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: 12


a. The water molecules will donate protons to the ammonia aqueous molecules, forming its conjugate acid, ammonium ion, and $OH^-$. $$NH_3(aq) + H_2O(l) \leftrightharpoons NH_{4}^+(aq) + OH^-(aq)$$ b. Ammonia will also act as a base, receiving on proton from the hydrogen chloride, resulting in $N{H_4}^+$ and $Cl^-$, the conjugate pairs of the reactants. The resulting products will form a solid ionic compound. $$NH_3(g) + HCl(g) \longrightarrow N{H_4}Cl(s)$$

Work Step by Step

According to the Bronsted-Lowry theory, ammonia $NH_3$ is a base, and is able to receive protons from Bronsted-Lowry acids, like water and gaseous hydrogen chloride.
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