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According to Bronsted-Lowry Acid-Base theory, stronger acids have weaker conjugate bases and vice-versa. $\ce{HCl}$, being a strong acid in water, it's conjugate base i.e $\ce{Cl-}$ is weak or it is more stable. Although it reacts with $\ce{H2O}$ but to a very less extent. Whereas in the case of $\ce{CH3COOH}$, it being a weak acid, it's conjugate base is a ...


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