A solution of 0.2 g of a compound containing `Cu^(2+) "and" C_(2)O_(4)^(2-)` ions on titration with 0.02 M `KMnO_(4)` in presence of `H_(2)SO_(4)` consumes 22.6 mL of the oxidant. The resultant solution is neutralized with `Na_(2)CO_(3)` acidified with dil. acetic acid and treated with excess KI. The liberated iodine requires 11.3 mL of 0.5 M `Na_(2)S_(2)O_(3)` solution for complete reduction. Find out the mole ratio of `Cu^(2+) "to" C_(2)O_(4)^(2-)` in the compound. Write down the balanced redox reactions involved in the above titrations.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Calculate the moles of KMnO4 used in the titration.

Given:
- Volume of KMnO4 = 22.6 mL = 0.0226 L
- Molarity of KMnO4 = 0.02 M

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