This process is made somewhat more complicated when oxidation and reduction are taking place. In a redox reaction, the electrons must be balanced in addition to the elements. The following steps provide a guide for balancing redox reactions.
(1) Split the reaction into two 'half-reactions,' one reduction and the other oxidation.
(2) If the reaction is taking place in acid, use to balance hydrogen. If the reaction is
taking place in base, use .
(3) Balance oxygen by adding .
(4) Because the number of electrons consumed must equal the number of electrons gained, cross multiply the number of electrons consumed in the oxidation half reaction with the stochiometric coefficients of the reduction half reaction. Then repeat this process by multiplying the original number of electrons gained in the reduction half reaction with the stochiometric coefficients of the oxidation half reaction.
(5) Add the two half-reactions together, canceling the electrons, , and species. The redox reaction should now be balanced.
