The pH of a 0.1 M aqueous solution of a very | vedclass

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(A) Given:$pH = 3$Concentration $(C) = 0.1 \ M$For a weak acid $HA \rightleftharpoons H^{+} + A^{-}$,the concentration of $H^{+}$ ions is given by $[H

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(A) Given:$pH = 3$Concentration $(C) = 0.1 \ M$For a weak acid $HA ightleftharpoons H^{+} + A^{-}$,the concentration of $H^{+}$ ions is given by $[H^{+}] = C \alpha$,where $\alpha$ is the degree of dissociation.From $pH = 3$,we have $[H^{+}] = 10^{-pH} = 10^{-3} \ M$.Substituting the values in the equation $[H^{+}] = C \alpha$:$10^{-3} = 0.1 	imes \alpha$$\alpha = \frac{10^{-3}}{10^{-1}} = 10^{-2}$To express the degree of dissociation as a percentage:$\alpha \% = 10^{-2} 	imes 100 = 1 \%$.

The $pH$ of a $0.1 \ M$ aqueous solution of a very weak acid $(HA)$ is $3$. What is its degree of dissociation in percentage?

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