Question

Complete and balance the following redox reaction in basic solution. Be sure to include the proper phases for all species within the reaction.

IO₃⁻ (aq) + Re(s)→ ReO₄⁻ (aq) + 10 (aq)

Answer 1

The balanaced equation is 4IO₃⁻ (aq) + Re (s) + 10OH⁻ (aq) -> 4ReO₄⁻ (aq) + 26H₂O (l)

To balance the redox reaction in basic solution, follow the steps for balancing redox reactions in basic media.

Step-by-step explanation:

To balance the redox reaction in basic solution, we can follow the steps for balancing redox reactions in basic media.

1. Write the balanced half-reactions for the oxidation and reduction processes:

Oxidation: IO₃⁻ (aq) -> ReO₄⁻ (aq) + 6H₂O (l) + 6e⁻

Reduction: Re (s) + 4OH⁻ (aq) -> ReO₄⁻ (aq) + 2H₂O (l) + 4e⁻

2. Balance the number of electrons transferred between the two half-reactions by multiplying the oxidation half-reaction by 4.

Oxidation: 4IO₃⁻ (aq) -> 4ReO₄⁻ (aq) + 24H₂O (l) + 24e⁻

Reduction: Re (s) + 4OH⁻ (aq) -> ReO₄⁻ (aq) + 2H₂O (l) + 4e⁻

3. Add the two half-reactions together:

4IO₃⁻ (aq) + Re (s) + 4OH⁻ (aq) -> 4ReO₄⁻ (aq) + 26H₂O (l)

4. Balance the charge by adding OH⁻ ions to both sides of the equation:

4IO₃⁻ (aq) + Re (s) + 10OH⁻ (aq) -> 4ReO₄⁻ (aq) + 26H₂O (l)

This balanced redox reaction occurs in basic solution.