In the acid-base relation:
$H C l + {C H}_{3} C O O H ⇌ {C l}^{-} + {C H}_{3} C O O H_{2}^{+}$
the conjugate acid of acetic acid is:

{C l}^{-}

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H C l

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{C H}_{3} C O O H_{2}^{+}

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H_{3} O^{+}

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Solution

The correct option is A ${C H}_{3} C O O H_{2}^{+}$
In the given equation,
$H C l + C H_{3} C O O H ⇌ {C l}^{-} + C H_{3} C O O H_{2} +$
$H C l$ donates proton to $C H_{3} C O O H$ to give $C H_{3} C O O H_{2} + .$
Since $H C l$ donates proton, $H^{+}$ , it is acid and its conjugate base will be $C l^{-} .$
And $C H_{3} C O O H_{2} +$ accepts proton, $H^{+}$ , It is base and its conjugate acid will be $C H_{3} C O O H_{2}^{+}$ .

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H C l + C H_{3} C O O H \to C l^{-} + C H_{3} C O O H_{2}^{+}

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