# Voltammetric Study of the Copper Pentacyanonitrosylferrate Adsorbed on the Silica Modified with a Poly(propylene)imine Hexadecylamine Dendrimer for Determination of  Nitrite

Authors: D. R. do Carmo; S. Gabriel; D. R. Silvestrini; U. O. Bicalho; L. R. Cumba
Journal: International Journal of Electrochemistry
 (2012)

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## Abstract

Poly(propylene)imine hexadecylamine dendrimer (DAB-Am-16) was anchored on the surface of 3-chloropropylsilyl silica gel and subsequently interacted with copper nitroprusside. The composite was characterized by infrared (FTIR), energy dispersive X-ray (EDX), and cyclic voltammetry. The above techniques confirmed the successful anchoring of the dendrimer on the silica gel modified surface and its interaction with copper nitroprusside. The cyclic voltammogram of CuNPSD was found to exhibit two redox couples with (Eθ′)1 = 0.30 V and (Eθ′)2 = 0.78 V versus Ag/AgCl (KCl=1.0 mol L−1; v=20 mV s−1) attributed to the redox processes Cu(I)/Cu(II) and Fe(II)(CN)5NO/Fe(III)(CN)5NO, respectively. The CuNPSD-modified graphite paste electrode was found to show a linear response of 5.0×10−4 to 9.0×10−3 mol L−1 for nitrite determination with a detection limit (DL) of 3.8×10−4 mol L−1 and an amperometric sensitivity of 25.0 mA/mol L−1. The CuNPSD-modified graphite paste electrode was found to show a good electrochemical stability and an excellent response to the electrocatalytic oxidation of sodium nitrite.


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## Body

## 1. Introduction

Dendrimers are monodispersed macromolecules with well-known nanometer dimensions, especially their symmetrical shape of its highly branched and spherical structure [1]. This class of polymers has received considerable interest with possible applications in micelles [2, 3] and the encapsulation of substances [4–6] such as liquid crystals [7]. In electroanalysis [8–10] dendrimers have particular applications in sensors [11], electroluminescent devices [12, 13], and catalysts [14, 15] due to their unique structure and properties. However, very little is known about the interaction of these compounds with nitroprusside.Nitroprusside- (NP-) based compounds have been, in recent years, the target of a large number of works mainly in the areas of electrochemistry [16, 17] and electroanalysis [18, 19]. This is due mainly to their high electrophilic character and reducibility capacity attributed to the NO+ ligand primarily responsible for the reactions of NP ions making these compounds highly interesting not only from the physicochemical standpoint through the coordination properties of groups nitrosyl [20] but also because of their important biological role primarily as a source of nitric oxide [21]. Some studies have been carried out on the use of nitroprusside ions as electron mediator in the electrocatalysis of substances of biological interest [19, 22, 23].In the present study, the poly(propylene)imine hexadecylamine dendrimer (DAB-Am-16) was anchored [24] on the surface of 3-chloropropylsilyl silica gel generating the composite (SD). DAB-Am-16 consists of a polar core and an apolar periphery [25], there are three generations of branches, and the outermost shell is composed of 16-NH2 groups. The chelating capacity of such amine dendrimers can be used to adsorb metal ions in the environmental and biological samples in organic or aqueous medium because amine dendrimers are macrochelating agents for transitions metals. Silica was chosen as substrate for anchoring DAB-Am-16 due to the high stability of complexes formed that permits their multiple uses in preconcentration and separation processes.In this context, this work have as purpose to prepare dendrimer supported on the silica gel surface to an analytical and electroanalytical application, using a direct and facile procedure. The idea is to combine the ion exchange properties with good ionic conductor, and this combination will facilitate charge transfer between CuNP and SD due to the cation diffusion within the CuNP mediated by SD component.Subsequent to being generated, the SD was made to adsorb cupric ions, the resulting material being CuSD, which then reacted with sodium nitroprusside (NP) to form a binuclear complex on the surface of silica (SD). A rigorous cyclic voltammetry study of this new compound formed, CuNPSD, was carried out to optimize the main electrochemical parameters and thus establish a system for the graphite paste electrode in which the dendrimer, modified on its surface, will be employed in the electrocatalytical determination of sodium nitrite. Nitrite, on the other hand, has a biological importance in environment-related questions, while, in the area of medicine, it serves as vasodilator with a direct action on smooth muscles and thus directly affects the levels of blood pressure in an individual [26]. In nature, nitrite ions are produced by the photolysis of nitrate ions and photodegradation of humic substances found mainly in aquatic environments [27].The literature describes various methods used in determining these compounds : titration, which involves reactions with potassium permanganate [28] or iodine [29], UV-VIS spectrophotometry [30], chromatographic methods such as HPLC [31], and electrochemical methods involving redox reactions [32]. Among these methods, the electrochemical methods are considered to be among the best because of their low cost and quick analysis [27] especially those in which modified electrodes are employed.


## 2. Experimental

### 2.1. Formation of DAB-Am-16 on the Surface of Silica Gel

1.0 × 10−3 mol of DAB-Am-16 was added to 10 g of 3-chloropropylsilyl silica gel suspended in 25 mL of methanol. The suspension was kept under reflux for 48 hrs. The resulting solid was then separated using a thin sintered plate funnel and washed several times with the solvent. The solid phase was properly packaged and transferred to a Soxhlet extractor and washed several times with dry toluene in order to eliminate excess unbonded dendrimer. The resulting material was dried at 80°C and kept in a vacuum desiccator in the dark. For brevity, the resulting composite was labeled SD.


### 2.2. Formation of Binuclear Complex with Modified Silica Gel (CuNPSD)

The Binuclear complex was prepared according to the procedure described in the literature [24] with some modifications: 1.0 g of modified silica (SD) was immersed in 25 mL of a 1.0 × 10−3 mol L−1 cupric ion (Cu2+) solution (99% (v/v) acetone). This mixture was stirred for 30 minutes at room temperature, and the solid phase was filtered and washed with deionized water thus forming the CuSD. After thorough washing, the CuSD was added to a 1.0 × 10−3 mol L−1 solution of the electroactive sodium nitroprusside compound, Na2[Fe(CN)5NO]. The resulting material was washed with enough deionized water and the compound obtained labeled as CuNPSD. A schematic presentation of this synthesis is represented by Figure 1.Figure 1
Schematic representation of the stages in the modification process of CuNPSD.


### 2.3. Characterization Measurements

The spectra in the infrared region were obtained by a Nicolet 5DXB FT-IR spectrometer (Nicolet Instruments, Madison, WI). The pastils for analysis were prepared using 150 mg of previously dried KBr PA of the Synth brand and 1.5 mg (1.0% (w/w)) of each sample. A minimum of 64 “scans” with a resolution of ±4 cm−1 in a band of 4000 to 400 cm−1 was used. EDX measurements were taken with a Jeol JTSM T-330 electron microscope. The samples of about 20 to 30 nm thickness were metallized in a BAL-TEC SCD 050 sputter for 120 s. The cyclic voltammetry readings were obtained by potentiostat of Microquímica (MQPG-01) on a scale ranging from −0.1 to 1.2 V (versus Ag/AgCl). The electrochemical system was composed of three electrodes: a working electrode (internal diameter 0.5 mm) of graphite paste modified with 20% CuNPSD, 25 μL Nujol, as reference electrode (Ag/AgCl(s)), and an auxiliary electrode made of platinum. In the electrochemical cell, the nitrite solutions used in voltammetric experiments were prepared immediately before use and were deaerated with purified nitrogen.


## 2.1. Formation of DAB-Am-16 on the Surface of Silica Gel

1.0 × 10−3 mol of DAB-Am-16 was added to 10 g of 3-chloropropylsilyl silica gel suspended in 25 mL of methanol. The suspension was kept under reflux for 48 hrs. The resulting solid was then separated using a thin sintered plate funnel and washed several times with the solvent. The solid phase was properly packaged and transferred to a Soxhlet extractor and washed several times with dry toluene in order to eliminate excess unbonded dendrimer. The resulting material was dried at 80°C and kept in a vacuum desiccator in the dark. For brevity, the resulting composite was labeled SD.


## 2.2. Formation of Binuclear Complex with Modified Silica Gel (CuNPSD)

The Binuclear complex was prepared according to the procedure described in the literature [24] with some modifications: 1.0 g of modified silica (SD) was immersed in 25 mL of a 1.0 × 10−3 mol L−1 cupric ion (Cu2+) solution (99% (v/v) acetone). This mixture was stirred for 30 minutes at room temperature, and the solid phase was filtered and washed with deionized water thus forming the CuSD. After thorough washing, the CuSD was added to a 1.0 × 10−3 mol L−1 solution of the electroactive sodium nitroprusside compound, Na2[Fe(CN)5NO]. The resulting material was washed with enough deionized water and the compound obtained labeled as CuNPSD. A schematic presentation of this synthesis is represented by Figure 1.Figure 1
Schematic representation of the stages in the modification process of CuNPSD.


## 2.3. Characterization Measurements

The spectra in the infrared region were obtained by a Nicolet 5DXB FT-IR spectrometer (Nicolet Instruments, Madison, WI). The pastils for analysis were prepared using 150 mg of previously dried KBr PA of the Synth brand and 1.5 mg (1.0% (w/w)) of each sample. A minimum of 64 “scans” with a resolution of ±4 cm−1 in a band of 4000 to 400 cm−1 was used. EDX measurements were taken with a Jeol JTSM T-330 electron microscope. The samples of about 20 to 30 nm thickness were metallized in a BAL-TEC SCD 050 sputter for 120 s. The cyclic voltammetry readings were obtained by potentiostat of Microquímica (MQPG-01) on a scale ranging from −0.1 to 1.2 V (versus Ag/AgCl). The electrochemical system was composed of three electrodes: a working electrode (internal diameter 0.5 mm) of graphite paste modified with 20% CuNPSD, 25 μL Nujol, as reference electrode (Ag/AgCl(s)), and an auxiliary electrode made of platinum. In the electrochemical cell, the nitrite solutions used in voltammetric experiments were prepared immediately before use and were deaerated with purified nitrogen.


## 3. Results and Discussion

Figure2 illustrates the infrared spectra of the NP (a) and CuNPSD (b). The CuNPSD was observed to exhibit two absorption bands at 2196 cm−1 and 1953 cm−1 (Figure 2(b)), which confirmed the formation copper pentacyanonitrosylferrate on the surface of the SD (CuNPSD). The absorption bands at 2211 and 1960 cm−1, attributed to the stretching of “ν”s (CN) and “ν”s (NO), were found to be in good agreement with values for transition metal pentacyanoferrates [24, 33, 34] reported in the literature. A close comparison of the “ν”s (CN) and “ν”s (NO) band shifts and those obtained for sodium nitroprusside (NP) confirms a bathochromic shift of the former relative to the latter (Figure 2(a)), thus characterizing the formation of the binuclear complex on the silica surface (SD).Figure 2
FTIR of (a) NP and (b) CuNPSD.Figure3 depicts the EDX spectra of SD (a) and CuNPSD (b). The absence of Cl in the SD is evident for the complete reaction of the functionalized silica and the dendrimer. On the other hand, the presence of Fe, Cu, and N in the EDX obtained for CuNPSD is easily perceived as expected. These data support the formation of copper on the surface of silica gel modified with the dendrimer. A complementary and detailed characterization of SD using nuclear magnetic resonance in the solid state (29Si and 13C NMR) has been performed and recently published [24].Figure 3
Energy dispersive X-ray (EDX) analysis of (a) SD and  (b) CuNPSD.


### 3.1. Electrochemical Characterization of CuNPSD

The cyclic voltammogram (CV) of the CuNPSD-modified graphite paste electrode was found to exhibit two redox couples, I and II, as illustrated in Figure4(a) (dashed line). The obtained formal potentials, (Eθ′)1 = 0.30 V and (Eθ′)2 = 0.78 V versus Ag/AgCl(s), were attributed to redox processes Cu(I)/Cu(II) and Fe(II)(CN)5NO/Fe(III)(CN)5NO respectively, as described by (1) and (2), where K+: on was used for charge balance.(1)K2Cu(I)[Fe(II)(CN)5NO]⇄KCu(II)[Fe(II)(CN)5NO]+K++e-(0.30V)(2)KCu(II)[Fe(II)(CN)5NO]⇄Cu(II)[Fe(III)(CN)5NO]+K++e-(0.78V).(a) Cyclic voltammogram of CuNPSD for different scanning rates:  10–100 mV s−1 (KCl = 1.0 mol L−1, pH = 7.0). (b) Linear dependence of the anodic and cathodic current intensity with the square root of scan rate (peak I). (c) Linear dependence of the anodic and cathodic current intensity with the scan rate (peak(II)).
(a)(b)(c)The redox process I illustrated in Figure4(a) was attributed to the redox couple Cu(I)/Cu(II), which is compatible to that observed by Shankaran and Narayanan [35] and De Sá et al. [36], while the redox process II is representative of the process [Fe(II)(CN)5NO]/[Fe(III)(CN)5NO] on the surface of the SD (2) with values found to be consistent with those reported in the literature for copper nitroprusside [18, 37, 38]. Studies on the voltammetric behavior of CuNPSD in different supporting electrolytes (LiCl, NaCl, KCl, and NH4Cl) ascertained that the nature of cations affects not only the current intensity but also the average potentials of the redox process II (Eθ)2 found to shift to more positive potentials according to the following order: NH4+ > K+ > Na+ > Li+. This behavior is quite similar to that observed for Prussian blue [39] thus suggesting that the cavity diameter of the structure of sodium nitroprusside appears to be very close to that found in the literature (0.32 nm) for similar compounds such as Prussian blue [40]. The nature of anions (Cl−, NO3-, SO42-, CLO4-) was found to hardly affect the average potential of the redox couples I and II. Table 1 lists the values of the mean/average potentials presented and the main electrochemical parameters of the above-mentioned compound.Table 1
Relationship between the diameter of hydrated cations and the electrochemical parameters of CuNPSD (electrolyte 1.0 mol L−1; v = 20 mV s−1; pH = 7.0).
Cation[Ipa/Ipc]1*(Eθ)1*ΔEp1 (V)[Ipa/Ipc]2(Eθ)2ΔEp2 (V)Diameter of hydrated cation (nm)**Li+1.220.310.2280.810.770.0330.470Na+1.050.320.2190.880.770.0330.360K+0.980.320.2160.950.790.0300.240NH4+0.860.310.1810.860.780.0310.245Eθ*(V) = (Epa+Epc)/2eΔEp (V) = |Epa-Epc|,Ref.** [38].Figure4(a) presents also cyclic voltammograms of the CuNPSD-modified graphite paste obtained for different scanning speeds. The redox process I found a linear dependence of the anode and cathode peaks on the square root of scan rate, thus characterizing a diffusion-controlled process, while, for the redox process II, there was a linear dependence on scan rate, hence characterizing an adsorptive process [41], as illustrated by the graphs in the Figures 4(b) and 4(c), respectively. It was observed that the redox peak I of CV has ΔEp > 200 mV (v = 100 mV s−1), because the kinetics of electrons transfer at the electrode surface is not fast enough. This may be due to the difficulty of diffusion of species through the electrolyte-electrode interface solution for charge balancing. However, the CV of peak II has ΔEp = 81 mV (v = 100 mV s−1). These results suggest that the two redox processes (I and II) showed distinct behaviors.The voltammetric studies carried out at different KCl concentrations (0.1–2.0 mol L−1) showed a linear increase of peak potential (Eθ′)1 and (Eθ′)2 to more positive (anodic) regions as the concentration of electrolyte increased (Figure 5). The estimated slopes of these lines were 34 mV and 47 mV per decade of concentration of potassium ions for the redox processes I and II, respectively, hence indicating a quasi-Nernstian process.The dependence of the formal potential of  CuNPSD on the logarithms of  K+ concentration (v = 20 mV s−1): (a) peak I and (b) peak II.
(a)(b)Additionally, a study of the voltammetric behavior of CuNPSD in different hydrogen ion concentrations showed that the average potentials (Eθ′) of the two redox processes remained virtually unchanged in the pH range between 2 and 8. For high hydrogen ion concentrations or when the pH attained values below 3, the formation of a new redox process with average potentials (Eθ′)3 = 0.48 V was found to take place, as shown in Figure 6, a behavior analogous to that shown by Prussia blue. From these studies we conclude that high concentrations of H+ ions compete with K+ ions in the system redox process forming one or more intermediate species [18]. Another explanation for the above observation is the protonation of the cyanide groups, which alter the electron density of the metal center of Fe and Cu in CuNPSD (backbonding).Figure 6
Cyclic voltammograms of CuNPSD at different pH values (8–2).


### 3.2. Application of CuNPSD in the Determination of Nitrite

In search for an electroanalytical application of CuNPSD, this compound was tested for its voltammetric determination of nitrite using a graphite paste electrode. The CuNPSD-modified graphite paste electrode in the presence of nitrite was investigated in support of the electrolyte chosen previously, KCl 1.0 mol L−1 at pH 7.0. Figures 7(c) and 7(a) present the cyclic voltammograms of the graphite paste electrode modified with CuNPSD (CuNPSD-GPE) and without CuNPSD, respectively. On addition of nitrite (Figure 7(d)), the anodic current intensity of CuNPS-GPE was observed to increase in peak II. This process was also noted to occur at a lower potential (about 80 mV) than that observed for graphite paste without CuNPS in the presence of 1.0 × 10−3 mol L−1 of nitrite (Figure 7(b)).Figure 7
Voltammetric behavior of (a) graphite paste electrode, (b) graphite paste electrode in 1.0 × 10−3 mol L−1 nitrite, (c) CuNPSD-modified graphite paste electrode, and (d) CuNPSD-modified graphite paste in the presence of  1.0 × 10−3 mol L−1 of nitrite (KCl = 1.0 mol L−1; v = 20 mV s−1).The increase in anodic current with the addition of sodium nitrite (Figure8) is due to moderate electrocatalytic oxidation of the nitrite by the electron mediator, CuNPSD, as described in (3) and (4). The nitrite chemically reduces Fe(III) to Fe(II) during the anodic scan, which again is electrochemically oxidized to Fe(III). The chemical step of the process [42, 43] at the interface of electrolyte solution is given by (4).(3)NO2-+H2O⟶NO3-+2H++2e-(4)Cu(II)[Fe(III)(CN)5NO]+K++12NO2-+12H2O⟶12NO3-+H++KCuII[FeII(CN)5NO].
Figure 9 shows the analytical curve for the determination of the nitrite. From the curve, it is easy to observe that a linear system of 5.0 × 10−4 to 9.0 × 10−3 mol of nitrite has a corresponding analytical equation Y(μA) = −5.78 + 25060.97 (nitrite) with a correlation coefficient of r=0.9993. The method was found to present a detection limit of 3.8 × 10−4 mol L−1 with an amperometric sensitivity of 25.0 mA/mol/L for nitrite.Figure 8
Cyclic voltammograms obtained for the CuNPSD-modified graphite paste electrode in the presence of different concentrations of nitrite (5.0 × 10−5 to 9.0 × 10−3 mol L−1, KCl = 1.0 mol L−1; pH = 7.0; v = 20 mV s−1).Figure 9
Analytical curve of the anodic peak (II) for the determination of nitrite using a CuNPSD-modified graphite paste electrode (KCl = 1.0 mol L−1; pH = 7.0; v = 20 mV s−1).


## 3.1. Electrochemical Characterization of CuNPSD

The cyclic voltammogram (CV) of the CuNPSD-modified graphite paste electrode was found to exhibit two redox couples, I and II, as illustrated in Figure4(a) (dashed line). The obtained formal potentials, (Eθ′)1 = 0.30 V and (Eθ′)2 = 0.78 V versus Ag/AgCl(s), were attributed to redox processes Cu(I)/Cu(II) and Fe(II)(CN)5NO/Fe(III)(CN)5NO respectively, as described by (1) and (2), where K+: on was used for charge balance.(1)K2Cu(I)[Fe(II)(CN)5NO]⇄KCu(II)[Fe(II)(CN)5NO]+K++e-(0.30V)(2)KCu(II)[Fe(II)(CN)5NO]⇄Cu(II)[Fe(III)(CN)5NO]+K++e-(0.78V).(a) Cyclic voltammogram of CuNPSD for different scanning rates:  10–100 mV s−1 (KCl = 1.0 mol L−1, pH = 7.0). (b) Linear dependence of the anodic and cathodic current intensity with the square root of scan rate (peak I). (c) Linear dependence of the anodic and cathodic current intensity with the scan rate (peak(II)).
(a)(b)(c)The redox process I illustrated in Figure4(a) was attributed to the redox couple Cu(I)/Cu(II), which is compatible to that observed by Shankaran and Narayanan [35] and De Sá et al. [36], while the redox process II is representative of the process [Fe(II)(CN)5NO]/[Fe(III)(CN)5NO] on the surface of the SD (2) with values found to be consistent with those reported in the literature for copper nitroprusside [18, 37, 38]. Studies on the voltammetric behavior of CuNPSD in different supporting electrolytes (LiCl, NaCl, KCl, and NH4Cl) ascertained that the nature of cations affects not only the current intensity but also the average potentials of the redox process II (Eθ)2 found to shift to more positive potentials according to the following order: NH4+ > K+ > Na+ > Li+. This behavior is quite similar to that observed for Prussian blue [39] thus suggesting that the cavity diameter of the structure of sodium nitroprusside appears to be very close to that found in the literature (0.32 nm) for similar compounds such as Prussian blue [40]. The nature of anions (Cl−, NO3-, SO42-, CLO4-) was found to hardly affect the average potential of the redox couples I and II. Table 1 lists the values of the mean/average potentials presented and the main electrochemical parameters of the above-mentioned compound.Table 1
Relationship between the diameter of hydrated cations and the electrochemical parameters of CuNPSD (electrolyte 1.0 mol L−1; v = 20 mV s−1; pH = 7.0).
Cation[Ipa/Ipc]1*(Eθ)1*ΔEp1 (V)[Ipa/Ipc]2(Eθ)2ΔEp2 (V)Diameter of hydrated cation (nm)**Li+1.220.310.2280.810.770.0330.470Na+1.050.320.2190.880.770.0330.360K+0.980.320.2160.950.790.0300.240NH4+0.860.310.1810.860.780.0310.245Eθ*(V) = (Epa+Epc)/2eΔEp (V) = |Epa-Epc|,Ref.** [38].Figure4(a) presents also cyclic voltammograms of the CuNPSD-modified graphite paste obtained for different scanning speeds. The redox process I found a linear dependence of the anode and cathode peaks on the square root of scan rate, thus characterizing a diffusion-controlled process, while, for the redox process II, there was a linear dependence on scan rate, hence characterizing an adsorptive process [41], as illustrated by the graphs in the Figures 4(b) and 4(c), respectively. It was observed that the redox peak I of CV has ΔEp > 200 mV (v = 100 mV s−1), because the kinetics of electrons transfer at the electrode surface is not fast enough. This may be due to the difficulty of diffusion of species through the electrolyte-electrode interface solution for charge balancing. However, the CV of peak II has ΔEp = 81 mV (v = 100 mV s−1). These results suggest that the two redox processes (I and II) showed distinct behaviors.The voltammetric studies carried out at different KCl concentrations (0.1–2.0 mol L−1) showed a linear increase of peak potential (Eθ′)1 and (Eθ′)2 to more positive (anodic) regions as the concentration of electrolyte increased (Figure 5). The estimated slopes of these lines were 34 mV and 47 mV per decade of concentration of potassium ions for the redox processes I and II, respectively, hence indicating a quasi-Nernstian process.The dependence of the formal potential of  CuNPSD on the logarithms of  K+ concentration (v = 20 mV s−1): (a) peak I and (b) peak II.
(a)(b)Additionally, a study of the voltammetric behavior of CuNPSD in different hydrogen ion concentrations showed that the average potentials (Eθ′) of the two redox processes remained virtually unchanged in the pH range between 2 and 8. For high hydrogen ion concentrations or when the pH attained values below 3, the formation of a new redox process with average potentials (Eθ′)3 = 0.48 V was found to take place, as shown in Figure 6, a behavior analogous to that shown by Prussia blue. From these studies we conclude that high concentrations of H+ ions compete with K+ ions in the system redox process forming one or more intermediate species [18]. Another explanation for the above observation is the protonation of the cyanide groups, which alter the electron density of the metal center of Fe and Cu in CuNPSD (backbonding).Figure 6
Cyclic voltammograms of CuNPSD at different pH values (8–2).


## 3.2. Application of CuNPSD in the Determination of Nitrite

In search for an electroanalytical application of CuNPSD, this compound was tested for its voltammetric determination of nitrite using a graphite paste electrode. The CuNPSD-modified graphite paste electrode in the presence of nitrite was investigated in support of the electrolyte chosen previously, KCl 1.0 mol L−1 at pH 7.0. Figures 7(c) and 7(a) present the cyclic voltammograms of the graphite paste electrode modified with CuNPSD (CuNPSD-GPE) and without CuNPSD, respectively. On addition of nitrite (Figure 7(d)), the anodic current intensity of CuNPS-GPE was observed to increase in peak II. This process was also noted to occur at a lower potential (about 80 mV) than that observed for graphite paste without CuNPS in the presence of 1.0 × 10−3 mol L−1 of nitrite (Figure 7(b)).Figure 7
Voltammetric behavior of (a) graphite paste electrode, (b) graphite paste electrode in 1.0 × 10−3 mol L−1 nitrite, (c) CuNPSD-modified graphite paste electrode, and (d) CuNPSD-modified graphite paste in the presence of  1.0 × 10−3 mol L−1 of nitrite (KCl = 1.0 mol L−1; v = 20 mV s−1).The increase in anodic current with the addition of sodium nitrite (Figure8) is due to moderate electrocatalytic oxidation of the nitrite by the electron mediator, CuNPSD, as described in (3) and (4). The nitrite chemically reduces Fe(III) to Fe(II) during the anodic scan, which again is electrochemically oxidized to Fe(III). The chemical step of the process [42, 43] at the interface of electrolyte solution is given by (4).(3)NO2-+H2O⟶NO3-+2H++2e-(4)Cu(II)[Fe(III)(CN)5NO]+K++12NO2-+12H2O⟶12NO3-+H++KCuII[FeII(CN)5NO].
Figure 9 shows the analytical curve for the determination of the nitrite. From the curve, it is easy to observe that a linear system of 5.0 × 10−4 to 9.0 × 10−3 mol of nitrite has a corresponding analytical equation Y(μA) = −5.78 + 25060.97 (nitrite) with a correlation coefficient of r=0.9993. The method was found to present a detection limit of 3.8 × 10−4 mol L−1 with an amperometric sensitivity of 25.0 mA/mol/L for nitrite.Figure 8
Cyclic voltammograms obtained for the CuNPSD-modified graphite paste electrode in the presence of different concentrations of nitrite (5.0 × 10−5 to 9.0 × 10−3 mol L−1, KCl = 1.0 mol L−1; pH = 7.0; v = 20 mV s−1).Figure 9
Analytical curve of the anodic peak (II) for the determination of nitrite using a CuNPSD-modified graphite paste electrode (KCl = 1.0 mol L−1; pH = 7.0; v = 20 mV s−1).


## 4. Conclusions

FTIR studies, along with EDX, confirm the modification of 3-chloropropylsilyl silica gel with DABAm-16 (SD), hexadecylamine poly (propylene) imine dendrimer. After two stages of synthesis, the modified silica, SD, was found to promote the formation of the binuclear compound, CuNPSD, subsequently characterized by voltammetric and spectroscopic techniques.The CuNPSD-modified graphite paste electrode was found to show a good electrochemical stability and excellent response to the electrocatalytic oxidation of sodium nitrite with a detection limit of 3.8 × 10−4 mol L−1 and an amperometric sensitivity of 25.0 mA/mol L−1. The use of CuNPSD-modified electrodes is advantageous because there is no need for any prior chemical treatment, and it is easily made, thus allowing the surface to be quickly renewed thereby decreasing the time spent in performing the analytical measurements.



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*Source: 527596-2012-05-08.xml*