The dissociation constants of monobasic acids | vedclass

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(A) For a weak monobasic acid,the concentration of $H^+$ ions is given by $[H^+] = \sqrt{K_a 	imes C}$.Since the concentration $C = 0.1 \ M$ is const

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$A < B < C < D$

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(A) For a weak monobasic acid,the concentration of $H^+$ ions is given by $[H^+] = \sqrt{K_a imes C}$.Since the concentration $C = 0.1 \ M$ is constant for all acids,$[H^+] \propto \sqrt{K_a}$.As $K_a$ increases,$[H^+]$ increases,and consequently,the $pH$ $(pH = -\log[H^+])$ decreases.The given dissociation constants are $K_a(A) = 6 imes 10^{-4}$,$K_a(B) = 5 imes 10^{-5}$,$K_a(C) = 3.6 imes 10^{-6}$,and $K_a(D) = 7 imes 10^{-10}$.The order of $K_a$ values is $A > B > C > D$.Therefore,the order of $[H^+]$ is $A > B > C > D$.Since $pH$ is inversely proportional to $[H^+]$,the order of $pH$ values is $A < B < C < D$.

The dissociation constants of monobasic acids $A$,$B$,$C$ and $D$ are $6 \times 10^{-4}$,$5 \times 10^{-5}$,$3.6 \times 10^{-6}$ and $7 \times 10^{-10}$ respectively. The $pH$ values of their $0.1 \ M$ aqueous solutions are in the order

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