Chemistry 10th Edition

Published by Brooks/Cole Publishing Co.
ISBN 10: 1133610668
ISBN 13: 978-1-13361-066-3

Chapter 10 - Reactions in Aqueous Solutions I: Acids, Bases, and Salts - Exercises - Bronsted-Lowry Theory - Page 368: 11


a. $HBr(aq) + H_2O(l) \longrightarrow Br^-(aq) + H_3O^+(aq)$ b. $C_2H_5COOH(aq) + H_2O(l) \leftrightharpoons {C_2H_5COO}^-(aq) + H_3O^+(aq)$ c. $H_2S(aq) + H_2O(l) \leftrightharpoons HS^-(aq) + H_3O^+(aq)$ d. $HCN(aq) + H_2O(l) \leftrightharpoons CN^-(aq) + H_3O^+(aq)$ e. $HF(aq) + H_2O(l) \leftrightharpoons F^-(aq) + H_3O^+(aq)$ f. $HClO_4(aq) + H_2O(l) \longrightarrow ClO{_4}^-(aq) + H_3O^+(aq)$

Work Step by Step

The pattern is: $$Acid(aq) + H_2O(l) \longrightarrow Conjugate \space base + H_3O^+(aq)$$ If the acid is a strong acid, we use the single right arrow, if the acid is weak, we use the double arrow. To get the conjugate base, remove a hydrogen and 1 from the charge of the molecule/ion.
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