Electrochemical oxidation of humic acid at the antimony- and nickel-doped tin oxide electrode

doi:10.1007/s11783-013-0545-9

Front.Environ.Sci.Eng.

2014, Vol. 8

Issue (3) : 337-344 https://doi.org/10.1007/s11783-013-0545-9

RESEARCH ARTICLE

Electrochemical oxidation of humic acid at the antimony- and nickel-doped tin oxide electrode

TANG Chengli,YAN Wei^1,(

),ZHENG Chunli

Department of Environmental Science and Engineering, Xi’an Jiaotong University, Xi’an 710049, China

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Abstract

This work investigated the degradation of humic acid (HA) in aqueous solution by electrochemical oxidation with Antimony- and Nickel-doped Tin oxide electrode (Ni-Sb-SnO₂/Ti electrode) as the anode. Initial concentrations of HA ranged from 3 to 9 mg·L^-1. Under such a concentration scope, the degradation of HA was a mass transfer controlled process. Degradation rate increased with the increase of HA initial concentration. Test on the effect of tert-butanol revealed that ·OH played an important role in the oxidation of HA. The absence of cation Ca²⁺ was beneficial to HA degradation, which suggested that both indirect and direct electrolyze happened during the whole electrochemical oxidation process. Alkaly (pH= 12) and neutral (pH= 7) conditions were benefical to HA degradation.

Keywords electrochemical oxidation humic acid (HA) natural water Ni-Sb-SnO₂/Ti electrode

Corresponding Author(s): YAN Wei

Issue Date: 19 May 2014

Cite this article:

TANG Chengli,YAN Wei,ZHENG Chunli. Electrochemical oxidation of humic acid at the antimony- and nickel-doped tin oxide electrode[J]. Front.Environ.Sci.Eng., 2014, 8(3): 337-344.

URL:

https://academic.hep.com.cn/fese/EN/10.1007/s11783-013-0545-9
https://academic.hep.com.cn/fese/EN/Y2014/V8/I3/337

Fig.1 SEM image of the prepared Ni-Sb-SnO₂/Ti electrode

Fig.2 Cyclic voltammetry curves of the electrode in 1M NaOH (pH= 12) in the presence (red line) and absence (black line) of HA (room temperature, scan rate 0.01 V·s^-1)

Fig.3 (a) Effect of HA concentration on degradation rate (b) ln[HA]⁰/ln[HA] vs reaction time at different HA concentrations (pH= 12, current density 28 mA·cm^-2, room temperature)

Fig.4 Effect of current density on the degradation rate of HA (initial HA concentration 5 mg·L^-1, pH 12, room temperature)

Fig.5 (a). Effect of Ca²⁺ addition on the degradation rate of HA (initial HA concentration 5 mg·L^-1, pH 12, current density 20 mA·cm^-2, room temperature) (b) cyclic voltammetry curves of the electrode in HA solution in the presence (red line) and absence (black line) of Ca²⁺ (room temperature, scan rate 0.01 V·s^-1)

Fig.6 Effect of t-butanol addition on the degradation rate of HA (initial HA concentration 5 mg·L^-1, pH 12, current density 20 mA·cm^-2, room temperature)

Fig.7 Effects of pH on the degradation rate of HA (initial HA concentration 5 mg·L^-1, current density 20 mA·cm^-2, room temperature)

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