We are being asked to balance the given redox reaction occurring in a basic solution.
When balancing redox reactions under basic conditions, we will follow the following steps.
Step 1: Separate the whole reaction into 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 reaction
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.
Balance the redox reaction under basic condition:
ClO−(aq) + Cr(OH)4−(aq) → CrO42−(aq) + Cl−(aq)
Balance the following reaction in basic solution.
ClO−(aq) + Cr(OH)−4(aq) → CrO42−(aq) + Cl−(aq)
A. 2OH− + 3ClO−(aq) + 2Cr(OH)4−(aq) → 2CrO42−(aq) + 3Cl−(aq) + 5H2O(l)
B. 2OH− + 2ClO−(aq) + Cr(OH)4−(aq) + 2Cl−(aq) + 3H2O(l)
C. 3ClO−(aq) + 2Cr(OH)4−(aq) → 2CrO42−(aq) + 3Cl−(aq) + 3H2O(l) + 2H+
D. 2ClO−(aq) + Cr(OH)4−(aq) → CrO42−(aq) + Cl−(aq) + H2O(l) + 2H+
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