CH_3COOH_{(aq)} + H_2O_{(l)} rightleftharpoon | vedclass

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Question

(A) According to the Bronsted-Lowry theory,the conjugate base of a weak acid is relatively strong,and the conjugate base of a strong acid is weak.$CH_

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$H_2O$

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(A) According to the Bronsted-Lowry theory,the conjugate base of a weak acid is relatively strong,and the conjugate base of a strong acid is weak.$CH_3COOH$ is a weak acid,so its conjugate base,$CH_3COO^{-}$,is a relatively strong base.$H_3O^{+}$ is a strong acid,so its conjugate base,$H_2O$,is a weak base.Therefore,$H_2O$ is the weaker base compared to $CH_3COO^{-}$.

$CH_3COOH_{(aq)} + H_2O_{(l)} \rightleftharpoons H_3O^{+}_{(aq)} + CH_3COO^{-}_{(aq)}$. Between $H_2O$ and $CH_3COO^{-}$,which one is the weaker base?

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