Chemistry (7th Edition)

Published by Pearson
ISBN 10: 0321943171
ISBN 13: 978-0-32194-317-0

Chapter 15 - Aqueous Equilibria: Acids and Bases - Worked Example - Page 606: 2


(a) $H_2CO_3$ (b) $HC{O_3}^-$ (c) $H_2O$ (d) $H_3PO_4$

Work Step by Step

The conjugate acid is the result of a base that receives one proton, therefore, you just need to add one hydrogen to the chemical formula, and sum 1 to the charge. For example: 1. Add the hydrogen: $H{CO_3}^- -- \gt H_2{CO_3}^-$ 2. Sum 1 to the charge: $H_2{CO_3}^- -- \gt H_2CO_3$
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