Chapter 10 - Reactions in Aqueous Solutions I: Acids, Bases, and Salts - Exercises - Bronsted-Lowry Theory - Page 368: 14

$NH_3(aq) + H_2O(l) \leftrightharpoons NH{_4}^+(aq) + OH^-(aq)$ $HS^-(aq) + H_2O(l) \leftrightharpoons H_2S(aq) + OH^-(aq)$ $CH_3COO^-(aq) + H_2O(l) \leftrightharpoons CH_3COOH(aq) + OH^-(aq)$ $O^{2-}(aq) + H_2O(l) \leftrightharpoons 2 OH^-(aq)$

Since these are bases, they will receive a proton from water, producing their conjugate acid and the hydroxide ion.