## Chemistry: A Molecular Approach (3rd Edition)

Bronsted-Lowry acid: $H_2O(l)$ Bronsted-Lowry base: $NH_3(aq)$ Conjugate acid: $NH_4^+(aq)$ Conjugate base: $OH^-(aq)$
According to the Bronsted-Lowry definition, Acid: proton ($H^{+}$ ion) donor Base: proton ($H^{+}$ ion) acceptor In the reaction, $H_{2}O$ is the acid because it donates a proton. $NH_3$ is the base because it accepts the proton. A conjugate acid is any base to which a proton has been added. So, $NH_4^+$ is the conjugate acid. A conjugate base is an acid from which a proton has been removed. So, $OH^-$ is the conjugate base.