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  2. Nernst equation - Wikipedia

    en.wikipedia.org/wiki/Nernst_equation

    In electrochemistry, the Nernst equation is a chemical thermodynamical relationship that permits the calculation of the reduction potential of a reaction (half-cell or full cell reaction) from the standard electrode potential, absolute temperature, the number of electrons involved in the redox reaction, and activities (often approximated by concentrations) of the chemical species undergoing ...

  3. Table of standard reduction potentials for half-reactions ...

    en.wikipedia.org/wiki/Table_of_standard...

    For obtaining the values of the reduction potential at pH = 7 for the redox reactions relevant for biological systems, the same kind of conversion exercise is done using the corresponding Nernst equation expressed as a function of pH. The conversion is simple, but care must be taken not to inadvertently mix reduction potential converted at pH ...

  4. Reduction potential - Wikipedia

    en.wikipedia.org/wiki/Reduction_potential

    In aqueous solutions, redox potential is a measure of the tendency of the solution to either gain or lose electrons in a reaction. A solution with a higher (more positive) reduction potential than some other molecule will have a tendency to gain electrons from this molecule (i.e. to be reduced by oxidizing this other molecule) and a solution with a lower (more negative) reduction potential ...

  5. Standard hydrogen electrode - Wikipedia

    en.wikipedia.org/wiki/Standard_hydrogen_electrode

    During the early development of electrochemistry, researchers used the normal hydrogen electrode as their standard for zero potential. This was convenient because it could actually be constructed by "[immersing] a platinum electrode into a solution of 1 N strong acid and [bubbling] hydrogen gas through the solution at about 1 atm pressure".

  6. Zeta potential - Wikipedia

    en.wikipedia.org/wiki/Zeta_potential

    The usual units are volts (V) or, more commonly, millivolts (mV). From a theoretical viewpoint, the zeta potential is the electric potential in the interfacial double layer (DL) at the location of the slipping plane relative to a point in the bulk fluid away from the interface.

  7. Reference electrode - Wikipedia

    en.wikipedia.org/wiki/Reference_electrode

    Most electrodes work over a limited range of conditions, such as pH or temperature, outside of this range the electrodes behavior becomes unpredictable. The advantage of a pseudo-reference electrode is that the resulting variation is factored into the system allowing researchers to accurately study systems over a wide range of conditions.

  8. Reversible hydrogen electrode - Wikipedia

    en.wikipedia.org/wiki/Reversible_hydrogen_electrode

    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] The name refers to the fact that the electrode is directly immersed in the actual electrolyte solution and not separated by a salt bridge. The hydrogen ion concentration is therefore not 1 mol/L, or ...

  9. pH meter - Wikipedia

    en.wikipedia.org/wiki/PH_meter

    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]