandong infusion
Hebei infusion
Levofloxacin Stada
Levofloxacin DHG
Ofloxacin mekopharm
Labeled amount (mg/form)
500/tablet
500/tablet
200/100 mL
200/100 mL
500/tablet
500/tablet
200/tablet
Recovery (%) ± SD
98.89 ± 0.23
101.20 ± 0.20
97.41 ± 0.42
97.69 ± 0.36
99.53 ± 0.17
101.01 ± 0.35
99.58 ± 0.46


### 3.5. Comparison with HPLC-MS Method

In order to validate the experimental data in determining some real drug samples, HPLC-MS was used with the conditions described on Section2.6 according to the previously published paper [13]. The comparison between the results determined by the present method with HPLC-MS method was indicated in Table 8.Table 8
Amount of some fluoroquinolone antibiotics determined by the proposed method and HPLC-MS.
Sample
Amount (mg/tablet)
Difference (%)
Proposed method
HPLC -MS
Ciprofloxacin-Hasancip table
494.45 ± 11.63
446.93 ± 15.84
10.63
Ofloxacin mekopharm
199.16 ± 0.85
202.00 ± 2.72
−1.41
Levofloxacin DHG
505.05 ± 17.33
480.55 ± 54.16
5.10
Levofloxacin Stada
497.65 ± 9.24
486.04 ± 9.24
2.39Table8 shows a good agreement between the proposed method and HPLC-MS where the relative differences of two methods were less than 11%. Furthermore, the standard deviation of the proposed method is almost lower than that of HPLC-MS. Our results indicate that the extractive spectrophotometric determination of FQs using BTB dye in chloroform is a very good method to quantify the FQ in pharmaceutical formulations.


## 3.1. Optimum Reaction Conditions

### 3.1.1. Effect of Extracting Solvent

Six organic solvents including chloroform, carbon tetrachloride, dichloromethane, dichloroethane, benzene, and toluene were used to study the effect of solvent to ion-pair formation between FQs and BTB. Figure2 shows that chloroform is the most suitable solvent for the extraction of three FQs with low blank absorbance, highest absorbances, and lowest standard deviations. It implies that chloroform is the best extracting solvent to achieve a good recovery of the complexes with the shortest time to reach the equilibrium processes.Figure 2
The effect of solvent on the ion-pair complex formation (10µg/mL of fluoroquinolones (FQs) with bromothymol blue (BTB)).


### 3.1.2. Effect of pH

The pH of solution plays an important role in the complex formations. The effect of pH on the formation of ion pairs was examined by varying the pH from 2.0 to 6.0 by adjusting 1 M HCl and 1 M NaOH. The maximum absorbances were observed at pH 3.3, 3.4, and 3.5 for the complexes of BTB and OFX, CFX, and LFX, respectively (Figure3). These pH values correspond to the initial pH of the examined drug and the dye. Therefore, it is not necessary to adjust the pH before extraction.Figure 3
Effect of pH on the absorbances of 10μg/mL of OFX, LFX, and CFX.


### 3.1.3. Effect of Dye Concentration

The effect of dye concentrations was studied by adding different volumes of 0.025% BTB from 1.0 to 6.0 mL with a fixed concentration of FQs (10μg/mL) (Figure 4). Figure 4 shows that the maximum absorbance of the complex was achieved with 4.0 mL of 0.025% of BTB in each case and excess dye did not affect the absorbance of the complex. Therefore, 4.0 mL of 0.025% of BTB is optimum dye volume and it is kept as constant for further studies.Figure 4
Effect of the volume of 0.025% BTB on the absorbance of 10μg/mL of OFX, LFX, and CFX.


### 3.1.4. Effect of Shaking Time

The effect of shaking time on the formation and stability of the ion-pair complex was investigated by measuring the absorbance of the extracted ion associates with increasing time from 0 to 4.0 min. Figure5 shows that the ion-pair complexes were formed instantaneously with 2.0 min shaking time. Thus, 2.0 min is the optimum shaking time and it is fixed for further studies.Figure 5
Effect of shaking time on the ion-pair complexes.


### 3.1.5. Stoichiometry of Ion-Pair Complexes

Job’s method of continuous variation of equimolar solutions was employed to evaluate stoichiometry of the complex. A 3.0 × 10−4 M standard solution of three FQs and 3.0 × 10−4 M solution of BTB were used. A series of the solutions were prepared in which the total volume of drug and reagent was kept in 10 mL, whereas the absorbances were measured at 420, 415, and 418 nm, for CFX, LFX, and OFX, respectively. The absorbances were plotted against the mole fraction of the drugs. The stoichiometry for each drug-dye ion-pair complex was found to be 1 : 1 (Figure 6).Figure 6
Job’s method of continuous variation graph for the reaction of drug with acid dyes BTB, [drug] = [dye] = 3.0 × 10−4 M.


### 3.1.6. Mechanism of Reaction and Absorption Spectra

Fluoroquinolones can contain a secondary amino group (CFX) and a tertiary amino group (LFX and OFX) that can be easily protonated under acidic conditions. On the one hand, the sulphonic acid group in BTB, that is, the only group undergoing dissociation in the pH range 1–5. The colour of BTB is on the basis of lactoid ring and subsequent formation of quinoid group. It is suggested that the two tautomers are plausible in equilibrium due to strong acidic nature of the sulphonic acid group. Thus, the quinoid body must predominate. Finally, the protonated fluoroquinolones form ion pairs with BTB dye that could be quantitatively extracted into chloroform. The possible reaction mechanisms are proposed and given in a scheme in Figure7.Figure 7
Proposal mechanism for the reaction between levofloxacin, ofloxacin, and bromothymol blue.The absorption spectra of the ion-pair complexes, which were formed between FQs and BTB, were measured in the wavelength range 350–500 nm against the blank solution and shown in Figure8.Figure 8
Absorption spectrum of ion-associate complexes of fluoroquinolones (10µg/mL) with BTB against reagent blank.Figure8 shows that absorption maxima for CFX-BTB, LFX-BTB, and OFX-BTB in chloroform were observed at 420, 415, and 418 nm, respectively. The reagent blanks under similar conditions have insignificant absorbances. At wavelengths 420, 415, and 418 nm, absorption spectrum of BTB does not affect the absorption spectrum of ion-associate complexes of FQs. Therefore, the selectivity of the proposed method for the determination of FQs is guaranteed.


### 3.1.7. Association Constants of Ion-Pair Complexes

The equation of association constant of ion-pair complex is(1)A/Am1−A/Amn+2CMnn,where A and Am are the observed absorbance and the maximum absorbance value when all the drug present is associated, respectively. CM is the molar concentration of the drugs at the maximum absorbance and n is the stoichiometry in which BTB ion associates with drugs. The conditional stability constants (Kf) of the ion-pair complexes according to Britton [32] for the cases of FQs were calculated from the continuous variation data using the following equation:(2)Kf=A/Am1−A/Amn+2CMnn.The conditional stability constants (Kf) of the ion-pair complexes for FQs are indicated in Table 1.Table 1
The conditional stability constants (Kf) of the ion-pair complexes for FQs.
Sample
V
drug (mL)
V
BTB (mL)
A
n
n
⋀
n
1
−
A
/
A
m
n
+
2
K
f
logKf
Mean
Ofloxacin
1
0.25
2.25
0.202
0.1111
0.7834
0.3116
50204.7802
4.7007
6.08
2
0.5
2
0.272
0.2500
0.7071
0.1486
157048.9127
5.1960
3
0.75
1.75
0.336
0.4286
0.6955
0.0512
572507.7789
5.7578
4
1
1.5
0.419
0.6667
0.7631
0.0035
9562329.8320
6.9806
5
1.25
1.25
0.476
1.0000
1.0000
0.0000
_
_
6
1.5
1
0.432
1.5000
1.8371
0.0002
59414177.6247
7.7739
7
1.75
0.75
0.356
2.3333
7.2213
0.0026
1172246.1806
6.0690
Levofloxacin
1
0.25
2.25
0.137
0.1111
0.7834
0.5749
14789.8587
4.1700
6.04
2
0.5
2
0.313
0.2500
0.7071
0.1856
115961.3839
5.0643
3
0.75
1.75
0.432
0.4286
0.6955
0.0426
708574.1920
5.8504
4
1
1.5
0.559
0.6667
0.7631
0.0005
67745245.6475
7.8309
5
1.25
1.25
0.594
1.0000
1.0000
0.0000
_
_
6
1.5
1
0.53
1.5000
1.8371
0.0004
34165312.8945
7.5336
7
1.75
0.75
0.426
2.3333
7.2213
0.0042
682897.0665
5.8344
Ciprofloxacin
1
0.25
2.25
0.392
0.1111
0.7834
0.2112
83530.0520
4.9218
5.91
2
0.5
2
0.452
0.2500
0.7071
0.1265
178145.0100
5.2508
3
0.75
1.75
0.564
0.4286
0.6955
0.0345
828480.0305
5.9183
4
1
1.5
0.661
0.6667
0.7631
0.0036
8522213.4055
6.9306
5
1.25
1.25
0.752
1.0000
1.0000
0.0000
_
_
6
1.5
1
0.615
1.5000
1.8371
0.0026
4572267.1248
6.6601
7
1.75
0.75
0.538
2.3333
7.2213
0.0043
608798.6008
5.7845
—, not determined.Table1 shows that the log Kf values of ion-pair associates for OFX-BTB, LFX-BTB, and CFX-BTB were 6.08 ± 0.46, 6.04 ± 0.58, and 5.91 ± 0.32, respectively (numbers of replicated experiments, n=6). The obtained results confirmed that the ion-pair formation complexes are of high stability.


## 3.1.1. Effect of Extracting Solvent

Six organic solvents including chloroform, carbon tetrachloride, dichloromethane, dichloroethane, benzene, and toluene were used to study the effect of solvent to ion-pair formation between FQs and BTB. Figure2 shows that chloroform is the most suitable solvent for the extraction of three FQs with low blank absorbance, highest absorbances, and lowest standard deviations. It implies that chloroform is the best extracting solvent to achieve a good recovery of the complexes with the shortest time to reach the equilibrium processes.Figure 2
The effect of solvent on the ion-pair complex formation (10µg/mL of fluoroquinolones (FQs) with bromothymol blue (BTB)).


## 3.1.2. Effect of pH

The pH of solution plays an important role in the complex formations. The effect of pH on the formation of ion pairs was examined by varying the pH from 2.0 to 6.0 by adjusting 1 M HCl and 1 M NaOH. The maximum absorbances were observed at pH 3.3, 3.4, and 3.5 for the complexes of BTB and OFX, CFX, and LFX, respectively (Figure3). These pH values correspond to the initial pH of the examined drug and the dye. Therefore, it is not necessary to adjust the pH before extraction.Figure 3
Effect of pH on the absorbances of 10μg/mL of OFX, LFX, and CFX.


## 3.1.3. Effect of Dye Concentration

The effect of dye concentrations was studied by adding different volumes of 0.025% BTB from 1.0 to 6.0 mL with a fixed concentration of FQs (10μg/mL) (Figure 4). Figure 4 shows that the maximum absorbance of the complex was achieved with 4.0 mL of 0.025% of BTB in each case and excess dye did not affect the absorbance of the complex. Therefore, 4.0 mL of 0.025% of BTB is optimum dye volume and it is kept as constant for further studies.Figure 4
Effect of the volume of 0.025% BTB on the absorbance of 10μg/mL of OFX, LFX, and CFX.


## 3.1.4. Effect of Shaking Time

The effect of shaking time on the formation and stability of the ion-pair complex was investigated by measuring the absorbance of the extracted ion associates with increasing time from 0 to 4.0 min. Figure5 shows that the ion-pair complexes were formed instantaneously with 2.0 min shaking time. Thus, 2.0 min is the optimum shaking time and it is fixed for further studies.Figure 5
Effect of shaking time on the ion-pair complexes.


## 3.1.5. Stoichiometry of Ion-Pair Complexes

Job’s method of continuous variation of equimolar solutions was employed to evaluate stoichiometry of the complex. A 3.0 × 10−4 M standard solution of three FQs and 3.0 × 10−4 M solution of BTB were used. A series of the solutions were prepared in which the total volume of drug and reagent was kept in 10 mL, whereas the absorbances were measured at 420, 415, and 418 nm, for CFX, LFX, and OFX, respectively. The absorbances were plotted against the mole fraction of the drugs. The stoichiometry for each drug-dye ion-pair complex was found to be 1 : 1 (Figure 6).Figure 6
Job’s method of continuous variation graph for the reaction of drug with acid dyes BTB, [drug] = [dye] = 3.0 × 10−4 M.


## 3.1.6. Mechanism of Reaction and Absorption Spectra

Fluoroquinolones can contain a secondary amino group (CFX) and a tertiary amino group (LFX and OFX) that can be easily protonated under acidic conditions. On the one hand, the sulphonic acid group in BTB, that is, the only group undergoing dissociation in the pH range 1–5. The colour of BTB is on the basis of lactoid ring and subsequent formation of quinoid group. It is suggested that the two tautomers are plausible in equilibrium due to strong acidic nature of the sulphonic acid group. Thus, the quinoid body must predominate. Finally, the protonated fluoroquinolones form ion pairs with BTB dye that could be quantitatively extracted into chloroform. The possible reaction mechanisms are proposed and given in a scheme in Figure7.Figure 7
Proposal mechanism for the reaction between levofloxacin, ofloxacin, and bromothymol blue.The absorption spectra of the ion-pair complexes, which were formed between FQs and BTB, were measured in the wavelength range 350–500 nm against the blank solution and shown in Figure8.Figure 8
Absorption spectrum of ion-associate complexes of fluoroquinolones (10µg/mL) with BTB against reagent blank.Figure8 shows that absorption maxima for CFX-BTB, LFX-BTB, and OFX-BTB in chloroform were observed at 420, 415, and 418 nm, respectively. The reagent blanks under similar conditions have insignificant absorbances. At wavelengths 420, 415, and 418 nm, absorption spectrum of BTB does not affect the absorption spectrum of ion-associate complexes of FQs. Therefore, the selectivity of the proposed method for the determination of FQs is guaranteed.


## 3.1.7. Association Constants of Ion-Pair Complexes

The equation of association constant of ion-pair complex is(1)A/Am1−A/Amn+2CMnn,where A and Am are the observed absorbance and the maximum absorbance value when all the drug present is associated, respectively. CM is the molar concentration of the drugs at the maximum absorbance and n is the stoichiometry in which BTB ion associates with drugs. The conditional stability constants (Kf) of the ion-pair complexes according to Britton [32] for the cases of FQs were calculated from the continuous variation data using the following equation:(2)Kf=A/Am1−A/Amn+2CMnn.The conditional stability constants (Kf) of the ion-pair complexes for FQs are indicated in Table 1.Table 1
The conditional stability constants (Kf) of the ion-pair complexes for FQs.
Sample
V
drug (mL)
V
BTB (mL)
A
n
n
⋀
n
1
−
A
/
A
m
n
+
2
K
f
logKf
Mean
Ofloxacin
1
0.25
2.25
0.202
0.1111
0.7834
0.3116
50204.7802
4.7007
6.08
2
0.5
2
0.272
0.2500
0.7071
0.1486
157048.9127
5.1960
3
0.75
1.75
0.336
0.4286
0.6955
0.0512
572507.7789
5.7578
4
1
1.5
0.419
0.6667
0.7631
0.0035
9562329.8320
6.9806
5
1.25
1.25
0.476
1.0000
1.0000
0.0000
_
_
6
1.5
1
0.432
1.5000
1.8371
0.0002
59414177.6247
7.7739
7
1.75
0.75
0.356
2.3333
7.2213
0.0026
1172246.1806
6.0690
Levofloxacin
1
0.25
2.25
0.137
0.1111
0.7834
0.5749
14789.8587
4.1700
6.04
2
0.5
2
0.313
0.2500
0.7071
0.1856
115961.3839
5.0643
3
0.75
1.75
0.432
0.4286
0.6955
0.0426
708574.1920
5.8504
4
1
1.5
0.559
0.6667
0.7631
0.0005
67745245.6475
7.8309
5
1.25
1.25
0.594
1.0000
1.0000
0.0000
_
_
6
1.5
1
0.53
1.5000
1.8371
0.0004
34165312.8945
7.5336
7
1.75
0.75
0.426
2.3333
7.2213
0.0042
682897.0665
5.8344
Ciprofloxacin
1
0.25
2.25
0.392
0.1111
0.7834
0.2112
83530.0520
4.9218
5.91
2
0.5
2
0.452
0.2500
0.7071
0.1265
178145.0100
5.2508
3
0.75
1.75
0.564
0.4286
0.6955
0.0345
828480.0305
5.9183
4
1
1.5
0.661
0.6667
0.7631
0.0036
8522213.4055
6.9306
5
1.25
1.25
0.752
1.0000
1.0000
0.0000
_
_
6
1.5
1
0.615
1.5000
1.8371
0.0026
4572267.1248
6.6601
7
1.75
0.75
0.538
2.3333
7.2213
0.0043
608798.6008
5.7845
—, not determined.Table1 shows that the log Kf values of ion-pair associates for OFX-BTB, LFX-BTB, and CFX-BTB were 6.08 ± 0.46, 6.04 ± 0.58, and 5.91 ± 0.32, respectively (numbers of replicated experiments, n=6). The obtained results confirmed that the ion-pair formation complexes are of high stability.


## 3.2. Validation of the Present Method

The proposed methods are validated according to ICH recommendations Q2(R1) [33]. The parameters that have been investigated are indicated below.


### 3.2.1. Linearity, Sensitivity, and Limits of Detection and Quantification

A linear relationship between the measured absorbance and the concentration range studied for each drug as shown in Figure9 and the correlation coefficient (R) of at least 0.997 were achieved. The limit of detection (LOD) and quantification (LOQ) of the method are determined by 3.3SD/b and 10SD/b, respectively, where SD is the standard deviation of blank absorbance values and b is the slope of the calibration curve equation.Figure 9
Calibration curves for OFX, LFX, and CFX at 418, 415, and 420 nm, respectively.The LOD and LOQ values, slope, and intercept of linear graphs for all the drugs and analytical parameters are indicated in Table2. The molar absorptivities and Sandell’s sensitivity of each methods were calculated and these values showed that the molar absorptivity of ion-pair complexes was in the order CFX-BTB > LFX-BTB > OFX-BTB.Table 2
Analytical characteristics of the proposed methods (n=6).
Parameters
Proposed methods
Ofloxacin
Levofloxacin
Ciprofloxacin
Colour
Yellow
Yellow
Yellow
Wavelengthsλmax (nm)
418
415
420
pH
3.3
3.5
3.4
Stability (h)
24
24
24
Shaking time (min)
2
2
2
Stoichiometric ratio
1 : 1
1 : 1
1 : 1
Beer’s law range (µg/mL)
1–35
0.5–25
0.5–25
Limit of detection, LOD (µg/mL)
0.105
0.101
0.084
Limit of quantitation, LOQ (µg/mL)
0.315
0.303
0.252
Molar absorptivity (L/mol.cm)
1.44 × 104
2.07 × 104
2.09 × 104
Sandell’s sensitivity (µg/cm2)
0.068
0.048
0.046
Regression equation (Y = bx + a), where Y is the absorbance, a is the intercept, b is the slope, and x is the concentration in μg/mL
Slope (b)
0.040
0.057
0.061
Intercept (a)
0.0165
0.072
0.089
Correlation coefficient (R)
0.998
0.997
0.998


### 3.2.2. Accuracy and Precision

The accuracy and precision of the methods were determined by preparing solutions of three different concentrations of drug and analyzing them in six replicates. The precision of the proposed methods was evaluated as percentage relative standard deviation (RSD%) and accuracy as percentage relative error (RE%). The percentage relative error was calculated using the following equation:(3)RE%=founded–addedadded×100.The accuracy and precision were summarized in Table3. The low values of the RSD and RE confirm the high precision and the good accuracy of the present method.Table 3
Evaluation of accuracy and precision of the proposed methods (n=6).
Method
Additive concentration (μg/mL)
Found concentration (μg/mL)
Recovery (%)
RSD (%)
RE (%)
Ofloxacin
5.00
5.11
102.19
2.31
2.2
10.00
10.26
102.64
1.34
2.6
15.00
14.89
99.25
0.88
−0.73
Levofloxacin
5.00
5.16
102.70
2.03
2.8
10.00
10.16
101.56
1.10
1.6
15.00
14.82
98.80
0.50
−1.2
Ciprofloxacin
5.00
5.13
102.71
1.92
2.6
10.00
9.74
97.41
0.52
−2.6
15.00
14.60
97.33
0.57
−2.7


### 3.2.3. Robustness and Ruggedness

For the evaluation of the method robustness, some parameters were interchanged: pH, dye concentration, wavelength range, and shaking time. The capacity remains unaffected by small deliberate variations. Method ruggedness was expressed as RSD% of the same procedure applied by two analysts and using different instruments on different days. The results showed no statistical differences between different analysts and instruments, suggesting that the developed methods were robust and rugged (Table4).Table 4
The results of analysis of pharmaceutical preparation and standard of fluoroquinolones by two different analysts and instruments (n=6).
Method
Different instruments
Different analysts
X
±SD
RSD (%)
X
±SD
RSD (%)
Ofloxacin-BTB pure ofloxacin (10µg·mL−1) Mekopharm (200 mg ofloxacin per tablet)
10.21
0.19
1.86
9.93
0.24
2.42
199
0.57
0.29
196
0.76
0.39
Levofloxacin-BTB pure levofloxacin (10µg·mL−1) Stada (500 mg levofloxacin per tablet)
10.16
0.15
1.48
10.19
0.21
2.06
498
0.61
0.12
501
0.85
0.17
Ciprofloxacin-BTB pure ciprofloxacin (10µg·mL−1) Hasancip (500 mg ciprofloxacin per tablet)
9.85
0.18
1.83
10.12
0.25
2.47
502
0.64
0.13
497
0.92
0.19


### 3.2.4. Selectivity and Effect of Interferences

The effect of commonly utilized excipients in drug formulation was studied. The investigated FQs were studied with various excipients such as magnesium stearate, glucose, lactose, starch, and sodium chloride which were prepared in the proportion corresponding to their amounts in the real drugs with a final dosage of 10µg/mL FQ. The effect of excipients on the determination of FQs was evaluated by recovery when determining FQs analyzed with the proposed method in the presence of excipient (Table 5).Table 5
The effect of excipients on the determination of fluoroquinolones (10µg/mL).
Recovery (%) ± SD
Excipients
Amount of excipient added (μg/mL)
Ofloxacin
Levofloxacin
Ciprofloxacin
Magnesium stearate
500
102.04 ± 0.12
101.23 ± 0.089
98.53 ± 0.91
Glucose
250
100.17 ± 0.16
99.04 ± 0.14
99.08 ± 0.062
Lactose
500
99.92 ± 0.21
100.20 ± 0.12
99.73 ± 0.21
Starch
200
100.96 ± 0.24
98.89 ± 0.13
101.31 ± 0.17
Sodium chloride
500
100.13 ± 0.24
100.15 ± 0.11
99.75 ± 0.16The results in Table5 show that the recoveries are in the range of 98.53–102.04, demonstrating that there is no interference of excipients when FQs in drugs are quantified by extractive spectrophotometric using ion-pair formation with BTB. In other words, the present method has a high selectivity for determining FQs in its dosage forms.


## 3.2.1. Linearity, Sensitivity, and Limits of Detection and Quantification

A linear relationship between the measured absorbance and the concentration range studied for each drug as shown in Figure9 and the correlation coefficient (R) of at least 0.997 were achieved. The limit of detection (LOD) and quantification (LOQ) of the method are determined by 3.3SD/b and 10SD/b, respectively, where SD is the standard deviation of blank absorbance values and b is the slope of the calibration curve equation.Figure 9
Calibration curves for OFX, LFX, and CFX at 418, 415, and 420 nm, respectively.The LOD and LOQ values, slope, and intercept of linear graphs for all the drugs and analytical parameters are indicated in Table2. The molar absorptivities and Sandell’s sensitivity of each methods were calculated and these values showed that the molar absorptivity of ion-pair complexes was in the order CFX-BTB > LFX-BTB > OFX-BTB.Table 2
Analytical characteristics of the proposed methods (n=6).
Parameters
Proposed methods
Ofloxacin
Levofloxacin
Ciprofloxacin
Colour
Yellow
Yellow
Yellow
Wavelengthsλmax (nm)
418
415
420
pH
3.3
3.5
3.4
Stability (h)
24
24
24
Shaking time (min)
2
2
2
Stoichiometric ratio
1 : 1
1 : 1
1 : 1
Beer’s law range (µg/mL)
1–35
0.5–25
0.5–25
Limit of detection, LOD (µg/mL)
0.105
0.101
0.084
Limit of quantitation, LOQ (µg/mL)
0.315
0.303
0.252
Molar absorptivity (L/mol.cm)
1.44 × 104
2.07 × 104
2.09 × 104
Sandell’s sensitivity (µg/cm2)
0.068
0.048
0.046
Regression equation (Y = bx + a), where Y is the absorbance, a is the intercept, b is the slope, and x is the concentration in μg/mL
Slope (b)
0.040
0.057
0.061
Intercept (a)
0.0165
0.072
0.089
Correlation coefficient (R)
0.998
0.997
0.998


## 3.2.2. Accuracy and Precision

The accuracy and precision of the methods were determined by preparing solutions of three different concentrations of drug and analyzing them in six replicates. The precision of the proposed methods was evaluated as percentage relative standard deviation (RSD%) and accuracy as percentage relative error (RE%). The percentage relative error was calculated using the following equation:(3)RE%=founded–addedadded×100.The accuracy and precision were summarized in Table3. The low values of the RSD and RE confirm the high precision and the good accuracy of the present method.Table 3
Evaluation of accuracy and precision of the proposed methods (n=6).
Method
Additive concentration (μg/mL)
Found concentration (μg/mL)
Recovery (%)
RSD (%)
RE (%)
Ofloxacin
5.00
5.11
102.19
2.31
2.2
10.00
10.26
102.64
1.34
2.6
15.00
14.89
99.25
0.88
−0.73
Levofloxacin
5.00
5.16
102.70
2.03
2.8
10.00
10.16
101.56
1.10
1.6
15.00
14.82
98.80
0.50
−1.2
Ciprofloxacin
5.00
5.13
102.71
1.92
2.6
10.00
9.74
97.41
0.52
−2.6
15.00
14.60
97.33
0.57
−2.7


## 3.2.3. Robustness and Ruggedness

For the evaluation of the method robustness, some parameters were interchanged: pH, dye concentration, wavelength range, and shaking time. The capacity remains unaffected by small deliberate variations. Method ruggedness was expressed as RSD% of the same procedure applied by two analysts and using different instruments on different days. The results showed no statistical differences between different analysts and instruments, suggesting that the developed methods were robust and rugged (Table4).Table 4
The results of analysis of pharmaceutical preparation and standard of fluoroquinolones by two different analysts and instruments (n=6).
Method
Different instruments
Different analysts
X
±SD
RSD (%)
X
±SD
RSD (%)
Ofloxacin-BTB pure ofloxacin (10µg·mL−1) Mekopharm (200 mg ofloxacin per tablet)
10.21
0.19
1.86
9.93
0.24
2.42
199
0.57
0.29
196
0.76
0.39
Levofloxacin-BTB pure levofloxacin (10µg·mL−1) Stada (500 mg levofloxacin per tablet)
10.16
0.15
1.48
10.19
0.21
2.06
498
0.61
0.12
501
0.85
0.17
Ciprofloxacin-BTB pure ciprofloxacin (10µg·mL−1) Hasancip (500 mg ciprofloxacin per tablet)
9.85
0.18
1.83
10.12
0.25
2.47
502
0.64
0.13
497
0.92
0.19


## 3.2.4. Selectivity and Effect of Interferences

The effect of commonly utilized excipients in drug formulation was studied. The investigated FQs were studied with various excipients such as magnesium stearate, glucose, lactose, starch, and sodium chloride which were prepared in the proportion corresponding to their amounts in the real drugs with a final dosage of 10µg/mL FQ. The effect of excipients on the determination of FQs was evaluated by recovery when determining FQs analyzed with the proposed method in the presence of excipient (Table 5).Table 5
The effect of excipients on the determination of fluoroquinolones (10µg/mL).
Recovery (%) ± SD
Excipients
Amount of excipient added (μg/mL)
Ofloxacin
Levofloxacin
Ciprofloxacin
Magnesium stearate
500
102.04 ± 0.12
101.23 ± 0.089
98.53 ± 0.91
Glucose
250
100.17 ± 0.16
99.04 ± 0.14
99.08 ± 0.062
Lactose
500
99.92 ± 0.21
100.20 ± 0.12
99.73 ± 0.21
Starch
200
100.96 ± 0.24
98.89 ± 0.13
101.31 ± 0.17
Sodium chloride
500
100.13 ± 0.24
100.15 ± 0.11
99.75 ± 0.16The results in Table5 show that the recoveries are in the range of 98.53–102.04, demonstrating that there is no interference of excipients when FQs in drugs are quantified by extractive spectrophotometric using ion-pair formation with BTB. In other words, the present method has a high selectivity for determining FQs in its dosage forms.


## 3.3. Comparison with Other Spectrophotometric Methods

The proposed method compares with other reported methods. It has been observed that the extractive spectrophotometric method with BTB in the present study is of high sensitivity than other ones (Table6). It also does not need heating, the product is stable for a longer time, and the interferences are minimum.Table 6
The comparison of present study with other spectrophotometric methods.
Drug
Reagent
λ
max (nm)
Range of determination (μg/mL)
Molar absorptivity (L/mol⋅cm)
Remarks
Reference
Ciprofloxacin
Co (II) tetrathiocyanate
623
20–240
8.38 × 102
Less sensitive
[34]
Supracene violet 3
575
2.5–30
8.62 × 103
Less sensitive
[35]
Eosin Y
547
2–8
3.56 × 104
Less stable colour
[36]
Merbromin
545
2–15
1.23 × 104
Addition of CN–to inhibit Hg+2 ions
Ce(IV)- MBTH
630
10–50
—
Involves shaking time
[17]
Tris(o-phenanthroline) iron(II)
510
0.04–7.2
3.4 × 104
Involves shaking time and heating
[18]
Tris (bipyridyl) iron(II)
522
0.05–9
2.95 × 104
Involves shaking time and heating
CL
520
16–96
—
Involves shaking time and heating
[16]
TCNE
335
0.25–15
—
Involves shaking time and heating
Sudan II
550
0.8–7.1
5.3 × 104
Narrow linear range
[8]
Congo red
517
0.5–6.0
2.83 × 104
Gentian violet
585
0.5–10
2.21 × 104
Brilliant blue G
610
0.5–6.0
2.86 × 104
Narrow linear range and required pH adjustment
[37]
Bromocresol green
412
1–20
2.28 × 104
Required pH adjustment
[14]
BTB
420
0.5–25
2.09 × 104
Highly sensitive with wide linear dynamic ranges, no heating, and no pH adjustment
This study
Levofloxacin
Chloranilic acid
521
15–250
1.2 × 103
Less sensitive
[14]
Bromocresol green
411
1–20
2.16 × 104
Required pH adjustment
Eosin Y
547
2–8
4.83 × 104
Less stable colour
[36]
Merbromin
545
2–15
1.58 × 104
Addition of CN–to inhibit Hg+2 ions
Cobalt (II) tetrathiocyanate
623
20–240
—
Less sensitive
[34]
Bromophenol blue
424
1.85–31.5
1.98 × 104
Required pH adjustment
[19]
Bromocresol green
428
1.85–25
1.82 × 104
BTB
415
0.5–25
2.07 × 104
Highly sensitive with wide linear dynamic ranges, no heating, and no pH-adjustment
This study
Ofloxacin
Supracene violet 3
575
2.5–25
1.09 × 104
Less sensitive
[35]
Tropaeolin 000
485
2.5–30
8.23 × 102
Less sensitive
Sudan II
560
0.8–8.4
2.97 × 104
Narrow linear range
[8]
Congo red
530
0.5–5.5
3.29 × 104
Gentian violet
575
0.8–11
2.51 × 104
Bromocresol purple
400
1.0–16.0
2. 4 × 104
Required pH adjustment
[38]
Bromocresol green
410
1.0–16.0
1.96 × 104
Required pH adjustment
Bromophenol blue
410
5–25
1.03 × 104
Required close pH control and involved extraction steps
[20]
Bromothymol blue
415
2–15
2.01 × 104
Bromocresol purple
410
2–20
1.64 × 104
Bromothymol blue
415
1–35
1.44 × 104
Highly sensitive with wide linear dynamic ranges, no heating, and no pH-adjustment
This study


## 3.4. Analysis of Pharmaceutical Formulations

The proposed method was applied successfully for the determination of studied drugs in the pharmaceutical formulations (tablets and infusion) and the results are presented in Table7. Six replicated determinations were measured. Table 7 shows that satisfactory recovery data were obtained and the recovery efficiency varies from 97.41% to 101.20%, indicating high accuracy of the present method in determining real pharmaceutical samples.Table 7
Determination of the studied drugs in their pharmaceutical preparations using the proposed method (n=6).
Pharmaceutical preparation
Hasancip tablet
Kacipro tablet
Shandong infusion
Hebei infusion
Levofloxacin Stada
Levofloxacin DHG
Ofloxacin mekopharm
Labeled amount (mg/form)
500/tablet
500/tablet
200/100 mL
200/100 mL
500/tablet
500/tablet
200/tablet
Recovery (%) ± SD
98.89 ± 0.23
101.20 ± 0.20
97.41 ± 0.42
97.69 ± 0.36
99.53 ± 0.17
101.01 ± 0.35
99.58 ± 0.46


## 3.5. Comparison with HPLC-MS Method

In order to validate the experimental data in determining some real drug samples, HPLC-MS was used with the conditions described on Section2.6 according to the previously published paper [13]. The comparison between the results determined by the present method with HPLC-MS method was indicated in Table 8.Table 8
Amount of some fluoroquinolone antibiotics determined by the proposed method and HPLC-MS.
Sample
Amount (mg/tablet)
Difference (%)
Proposed method
HPLC -MS
Ciprofloxacin-Hasancip table
494.45 ± 11.63
446.93 ± 15.84
10.63
Ofloxacin mekopharm
199.16 ± 0.85
202.00 ± 2.72
−1.41
Levofloxacin DHG
505.05 ± 17.33
480.55 ± 54.16
5.10
Levofloxacin Stada
497.65 ± 9.24
486.04 ± 9.24
2.39Table8 shows a good agreement between the proposed method and HPLC-MS where the relative differences of two methods were less than 11%. Furthermore, the standard deviation of the proposed method is almost lower than that of HPLC-MS. Our results indicate that the extractive spectrophotometric determination of FQs using BTB dye in chloroform is a very good method to quantify the FQ in pharmaceutical formulations.


## 4. Conclusions

We have reported a new method when using BTB as an anionic dyes for the extractive spectrophotometric determination of ciprofloxacin (CFX), levofloxacin (LFX), and ofloxacin (OFX) in different pharmaceutical drugs (tablets and infusions). The methods have the advantages of simplicity without heating, pH-adjustment, and high sensitivity. The limit of detection (LOD) values are 0.084µg/mL for CFX, 0.101 µg/mL for LFX, and 0.105 µg/mL for OFX. No interference from common excipients was confirmed. The stoichiometry complexes of FQs and BTB determined by Job’s method of continuous variation were found to be 1 : 1. The developed and validated methods are indicated as the acceptable precision and accuracy, and recovery of the drugs and suitable for routine analysis of drugs in pharmaceutical formulations. The results of some real samples by the present method that were compared with HPLC-MS method with the relative differences are less than 11%, indicating that the present method is good for determination of FQs in pharmaceutical formulations.



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