# Chapter 14 - Acids and Bases - Questions for Review and Thought - Topical Questions - Page 652c: 43f

$H_2SO_4(aq) + H_2O(l) \lt -- \gt H{SO_4}^-(aq) + H_3O^+(aq)$ $K_a = \frac{[H_3O^+][H{SO_4}^-]}{[H_2SO_4]}$

#### Work Step by Step

1. Write the ionization chemical equation: - Since $H_2SO_4$ is an acid, write the reaction where it donates a proton to a water molecule: $H_2SO_4(aq) + H_2O(l) \lt -- \gt H{SO_4}^-(aq) + H_3O^+(aq)$ 2. Now, write the $K_a$ expression: - The $K_a$ expression is the concentrations of the products divided by the concentration of the reactants: $K_a = \frac{[Products]}{[Reactants]}$ $K_a = \frac{[H_3O^+][H{SO_4}^-]}{[H_2SO_4]}$ *** We don't consider the $[H_2O]$, because it is the solvent of the solution.

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.