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Question: Ionic dissociation of acetic acid is represented as: \(C{H_3}COOH + {H_2}O \rightleftharpoons C{H_...

Ionic dissociation of acetic acid is represented as:
CH3COOH+H2OCH3COO+H3O+C{H_3}COOH + {H_2}O \rightleftharpoons C{H_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

Explanation

Solution

Bronsted lowry concept is developed to overcome the limitations of Arrhenius concept such as bronsted lowry concept can explain reactions in an non aqueous medium and is not limited to molecules only but includes even the ionic species.

Complete step by step answer:
According to Bronsted-lowry acid-base theory, any substance which has a tendency to donate its proton (H+H^{+}) is acid and a substance that has a tendency to accept a proton (H+H^{+}) is called the base. A conjugate pair of acid and a base differs only by a proton (H+H^{+}). In the question we are given with the ionic dissociation of acetic acid.
In the reaction:
CH3COOH+H2OCH3COO+H3O+C{H_3}COOH + {H_2}O \rightleftharpoons C{H_3}CO{O^ - } + {H_3}{O^ + }
CH3COOHC{H_3}COOH is donating its proton to H2O{H_2}O to form H3O+{H_3}{O^ + }.Hence due the bronsted lowry concept CH3COOHC{H_3}COOHis an acid, as it donating H+H_{+} it acts as an acid and H2O{H_2}O is base, as it accepting H+H^{+} .
In the products side, the CH3COOC{H_3}CO{O^ - } is the conjugate base of acid CH3COOHC{H_3}COOH and H3O+{H_3}​O^+ is the conjugate acid of the base H2O{H_2}O. therefore the two conjugate pairs in the reaction are
conjugate acid-base where CH3COOHC{H_3}COOH is acid and CH3COOC{H_3}CO{O^ - } is its base
conjugate acid-base where H2O{H_2}O is the base and H3O+{H_3}{O^ + } is its acid.
So in total, 2 acids and 2 bases are present in the reaction.

Hence the correct option is option B.

Additional information: Classic concept of acid base has been defined by three theories which are Arrhenius acid and base- a substance which donates H+H^{+} is an acid, and a substance which donates OHOH^{-} is a base.
According to Bronsted-lowry acid-base theory- any substance which donates its proton (H+H^{+}) is acid and which accepts a proton (H+H^{+}) is called the base.
According to Lewis acid-base theory- any substance which accepts electron pairs is acid, and which donates electron pairs is a base.
All the theories complete each other's limitation Arrhenius theory’s limitation were completed by bronsted lowry concept and so on.

Note:
All Arrhenius acids are also bronsted acids but all Arrhenius bases can not be bronsted bases because bronsted base accepting protons may not have OHOH^{-}.