When $\ce{KMnO_4}$ solution is added to oxalic acid solution, the decolourisation is slow in the beginning but becomes instantaneous after some time because
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When $\ce{KMnO_4}$ solution is added to oxalic acid solution, the decolourisation is slow in the beginning but becomes instantaneous after some time because $Mn^{2+}$ acts as an autocatalyst.
Reduction half $\text{MnO}^-_4+8\text{H}^++5\text{e}^-\rightarrow\text{Mn}^{2+}+4\text{H}_2\text{O]}\times2$
Oxidation half $\text{C}_2\text{O}_4^{2-}\rightarrow2\text{CO}_2+2\text{e}^-]\times5$
Overall equation $2\text{MnO}_4^-+16\text{H}^++5\text{C}_2\text{O}_4^{2-}\rightarrow2\text{Mn}^{2+}+10\text{CO}_2+8\text{H}_2\text{O}$
End point of this reaction Colourless to light pink
Reduction half $\text{MnO}^-_4+8\text{H}^++5\text{e}^-\rightarrow\text{Mn}^{2+}+4\text{H}_2\text{O]}\times2$
Oxidation half $\text{C}_2\text{O}_4^{2-}\rightarrow2\text{CO}_2+2\text{e}^-]\times5$
Overall equation $2\text{MnO}_4^-+16\text{H}^++5\text{C}_2\text{O}_4^{2-}\rightarrow2\text{Mn}^{2+}+10\text{CO}_2+8\text{H}_2\text{O}$
End point of this reaction Colourless to light pink
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