1. Balancing Redox ½ Reaction (Basic)

2. Balancing Basic
Balancing in basic solution is just like acidic with one additional step
When balancing in acidic you will have H+ at the end
In basic you don’t want H+, you want OH-

3. To change to basic
To change to basic, simply add an equivalent number of OH- to each side and simplify

4. Example
Balancing the following by using the ½ reaction method in a basic solution
AsO4-3 + Zn  H3As + Zn +2
Acidic:
11H+ + AsO Zn  H3As + 4 H2O + 4Zn+2
Basic:
+11 OH OH-
11 H2O + AsO Zn  H3As + 4 H2O + 4Zn+2+ 11OH-
7 H2O + AsO Zn  H3As + 4Zn+2+ 11OH-

5. Another Example Ag + NO3-  Ag + + N+2 Acidic:
3Ag +6 H+ + NO3-  3Ag + + N+2+ 3H2O
Basic:
+ 6OH OH-
3Ag +6H2O + NO3-  3Ag + + N+2+ 3H2O + 6OH-
3Ag +3H2O + NO3-  3Ag + + N+2 + 6OH-

6. One More Mn(NO3)2 + NaBiO3 + HNO3  NaMnO4 + Bi(NO3)3 + H2O + NaNO3
Acidic:
2Mn H+ + 5 BiO3-  2MnO4- + 5Bi H2O
Basic:
+ 14 OH OH-
2Mn H2O + 5 BiO3-  2MnO4- + 5Bi H2O+ 14 OH-
2Mn+2 + 7H2O + 5 BiO3-  2MnO4- + 5Bi OH-