The open circuit potential of hydrogen peroxide at noble and glassy carbon electrodes in acidic and basic electrolytes

• Published in: Journal of electroanalytical chemistry (Lausanne, Switzerland) Vol. 658; no. 1-2; pp. 46 - 51
• Main Authors: Jing, Xia, Cao, Dianxue, Liu, Yao, Wang, Guiling, Yin, Jinling, Wen, Qing, Gao, Yinyi
• Format: Journal Article
• Language: English
• Published: Kidlington Elsevier B.V 15.07.2011; Elsevier
• Subjects: Applied sciences; carbon; chemistry; electrodes; electrolytes; Energy; Energy. Thermal use of fuels; equations; Equipments for energy generation and conversion: thermal, electrical, mechanical energy, etc; Exact sciences and technology; Fuel cell; Fuel cells; Glassy carbon electrode; gold; Hydrogen peroxide; Noble metal electrodes; Open circuit potential; protons; sodium hydroxide; sulfuric acid; temperature; Glassy carbon electrode; Hydrogen peroxide; Noble metal electrodes; Open circuit potential; Fuel cell; Gold; Basic solution; Transition metal; Palladium; Carbon; Acidic solution; Open circuit voltage; Electrodes; Chemical reduction; Platinum; Reaction mechanism; Noble metal; Oxidation; Electrochemical reaction; Platinoid; Glassy state
• DOI: 10.1016/j.jelechem.2011.04.025
• ISSN: 1572-6657

► OCP of H2O2 is a mixed potential of H2O2 electrooxidation and electroreduction. ► OCP of H2O2 is closer to the equilibrium potential of H2O2 electrooxidation. ► OCP of H2O2 is around 0.8V in acidic solution and around 0V in basic solution. The open circuit potentials (OCPs) of H2O2 at Pt, Pd, Au, and glassy carbon electrodes are measured in H2SO4 and NaOH electrolyte solutions. Effects of concentration of H+, OH− and H2O2 as well as temperature on the OCP of H2O2 are investigated. The OCP of H2O2 is much lower than its theoretical reduction potential in both acidic and basic medium. The OCP is actually a mixed potential of H2O2 electroreduction and electrooxidation simultaneously occurring at electrode surfaces and it is more close to the equilibrium potential of H2O2 electrooxidation rather than electroreduction. The OCP of H2O2 is around 0.77–0.80V at [H+]=[H2O2]=1.0moldm−3 in H2SO4 solution and is about 0–0.06V at [OH−]=[H2O2]=1.0moldm−3 in NaOH at 298K on Pt, Pd, Au and GC electrodes. The OCP of H2O2 is independent of H2O2 concentration within the range of 0.01 to 1.0moldm−3. It increases approximately linearly with the logarithm of H+ concentration from 0.02 to 2.0moldm−3, decreases with the logarithm of OH− concentration from 0.01 to 1.0moldm−3 and decreases with increase of temperature from 278K to 333K. The linear equations were presented and discussed.