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

Answer

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.
Update this answer!

You can help us out by revising, improving and updating this answer.

Update this answer

After you claim an answer you’ll have 24 hours to send in a draft. An editor will review the submission and either publish your submission or provide feedback.