JEE Advance - Chemistry (1991 - No. 5)
A solution of 0.2 g of a compound containing Cu2+ and $$C_2O_4^{2-}$$ ions on titration with 0.02M $$KMnO_4$$ in presence of $$H_2SO_4$$ consumes 22.6 ml. of the oxidant. The resultant solution in neutralized with Na2CO3, acidified with dil. acetic acid and treated with excess KI. The liberated iodine requires 11.3 ml of 0.05M Na2S2O3 solution for complete reduction.
Find out the molar ratio of Cu2+ to $$C_2O_4^{2-}$$ in the compound.Write down the balanced redox reactions involved in the above titrations.
Find out the molar ratio of Cu2+ to $$C_2O_4^{2-}$$ in the compound.Write down the balanced redox reactions involved in the above titrations.
1:1
1:2
2:1
1:3
3:1