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Chapter 22: Problem 45

Explain, giving one example in each case, why nitrous acid can act as both a reducing agent and an oxidizing agent.

Short Answer

Expert verified
Nitrous acid (HNO2) can act as both a reducing agent, as illustrated in the reaction HNO2 + 2KMnO4 → K2MnO4 + HNO3 + H2O, where HNO2 is oxidized and KMnO4 is reduced; and an oxidizing agent, as shown in the reaction HNO2 + Zn → Zn(NO2)2 + H2, where HNO2 is reduced and Zn is oxidized.

Step by step solution

01

Identify Nitrous Acid as a Reducing Agent

This involves identifying a reaction in which nitrous acid (HNO2) acts as a reducing agent. As a reducing agent, HNO2 is oxidized, meaning it loses electrons and its oxidation state increases. Consider the reaction between nitrous acid and potassium permanganate (KMnO4):\[HNO2 + 2KMnO4 \rightarrow K2MnO4 + HNO3 + H2O\]In this reaction, nitrous acid is oxidized from a +3 oxidation state to a +5 state in nitric acid (HNO3), thereby reducing KMnO4 into K2MnO4 by decreasing the oxidation state of manganese from +7 to +6.
02

Identify Nitrous Acid as an Oxidizing Agent

This involves identifying a reaction where nitrous acid (HNO2) acts as an oxidizing agent. As an oxidizing agent, HNO2 is reduced, meaning it gains electrons and its oxidation state decreases. Consider the reaction between nitrous acid and zinc (Zn):\[HNO2 + Zn \rightarrow Zn(NO2)2 + H2\]In this reaction, nitrous acid is reduced from a +3 oxidation state to a +2 state in zinc nitrite (Zn(NO2)2), thereby oxidizing zinc from an oxidation state of 0 to +2.

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Most popular questions from this chapter

Briefly discuss the preparation and properties of carbon monoxide and carbon dioxide.

Describe two chemical differences between CO and \(\mathrm{CO}_{2}\).

Write a balanced equation for each of the following processes: (a) On heating, ammonium nitrate produces nitrous oxide. (b) On heating, potassium nitrate produces potassium nitrite and oxygen gas. (c) On heating, lead nitrate produces lead(II) oxide, nitrogen dioxide \(\left(\mathrm{NO}_{2}\right),\) and oxygen gas.

Draw molecular orbital energy level diagrams for \(\mathrm{O}_{2}, \mathrm{O}_{2}^{-},\) and \(\mathrm{O}_{2}^{2-}\).

When \(1.645 \mathrm{~g}\) of white phosphorus are dissolved in \(75.5 \mathrm{~g}\) of \(\mathrm{CS}_{2},\) the solution boils at \(46.709^{\circ} \mathrm{C}\) whereas pure \(\mathrm{CS}_{2}\) boils at \(46.300^{\circ} \mathrm{C}\). The molal boiling-point elevation constant for \(\mathrm{CS}_{2}\) is \(2.34^{\circ} \mathrm{C} / \mathrm{m}\). Calculate the molar mass of white phosphorus and give the molecular formula.
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