Which of the following correctly give the moles of acidified $KMnO X_{4}$ needed per mole of the substance (each product is the highest stable oxidation state: oxalate to $CO X_{2}$ , nitrite to nitrate, $Fe X^{2 +}$ to $Fe X^{3 +}$ , $Fe X^{3 +}$ is not oxidised further)?

A $NaNO X_{2}$ : 0.4 mol
B $H X_{2} C X_{2} O X_{4}$ : 0.4 mol
C $Fe X_{2} (C X_{2} O X_{4}) X_{3}$ : 0.6 mol
D $FeC X_{2} O X_{4}$ : 0.6 mol

Answer: A, B, D

Moles of KMnO4 = (electrons lost per mole)/5. FeC2O4 loses 3 e-, so 0.6 mol; H2C2O4 loses 2 e-, so 0.4 mol; NaNO2 loses 2 e-, so 0.4 mol. In Fe2(C2O4)3 only the three oxalates react: 6 e-, so 1.2 mol, not 0.6.

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Which of the following correctly give the moles of acidified KMnOX4​ needed per mole of the substance (each product is the highest stable oxidation state: oxalate to COX2​, nitrite to nitrate, FeX2+ to FeX3+, FeX3+ is not oxidised further)?

Answer: A, B, D

More questions on Redox titrations with KMnO4 and K2Cr2O7

Which of the following correctly give the moles of acidified $KMnO X_{4}$ needed per mole of the substance (each product is the highest stable oxidation state: oxalate to $CO X_{2}$ , nitrite to nitrate, $Fe X^{2 +}$ to $Fe X^{3 +}$ , $Fe X^{3 +}$ is not oxidised further)?