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.
$\mathrm{HCl}+\mathrm{CH}_{3} \mathrm{COOH}=\mathrm{Cl}^{-}+\mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}$
The set that characterises the conjugate acidbase pairs is
  1. $\left(\mathrm{HCl}, \mathrm{CH}_{3} \mathrm{COOH}ight)$ and $\left(\mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}, \mathrm{Cl}^{-}ight)$
  2. $\left(\mathrm{HCl}, \mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}ight)$ and $\left(\mathrm{CH}_{3} \mathrm{COOH}, \mathrm{Cl}^{-}ight)$
  3. $\left(\mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}, \mathrm{HCl}ight)$ and $\left(\mathrm{Cl}^{-}, \mathrm{CH}_{3} \mathrm{COOH}ight)$
  4. $\quad\left(\mathrm{HCl}, \mathrm{Cl}^{-}ight)$ and $\left(\mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}, \mathrm{CH}_{3} \mathrm{COOH}ight)$

Solution

$\mathrm{HCl}$ is stronger acid than $\mathrm{CH}_{3} \mathrm{COOH}$ and $\mathrm{Cl}^{-}$ is a stronger base than $\mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}$
and is the conjugate base of $\mathrm{HCl}$.
\(\begin{array}{cc}
\mathrm{HCl} & + & \mathrm{CH}_3 \mathrm{COOH} & ightleftharpoons & \mathrm{Cl}^{-} & + & \mathrm{CH}_3 \mathrm{COOH}_2^{+} \\
\mathrm{acid}_1 & & \text { base }_2 & & \text {base }_1 & & \text { acid }_2
\end{array}\)

Asked in: JEE-TOPICTESTS-CHEMISTRY

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