AP Chemistry
4.9 Oxidation-Reduction (Redox) Reactions
A student titrates an acidic solution of oxalic acid, \(\text{H}_2\text{C}_2\text{O}_4\text{(aq)}\), with a standardized potassium permanganate solution, \(\text{KMnO}_4\text{(aq)}\). The balanced net-ionic equation for the redox titration reaction is shown below:
\[2\text{MnO}_4^-\text{(aq)} + 5\text{H}_2\text{C}_2\text{O}_4\text{(aq)} + 6\text{H}^+\text{(aq)} \rightarrow 2\text{Mn}^{2+}\text{(aq)} + 10\text{CO}_2\text{(g)} + 8\text{H}_2\text{O(l)}\]
Which species acts as the reducing agent in this reaction, and what is the change in the oxidation number of the atom being oxidized?
\[2\text{MnO}_4^-\text{(aq)} + 5\text{H}_2\text{C}_2\text{O}_4\text{(aq)} + 6\text{H}^+\text{(aq)} \rightarrow 2\text{Mn}^{2+}\text{(aq)} + 10\text{CO}_2\text{(g)} + 8\text{H}_2\text{O(l)}\]
Which species acts as the reducing agent in this reaction, and what is the change in the oxidation number of the atom being oxidized?
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