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Question #e3e9a

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Answer 1 · 2016-04-14T09:23:00

It appears to be an oxidation reaction of ferrous oxalate dihydrate by Potassium Permanganate.
Potassium permanganate is a very strong oxidizing agent, oxidizes both the ${Fe}^{2 +}$ $"Fe"^(2+)$ ion and the oxalate ion.

Explanation:

Redox reactions for oxidation of both are shown below:

Oxalate oxidation:
$2 {MnO}_{4}^{-} + 16 H^{+} + 5 C_{2} O_{4}^{2 -} \to 2 {Mn}^{2 +} + 8 H_{2} O + 10 {CO}_{2}$ $2"MnO"_4^(-) + 16"H"^+ + 5"C"_2"O"_4^(2-)-> 2"Mn"^(2+) + 8"H"_2"O" + 10"CO"_2$

Iron(II) oxidation:
${MnO}_{4}^{-} + 8 H^{+} + 5 {Fe}^{2 +} \to {Mn}^{2 +} + 4 H_{2} O + 5 {Fe}^{3 +}$ $"MnO"_4^(-) + 8"H"^+ + 5"Fe"^(2+) -> "Mn"^(2+) + 4"H"_2"O" + 5"Fe"^(3+)$

First the ferrous oxalate dihydrate is dissolved in Sulfuric acid, $H_{2} {SO}_{4}$ $"H"_2"SO"_4$

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