Multiple Choice
Which of the following is the correctly balanced equation for the oxidation reaction of Cr2O7^2-(aq) and C2O4^2-(aq) in a basic solution using the half-reaction method?
6. Chemical Quantities & Aqueous Reactions
Balancing Redox Reactions: Basic Solutions
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Which of the following is the correct balanced equation for the redox reaction occurring in a basic solution involving ClO⁻(aq) and Cr(OH)₃(s)?
A
ClO⁻(aq) + Cr(OH)₃(s) + 5 OH⁻(aq) --> Cl⁻(aq) + CrO₄²⁻(aq) + H₂O(l)
B
ClO⁻(aq) + Cr(OH)₃(s) + 4 OH⁻(aq) --> Cl⁻(aq) + CrO₄²⁻(aq) + 2 H₂O(l)
C
ClO⁻(aq) + Cr(OH)₃(s) + 2 OH⁻(aq) --> Cl⁻(aq) + CrO₄²⁻(aq) + 4 H₂O(l)
D
ClO⁻(aq) + Cr(OH)₃(s) + 3 OH⁻(aq) --> Cl⁻(aq) + CrO₄²⁻(aq) + 3 H₂O(l)
Verified step by step guidance1
Identify the oxidation and reduction half-reactions. In this case, ClO⁻ is reduced to Cl⁻, and Cr(OH)₃ is oxidized to CrO₄²⁻.
Write the half-reactions separately. For reduction: ClO⁻ → Cl⁻. For oxidation: Cr(OH)₃ → CrO₄²⁻.
Balance each half-reaction for mass and charge. Add water (H₂O) to balance oxygen atoms and hydroxide ions (OH⁻) to balance hydrogen atoms in a basic solution.
Combine the balanced half-reactions, ensuring that the electrons lost in the oxidation half-reaction equal the electrons gained in the reduction half-reaction.
Verify that the final equation is balanced for both mass and charge, and that it matches one of the given options.
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