A solution contains 0.0100 mol Fe^2+ and 0.0100 mol C2O4^2- (no other reductant). Which of the following are correct?

If a titrant oxidised only Fe^2+, then 0.0200 M K2Cr2O7 would need 83.3 mL.

Complete oxidation of both needs 300 mL of 0.0200 M acidified KMnO4.

The normality of 0.0200 M KMnO4 in acidic medium is 0.100 N.

The oxalate alone would need 100 mL of 0.0200 M acidified KMnO4.

If a titrant oxidised only Fe^2+, then 0.0200 M K2Cr2O7 would need 83.3 mL.

Complete oxidation of both needs 300 mL of 0.0200 M acidified KMnO4.

The normality of 0.0200 M KMnO4 in acidic medium is 0.100 N.

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JEE Advanced levelOne or more correct optionsDifficulty 3 of 3eq073

A solution contains $0.0100$ mol $Fe X^{2 +}$ and $0.0100$ mol $C X_{2} O X_{4} X^{2 -}$ (no other reductant). Which of the following are correct?

AThe oxalate alone would need 100 mL of $0.0200 M$ acidified $KMnO X_{4}$ .
BIf a titrant oxidised only $Fe X^{2 +}$ , then $0.0200 M$ $K X_{2} Cr X_{2} O X_{7}$ would need 83.3 mL.
CComplete oxidation of both needs 300 mL of $0.0200 M$ acidified $KMnO X_{4}$ .
DThe normality of $0.0200 M$ $KMnO X_{4}$ in acidic medium is $0.100 N$ .

Answer: B, C, D

Total electrons = 0.0100 + 0.0200 = 0.0300 mol, so KMnO4 = 0.0060 mol = 300 mL; N = 5 x 0.0200 = 0.100. Dichromate for Fe2+ alone: 0.0100/6 = 1.667e-3 mol = 83.3 mL. Oxalate alone: 0.0200/5 = 4.00e-3 mol = 200 mL, not 100 mL.

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A solution contains 0.0100 mol FeX2+ and 0.0100 mol CX2​OX4​X2− (no other reductant). Which of the following are correct?

Answer: B, C, D

More questions on Redox titrations with KMnO4 and K2Cr2O7

A solution contains $0.0100$ mol $Fe X^{2 +}$ and $0.0100$ mol $C X_{2} O X_{4} X^{2 -}$ (no other reductant). Which of the following are correct?