# Chapter 15 - Sections 15.1-15.12 - Exercises - Problems by Topic: 36c

Bronsted-Lowry acid: $H_{2}O$ Bronsted-Lowry base: $CO_3^{2-}$ Conjugate acid: $HCO_3^-$ Conjugate base: $OH^{-}$

#### Work Step by Step

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. $CO_3^{2-}$ is the base because it accepts the proton. A conjugate acid is any base to which a proton has been added. So, $HCO_3^-$ is the conjugate acid. A conjugate base is an acid from which a proton has been removed. So, $OH^{-}$ is the conjugate base.

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