Question

For a particular redox reaction, ClO₂ is oxidized to CIO and Ag+ is reduced to Ag. Complete and balance the equation for this

reaction in basic solution. Phases are optional.
balanced redox reaction: CIO-2 + Ag+ —> CIO-4 + Ag

Answer 1

To balance the redox reaction in basic solution, follow these steps:

Assign oxidation numbers to each element in the reaction:

Cl in ClO₂: +4

Cl in CIO: +1

Ag in Ag⁺: +1

Ag in Ag: 0

Identify the elements undergoing oxidation and reduction:

Oxidation: Cl in ClO₂ is going from +4 to +1.

Reduction: Ag⁺ is going from +1 to 0.

Balance the number of atoms for each element except for H and O:

ClO₂ + Ag⁺ → CIO + Ag

Balance the oxygen atoms by adding water (H₂O) molecules:

ClO₂ + Ag⁺ → CIO + Ag + H₂O

Balance the hydrogen atoms by adding hydroxide ions (OH⁻):

ClO₂ + Ag⁺ + H₂O → CIO + Ag + OH⁻

Balance the charge by adding electrons (e⁻):

ClO₂ + 2Ag⁺ + 2H₂O → CIO + 2Ag + 2OH⁻ + 2e⁻

Make sure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.

The balanced redox reaction in basic solution is:

ClO₂ + 2Ag⁺ + 2H₂O → CIO + 2Ag + 2OH⁻