A) \[(HCl,C{{H}_{3}}COOH)and(C{{H}_{3}}COOH_{2}^{+},C{{l}^{-}})\]
B) \[(HCl,C{{H}_{3}}COOH_{2}^{+})and(C{{H}_{3}}COOH,C{{l}^{-}})\]
C) \[(C{{H}_{3}}COOH_{2}^{+},HCl)and(C{{l}^{-}},C{{H}_{3}}COOH)\]
D) \[(HCl,C{{l}^{-}})and(C{{H}_{3}}COOH_{2}^{+},C{{H}_{3}}COOH)\]
Correct Answer: D
Solution :
[d] \[HCl\] 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\[HCl\]. \[\underset{aci{{d}_{1}}}{\mathop{HCl}}\,+C{{H}_{3}}C\underset{bas{{e}_{2}}}{\mathop{OOH}}\,\,\rightleftharpoons \,\,\underset{bas{{e}_{1}}}{\mathop{C{{l}^{-}}}}\,+\underset{aci{{d}_{2}}}{\mathop{C{{H}_{3}}COOH_{2}^{+}}}\,\]
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