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(A) For a weak acid $HA \rightleftharpoons H^{+} + A^{-}$,the dissociation constant $K_a$ is given by $K_a = \frac{[H^{+}][A^{-}]}{[HA]}$.Upon dilutio

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Strength of the acid

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(A) For a weak acid $HA \rightleftharpoons H^{+} + A^{-}$,the dissociation constant $K_a$ is given by $K_a = \frac{[H^{+}][A^{-}]}{[HA]}$.Upon dilution,the degree of dissociation $(\alpha)$ increases according to Ostwald's dilution law,$\alpha = \sqrt{\frac{K_a}{C}}$.As $\alpha$ increases,$[H^{+}]$ changes,and consequently,the $pH$ changes.However,the equilibrium constant $K_a$ is a characteristic property of the acid at a constant temperature and does not change upon dilution.

$A$ solution of a weak acid is diluted by adding an equal volume of water. Which of the following will not change?

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