# Thionine-Bromate as a New Reaction System for Kinetic Spectrophotometric Determination of Hydrazine in Cooling Tower Water Samples

Authors: Masoud Reza Shishehbore; Ali Sheibani; Masoumeh Eslami
Journal: Journal of Chemistry
 (2013)

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## Abstract

A simple, selective, and inexpensive kinetic method was developed for the determination of hydrazine based on its inhibitory effect on the thionine-bromate system in sulfuric acid media. The reaction was monitored spectrophotometrically at 601 nm by a fixed time method. The effect of different parameters such as concentration of reactants, ionic strength, temperature, and time on the rate of reaction was investigated, and the optimum conditions were obtained. Under optimum conditions, the calibration curve was linear in the concentration range from 0.8–23.0μg mL−1 of hydrazine, and the detection limit of the method was 0.22 μg mL−1. The relative standard deviation for five replicate determinations of 1.0 μg mL−1 of hydrazine was 0.74%. The potential of interfering effect of foreign species on the hydrazine determination was studied. The proposed method was successfully applied for the determination of hydrazine in different water samples.


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## Body

## 1. Introduction

Hydrazine is a strong reducing agent that is used as an oxygen scavenger in boilers. Hydrazine and its derivatives are also used widely in industry and agriculture as fuel in rockets and fuel cells, antioxidant, corrosion inhibitor, catalyst, emulsifier, insecticide and pesticide, plant-growth regulator, photographic developer, dyes stuff, explosive, and blowing agent for plastics [1–3]. Hydrazine that can be absorbed through skin has carcinogenic and hepatotoxic effects. It affects the liver, the kidney, and the brain; therefore, it is important in pharmacology. Furthermore, hydrazine is suspected of being a mutagen and carcinogenic compound [4]. Since the toxicity of hydrazine is well known, a sensitive and accurate method requires for the determination of trace amounts of hydrazine in different samples.Various instrumental methods were used for the determination of hydrazine. These include chromatography [5, 6], capillary electrophoresis [7], voltammetry [8, 9], spectrophotometry [10], spectrofluorimetry [11], chemiluminescence [12], potentiometry [13], and amperometry [14]. Some of these methods have limitations such as hard operation and high cost. Catalytic spectrophotometric methods, because of their excellent sensitivity, sufficient accuracy, simple procedure, and inexpensive apparatus, are more attractive for the determination of hydrazine and a large group of compounds in different matrices [15–24].In this paper, a kinetic spectrophotometric method was developed for the determination of hydrazine based on its inhibitory effect on the reaction of bromate with thionine in acidic media. The developed method surpasses reported kinetic spectrophotometric methods in the linear dynamic range [20, 22–24] and detection limit [19, 21] for hydrazine determination. However, lower detection limit [18] and wider linear dynamic range [21] were also reported. The method has been successfully applied for the determination of hydrazine in different water samples.


## 2. Experimental

### 2.1. Reagents and Chemicals

Doubly distilled water and analytical grade chemical reagents were used. The hydrazine solution (200.0μg mL−1) was prepared by dilution of concentrated hydrazine (a=80%, d=1.03 g mL−1, Merck) to 250 mL with water as daily. A solution of Thionine (300.0 μmol L−1) was prepared by dissolving 0.0862 g of thionine (Merck) in water and diluting to 1000 mL in a volumetric flask. Sulfuric acid solution (4.0 mol L−1) was prepared by diluting 217.4 mL of concentrated sulfuric acid (a=98%, d=1.84 kg L−1, Merck) to 1000 mL. A potassium bromate solution (50.0 mmol L−1) was prepared by dissolving 8.3540 g of potassium bromate (Merck) in water and diluting to 1000 mL in a volumetric flask.


### 2.2. Apparatus

A Shimadzu UV-VIS spectrophotometer (160-A, Japan) with 1 cm matched glass cells was used to measure the absorbance. A thermostated water bath (Heidolph, Germany) was used to keep the reaction at desired temperature. A stopwatch was applied to record the reaction time.


### 2.3. General Procedure

The inhibited reaction was studied spectrophotometrically by monitoring the change in absorbance of the reaction mixture at 601 nm. For this purpose, to a series of 10 mL volumetric flasks, 1.9 mL of 4.0 mol L−1 sulfuric acid solution, 1.2 mL of 300.0 μmol L−1 thionine solution, and the sample or standard solutions containing 8.0–230.0 μg of hydrazine were added. The solution was mixed and diluted to 8 mL with water. Then, 0.08 mL of 50.0 mmol L−1 bromate solution was added and diluted to the mark. The solution was mixed thoroughly and a portion of it was transferred to a glass cell. The absorbance of inhibited reaction (ΔAs) was measured against water at 601 nm for time interval 0.5–2.5 min. The measurement in the absence of hydrazine was repeated to obtain the values for the uninhibited reaction (ΔAb). Finally, the difference in the absorbance change was considered as the response (ΔA=ΔAb-ΔAs).


## 2.1. Reagents and Chemicals

Doubly distilled water and analytical grade chemical reagents were used. The hydrazine solution (200.0μg mL−1) was prepared by dilution of concentrated hydrazine (a=80%, d=1.03 g mL−1, Merck) to 250 mL with water as daily. A solution of Thionine (300.0 μmol L−1) was prepared by dissolving 0.0862 g of thionine (Merck) in water and diluting to 1000 mL in a volumetric flask. Sulfuric acid solution (4.0 mol L−1) was prepared by diluting 217.4 mL of concentrated sulfuric acid (a=98%, d=1.84 kg L−1, Merck) to 1000 mL. A potassium bromate solution (50.0 mmol L−1) was prepared by dissolving 8.3540 g of potassium bromate (Merck) in water and diluting to 1000 mL in a volumetric flask.


## 2.2. Apparatus

A Shimadzu UV-VIS spectrophotometer (160-A, Japan) with 1 cm matched glass cells was used to measure the absorbance. A thermostated water bath (Heidolph, Germany) was used to keep the reaction at desired temperature. A stopwatch was applied to record the reaction time.


## 2.3. General Procedure

The inhibited reaction was studied spectrophotometrically by monitoring the change in absorbance of the reaction mixture at 601 nm. For this purpose, to a series of 10 mL volumetric flasks, 1.9 mL of 4.0 mol L−1 sulfuric acid solution, 1.2 mL of 300.0 μmol L−1 thionine solution, and the sample or standard solutions containing 8.0–230.0 μg of hydrazine were added. The solution was mixed and diluted to 8 mL with water. Then, 0.08 mL of 50.0 mmol L−1 bromate solution was added and diluted to the mark. The solution was mixed thoroughly and a portion of it was transferred to a glass cell. The absorbance of inhibited reaction (ΔAs) was measured against water at 601 nm for time interval 0.5–2.5 min. The measurement in the absence of hydrazine was repeated to obtain the values for the uninhibited reaction (ΔAb). Finally, the difference in the absorbance change was considered as the response (ΔA=ΔAb-ΔAs).


## 3. Results and Discussion

Figures1(a) and 1(b) show the absorption spectra of the reaction mixture (sulfuric acid, thionine, and bromate) in presence and absence of hydrazine, respectively. Since the absorbance change was reduced signficantly in presence of hydrazine, the proposed reaction system can be used for the determination of hydrazine. The possible mechanism of the reactions can be described as follows:
(1)BrO3-+H++Thionine(Red)→Br-+Thionine(Ox)BrO3-+H++Br-→Br2+H2OBr2+H++Thionine(Red)→Br-+Thionine(Ox),
where Red is the reduced form and Ox is the oxidized form of reactant. The presence of reducing agents that react slowly with bromate but rapidly with bromine inhibits the decolorizing reaction. According to the following reaction, hydrazine reacts with bromine and causes an inhibitory effect on the decolorization of Thionine by bromine. 						(2)Br2+H++Hydrazine(Red)→Br-+Hydrazine(Ox).
The level of inhibition depends on the amount of hydrazine in the reaction mixture. Therefore, this behavior allows developing an analytical method for the determination of hydrazine.Absorption spectra of (a) inhibited and (b) uninhibited reactions. Conditions: sulfuric acid, 0.5 mol L−1; thionine, 30.0 μmol L−1; hydrazine, 2.0 μg mL−1; bromate, 0.5 mmol L−1; 25°C and 4.0 min.
(a)
(b)


### 3.1. Effect of Variables

The effective parameters on the reaction rate including the reagents concentration, ionic strength, temperature, and time must be optimized to take full advantages. For this purpose, each parameter was optimized by setting other parameters constant. The maximum difference between the blank and sample absorbance change (ΔA) was considered to obtain more sensitive results.The influence of sulfuric acid concentration on the sensitivity was investigated in the range from 0.4–1.0 mol L−1 (Figure 2). The results show that the response was increased with increasing the sulfuric acid concentration up to 0.76 mol L−1 and decreased at higher concentrations. This may be attributed to protonation of thionine that might stop oxidation or make it quite difficult to occur. Therefore, 0.76 mol L−1 was selected as the optimum concentration of sulfuric acid.Figure 2
Effect of sulfuric acid concentration on the rate of uninhibited (ΔAb) and inhibited (ΔAs) reaction and response (ΔA). Conditions: thionine, 30.0 μmol L−1; hydrazine, 2.0 μg mL−1; bromate, 0.5 mmol L−1; 25°C and 4.0 min.The effect of thionine concentration was studied in the range from 18.0–75.0μmol L−1 at 0.76 mol L−1 of H2SO4 (Figure 3). According to Figure 3, the sensitivity was increased with increasing the thionine concentration up to 60.0 μmol L−1. Thus, 60.0 μmol L−1 was selected as the optimum value for thionine.Figure 3
Effect of thionine concentration on the rate of uninhibited (ΔAb) and inhibited (ΔAs) reaction and response (ΔA). Conditions: sulfuric acid, 0.76 mol L−1; bromate, 0.5 mmol L−1; 25°C and 4.0 min.Under the optimum concentrations of sulfuric acid and thionine, the effect of bromate concentration was investigated over the range from 0.25–0.55 mmol L−1 (Figure 4). As it can be seen in Figure 4, the maximum response was obtained at 0.4 mmol L−1 of bromate concentration. Therefore, this concentration was selected for further study.Figure 4
Effect of  bromate concentration on the rate of uninhibited (ΔAb) and inhibited (ΔAs) reaction and response (ΔA). Conditions: sulfuric acid, 0.76 mol L−1; thionine, 60.0 μmol L−1; 25°C and 4.0 min.Under the optimum reagents concentration, the effect of the ionic strength was studied in the range from 0.00–0.75 mol L−1 by using a sodium sulfate solution (3.0 mol L−1). The experimental results show that the response was not varied regularly with increasing the sodium sulfate concentration and the most sensitivity was obtained in absence of it. This may be attributed to the absorption behavior of thionine. In presence of sodium sulfate, the closeness of ions to thionine alters the molar absorptivity of it due to electrostatic interactions. Therefore, the effect of this parameter was overlooked.The influence of temperature on the reaction rate was studied in the range from 15–45°C with the obtained optimum conditions. The results in Figure5 show a maximum at 20°C. Therefore, this value was selected as the optimum temperature.Figure 5
Effect of temperature on the rate of uninhibited (ΔAb) and inhibited (ΔAs) reaction and response (ΔA). Conditions: sulfuric acid, 0.76 mol L−1; thionine, 60.0 μmol L−1; bromate, 0.4 mol L−1; and 4.0 min.The optimum time of reaction was found by measuring the change in the absorbance from 0.5–4.0 min. The reaction rate increased up to 2.5 min, and in longer times it was almost constant. Therefore, 2.5 min was selected as the optimum value.


### 3.2. Analytical Parameters

Under optimum conditions (sulfuric acid: 0.76 mol L−1; thionine: 60.0 μmol L−1; bromate: 0.4 mmol L−1; temperature: 20°C; time: 2.5 min), a linear calibration curve was obtained over the concentration range from 0.8–23.0 μg mL−1 of hydrazine including two linear segments of 0.8–6.0 and 6.0–23.0 μg mL−1. The data analysis gave the regression equations for the first and second linear segments of (3) as follows:
(3)ΔA=0.1393[C]+0.0074(R2=0.9994)ΔA=0.0312[C]+0.6576(R2=0.9996)
where ΔA is the difference in the absorbance changes between the blank and sample (response), C is the concentration of hydrazine (μg mL−1), and R2 is the correlation coefficient.The relative standard deviation of five replicate determinations was 0.74% for a solution of 1.0μg mL−1 of hydrazine. The detection limit, defined as D.L. = 3sb/m, where sb is standard deviation of the blank signal and m is the slope of the calibration curve, was 0.22 μg mL−1 of hydrazine.To study the selectivity of the proposed method, the effect of various species on the determination of 1.0μg mL−1 of hydrazine was investigated (Table 1). The tolerance limit was defined as the concentration of added species causing a relative error less than 5%. As it can be seen in Table 1, most of species did not interfere even when present in 100-fold excess over hydrazine.Table 1
Tolerance limit for various species for the determination of 1.0μg mL−1 of hydrazine.
Foreign species
Tolerance limit (wspecies/whydrazine)
EDTA, sulfamic acid
1000
Li+, Na+, K+, Ca2+, Mg2+
1000
NO
3
-, SO42-, PO43-, CH3CO2-, CO32-, HCO3-
1000
aFe3+, Cr3+, Zn2+
950
b
N
O
2
-
760
aFe2+
600
Cl−
50
aAfter adding 3 mL of 5% EDTA.
bAfter adding 3 mL of 3% sulfamic acid.In Table2, some of the analytical parameters obtained in this work are compared with those previously reported in the literature [21, 22, 24]. According to Table 2, the proposed method is comparable to other catalytic kinetic spectrophotometric methods. Therefore, the proposed method has the potential to offer itself as an alternative method for hydrazine analysis.Table 2
Comparison of some analytical parameters of catalytic spectrophotometric methods to proposed method.
Reaction system
Method
Effect on reaction system
L.R. (μg mL−1)
D.L. (μg mL−1)
Sample
Ref.
Mo(VI)-HCl
Fixed time
Inhibitory
3.2–448.0
1.0
Not applied
[21]
Neutral red-NO2-
Fixed time
Inhibitory
0.15–0.99
0.1
Water
[22]
HCl-BrO3-
Fixed time
Inhibitory
0.0096–1.02
0.0027
Water
[24]
Thionine-BrO3-
Fixed time
Inhibitory
0.8–23.0
0.22
Water and cooling tower water
This work


### 3.3. Application

In order to evaluate the capability of the proposed method, it was applied to the determination of hydrazine in different water samples. For this purpose, four water samples from three sources were examined. The distilled water and drinking water were spiked with 1.0μg mL−1 and 5.0 μg mL−1 of hydrazine. Cooling tower water samples were prepared from Yazd Power Generation Co and analysed as received. The obtained results were given in Table 3. The recoveries (n=3) were between 98.0 and 103.4% that confirm the reliability of the proposed method. Also, the same samples were analysed using ASTM method [25]. The recoveries vary over the range 98.7–102.4% for ASTM method. As it can be seen, the recoveries obtained from the two methods are in good agreement together. Moreover, the t-test for three replicate determinations at 95% confidence limit did not show a significant difference between the results obtained from the two methods.Table 3
The recovery results on the determination of hydrazine in the different water samples using the proposed method and the standard ASTM method.
Hydrazine (μg mL−1)
Sample
Proposed method
ASTM method
Statistical test
Added
Founda
Recovery (%)
Added
Founda
Recovery (%)
t testb
Distilled water
1.0
1.01 ± 0.01
102.0
1.0
0.99 ± 0.01
99.0
3.40
5.0
4.98 ± 0.05
99.6
5.0
5.01 ± 0.03
100.2
1.04
Drinking water
1.0
0.99 ± 0.03
99.0
1.0
1.01 ± 0.01
101.0
1.15
5.0
5.03 ± 0.04
100.6
5.0
4.98 ± 0.05
99.6
2.16
—
2.12 ± 0.02
—
2.09 ± 0.02
2.59
Cooling tower water (1)
1.0
3.14 ± 0.03
100.6
1.0
3.08 ± 0.03
98.7
3.46
5.0
7.05 ± 0.08
99.0
5.0
7.15 ± 0.08
102.4
2.16
15.0
17.19 ± 0.15
100.4
15.0
17.38 ± 0.18
101.7
2.19
—
2.25 ± 0.02
—
2.27 ± 0.02
1.73
Cooling tower water (2)
10.0
12.19 ± 0.11
99.5
10.0
12.28 ± 0.12
100.9
1.42
20.0
22.31 ± 0.21
100.3
20.0
22.08 ± 0.19
99.6
1.89
aMean ± standard deviation (n=3).
bTabulated t-value for three replicate determinations at P (0.95) is 4.30.


## 3.1. Effect of Variables

The effective parameters on the reaction rate including the reagents concentration, ionic strength, temperature, and time must be optimized to take full advantages. For this purpose, each parameter was optimized by setting other parameters constant. The maximum difference between the blank and sample absorbance change (ΔA) was considered to obtain more sensitive results.The influence of sulfuric acid concentration on the sensitivity was investigated in the range from 0.4–1.0 mol L−1 (Figure 2). The results show that the response was increased with increasing the sulfuric acid concentration up to 0.76 mol L−1 and decreased at higher concentrations. This may be attributed to protonation of thionine that might stop oxidation or make it quite difficult to occur. Therefore, 0.76 mol L−1 was selected as the optimum concentration of sulfuric acid.Figure 2
Effect of sulfuric acid concentration on the rate of uninhibited (ΔAb) and inhibited (ΔAs) reaction and response (ΔA). Conditions: thionine, 30.0 μmol L−1; hydrazine, 2.0 μg mL−1; bromate, 0.5 mmol L−1; 25°C and 4.0 min.The effect of thionine concentration was studied in the range from 18.0–75.0μmol L−1 at 0.76 mol L−1 of H2SO4 (Figure 3). According to Figure 3, the sensitivity was increased with increasing the thionine concentration up to 60.0 μmol L−1. Thus, 60.0 μmol L−1 was selected as the optimum value for thionine.Figure 3
Effect of thionine concentration on the rate of uninhibited (ΔAb) and inhibited (ΔAs) reaction and response (ΔA). Conditions: sulfuric acid, 0.76 mol L−1; bromate, 0.5 mmol L−1; 25°C and 4.0 min.Under the optimum concentrations of sulfuric acid and thionine, the effect of bromate concentration was investigated over the range from 0.25–0.55 mmol L−1 (Figure 4). As it can be seen in Figure 4, the maximum response was obtained at 0.4 mmol L−1 of bromate concentration. Therefore, this concentration was selected for further study.Figure 4
Effect of  bromate concentration on the rate of uninhibited (ΔAb) and inhibited (ΔAs) reaction and response (ΔA). Conditions: sulfuric acid, 0.76 mol L−1; thionine, 60.0 μmol L−1; 25°C and 4.0 min.Under the optimum reagents concentration, the effect of the ionic strength was studied in the range from 0.00–0.75 mol L−1 by using a sodium sulfate solution (3.0 mol L−1). The experimental results show that the response was not varied regularly with increasing the sodium sulfate concentration and the most sensitivity was obtained in absence of it. This may be attributed to the absorption behavior of thionine. In presence of sodium sulfate, the closeness of ions to thionine alters the molar absorptivity of it due to electrostatic interactions. Therefore, the effect of this parameter was overlooked.The influence of temperature on the reaction rate was studied in the range from 15–45°C with the obtained optimum conditions. The results in Figure5 show a maximum at 20°C. Therefore, this value was selected as the optimum temperature.Figure 5
Effect of temperature on the rate of uninhibited (ΔAb) and inhibited (ΔAs) reaction and response (ΔA). Conditions: sulfuric acid, 0.76 mol L−1; thionine, 60.0 μmol L−1; bromate, 0.4 mol L−1; and 4.0 min.The optimum time of reaction was found by measuring the change in the absorbance from 0.5–4.0 min. The reaction rate increased up to 2.5 min, and in longer times it was almost constant. Therefore, 2.5 min was selected as the optimum value.


## 3.2. Analytical Parameters

Under optimum conditions (sulfuric acid: 0.76 mol L−1; thionine: 60.0 μmol L−1; bromate: 0.4 mmol L−1; temperature: 20°C; time: 2.5 min), a linear calibration curve was obtained over the concentration range from 0.8–23.0 μg mL−1 of hydrazine including two linear segments of 0.8–6.0 and 6.0–23.0 μg mL−1. The data analysis gave the regression equations for the first and second linear segments of (3) as follows:
(3)ΔA=0.1393[C]+0.0074(R2=0.9994)ΔA=0.0312[C]+0.6576(R2=0.9996)
where ΔA is the difference in the absorbance changes between the blank and sample (response), C is the concentration of hydrazine (μg mL−1), and R2 is the correlation coefficient.The relative standard deviation of five replicate determinations was 0.74% for a solution of 1.0μg mL−1 of hydrazine. The detection limit, defined as D.L. = 3sb/m, where sb is standard deviation of the blank signal and m is the slope of the calibration curve, was 0.22 μg mL−1 of hydrazine.To study the selectivity of the proposed method, the effect of various species on the determination of 1.0μg mL−1 of hydrazine was investigated (Table 1). The tolerance limit was defined as the concentration of added species causing a relative error less than 5%. As it can be seen in Table 1, most of species did not interfere even when present in 100-fold excess over hydrazine.Table 1
Tolerance limit for various species for the determination of 1.0μg mL−1 of hydrazine.
Foreign species
Tolerance limit (wspecies/whydrazine)
EDTA, sulfamic acid
1000
Li+, Na+, K+, Ca2+, Mg2+
1000
NO
3
-, SO42-, PO43-, CH3CO2-, CO32-, HCO3-
1000
aFe3+, Cr3+, Zn2+
950
b
N
O
2
-
760
aFe2+
600
Cl−
50
aAfter adding 3 mL of 5% EDTA.
bAfter adding 3 mL of 3% sulfamic acid.In Table2, some of the analytical parameters obtained in this work are compared with those previously reported in the literature [21, 22, 24]. According to Table 2, the proposed method is comparable to other catalytic kinetic spectrophotometric methods. Therefore, the proposed method has the potential to offer itself as an alternative method for hydrazine analysis.Table 2
Comparison of some analytical parameters of catalytic spectrophotometric methods to proposed method.
Reaction system
Method
Effect on reaction system
L.R. (μg mL−1)
D.L. (μg mL−1)
Sample
Ref.
Mo(VI)-HCl
Fixed time
Inhibitory
3.2–448.0
1.0
Not applied
[21]
Neutral red-NO2-
Fixed time
Inhibitory
0.15–0.99
0.1
Water
[22]
HCl-BrO3-
Fixed time
Inhibitory
0.0096–1.02
0.0027
Water
[24]
Thionine-BrO3-
Fixed time
Inhibitory
0.8–23.0
0.22
Water and cooling tower water
This work


## 3.3. Application

In order to evaluate the capability of the proposed method, it was applied to the determination of hydrazine in different water samples. For this purpose, four water samples from three sources were examined. The distilled water and drinking water were spiked with 1.0μg mL−1 and 5.0 μg mL−1 of hydrazine. Cooling tower water samples were prepared from Yazd Power Generation Co and analysed as received. The obtained results were given in Table 3. The recoveries (n=3) were between 98.0 and 103.4% that confirm the reliability of the proposed method. Also, the same samples were analysed using ASTM method [25]. The recoveries vary over the range 98.7–102.4% for ASTM method. As it can be seen, the recoveries obtained from the two methods are in good agreement together. Moreover, the t-test for three replicate determinations at 95% confidence limit did not show a significant difference between the results obtained from the two methods.Table 3
The recovery results on the determination of hydrazine in the different water samples using the proposed method and the standard ASTM method.
Hydrazine (μg mL−1)
Sample
Proposed method
ASTM method
Statistical test
Added
Founda
Recovery (%)
Added
Founda
Recovery (%)
t testb
Distilled water
1.0
1.01 ± 0.01
102.0
1.0
0.99 ± 0.01
99.0
3.40
5.0
4.98 ± 0.05
99.6
5.0
5.01 ± 0.03
100.2
1.04
Drinking water
1.0
0.99 ± 0.03
99.0
1.0
1.01 ± 0.01
101.0
1.15
5.0
5.03 ± 0.04
100.6
5.0
4.98 ± 0.05
99.6
2.16
—
2.12 ± 0.02
—
2.09 ± 0.02
2.59
Cooling tower water (1)
1.0
3.14 ± 0.03
100.6
1.0
3.08 ± 0.03
98.7
3.46
5.0
7.05 ± 0.08
99.0
5.0
7.15 ± 0.08
102.4
2.16
15.0
17.19 ± 0.15
100.4
15.0
17.38 ± 0.18
101.7
2.19
—
2.25 ± 0.02
—
2.27 ± 0.02
1.73
Cooling tower water (2)
10.0
12.19 ± 0.11
99.5
10.0
12.28 ± 0.12
100.9
1.42
20.0
22.31 ± 0.21
100.3
20.0
22.08 ± 0.19
99.6
1.89
aMean ± standard deviation (n=3).
bTabulated t-value for three replicate determinations at P (0.95) is 4.30.


## 4. Conclusion

A simple, selective and sensitive kinetic spectrophotometric method for the determination of hydrazine was developed based on its inhibitory effect on the oxidation of thionine with bromate in the acidic media. The method was suitable for the determination of hydrazine in different water samples with satisfactory results.



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*Source: 861625-2012-09-26.xml*