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) A)Br₂= 1,OH^⁻ = 2 B)Br₂= 2,OH^⁻ = 5 C)Br₂= 3,OH^⁻ = 3 D)Br₂= 3,OH^⁻ = 6 E)Br₂= 1,OH^⁻ = 6

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First, we need to identify the oxidation states of each element: Br₂(l) → BrO₃⁻(aq) + Br⁻(aq) Br: 0 → -1 S: -1 → 0 B: +1 → +3 O: -2 → -2 Next, we balance the atoms: Br₂(l) + 3OH⁻(aq) → BrO₃⁻(aq) + Br⁻(aq) + 3H2O(l) Note that we add 3OH⁻(aq) to balance the oxygens and create water molecules on the product side. However, this introduces additional hydrogens that we need to balance by adding 3H2O(l) on the reactant side. Finally, we balance the charges by adding electrons: Br₂(l) + 3OH⁻(aq) → BrO₃⁻(aq) + Br⁻(aq) + 3H2O(l) + 2e⁻ We can see that the coefficients in front of Br₂, OH⁻, and Br⁻ are 1, 3, and 1 respectively. The coefficient in front of BrO₃⁻ is not needed since it is equal to 1. Therefore, the answer is choice letter D.

Balance the Following Redox Reaction If It Occurs in Basic