We can summarize the procedure that we use to balance a redox reaction that occurs in solution:

In acidic solution do steps 1 –5. In basic solution do steps 1-8.

1.Divide the equation into two incomplete half-reactions, one for oxidation and the other for reduction.

2.Balance each half-reaction.
2a.First, balance the elements other than H and O.
2b.Next, balance the O atoms by adding H₂O.
2c.Then, balance the H atoms by adding H⁺.
2d.Finally, balance the charge by adding e^- to the side with the greater overall positive charge.

3.Multiply each half-reaction by an integer so that the number of electrons lost in one half-reaction equals the number gained in the other.

4.Add the two half-reactions and simplify where possible by canceling species appearing on both sides of the equation.

5.Check the equation to make sure that there are the same number of atoms of each kind and the same total charge on both sides.

6.Add OH^- ions to both sides of the equation, the number of OH^- you add is equal to the number of H⁺ ions in the balanced equation.

7.Cancel the OH^- and H⁺ ions where they appear on the same side of the equation and make them equal H₂O molecules and then
cancel the H₂O molecules across the left hand side and right hand sides of the balanced equation.

8.Check the equation to make sure that there are the same number of atoms of each kind and the same total charge on both sides.