One mole of an equimolar mixture of ferric oxalate, , and ferrous oxalate, , required exactly moles — Redox Reactions and Volumetric Analysis Chemistry Question

💡 Solution & Explanation

1 mole of an equimolar mixture contains 0.5 moles of each. For $Fe_2(C_2O_4)_3$ : $Fe^{3+}$ cannot oxidize further; 3 oxalate groups oxidize to $6CO_2$ (n=6). Equivalents = $0.5 \times 6 = 3.0$ . For $FeC_2O_4$ : Fe loses 1e-, oxalate loses 2e- (n=3). Equivalents = $0.5 \times 3 = 1.5$ . Total equivalents = 4.5. $KMnO_4$ has n=5. Moles = 4.5 / 5 = 0.9.