Complete and balance the equation for this reaction in acidic solution.

BrO−3+Sb3+⟶Br−+Sb5+

6 H⁺ + BrO₃⁻ + 3 Sb³⁺ ⟶ Br⁻ + 3 H₂O + 3 Sb⁵⁺

Explanation:

Step 1: Write the unbalanced reaction

BrO₃⁻ + Sb³⁺ ⟶ Br⁻ + Sb⁵⁺

Step 2: Identify both half-reactions

Reduction: BrO₃⁻ ⟶ Br⁻

Oxidation: Sb³⁺ ⟶ Sb⁵⁺

Step 3: Perform the mass balance, adding H⁺ and H₂O where appropriate

6 H⁺ + BrO₃⁻ ⟶ Br⁻ + 3 H₂O

Sb³⁺ ⟶ Sb⁵⁺

Step 4: Perform the charge balance, adding electrons where appropriate

6 H⁺ + BrO₃⁻ + 6 e⁻ ⟶ Br⁻ + 3 H₂O

Sb³⁺ ⟶ Sb⁵⁺ + 2 e⁻

Step 5: Multiply both half-reactions by numbers that assure that the number of electrons gained and lost is the same

1 × (6 H⁺ + BrO₃⁻ + 6 e⁻ ⟶ Br⁻ + 3 H₂O)

3 × (Sb³⁺ ⟶ Sb⁵⁺ + 2 e⁻)

Step 6: Add both half-reactions and cancel what is repeated in both sides

6 H⁺ + BrO₃⁻ + 3 Sb³⁺ ⟶ Br⁻ + 3 H₂O + 3 Sb⁵⁺

Option A is correct way of representation of electronic configuration.