Question

In a particular redox reaction, ClO²⁻ is oxidized to ClO⁴⁻ and Ag is reduced to Ag. Complete and balance the equation for this reaction in acidic solution. Phases are optional.

ClO²⁻ + Ag⁺ --> ClO⁴⁻+ Ag

Answer 1

To balance the redox reaction where ClO²⁻ is oxidized to ClO⁴⁻ and Ag⁺ is reduced to Ag, the balanced equation in an acidic solution is ClO²⁻ + 4Ag⁺ + 6H⁺ → ClO⁴⁻ + 4Ag + 3H₂O.

Step-by-step explanation:

To complete and balance the equation for the redox reaction in acidic solution where ClO²⁻ is oxidized to ClO⁴⁻ and Ag is reduced to Ag, we must first determine the oxidation states of chlorine in ClO²⁻ and ClO⁴⁻. Chlorine's oxidation state increases from +3 in ClO²⁻ to +7 in ClO⁴⁻, indicating that chlorine undergoes oxidation and ClO²⁻ is the reducing agent. For silver, Ag⁺ is reduced to Ag, so Ag⁺ is the oxidant. The balanced equation in acidic solution can be represented as:

ClO²⁻ + 4Ag⁺ + 6H⁺ → ClO⁴⁻ + 4Ag + 3H₂O

This equation is balanced with respect to both mass and charge. In acidic solution, H⁺ ions and water molecules are added as needed to balance hydrogen and oxygen atoms.