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A reversible hydrogen electrode ( RHE) is a reference electrode, more specifically a subtype of the standard hydrogen electrodes, for electrochemical processes. Unlike the standard hydrogen electrode, its measured potential does change with the pH, so it can be directly used in the electrolyte. [1] [2] [3]
In electrochemistry, the standard hydrogen electrode (abbreviated SHE ), is a redox electrode which forms the basis of the thermodynamic scale of oxidation-reduction potentials.
Table of standard electrode potentials. Legend: ( s) – solid; ( l) – liquid; ( g) – gas; ( aq) – aqueous (default for all charged species); ( Hg) – amalgam; bold – water electrolysis equations. See also. Galvanic series lists electrode potentials in saltwater. Standard apparent reduction potentials in biochemistry at pH 7.
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A reference electrode is an electrode that has a stable and well-known electrode potential. The overall chemical reaction taking place in a cell is made up of two independent half-reactions, which describe chemical changes at the two electrodes.
A pH meter is a scientific instrument that measures the hydrogen-ion activity in water-based solutions, indicating its acidity or alkalinity expressed as pH. [2] .
External links. pH. Test tubes containing solutions of pH 1–10 colored with an indicator. In chemistry, pH ( / piːˈeɪtʃ / pee-AYCH ), also referred to as acidity or basicity, historically denotes " potential of hydrogen " (or "power of hydrogen"). [1] . It is a logarithmic scale used to specify the acidity or basicity of aqueous solutions.
The aqueous phase in contact with the mercury and the mercury (I) chloride (Hg 2 Cl 2, "calomel") is a saturated solution of potassium chloride in water. The electrode is normally linked via a porous frit (sometimes coupled to a salt bridge) to the solution in which the other electrode is immersed. In cell notation the electrode is written as:
