Chemistry: A Molecular Approach (3rd Edition)

Published by Prentice Hall
ISBN 10: 0321809246
ISBN 13: 978-0-32180-924-7

Chapter 15 - Sections 15.1-15.12 - Exercises - Problems by Topic - Page 746: 36d


Bronsted-Lowry acid: $HBr$ Bronsted-Lowry base: $H_{2}O$ Conjugate acid: $H_{3}O^+$ Conjugate base: $Br^{-}$

Work Step by Step

According to the Bronsted-Lowry definition, Acid: proton ($H^{+}$ ion) donor Base: proton ($H^{+}$ ion) acceptor In the reaction, $HBr$ is the acid because, in solution, it donates a proton to water. $H_{2}O$ is the base because it accepts the proton. A conjugate acid is any base to which a proton has been added. So, $H_3O^+$ is the conjugate acid. A conjugate base is an acid from which a proton has been removed. So, $Br^-$ is the conjugate base.
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