Redox Titration - Oxalic Acid vs $$\text{KMnO}_4$$

Formula / Core Reaction:

$$2\text{MnO}_4^- + 5\text{C}_2\text{O}_4^{2-} + 16\text{H}^+ \xrightarrow{60-70^\circ\text{C}} 2\text{Mn}^{2+} + 10\text{CO}_2 \uparrow + 8\text{H}_2\text{O}$$

Concept: Redox titration where permanganate ($$\text{MnO}_4^-$$) oxidizes oxalate ion ($$\text{C}_2\text{O}_4^{2-}$$) to carbon dioxide in acidic medium. Heating to $$60-70^\circ\text{C}$$ is required to accelerate the initial slow kinetics until autocatalytic $$\text{Mn}^{2+}$$ forms.

Notation / Key Observation:

• n-factor of $$\text{KMnO}_4 = 5$$ ($$\text{Mn}^{+7} \rightarrow \text{Mn}^{+2}$$);
• n-factor of Oxalic acid ($$\text{H}_2\text{C}_2\text{O}_4$$) = 2 ($$\text{C}^{+3}_2 \rightarrow 2\text{C}^{+4}$$);
• Equivalence relation: $$N_1V_1 = N_2V_2 \implies 5 \cdot M_{\text{KMnO}_4} \cdot V_{\text{KMnO}_4} = 2 \cdot M_{\text{oxalic}} \cdot V_{\text{oxalic}}$$.