At 25° C, the dissociation constant of a weak monoprotic acid HAKa is numerically equal to the dissociation constant of its conjugate base A− (Kb) Which of the following statement(s) is are correct?

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At 25° C, the dissociation constant of a weak monoprotic acid $H A (K_{a})$ is numerically equal to the dissociation constant of its conjugate base $A^{-} (K_{b})$ Which of the following statement(s) is are correct?

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The pH of 0.1 M aqueous solution of the conjugate base $(A^{-})$ is 10.0.

The pH of 0.1 M aqueous solution of the acid, HA, is 4.0.

The pH of an aqueous solution containing $0.1 M - HA$ and $0.01$ $M - HCl$ is $2.0 .$

The dissociation constant of the acid, HA, is $10^{- 7} at 25^{\circ} C$

answer is A, B, C, D.

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Detailed Solution

(a) $K_{a} \times K_{b} = K_{w}$ (always)

If $K_{a} = K_{b} \Rightarrow K_{a} = 10^{- 7}$

(b) $pH = \frac{1}{2} [7 - \log 0.1] = 4.0$

(d) ${[H^{+}]}_{Total} = {[H^{+}]}_{HCl} = 0.01$

So, $pH = 2$

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