During a highly precise redox titration conducted in an acidified laboratory medium, exactly mole of — d and f Block Elements Chemistry Question
Question
During a highly precise redox titration conducted in an acidified laboratory medium, exactly $1$ mole of pure Ferrous Oxalate ($FeC_2O_4$) is subjected to complete oxidation by Potassium Permanganate. What is the total, exact number of moles of electrons strictly lost by that single mole of Ferrous Oxalate during its complete transformation?
💡 Solution & Explanation
Ferrous Oxalate ($FeC_2O_4$) acts as a potent reducing agent where BOTH the cation and the anion undergo simultaneous oxidation. The $Fe^{2+}$ is oxidized to $Fe^{3+}$ (losing exactly $1$ mole of electrons). Concurrently, the entire oxalate ion ($C_2O_4^{2-}$) is oxidized to $2$ moles of $CO_2$ gas (losing exactly $2$ moles of electrons). The total moles of electrons lost by one mole of the compound is strictly $1 + 2 = 3$.