## Chemistry: The Central Science (13th Edition)

Bronsted-Lowry Acid: $H_3O^+(aq)$ Bronsted-Lowry Base: ${HSO_3}^{-}(aq)$ Conjugate Acid: $H_2SO_3(aq)$ Conjugate Base: $H_2O(l)$
${H_3O}^+(aq) + H{SO_3}^-(aq) H_2{SO_3}^{}(aq) + H_2O(l)$ Since $H_3O^+$ donates one proton, it is the acid; Since $H{SO_3}^-$ receives one proton, it is the base; $H_2O$ is the conjugate base because it is the acid ($H_3O^+$) after donating a proton $H_2SO_3$ is the conjugate acid because it is the base ($H{SO_3}^-$) after receiving a proton.