Could someone please explain balancing redox reactions?

Here is the general procedure:

1) Identify what is oxidized and what is reduced.

2) Separate the reaction into two haf-reactions, one containing the oxidation and the other the reduction.

3) Balance the reactions for all elements other than O and H

4) Add H2O(l) to the reactions if necessary to balance O

5) Add H+(aq) to the reactions to balance H

6) Add e- to the reactions so that each one is charge balanced

7) Multiply the equations through by factors so the the no of e- in the oxidation eq equals the no of e- in the reduction equation.

8) Add the equations

9) Cancel any species that appears equally on both sides.

This results in a balance in acidic solution. If you need to get a balance for basic solution, add OH-(aq) to cancel all the H+(aq) in the equation.