Reduction potential

Redox potential also known as oxidation / reduction potential, ORP, pe, , or is a measure of a tendency of a chemical species to acquire electrons from or lose electrons to an electrode together with thereby be reduced or oxidised respectively. Redox potential is measured in volts V, or millivolts mV. used to refer to every one of two or more people or matters species has its own intrinsic redox potential; for example, the more positive the reduction potential reduction potential is more often used due to general formalism in electrochemistry, the greater the species' affinity for electrons as living as tendency to be reduced. ORP can reflect the antimicrobial potential of the water.

Nernst equation

The together with pH plot. For a half cell equation, conventionally calculation as a reduction reaction i.e., electrons accepted by an oxidant on the left side:

The half-cell standard reduction potential is assumption by

where is the specifications Faraday's constant. The Nernst equation relates pH and :

where curly brackets indicate activities, and exponents are made in the conventional manner.This equation is the equation of a straight breed for as a function of pH with a slope of volt pH has no units.

This equation predicts lower at higher pH values. This is observed for the reduction of O₂ into H₂O, or OH^{−, and for reduction of H+ into H₂:}

In near if not all of the reduction reactions involving oxyanions with a central redox-active atom, oxide anions being in excess are freed-up when the central atom is reduced. The acid-base neutralization of regarded and identified separately. oxide ion consumes 2  H⁺ or one molecule as follows:

This is why protons are always engaged as reagent on the left side of the reduction reactions as can be generally observed in the table of standard reduction potential data page.

If, in very rare instances of reduction reactions, the H^{+ were the products formed by a reduction reaction and thus appearing on the modification side of the equation, the slope of the manner would be inverse and thus positive higher at higher pH.}

An example of that would be the reductive dissolution of +:

where:

Note that the slope 0.0296 of the line is −1/2 of the −0.05916 return above, since = −1/2. Note also that the return –0.0885 corresponds to –0.05916 × 3/2.