Final answer:
Balancing a redox reaction in acidic solution involves writing half-reactions for oxidation and reduction, balancing atoms and charges with H+ ions and electrons, combining the half-reactions, and verifying mass and charge balance.
Step-by-step explanation:
To balance the redox reaction Cl⁻(aq) + IO₃⁻(aq) → Cl₂(g) + I₂(s) in acidic solution, we need to follow several steps. First, write the half-reactions for oxidation and reduction. The oxidation half-reaction is Cl⁻ → Cl₂ and requires the addition of electrons on the product side. Similarly, the reduction half-reaction is IO₃⁻ → I₂ and electrons will be added to the reactants side. Next, balance the atoms in each half-reaction, followed by balancing the charges by adding H⁺⁻ ions and electrons.
Once both half-reactions are balanced by atoms and charge, combine them, ensuring that the electrons cancel out. The final balanced reaction may require coefficients to ensure both mass and charge balance. Remember that the reaction takes place in acidic solution, so it is necessary to adjust the half-reactions with the appropriate number of H⁺⁻ ions. After combining the half-reactions, make sure to check the balance for both atoms and charges.