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Answer: According to the acid-base theory of Bronsted and Lowry, acids are proton givers whereas bases are proton acceptors. In order to describe conjugate acid-base pairs. Let’s examine the following response:
CH3COOH + H2O → CH3COO– + H3O+
In the process described above, acetic acid (CH3COOH) contributes to a proton and produces acetate ion (CH3COO–). The substance formed when an acid donates a proton is known as a conjugate base. The acetate ion (CH3COO–) is hence the conjugate base of acetic acid. Similarly, water (H2O) takes a proton and functions as a base, producing the hydronium ion (H3O+). The substance formed when a base accepts a proton is known as conjugate acid. Hydronium ion (H3O+) is hence the conjugate acid of water (base).
Therefore, H2O and H3O+ are instances of conjugate acid-base pairings.
