In a particular redox reaction, BrO− is oxidized to BrO−3 and Ag + is reduced to Ag.
Complete and balance the equation for this reaction in acidic solution. Phases are optional.
BrO ⁻ + Ag ⁺ → BrO₃ ⁻ + Ag

4 Ag⁺ + 2 H₂O + BrO⁻ → 4 Ag + BrO₃⁻ + 4 H⁺

Explanation:

In order to balance a redox reaction, we will use the ion-electron method.

Step 1: Identify both half-reactions

Reduction: Ag⁺ → Ag

Oxidation: BrO⁻ → BrO₃⁻

Step 2: Perform the mass balance adding H⁺ and H₂O where necessary

Ag⁺ → Ag

2 H₂O + BrO⁻ → BrO₃⁻ + 4 H⁺

Step 3: Perform the electrical balance adding electrons where necessary

1 e⁻ + Ag⁺ → Ag

2 H₂O + BrO⁻ → BrO₃⁻ + 4 H⁺ + 4 e⁻

Step 4: Multiply both half-reactions by numbers that secure that the number of electrons gained and lost are equal

4 × (1 e⁻ + Ag⁺ → Ag)

1 × (2 H₂O + BrO⁻ → BrO₃⁻ + 4 H⁺ + 4 e⁻)

Step 5: Add both half-reactions

4 e⁻ + 4 Ag⁺ + 2 H₂O + BrO⁻ → 4 Ag + BrO₃⁻ + 4 H⁺ + 4 e⁻

4 Ag⁺ + 2 H₂O + BrO⁻ → 4 Ag + BrO₃⁻ + 4 H⁺

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