A solution of `0.2` g of a compound containing `Cu^(2+)` and `C_2O_4^(2−)` ions on titration with `0.02`M `KMnO_4` i

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Q 1119067819.     A solution of `0.2` g of a compound containing `Cu^(2+)` and `C_2O_4^(2−)` ions on titration with `0.02`M `KMnO_4` in presence of `H_2SO_4` consumes `22.6` mL of the oxidant. The resultant solution is neutralized with `Na_2CO_3`, acidified with dilute acetic acid and treated with excess `KI`. The liberated iodine requires `11.3` mL of `0.05` M `Na_2S_2O_3` solution for complete reduction. Calculate the mole ratio of `Cu^( 2+` to `C_2O_4^(2−)` in the compound.
JEE 1991
A

`1 : 3`

B

`2 : 3`

C

`1 : 4`

D

`1 : 2`

HINT


Solution
(Provided By a Student and Checked/Corrected by EXXAMM.com Team)

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