## Chemistry: The Central Science (13th Edition)

Published by Prentice Hall

# Chapter 16 - Acid-Base Equilibria - Exercises: 16.18a

#### Answer

Acid in the left side: $HBrO(aq)$ Base in the left side: $H_2O(l)$ Conjugate Acid: $H_3O^+(aq)$ Conjugate Base: $BrO^-(aq)$

#### Work Step by Step

$HBrO(aq) + H_2O(l) BrO^-(aq) + H_3O^+(aq)$ Since $HBrO$ donates a proton, it is the Bronsted-Lowry Acid. Since $H_2O$ receives a proton, it is the Bronsted-Lowry Base. $BrO^-$ is the conjugate base because it derives from the acid ($HBrO$) $H_3O^+$ is the conjugate acid because it derives from the base ($H_2O$)

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