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The determination of an equilibrium constant using electrode potential measurement is based on the relationship between the Gibbs free energy change and the cell potential, which is described by electrochemical principles. In electro-analytical chemistry, this approach allows one to study redox reactions and their equilibria quantitatively. For a general redox reaction, consider the reaction: $$ aA + bB \rightleftharpoons cC + dD $$ where $A$ and $B$ are reactants, and $C$ and $D$ are products. The standard Gibbs free energy change ($\Delta G^\circ$) for this reaction is related to the equilibrium constant $K$ by the equation: $$ \Delta G^\circ = -RT \ln K ______ ___ ____ _________ _____ ______ ____ ______ ________ ________.
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