When balancing redox reactions under acidic conditions, we will follow the following steps.
Step 1: Separate the whole reaction into two half-reactions.
Step 2: Balance the non-hydrogen and non-oxygen elements first.
Step 3: Balance oxygen by adding H2O to the side that needs oxygen. (1 O: 1 H2O)
Step 4: Balance hydrogen by adding H+ to the side that needs hydrogen. (1 H: 1 H+)
Step 5: Balance the charges: add electrons to the more positive side (or less negative side).
Step 6: Balance electrons on the two half-reactions.
Step 7: Get the overall reaction by adding the two reactions.
When balancing under basic conditions, additional steps are required:
Step 8: Balance remaining H+ by adding an equal amount of OH– ions to both sides.
Step 9: H+(aq) will combine with OH–(aq) to form H2O(l).
Step 10: Cancel out common species.
a. H2O2(aq) + ClO2(aq) → ClO2-(aq) +O2(g)
(1-2): Separate and balance non-H and O atoms
H2O2(aq) → O2(g)
ClO2(aq) → ClO2-(aq)
(3): Add H2O
H2O2(aq) → O2(g)
ClO2(aq) → ClO2-(aq)
(4): Add H+
H2O2(aq) → O2(g) + 2 H+ (aq)
ClO2(aq) → ClO2-(aq)
(5): Balance charges
H2O2(aq) → O2(g) + 2 H+ (aq) + 2 e-
ClO2(aq) + 1 e- → ClO2-(aq)
Balance each of the following redox reactions occurring in basic solution.
a. H2O2(aq) + ClO2(aq) → ClO2-(aq) +O2(g)
b. Al(s)+MnO4-(aq) → MnO2(s) + Al(OH)4-(aq)
c. Cl2(g) → Cl−(aq)+ ClO−(aq)
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