---
title: "A student investigates the redox behavior of the nitrite ion, \\(\\text{NO}_2^-\\text{(aq)}\\), by carrying out two separate reactions in acidic solution:  Reaction 1: \\[ 5\\,\\text{NO}_2^-\\text{(aq)} + 2\\,\\text{MnO}_4^-\\text{(aq)} + 6\\,\\text{H}^+\\text{(aq)} \\rightarrow 5\\,\\text{NO}_3^-\\text{(aq)} + 2\\,\\text{Mn}^{2+}\\text{(aq)} + 3\\,\\text{H}_2\\text{O(l)} \\]  Reaction 2: \\[ 2\\,\\text{NO}_2^-\\text{(aq)} + 2\\,\\text{I}^-\\text{(aq)} + 4\\,\\text{H}^+\\text{(aq)} \\rightarrow 2\\,\\text{NO(g)} + \\text{I}_2\\text{(aq)} + 2\\,\\text{H}_2\\text{O(l)} \\]  Which of the following statements best justifies the chemical behavior of \\(\\text{NO}_2^-\\text{(aq)}\\) in these two reactions?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/123629/"
date_modified: "2026-09-28T12:01:50+00:00"
---

# A student investigates the redox behavior of the nitrite ion, \(\text{NO}_2^-\text{(aq)}\), by carrying out two separate reactions in acidic solution:

Reaction 1:
\[ 5\,\text{NO}_2^-\text{(aq)} + 2\,\text{MnO}_4^-\text{(aq)} + 6\,\text{H}^+\text{(aq)} \rightarrow 5\,\text{NO}_3^-\text{(aq)} + 2\,\text{Mn}^{2+}\text{(aq)} + 3\,\text{H}_2\text{O(l)} \]

Reaction 2:
\[ 2\,\text{NO}_2^-\text{(aq)} + 2\,\text{I}^-\text{(aq)} + 4\,\text{H}^+\text{(aq)} \rightarrow 2\,\text{NO(g)} + \text{I}_2\text{(aq)} + 2\,\text{H}_2\text{O(l)} \]

Which of the following statements best justifies the chemical behavior of \(\text{NO}_2^-\text{(aq)}\) in these two reactions?

A student investigates the redox behavior of the nitrite ion, \(\text{NO}_2^-\text{(aq)}\), by carrying out two separate reactions in acidic solution:

Reaction 1:
\[ 5\,\text{NO}_2^-\text{(aq)} + 2\,\text{MnO}_4^-\text{(aq)} + 6\,\text{H}^+\text{(aq)} \rightarrow 5\,\text{NO}_3^-\text{(aq)} + 2\,\text{Mn}^{2+}\text{(aq)} + 3\,\text{H}_2\text{O(l)} \]

Reaction 2:
\[ 2\,\text{NO}_2^-\text{(aq)} + 2\,\text{I}^-\text{(aq)} + 4\,\text{H}^+\text{(aq)} \rightarrow 2\,\text{NO(g)} + \text{I}_2\text{(aq)} + 2\,\text{H}_2\text{O(l)} \]

Which of the following statements best justifies the chemical behavior of \(\text{NO}_2^-\text{(aq)}\) in these two reactions?

- **A.** \(\text{NO}_2^-\text{(aq)}\) acts as a reducing agent in Reaction 1 and an oxidizing agent in Reaction 2 because nitrogen is in an intermediate oxidation state of \(+3\), allowing it to lose electrons to form \(\text{NO}_3^-\) or gain electrons to form \(\text{NO}\).
- **B.** \(\text{NO}_2^-\text{(aq)}\) acts as an oxidizing agent in Reaction 1 and a reducing agent in Reaction 2 because the negative charge on the nitrite ion allows it to accept electrons from cations and donate electrons to anions.
- **C.** \(\text{NO}_2^-\text{(aq)}\) acts as a reducing agent in Reaction 1 and an oxidizing agent in Reaction 2 because oxygen atoms in \(\text{NO}_2^-\) change their oxidation states from \(-2\) to \(0\) and \(-1\), while the oxidation state of the nitrogen atom remains constant at \(+3\).
- **D.** \(\text{NO}_2^-\text{(aq)}\) acts exclusively as a Brønsted-Lowry base in both reactions because the lone pair on the nitrogen atom accepts protons from \(\text{H}^+\text{(aq)}\), which drives the conversion into other nitrogen-containing species.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123629/*