Chemistry: The Central Science (13th Edition)

Published by Prentice Hall
ISBN 10: 0321910419
ISBN 13: 978-0-32191-041-7

Chapter 16 - Acid-Base Equilibria - Exercises - Page 717: 16.18b


Bronsted-Lowry Acid: $H{SO_4}^-(aq)$ Bronsted-Lowry Base: $H{CO_3}^-(aq)$ Conjugate Base: $S{O_4}^{2-}(aq)$ Conjugate Acid: $H_2CO_3(aq)$

Work Step by Step

$H{SO_4}^-(aq) + H{CO_3}^-(aq) S{O_4}^{2-}(aq) + H_2CO_3(aq)$ Since $H{SO_4}^-$ donates one proton, it is the acid; Since $H{CO_3}^-$ receives one proton, it is the base; $S{O_4}^{2-}$ is the conjugate base because it is the acid ($H{SO_4}^-$) after donating a proton $H_2CO_3$ is the conjugate acid because it is the base ($H{CO_3}^-$) after receiving a proton.
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