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: 36b

Answer

Bronsted-Lowry acid: $H_{2}O$ Bronsted-Lowry base: $CH_3NH_2$ Conjugate acid: $CH_3NH_3^+$ Conjugate base: $OH^{-}$

Work Step by Step

According to the Bronsted-Lowry definition, Acid: proton ($H^{+}$ ion) donor Base: proton ($H^{+}$ ion) acceptor In the reaction, $H_{2}O$ is the acid because it donates a proton to water. $CH_3NH_2$ is the base because it accepts the proton. A conjugate acid is any base to which a proton has been added. So, $CH_3NH_3^+$ is the conjugate acid. A conjugate base is an acid from which a proton has been removed. So, $OH^-$ is the conjugate base.
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