A solution of 0.2 g of a compound containing Cu2+ and C2O2–4 ions on titration with 0.02 M KMnO4 in presence of H2SO4 consumes 22.6 mL of the oxidant. The resultant solution is neutralized with Na2CO3, acidified with dil. acetic acid and treated with excess KI.The liberated iodine requires 11.3 mL of 0.05MNa2S3O3 solution for complete reduction. Find out the mole ratio of Cu2+ to C2O2–4 in the compound is a:b. The sum of a+b is

A solution of 0.2 g of a compound containing Cu2+ and C2O2–4 ions on

1.	A solution of 0.2 g of a compound containing Cu2+ and C2O2–4 ions on titration with 0.02 M KMnO4 in presence of H2SO4 consumes 22.6 mL of the oxidant. The resultant solution is neutralized with Na2CO3, acidified with dil. acetic acid and treated with excess KI.The liberated iodine requires 11.3 mL of 0.05MNa2S3O3 solution for complete reduction. Find out the mole ratio of Cu2+ to C2O2–4 in the compound is a:b. The sum of a+b is
Answer» A solution of $0.2 g$ of a compound containing $C u^{2 +}$ and $C_{2} O_{4}^{2 -}$ ions on titration with $0.02 M K M n O_{4}$ in presence of $H_{2} S O_{4}$ consumes $22.6 m L$ of the oxidant. The resultant solution is neutralized with $N a_{2} C O_{3}$ , acidified with dil. acetic acid and treated with excess $K I$ .The liberated iodine requires $11.3 m L$ of $0.05 M N a_{2} S_{3} O_{3}$ solution for complete reduction. Find out the mole ratio of $C u^{2 +}$ to $C_{2} O_{4}^{2 -}$ in the compound is $a : b$ . The sum of $a + b$ is