Question

Ionic dissociation of acetic acid is represented as:

${CH}_{3}COOH+H_{2}O\rightleftharpoons {CH}_{3}CO{O}^{-}+H_3{O}^{+}$

According to Lowry and Bronsted, the reaction possesses:

• A. An acid and three bases
• B. Two acids and two bases
• C. An acid and a base
• D. Three acids and a base

Answer 1

The correct option is B Two acids and two bases

According to Bronsted-lowry acid-base theory, any electrolyte which donates its proton ($H^{+}$) is acid and which accepts a proton ($H^{+}$) is called base.

Given reaction:

${CH}_{3}COOH+H_{2}O\rightleftharpoons {CH}_{3}CO{O}^{-}+H_3{O}^{+}$

$C{H}_{3}COOH$ is donating its proton to $H_{2}O$.

Here $C{H}_{3}COOH$ is acid,as it donating $H^{+}$and $H_{2}O$ is base, as it accepting $H^{+}$

In products side, the $C{H}_{3}CO{O}^{-}$ is conjugate base of acid $C{H}_{3}COOH$ and $H_3{O}^{+}$ is conjugate acid of base $H_{2}O$.

So in total, 2 acids and 2 bases are present in the reaction.

Hence, option $B$ is correct.