# Cobalt Hexacyanoferrate-Decorated Titania Nanotube: CoHCF@TNT Modified GCE as an Electron Transfer Mediator for the Determination of Hydrazine in Water Samples

Authors: S. Jancy Sophia; S. Devi; K. Pandian
Journal: ISRN Analytical Chemistry
 (2012)

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## Abstract

The cobalt hexacyanoferrate-decorated titania nanotube (CoHCF@TNT) was prepared by dispersing 100 mg of titania nanotube (TNT) to a solution of an equimolar concentration of CoCl2 · 6H2O and K3[Fe(CN)6] containing 0.05 M KCl solution (35 mL). The TNT was synthesized by hydrothermal method using Degussa P-25 TiO2 in 2 M NaOH as reported in the literature. The CoHCF@TNT was isolated and characterized by DRS-UV, FE-SEM, FT-IR, and XRD analysis. The electrochemical behavior of the CoHCF@TNT was carried out in 0.1 M phosphate buffer. The CoHCF@TNT modified system showed an excellent electron transfer mediator for the oxidation of hydrazine at +0.5 V versus Ag wire. The proposed method can be utilized for the amperometry detection of hydrazine from environmental samples. A calibration plot was constructed by plotting the concentration of hydrazine against the peak current. The current response was linear in the ranges of the hydrazine concentration from 5 × 10−4 M to 2.5 × 10−3 M with a slope of 72.8 μAmM−1 and the linear correlation coefficient of 0.9972. The detection limit was found to be 1 × 10−3 M.


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## Body

## 1. Introduction

There is an increasing demand for the development of a novel electrocatalytic mediator which has been used for various kinds of sensors for the detection of environmentally important pollutant in recent days. Though metal hexacyanoferrates are most studied as an important class of electron transfer mediator for the electrocatalytic oxidation and reduction, still there are numerous developments have been made to study their unique inherent physicochemical properties and electron transfer characteristics. The metal hexacyanoferrate-modified electrode shows excellent electrocatalytic behavior and selectivity. They can be widely used in various fields of research including photomagnetic [1], solid batteries [2], electrocatalysis [3], and biosensors [4]. Itaya et al., [5] and others have extensively studied the electrochemical behavior and stability of the Prussian blue and its analogues due to their similar electrochemical behavior, stability, and wider electrochemical window. These metal hexacyanoferrate-modified electrodes have mostly been utilized for the electrocatalytic detection of biological important thiols [6], selective detection of neurotransmitters [7], and environmental important pollutants like hydrazine [8], peroxide [9], and thiosulfate [10]. Because of its zeolite-like characteristics, PB and its analogues have been utilized for selective removal of radioactive Cs and toxic metals like Tl [11, 12].To improve the electrochemical stability of the modified electrode and avoid fouling of the electrode, various strategies have been demonstrated. For instant, sol-gel method, by using perm selective coating using nafion and other polymers and direct coating in presence of conducting polymer are some of the few examples [13, 14]. Recently mesoporous carbons [15], carbon nanotube [16], and graphene [17] have been utilized to stabilize PB and analogues. In the present work, we have taken an initiative to use titania nanotube as template to immobilize metal hexacyanoferrates. It is well known that titania and its nanotube can be used as electrode substrate for the electrocatalytic reaction and solar cell applications [18, 19]. We have made an attempt to use titania nanotube as template to immobilize cobalt hexacyanoferrate by sequential deposition method [20]. The film thickness and electron transfer reaction can be controlled by the help of the sequential deposition method. The aim of the present investigation is to utilize CoHCF@TNT, for the electrocatalytic detection of hydrazine in water samples. Hydrazine is widely used in industry and agriculture as fuel cells, insecticides, explosives, rocket propellants, metal film manufactures, and pharmaceuticals [21]. Hydrazine is found to be a neurotoxin and produces carcinogenic and mutagenic effects [22]. Its poisoning induces vomiting, severe irritation of the respiratory track, and long-term exposure affects the central nervous system. Hydrazine can be determined by several instrumental methods including chromatography [23], spectrophotometry [24], capillary electrophoresis [25] and fluorimetry [26]. Among these techniques, the electrochemical method is found to be a simple and an easy way to estimate hydrazine.Electroanalytical techniques seem to provide direct and efficient methods for the detection of hydrazine at trace level. This technique offers the opportunity for portable, cheap, and rapid methodologies. However, electrochemical oxidations of hydrazine are sluggish, and a relatively high overpotential is required at conventional electrodes. Several approaches have been investigated to minimize this problem. Therefore, chemically modified electrodes have been developed for the determination of hydrazine. Several types of modified electrode have been used for the electrocatalytic oxidation of hydrazine such as metal phthalocyanine [27, 28], metal porphyrin [29], metal hexacyanoferrate [30, 31], metal complexes [32], metal nanoparticles [33], and metal nanoparticles-modified MWCNT-[34] modified electrodes. Among these electron transfer mediators, metal hexacyanoferrates [35], metal hexacyanoferrate-modified metal oxide [36], and metal hexacyanoferrate-modified carbon nanotube [37] have been widely used for the electrocatalytic detection of hydrazine in various sources. Here, we are aiming to use CoHCF@TNT for the quantitative detection of hydrazine in water sources by amperometry method for the first time.


## 2. Experimental Section

### 2.1. Chemicals

All chemicals were purchased from commercial sources. TiO2 was purchased from Aldrich chemical, USA. Cobalt(II) chloride, and potassium ferricyanide, potassium chloride were used as received from SD fine chemicals Pvt, Ltd, India. All solutions were prepared using high-purity Milli-Q water (resistivity of 18.1 MΩ).


### 2.2. Instrumental Method

The FT-IR spectra were recorded using Perkin-Elmer 360 model FT-IR double beam spectrophotometer. Diffusive reflectance spectrum was recorded in DRS UV-visible spectrophotometer lambda 35. XRD patterns of the samples were recorded with a JSO DEBYE FLEX 2002 Seifert diffractometer. SEM images were obtained with a field emission JEOL-JSM-6360 instrument, USA. The CV experiment was carried out using CHI 660A electrochemical instrument, USA. A three-electrode system with a single compartment cell system was used for the electrochemical studies. A GCE and platinum were used as working and counter electrode, respectively. Ag wire was used as reference electrode. All potentials were measured against the Ag wire as reference electrode.


### 2.3. Preparation of CoHCF@TNT-Modified GCE

The glassy carbon (GC) surface was polished to a mirror-like smoothness with emery paper and then sonicated in ethanol and distilled water for 5 minutes. Following drying with a stream of high purity of nitrogen gas, the GC substrate was modified with drops of CoHCF@TNT suspension and then dried. A CoHCF@TNT-coated GC electrode was thus prepared for measurements, after the GC was removed from the deposited solution throughly rinsed with water, and dried with nitrogen gas.


### 2.4. Synthesis of TNT

We have synthesized TNT based on previous literature report [38]. In brief, 2 g of the TiO2 (P-25 Degussa) was mixed with 70 mL of 10 N NaOH solution, and the resulting homogeneous mixture was allowed to heat treatment at 110–150°C in a Teflon-lined autoclave for 24 h. After the treatment, the filtered sample was then neutralized by mixing with 1 L of 0.1 N HCl solutions for several times, until the pH value of the rinsing solution was less than 7. The powder was dried at 100°C for 3 h to give the as-synthesized nanotube product. To improve the thermal stability, the as-synthesized nanotubes were calcined at different temperatures for 1 h. The appearance of white color powder indicates the formation of TNT. The CoHCF@TNT was prepared by using an equimolar concentration of CoCl2·6H2O and K3[Fe(CN)6] containing 0.05 M KCl solution in presence of 100 mg of TNT [39]. Finally, the CoHCF@TNT was thoroughly washed with ultrapure water to remove the physisorbed ions. The CoHCF@TNT is dried under nitrogen atmosphere for overnight and stored in a dark.


## 2.1. Chemicals

All chemicals were purchased from commercial sources. TiO2 was purchased from Aldrich chemical, USA. Cobalt(II) chloride, and potassium ferricyanide, potassium chloride were used as received from SD fine chemicals Pvt, Ltd, India. All solutions were prepared using high-purity Milli-Q water (resistivity of 18.1 MΩ).


## 2.2. Instrumental Method

The FT-IR spectra were recorded using Perkin-Elmer 360 model FT-IR double beam spectrophotometer. Diffusive reflectance spectrum was recorded in DRS UV-visible spectrophotometer lambda 35. XRD patterns of the samples were recorded with a JSO DEBYE FLEX 2002 Seifert diffractometer. SEM images were obtained with a field emission JEOL-JSM-6360 instrument, USA. The CV experiment was carried out using CHI 660A electrochemical instrument, USA. A three-electrode system with a single compartment cell system was used for the electrochemical studies. A GCE and platinum were used as working and counter electrode, respectively. Ag wire was used as reference electrode. All potentials were measured against the Ag wire as reference electrode.


## 2.3. Preparation of CoHCF@TNT-Modified GCE

The glassy carbon (GC) surface was polished to a mirror-like smoothness with emery paper and then sonicated in ethanol and distilled water for 5 minutes. Following drying with a stream of high purity of nitrogen gas, the GC substrate was modified with drops of CoHCF@TNT suspension and then dried. A CoHCF@TNT-coated GC electrode was thus prepared for measurements, after the GC was removed from the deposited solution throughly rinsed with water, and dried with nitrogen gas.


## 2.4. Synthesis of TNT

We have synthesized TNT based on previous literature report [38]. In brief, 2 g of the TiO2 (P-25 Degussa) was mixed with 70 mL of 10 N NaOH solution, and the resulting homogeneous mixture was allowed to heat treatment at 110–150°C in a Teflon-lined autoclave for 24 h. After the treatment, the filtered sample was then neutralized by mixing with 1 L of 0.1 N HCl solutions for several times, until the pH value of the rinsing solution was less than 7. The powder was dried at 100°C for 3 h to give the as-synthesized nanotube product. To improve the thermal stability, the as-synthesized nanotubes were calcined at different temperatures for 1 h. The appearance of white color powder indicates the formation of TNT. The CoHCF@TNT was prepared by using an equimolar concentration of CoCl2·6H2O and K3[Fe(CN)6] containing 0.05 M KCl solution in presence of 100 mg of TNT [39]. Finally, the CoHCF@TNT was thoroughly washed with ultrapure water to remove the physisorbed ions. The CoHCF@TNT is dried under nitrogen atmosphere for overnight and stored in a dark.


## 3. Results and Discussion

### 3.1. SEM Images of CoHCF@TNT

Figure1(a) depicted the typical SEM images of products prepared by hydrothermal treatments of P-25 Degussa type TiO2 at 383 K for 24 h. Furthermore, the effect of the sodium content on the microstructure of nanotubes is important. Therefore, energy-dispersive X-ray (EDX) (Figure 2(a)) evaluation was carried out for products prepared by hydrothermal treatment for 24 h. The Na/Ti atomic ratio for products prepared by hydrothermal treatment for 24 h was approximately 0.2 without acid treatment. On the contrary, after acid treatment with a 0.1 M HCl aqueous solution, only a trace amount of sodium could be detected in this sample by EDX analysis (Figure 2(b)). This has been ascribed to the decrease of Na/Ti ratio of TiO2-derived TNT caused by the replacement of Na+ with H+ during the acid treatment with dil.HCl [40].SEM images of TNT (a) and after modifying with CoHCF (b).
(a)(b)EDAX images of TNT (a) and after modifying with CoHCF (b).
(a)(b)SEM image of CoHCF@TNT is shown in Figure1(b). From SEM analysis, the size and shape of the nanotube were calculated. After exposure of the CoHCF solution, the nanotubes are aggregated and form a big-size composite fiber-like structure. The approximate composition of CoHCF treated TNT was calculated from EDX analysis.


### 3.2. XRD Pattern of CoHCF@TNT

The XRD pattern of pure TNTs and CoHCF@TNT is shown in Figure3. The XRD pattern profile of the TNTs is exactly similar to those observed in the literature [41], which suggests a crystalline structure of lepidocrocite-type TNTs with a general formula HxTi2–x/4□x/4O4 (□: vacancy). The X-ray diffractograms are typical of layered materials, which suggest that the nanotubes are multiwalled in nature. The layered structures give rise to a characteristic (200) reflection with a lower 2θ values of 11.3° which corresponds to interlayer distance of TNT. The peak position shows red shift when compared with the literature reports, and it is due to the sodium ions present in the TNT interlayers. A high-intense peak at 2θ = 48.6° was found, and it is due to the edge sharing TiO6 octahedral. The other peaks at 2θ~25.1 correspond to the titanate phase. All other peaks are in close agreement with reported values. The (200) peak at 11.3° was not altered even after intercalation of CoHCF into TNT lattices, indicating that the interlayer spacing was not expanded with intercalation of CoHCF into the interlayer of TNT. The X-ray powder diffraction (XRD) pattern of the composite material showed peaks at 17.32°(200), 25.48°(220), 34.86°(400), and 39.05°(420), which can be indexed as the face-centred cubic (fcc) crystal structure [42].Figure 3
XRD pattern of (a) TNT (b) CoHCF@TNT.


### 3.3. UV-Vis Diffuse Reflectance Spectra

UV-Vis diffuse reflectance spectroscopy is used to measure the change in the electronic absorption spectrum of the materials. Figure4 shows the UV-Vis absorption spectra of TNT, (b) CoHCF, and (c) CoHCF@TNT. It is evident that for the protonic lepidocrocite TNT, there is broadband absorption from 268 to 314 nm, due to the transition from the O2− antibonding orbital to the lowest empty orbital of Ti4+. The addition of CoHCF to the TNT structure shifts the band edge absorption to about 410 nm, thus making it possible to use these CoHCF@TNTs as photocatalysts operating with excitation in the violet-blue region of the electromagnetic spectrum. This red shift in the band edge absorption can be understood as being due to the effects of CoHCF addition (intercalation), which change the band gap energy of the system. A similar band gap shift toward the visible range was also observed for TNTs intercalated with other metals, such as Fe, Bi, Cd, Ni, and Co [43]. By using standard Kubelka-Munk methodology, we can estimate the band gap for TNT and CoHCF as being 3.06 and 2.94 eV, respectively. The photoabsorption of CoHCF@TNT in the range 410–760 nm is attributed due to the existence of the Co 3d bands above the O 2p bands [43, 44].Figure 4
UV-Vis diffuse reflectance spectrum of TNT (a), CoHCF (b), and CoHCF@TNT (c).


### 3.4. FT-IR Spectral Studies for TNT and CoHCF@TNT

The formation of CoHCF@TNT was further confirmed by the FTIR spectrum. Figure5 shows the FTIR spectrum of (a) CoHCF@TNT; (b) TNT. In the FT-IR spectrum of TNT (Figure 5(b)), three absorption bands centered at 1630, 3482, and 914 cm−1 are assigned for bending vibration of H–O–H, stretching vibrations of OH group of physisorbed water and Ti–O bonds, respectively. These results indicate the most replacement of Na+ in the nanotubular product by H+ and also the presence of large amount of water molecules and hydroxyl groups present in TNT. A band at 914 cm−1 was affected by the intercalation of CoHCF, which leads to a decrease in vibrational energy of the Ti–O octahedrons. The changes in the stretching modes for terminal Ti–O bonds (914 cm−1) was understood in terms of the interaction of the CoHCF with the terminal Ti–O bonds. In the FT-IR spectra of CoHCF@TNT, the intense and a strong absorption band at 2121 cm−1 is due to the common characteristics of CoHCF and its analogues, corresponding to the stretching vibration of the –C≡N–group, and the absorption band at 483 cm−1 is due to the formation of M–CN–M, which indicate the presence of CoHCF. In addition, the absorption bands at 3404 and 1608 cm−1 indicates the O–H stretching mode and H–O–H bending mode, respectively. These results highlight the presence of water molecules in a interstitial position, and also the stretching vibration of water molecules produces another broad peak at 3635 cm−1 which further confirm that the samples are hydrated [40, 43, 45].Figure 5
FT-IR spectra of (a) CoHCF@TNT (b) TNT.


### 3.5. Electrochemical Behavior of CoHCF@TNT

The electrochemical behavior of the CoHCF@TNT was investigated using cyclic voltammetric technique (Figure6). A reversible cyclic voltammogram is obtained for the CoHCF@TNT in 0.1 M PBS medium. The cyclic voltammogram of CoHCF@TNT-modified electrodes exhibits an enhancement in redox signals, which confirms the high sensitivity of the electrode and also confirms the modification of TNT by CoHCF.Figure 6
Cyclic voltammograms of (a) bare, (b) bare with 0.1 mM hydrazine, (c) CoHCF@TNT-modified GC electrode and (d) same as (c) in 0.1 mM hydrazine at pH 7 (0.1 M phosphate buffer): scan rate: 50 mV/sec.We have compared the current density and the peak potential changes of bare and CoHCF@TNT-modified electrodes on electrocatalytic oxidation of hydrazine, and the resulting cyclic voltammograms are shown in Figure6. It was observed that there is a decrease in over potential for CoHCF@TNT modified electrode than the bare GCE. Also there is a remarkable increase in the anodic peak current were noted in the case of CoHCF@TNT modified electrode. This result confirms that the CoHCF@TNT acts as a better electrocatalyst on electrochemical oxidation of hydrazine at neutral pH ranges.The electrochemical behavior of CoHCF@TNT was tested in 0.1 M PBS, and the resulting voltammogram is shown in Figure7. From the cyclic voltammogram, it can be seen that the redox peak current for both Co2+/Co3+ and Fe(CN)6 4−/Fe(CN)6 3− systems, and the separate redox peaks were merged together and showing a single redox peak. The increase in peak currents when increasing potential scan rates, confirming the redox behavior is due to the surface confinement of the redox species and also suggests that the redox reaction is purely diffusion-controlled one [30].Figure 7
Cyclic voltammograms of CoHCF@TNT-modified electrode in 0.1 M phosphate buffer (pH 7) at scan rates of 20, 50, 75, and 100 mV s−1 (bottom to top).


## 3.1. SEM Images of CoHCF@TNT

Figure1(a) depicted the typical SEM images of products prepared by hydrothermal treatments of P-25 Degussa type TiO2 at 383 K for 24 h. Furthermore, the effect of the sodium content on the microstructure of nanotubes is important. Therefore, energy-dispersive X-ray (EDX) (Figure 2(a)) evaluation was carried out for products prepared by hydrothermal treatment for 24 h. The Na/Ti atomic ratio for products prepared by hydrothermal treatment for 24 h was approximately 0.2 without acid treatment. On the contrary, after acid treatment with a 0.1 M HCl aqueous solution, only a trace amount of sodium could be detected in this sample by EDX analysis (Figure 2(b)). This has been ascribed to the decrease of Na/Ti ratio of TiO2-derived TNT caused by the replacement of Na+ with H+ during the acid treatment with dil.HCl [40].SEM images of TNT (a) and after modifying with CoHCF (b).
(a)(b)EDAX images of TNT (a) and after modifying with CoHCF (b).
(a)(b)SEM image of CoHCF@TNT is shown in Figure1(b). From SEM analysis, the size and shape of the nanotube were calculated. After exposure of the CoHCF solution, the nanotubes are aggregated and form a big-size composite fiber-like structure. The approximate composition of CoHCF treated TNT was calculated from EDX analysis.


## 3.2. XRD Pattern of CoHCF@TNT

The XRD pattern of pure TNTs and CoHCF@TNT is shown in Figure3. The XRD pattern profile of the TNTs is exactly similar to those observed in the literature [41], which suggests a crystalline structure of lepidocrocite-type TNTs with a general formula HxTi2–x/4□x/4O4 (□: vacancy). The X-ray diffractograms are typical of layered materials, which suggest that the nanotubes are multiwalled in nature. The layered structures give rise to a characteristic (200) reflection with a lower 2θ values of 11.3° which corresponds to interlayer distance of TNT. The peak position shows red shift when compared with the literature reports, and it is due to the sodium ions present in the TNT interlayers. A high-intense peak at 2θ = 48.6° was found, and it is due to the edge sharing TiO6 octahedral. The other peaks at 2θ~25.1 correspond to the titanate phase. All other peaks are in close agreement with reported values. The (200) peak at 11.3° was not altered even after intercalation of CoHCF into TNT lattices, indicating that the interlayer spacing was not expanded with intercalation of CoHCF into the interlayer of TNT. The X-ray powder diffraction (XRD) pattern of the composite material showed peaks at 17.32°(200), 25.48°(220), 34.86°(400), and 39.05°(420), which can be indexed as the face-centred cubic (fcc) crystal structure [42].Figure 3
XRD pattern of (a) TNT (b) CoHCF@TNT.


## 3.3. UV-Vis Diffuse Reflectance Spectra

UV-Vis diffuse reflectance spectroscopy is used to measure the change in the electronic absorption spectrum of the materials. Figure4 shows the UV-Vis absorption spectra of TNT, (b) CoHCF, and (c) CoHCF@TNT. It is evident that for the protonic lepidocrocite TNT, there is broadband absorption from 268 to 314 nm, due to the transition from the O2− antibonding orbital to the lowest empty orbital of Ti4+. The addition of CoHCF to the TNT structure shifts the band edge absorption to about 410 nm, thus making it possible to use these CoHCF@TNTs as photocatalysts operating with excitation in the violet-blue region of the electromagnetic spectrum. This red shift in the band edge absorption can be understood as being due to the effects of CoHCF addition (intercalation), which change the band gap energy of the system. A similar band gap shift toward the visible range was also observed for TNTs intercalated with other metals, such as Fe, Bi, Cd, Ni, and Co [43]. By using standard Kubelka-Munk methodology, we can estimate the band gap for TNT and CoHCF as being 3.06 and 2.94 eV, respectively. The photoabsorption of CoHCF@TNT in the range 410–760 nm is attributed due to the existence of the Co 3d bands above the O 2p bands [43, 44].Figure 4
UV-Vis diffuse reflectance spectrum of TNT (a), CoHCF (b), and CoHCF@TNT (c).


## 3.4. FT-IR Spectral Studies for TNT and CoHCF@TNT

The formation of CoHCF@TNT was further confirmed by the FTIR spectrum. Figure5 shows the FTIR spectrum of (a) CoHCF@TNT; (b) TNT. In the FT-IR spectrum of TNT (Figure 5(b)), three absorption bands centered at 1630, 3482, and 914 cm−1 are assigned for bending vibration of H–O–H, stretching vibrations of OH group of physisorbed water and Ti–O bonds, respectively. These results indicate the most replacement of Na+ in the nanotubular product by H+ and also the presence of large amount of water molecules and hydroxyl groups present in TNT. A band at 914 cm−1 was affected by the intercalation of CoHCF, which leads to a decrease in vibrational energy of the Ti–O octahedrons. The changes in the stretching modes for terminal Ti–O bonds (914 cm−1) was understood in terms of the interaction of the CoHCF with the terminal Ti–O bonds. In the FT-IR spectra of CoHCF@TNT, the intense and a strong absorption band at 2121 cm−1 is due to the common characteristics of CoHCF and its analogues, corresponding to the stretching vibration of the –C≡N–group, and the absorption band at 483 cm−1 is due to the formation of M–CN–M, which indicate the presence of CoHCF. In addition, the absorption bands at 3404 and 1608 cm−1 indicates the O–H stretching mode and H–O–H bending mode, respectively. These results highlight the presence of water molecules in a interstitial position, and also the stretching vibration of water molecules produces another broad peak at 3635 cm−1 which further confirm that the samples are hydrated [40, 43, 45].Figure 5
FT-IR spectra of (a) CoHCF@TNT (b) TNT.


## 3.5. Electrochemical Behavior of CoHCF@TNT

The electrochemical behavior of the CoHCF@TNT was investigated using cyclic voltammetric technique (Figure6). A reversible cyclic voltammogram is obtained for the CoHCF@TNT in 0.1 M PBS medium. The cyclic voltammogram of CoHCF@TNT-modified electrodes exhibits an enhancement in redox signals, which confirms the high sensitivity of the electrode and also confirms the modification of TNT by CoHCF.Figure 6
Cyclic voltammograms of (a) bare, (b) bare with 0.1 mM hydrazine, (c) CoHCF@TNT-modified GC electrode and (d) same as (c) in 0.1 mM hydrazine at pH 7 (0.1 M phosphate buffer): scan rate: 50 mV/sec.We have compared the current density and the peak potential changes of bare and CoHCF@TNT-modified electrodes on electrocatalytic oxidation of hydrazine, and the resulting cyclic voltammograms are shown in Figure6. It was observed that there is a decrease in over potential for CoHCF@TNT modified electrode than the bare GCE. Also there is a remarkable increase in the anodic peak current were noted in the case of CoHCF@TNT modified electrode. This result confirms that the CoHCF@TNT acts as a better electrocatalyst on electrochemical oxidation of hydrazine at neutral pH ranges.The electrochemical behavior of CoHCF@TNT was tested in 0.1 M PBS, and the resulting voltammogram is shown in Figure7. From the cyclic voltammogram, it can be seen that the redox peak current for both Co2+/Co3+ and Fe(CN)6 4−/Fe(CN)6 3− systems, and the separate redox peaks were merged together and showing a single redox peak. The increase in peak currents when increasing potential scan rates, confirming the redox behavior is due to the surface confinement of the redox species and also suggests that the redox reaction is purely diffusion-controlled one [30].Figure 7
Cyclic voltammograms of CoHCF@TNT-modified electrode in 0.1 M phosphate buffer (pH 7) at scan rates of 20, 50, 75, and 100 mV s−1 (bottom to top).


## 4. Amperometric Response of CoHCF@TNT

Because of the increase in peak at 0.5 V in Figure8 for the electrochemical oxidation of hydrazine using CoHCF@TNT many fold when compared with bare GCE, we have developed amperometry method for the quantitative detection of hydrazine in water samples. The typical hydrazine current response at 0.5 V versus Ag wire during the successive addition of 50 μL of 0.1 M hydrazine in 8 mL 0.1 M PBS under constant stirring condition and the resulting current response at regular time intervals are shown in Figure 8. A well-defined amperometric response with a response time of less than 5 s was observed, which demonstrates the stable and efficient catalytic ability of CoHCF@TNT. The response current was linear with the hydrazine concentration from 5 × 10−4M to 2.5 × 10−3M with a slope of 72.8 μAmM−1 and linear correlation coefficient of 0.9972. The detection limit was found to be 1 × 10−3M. The detection limit value is comparable with the reported in the literature which was shown in Table 1.Table 1
A comparison of electrocatalytic detection of hydrazine using various types of modified electrode systems.
S. numbersElectrode systempHPotentialConcentration rangesReference(1)CeHCF/mesoporous carbon1.5+0.34 V versus Ag/AgCl (satd KCl)1–163μM[14](2)Ni(II)-bicalein complex/MWCNT13+0.65 V versus Ag/AgCl (satd KCl)2.5μM to 0.2 mM[21](3)Pd/boron-doped diamond7+0.11 V versus Ag/AgCl (satd KCl)10 mM to 102 mM.[20](4)Pd/CNT10.27 versus Ag/AgCl (satd KCl)2.5–700μM[33](5)CoHCF@TNT6.9+0.50 V versus Ag wire0.5–2.5 mMPresent workFigure 8
Amperometric response of CoHCF@TNT in 0.1 M phosphate buffer medium by successive addition of 50μL hydrazine. Applied potential: +0.5 V. (Inset figure plot of ip versus c hydrazine).For the detection of hydrazine in real water samples, standard addition method was carried out. The results are given in Table2 for triplicate, and the results were consistent. The recovery was found to close to 100% in most cases.Table 2
Determination of hydrazine in real samples.
SamplesAdded/10−4MFound/10−4MRecovery (%)Average recovery (%)River water1010.1101102.51515.31022021.21062525.2100.8Drinking water109.999103.21516.21082021.11062524.999.6


## 5. Conclusion

In conclusion, we have successfully developed a methodology for synthesis of CoHCF@TNT. The surface morphology and structural features of the system were investigated by using various instrumental methods such as scanning electron microscopy (SEM), X-ray powder diffraction method (XRD), and FT-IR spectrophotometer. The electrochemical behavior of the CoHCF@TNT was investigated using cyclic voltammetry technique, and the cyclic voltammogram of CoHCF@TNT showed reversible electron transfer behavior of CoHCF. The CoHCF@TNT-modified GC electrode showed an excellent electrocatalytic oxidation of hydrazine in 0.1 M PBS medium. An enhanced electrochemical response was noted when compared with bare GCE with lower over potential ranges. For the quantitative detection of hydrazine, the amperometry method was adopted under optimum experimental conditions with an operating potential of 0.5 V versus Ag wire. This proposed method can be applied for quantitative detection of hydrazine in water samples. The results were given in a tabular form, and it was found that the electrochemical response stable for repeated usage of the electrode without loss of its activity.



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*Source: 192698-2012-04-11.xml*