The copper–copper(II) sulfate electrode is a reference electrode of the first kind, [1] based on the redox reaction with participation of the metal ( copper) and its salt, copper(II) sulfate. It is used for measuring electrode potential and is the most commonly used reference electrode for testing cathodic protection corrosion control systems. [2] The corresponding equation can be presented as follow:
- Cu2+ + 2e− → Cu0(metal)
This reaction characterized by reversible and fast electrode kinetics, [3] meaning that a sufficiently high current can be passed through the electrode with the 100% efficiency of the redox reaction ( dissolution of the metal or cathodic deposition of the copper-ions).
The Nernst equation below shows the dependence of the potential of the copper-copper(II) sulfate electrode on the activity or concentration copper-ions:
Commercial reference electrodes consist of a plastic tube holding the copper rod and saturated solution of copper sulfate. A porous plug on one end allows contact with the copper sulfate electrolyte. The copper rod protrudes out of the tube. A voltmeter negative lead is connected to the copper rod.
The potential of a copper–copper sulfate electrode is +0.314 volt with respect to the standard hydrogen electrode.[ citation needed] Copper–copper(II) sulfate electrode is also used as one of the half cells in the galvanic Daniel-Jakobi cell.
- E. Protopopoff and P. Marcus, Potential Measurements with Reference Electrodes, Corrosion: Fundamentals, Testing, and Protection, Vol 13A, ASM Handbook, ASM International, 2003, p 13-16
- A.W. Peabody, Peabody's Control of Pipeline Corrosion, 2nd Ed., 2001, NACE International. ISBN 1-57590-092-0
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The copper–copper(II) sulfate electrode is a reference electrode of the first kind, [1] based on the redox reaction with participation of the metal ( copper) and its salt, copper(II) sulfate. It is used for measuring electrode potential and is the most commonly used reference electrode for testing cathodic protection corrosion control systems. [2] The corresponding equation can be presented as follow:
- Cu2+ + 2e− → Cu0(metal)
This reaction characterized by reversible and fast electrode kinetics, [3] meaning that a sufficiently high current can be passed through the electrode with the 100% efficiency of the redox reaction ( dissolution of the metal or cathodic deposition of the copper-ions).
The Nernst equation below shows the dependence of the potential of the copper-copper(II) sulfate electrode on the activity or concentration copper-ions:
Commercial reference electrodes consist of a plastic tube holding the copper rod and saturated solution of copper sulfate. A porous plug on one end allows contact with the copper sulfate electrolyte. The copper rod protrudes out of the tube. A voltmeter negative lead is connected to the copper rod.
The potential of a copper–copper sulfate electrode is +0.314 volt with respect to the standard hydrogen electrode.[ citation needed] Copper–copper(II) sulfate electrode is also used as one of the half cells in the galvanic Daniel-Jakobi cell.
- E. Protopopoff and P. Marcus, Potential Measurements with Reference Electrodes, Corrosion: Fundamentals, Testing, and Protection, Vol 13A, ASM Handbook, ASM International, 2003, p 13-16
- A.W. Peabody, Peabody's Control of Pipeline Corrosion, 2nd Ed., 2001, NACE International. ISBN 1-57590-092-0
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| This electrochemistry-related article is a stub. You can help Wikipedia by expanding it. |