The pH of 1, N aqueous solutions of HCl,CH_{3 | vedclass

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(C) The acidic strength of an acid depends on the stability of its conjugate base. Stronger acids have more stable conjugate bases.The dissociation re

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$CH_{3}COOH > HCOOH > HCl$

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(C) The acidic strength of an acid depends on the stability of its conjugate base. Stronger acids have more stable conjugate bases.The dissociation reactions are:$HCl \rightleftharpoons H^{+} + Cl^{-}$$HCOOH \rightleftharpoons H^{+} + HCOO^{-}$$CH_{3}COOH \rightleftharpoons H^{+} + CH_{3}COO^{-}$The stability of the conjugate bases follows the order: $Cl^{-} > HCOO^{-} > CH_{3}COO^{-}$.Therefore,the acidic strength follows the order: $HCl > HCOOH > CH_{3}COOH$.Since $pH = -\log[H^{+}]$,a higher concentration of $H^{+}$ ions results in a lower $pH$ value.Thus,the order of $pH$ for $1\, N$ aqueous solutions is: $CH_{3}COOH > HCOOH > HCl$.

The $pH$ of $1\, N$ aqueous solutions of $HCl$,$CH_{3}COOH$ and $HCOOH$ follows the order

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