A Cyclic Voltammetric Study of the Redox Reaction of Cu(II) in Presence of Ascorbic Acid in Different pH Media

Abstract

The electrochemical redox behavior of Cu(II), and Cu(II) in presence of ascorbic acid has been investigated at glassy carbon electrode (GCE) in aqueous phosphate buffer solution (PBS) at various pH. In the studied pH range the voltammogram consists of a cathodic and an anodic peak. Cu(II) follows one step two-electron transfer electrochemical redox reaction. The intensities of both cathodic and anodic peak current increase with increasing scan rate that are consistent with Randles-Sevcik equation. The linear behavior of peak current with the square root of scan rate indicates that the electrochemical processes are diffusion controlled. In presence of ascorbic acid both of the cathodic and anodic peak current of Cu(II) is reduced and peak positions are shifted compared to those of Cu(II) alone. These observation suggest that Cu(II) undergoes a strong interaction with ascorbic acid in the studied medium.

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“…The first anodic peak at approximate potential of -0.07 V, could be attributed to the conversion of Cu(0) to Cu(I) [48]. The second peak positioned at approximate potential of 0.21 V was also resulted from the conversion of Cu species to Cu(II) on GCE surface [49]. In reverse direction, the cathodic peak at -0.04 V was belonged to the reduction of Cu species [49].…”

“…The second peak positioned at approximate potential of 0.21 V was also resulted from the conversion of Cu species to Cu(II) on GCE surface [49]. In reverse direction, the cathodic peak at -0.04 V was belonged to the reduction of Cu species [49]. The voltammogram in Fig.…”

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“…This study found that electrochemical reactions were diffusion-controlled according to the linear relation between the square root of scan rate and the peak current. In presence of ascorbic acid, both of the cathodic and anodic peak currents of Cu (II) reduced and peak positions shifted compared to those of Cu (II) alone [12].…”

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“…The experiments were performed using CV techniques at different scan rates (10-100 mV/s). Figure 4b shows that cathodic peak currents were directly proportional to the square root of the scan rate (v 1 2 ), indicating the diffusion-controlled redox process [36]. The active surface area of bare SPCE and CdSe/ZnS QD/SiNPs/SPCE was calculated at 0.0792 and 0.3281 cm 2 , respectively, which means that the active surface area of CdSe/ZnS QD/SiNPs/SPCE was 4.14-fold higher than bare SPCE.…”