Balancing Oxidation-Reduction Reactions
Grade 12 Chemistry worksheet on balancing redox reactions using the half-reaction method in acidic and basic solutions.
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Standards
Balancing Oxidation-Reduction Reactions
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Date:
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Read each question carefully and follow the instructions to balance the given oxidation-reduction reactions. Show all your work for full credit.
1. In the reaction: MnO₄⁻(aq) + C₂O₄²⁻(aq) → Mn²⁺(aq) + CO₂(g) (acidic solution), what is the oxidation state of carbon in C₂O₄²⁻?
+2
+3
+4
+6
2. Which of the following acts as the oxidizing agent in the reaction: Cr₂O₇²⁻(aq) + SO₃²⁻(aq) → Cr³⁺(aq) + SO₄²⁻(aq) (acidic solution)?
Cr₂O₇²⁻
SO₃²⁻
Cr³⁺
SO₄²⁻
3. In an acidic solution, to balance oxygen atoms, we add to the side lacking oxygen.
4. To balance hydrogen atoms in a basic solution, we first add H⁺ ions, then add an equal number of to both sides of the equation.
5. Balance the following redox reaction in acidic solution:
IO₃⁻(aq) + I⁻(aq) → I₂(s)
6. Balance the following redox reaction in basic solution:
MnO₄⁻(aq) + Br⁻(aq) → MnO₂(s) + BrO₃⁻(aq)
7. The number of electrons gained in a reduction half-reaction must equal the number of electrons lost in an oxidation half-reaction.
True
False
8. When balancing a redox reaction, spectator ions are typically included in the half-reactions.
True
False
9. Explain the key differences in balancing redox reactions in acidic versus basic solutions, specifically regarding the use of H⁺, OH⁻, and H₂O.