Question
The following equilibrium is established when hydrogen chloride is dissolved in acetic acid.
The following equilibrium is established when hydrogen chloride is dissolved in acetic acid.
The set that characterises the conjugate acidbase pairs is
A.
$$\left( {HCl,C{H_3}COOH} \right){\text{and}}\left( {C{H_3}COOH_2^ + ,C{l^ - }} \right)$$
B.
$$\left( {HCl,C{H_3}COOH_2^ + } \right){\text{and}}\left( {C{H_3}COOH,C{l^ - }} \right)$$
C.
$$\left( {C{H_3}COOH_2^ + ,HCl} \right){\text{and}}\left( {C{l^ - },C{H_3}COOH} \right)$$
D.
$$\left( {HCl,C{l^ - }} \right){\text{and}}\left( {C{H_3}COOH_2^ + ,C{H_3}COOH} \right)$$
Answer :
$$\left( {HCl,C{l^ - }} \right){\text{and}}\left( {C{H_3}COOH_2^ + ,C{H_3}COOH} \right)$$
Solution :
$$HCl$$ is stronger acid than $$C{H_3}COOH$$ and $$C{l^ - }$$ is a stronger base than $$C{H_3}COOH_2^ + $$ and is the conjugate base of $$HCl.$$
$$\mathop {HCl}\limits_{{\text{aci}}{{\text{d}}_{\text{1}}}} + \mathop {C{H_3}COOH}\limits_{{\text{bas}}{{\text{e}}_{\text{2}}}} \rightleftharpoons \mathop {C{l^ - }}\limits_{{\text{bas}}{{\text{e}}_1}} + \mathop {C{H_3}COOH_2^ + }\limits_{{\text{aci}}{{\text{d}}_2}} $$
$$HCl$$ is stronger acid than $$C{H_3}COOH$$ and $$C{l^ - }$$ is a stronger base than $$C{H_3}COOH_2^ + $$ and is the conjugate base of $$HCl.$$
$$\mathop {HCl}\limits_{{\text{aci}}{{\text{d}}_{\text{1}}}} + \mathop {C{H_3}COOH}\limits_{{\text{bas}}{{\text{e}}_{\text{2}}}} \rightleftharpoons \mathop {C{l^ - }}\limits_{{\text{bas}}{{\text{e}}_1}} + \mathop {C{H_3}COOH_2^ + }\limits_{{\text{aci}}{{\text{d}}_2}} $$