Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Br₂and OH^- in the balanced reaction?
Br₂(l) → BrO₃^- (aq) + Br^- (aq)

Question

Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Br₂and OH^- in the balanced reaction? Br₂(l)→ BrO₃^- (aq)+ Br^- (aq)

Quizplus · Accepted Answer

1) Assign oxidation numbers to all elements: Br₂(l)→ BrO₃^- (aq)+ Br^- (aq) Br: 0 → +5 S: -2 → -2 B: +1 → +3, +2 → +3 O: -2 → -2, 0 → -2 H: +1 → +1 P: 0 → -3 2) Separate the redox reaction into half-reactions: Oxidation: Br → BrO Reduction: B → P 3) Balance all elements except H and O in each half-reaction: Oxidation: Br → BrO3 Reduction: 3B → P 4) Balance O by adding H2O to the side lacking oxygen: Oxidation: Br → BrO3 + 6H2O Reduction: 3B → P + 3H2O 5) Balance H by adding H+ to the side lacking hydrogen: Oxidation: Br + 6H2O → BrO3 + 6H+ Reduction: 3B + 6H+ → P + 3H2O 6) Balance the charge by adding electrons (e-) to the more positive side: Oxidation: Br + 6H2O → BrO3 + 6H+ + 6e- Reduction: 3B + 6H+ + 9e- → P + 3H2O 7) Multiply half-reactions by integers to equalize the number of electrons in both half-reactions: Oxidation (x3): 3Br + 18H2O → 3BrO3 + 18H+ + 18e- Reduction: 3B + 6H+ + 9e- → 3P + 9H2O 8) Add half-reactions together and cancel out any species that appear on both sides: 3Br + 18H2O + 3B + 6H+ + 9e- → 3BrO3 + 18H+ + 18e- + 3P + 9H2O 3Br + 3B + 6H+ → 3BrO3 + 3P + 15H2O 9) In basic solution, add OH- to both sides to neutralize the H+: 3Br + 3B + 6OH- → 3BrO3 + 3P + 15H2O + 6OH- The coefficients in front of Br₂, OH^-, and Br^- are all 3, so the answer is D.

Balance the Following Redox Reaction If It Occurs in Basic