(i)    Write the given skeleton equation for the reaction and complete it. Determine the oxidation state of all the atoms to identify the atom undergoing oxidation (increase in oxidation state) and reduction (decrease in oxidation state).

(ii)    Write oxidation and reduction separately only in terms of the element (not compound). It must be remembered that the number of atoms should be same as that in the compound present in skeleton equation. At this stage the stoichiometric coefficient should be unity.e.g.

(iii)    Balance the number of atoms undergoing change in oxidation state by changing stoichiometric coefficient. Then write suitable number of electrons lost or gained by those atoms (electrons lost or gained by one atom is equal to the increase or decrease in oxidation state, respectively).
(iv)    Multiply the oxidation and reduction equations obtained above by suitable numbers so that electrons lost become equal to electrons gained.

(v)    Replace the stoichiometric coefficient of species obtained above to the given skeleton equation.

(vi)    Balance all other atoms except hydrogen and oxygen by changing stoichiometric coefficients of those substances which contain that element. Following points should be remembered while doing this:
(a)    The element occuring at minimum places is to be balanced first.
(b)    While balancing other atoms avoid, if possible, changing stoichiometric coefficients of substances having any atom whose oxidation state changes.
(vii) Balance the charge on the basis of medium of the reaction.
(a)    Balance charge by adding H+ to the side deficient in positive charge if the medium is acidic.
(b)    Balance charge by adding OH to the side deficient in negative charge if the medium is basic.

(viii) Balance hydrogen by adding H2O to the side deficient in hydrogen.

(ix)    Cancel any term common in the equation obtained.