How do we represent the oxidation of oxalate ion by permanganate ion?

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How do we represent the oxidation of oxalate ion by permanganate ion?

How do we represent the oxidation of oxalate ion by permanganate ion by the half-equation method? What colour change would we observe in the titration?

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Answer 1 · 2017-09-11T19:20:37

$"Permanganate ion"$ is coloured a bright purple....

Explanation:

And conveniently, it is reduced to $Mn^(2+)$ , which is almost colourless. This change is very recognizable, and the stoichiometric endpoint is very accessible.

$"Reduction half equation:"$

$underbrace(MnO_4^(-))_"bright purple" + 8H^(+)+5e^(-) rarr Mn^(2+)+4H_2O(l)$ $(i)$

$"Oxidation half equation:"$

$C_2O_4^(2-) rarr 2CO_2(g)+2e^(-)$ $(ii)$

And so we take $2xx(i)+5xx(ii)$ to give.....

$2MnO_4^(-) +5C_2O_4^(2-)+ 16H^(+)rarr 2Mn^(2+)+10CO_2(g)+8H_2O(l)$

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How do we represent the oxidation of oxalate ion by permanganate ion?