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title: "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?"
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url: "https://nerd-notes.com/ubq/119204/"
date_modified: "2026-08-19T12:39:21+00:00"
---

# 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?

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?

- **A.** \(\text{H}_2\text{C}_2\text{O}_4\text{(aq)}\), in which the oxidation number of \(\text{C}\) increases from \(+3\) to \(+4\)
- **B.** \(\text{MnO}_4^-\text{(aq)}\), in which the oxidation number of \(\text{Mn}\) decreases from \(+7\) to \(+2\)
- **C.** \(\text{H}^+\text{(aq)}\), in which the oxidation number of \(\text{H}\) increases from \(+1\) to \(+2\)
- **D.** \(\text{H}_2\text{C}_2\text{O}_4\text{(aq)}\), in which the oxidation number of \(\text{C}\) increases from \(+2\) to \(+4\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119204/*