---
title: "A student mixes an acidic solution containing  \\(\\text{VO}_2^+\\text{(aq)}\\) ions with a solution containing \\(\\text{SO}_3^{2-}\\text{(aq)}\\) ions. The balanced net ionic equation for the reaction is represented below.  \\[ 2\\,\\text{VO}_2^+\\text{(aq)} + \\text{SO}_3^{2-}\\text{(aq)} + 2\\,\\text{H}^+\\text{(aq)} \\rightarrow 2\\,\\text{VO}^{2+}\\text{(aq)} + \\text{SO}_4^{2-}\\text{(aq)} + \\text{H}_2\\text{O(l)} \\]  Which of the following correctly identifies the reducing agent and explains the change that occurs during the reaction?"
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url: "https://nerd-notes.com/ubq/121460/"
date_modified: "2026-08-23T05:04:38+00:00"
---

# A student mixes an acidic solution containing 
\(\text{VO}_2^+\text{(aq)}\) ions with a solution containing \(\text{SO}_3^{2-}\text{(aq)}\) ions. The balanced net ionic equation for the reaction is represented below.

\[ 2\,\text{VO}_2^+\text{(aq)} + \text{SO}_3^{2-}\text{(aq)} + 2\,\text{H}^+\text{(aq)} \rightarrow 2\,\text{VO}^{2+}\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} + \text{H}_2\text{O(l)} \]

Which of the following correctly identifies the reducing agent and explains the change that occurs during the reaction?

A student mixes an acidic solution containing 
\(\text{VO}_2^+\text{(aq)}\) ions with a solution containing \(\text{SO}_3^{2-}\text{(aq)}\) ions. The balanced net ionic equation for the reaction is represented below.

\[ 2\,\text{VO}_2^+\text{(aq)} + \text{SO}_3^{2-}\text{(aq)} + 2\,\text{H}^+\text{(aq)} \rightarrow 2\,\text{VO}^{2+}\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} + \text{H}_2\text{O(l)} \]

Which of the following correctly identifies the reducing agent and explains the change that occurs during the reaction?

- **A.** \(\text{VO}_2^+\text{(aq)}\), because vanadium gains electrons and its oxidation state decreases from \(+5\) to \(+4\).
- **B.** \(\text{VO}_2^+\text{(aq)}\), because vanadium loses electrons and its oxidation state increases from \(+4\) to \(+5\).
- **C.** \(\text{SO}_3^{2-}\text{(aq)}\), because sulfur loses electrons and its oxidation state increases from \(+4\) to \(+6\).
- **D.** \(\text{SO}_3^{2-}\text{(aq)}\), because sulfur gains electrons and its oxidation state decreases from \(+6\) to \(+4\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121460/*