A solution containing `Cu^(+2), C_2 O_(4)^(-2)` ions: The solution requires 22.6 mL of 0.02 `M KMnO_4` in the presence of `H_2 SO_4` for oxidation. The resulting solution is neutralized and added excess KI. The iodine is liberated according to this equation `Cu^(2+) + I^(-) to Cu_2 I_2 ` The iodine liberated requires 11.3 mL of 0.05 M `Na_2 S_2 O_3` solution. The molar ratio of `Cu^(2+) , C_2 O_(4)^(-2)` in solution is

Options

A. `1:1`
B. `1:2`
C. `2:1`
D. `1:3`

Answer

B

Explanation

Mole of ` Cu^(+2) = (11.3 xx 0.05 )/(1000) = 0.565 xx 10^(-3) , ` mole of ` C_2 O_(4)^(-2)=( 22.6 xx 0.02 xx 5)/(2000 ) = 1.13 xx 10^(-3)`