Which of the following will occur if a 0.1 , | vedclass

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(C) For a weak acid $HA \rightleftharpoons H^+ + A^-$,the degree of dissociation $\alpha$ is given by $\alpha = \sqrt{K_a / C}$.As the concentration $

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Percentage ionization will increase

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(C) For a weak acid $HA ightleftharpoons H^+ + A^-$,the degree of dissociation $\alpha$ is given by $\alpha = \sqrt{K_a / C}$.As the concentration $C$ decreases (dilution),the degree of dissociation $\alpha$ increases.Since $[H^+] = C 	imes \alpha = \sqrt{K_a 	imes C}$,as $C$ decreases,$[H^+]$ also decreases.However,the decrease in $[H^+]$ is not proportional to the decrease in $C$ because $\alpha$ increases.Since $[H^+]$ decreases,the $pH = -\log[H^+]$ will increase.Therefore,the percentage ionization increases upon dilution,while the $pH$ increases (not decreases).

Which of the following will occur if a $0.1 \, M$ solution of a weak acid is diluted to $0.01 \, M$ at constant temperature?

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