# Chapter 14 - Acids and Bases - Questions for Review and Thought - Topical Questions - Page 652d: 68a

This reation is reactant-favored. - $H_2O(l) + HNO_3(aq) \lt -- \gt H_3O^{+}(aq) + N{O_3}^-(aq)$ --- Other reactions: - $H_2O(l) + N{O_3}^-(aq) \lt -- \gt OH^-(aq) + HNO_3(aq)$** ** This reaction is very insignificant, because $N{O_3}^-$ is a very weak acid. - $2H_2O(l) \lt -- \gt H_3O^+(aq) + OH^-(aq)$

#### Work Step by Step

1. Identify the acids and bases: - $H_2O$ is amphiprotic. - $HNO_3$ is an acid. - Therefore, the only reaction that can occur is with $HNO_3$ as an acid. 2. Write the reaction - $H_2O(l) + HNO_3(aq) \lt -- \gt H_3O^{+}(aq) + N{O_3}^-(aq)$ 3. Identify the weaker acid (or base). $HNO_3$ and $H_3O^+$: $H_3O^+$ is weaker. Therefore, the side that has the $H_3O^+$ is favored; Other possible reaction? - $H_2O$ can act as an acid too: $H_2O(l) + N{O_3}^-(aq) \lt -- \gt OH^-(aq) + HNO_3(aq)$ $HNO_3$ can act only as an acid. $H_3O^+$ can act only as an acid. $N{O_3}^-$ can act only as a base. And we have the auto-ionization of water: $2H_2O(l) \lt -- \gt H_3O^+(aq) + OH^-(aq)$

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