$A$ weak monoacidic base is $1.2 \%$ dissociated in its $0.2 \ M$ solution. What is the value of dissociation constant?

In its $0.2 \, M$ solution,an acid ionises to an extent of $60 \%$. Its hydrogen ion concentration is.....$M$

Calculate the $pH$ of a $0.08 \ M$ solution of hypochlorous acid,$HOCl$. The ionization constant of the acid is $2.5 \times 10^{-5}$. Determine the percent dissociation of $HOCl$.

The dissociation constant of a base $BOH$ at $25^{\circ} C$ is $1.0 \times 10^{-12}$. The concentration of $OH^{-}$ in a $0.01 \ M$ aqueous solution is .......

If $1 \ mM$ solution of ethylamine produces $pH = 9$,then the ionization constant $(K_b)$ of ethylamine is $10^{-x}$. The value of $x$ is . . . . . . (nearest integer). [The degree of ionization of ethylamine can be neglected with respect to unity.]

$A$ centimolar solution of a weak acid is $1.3 \%$ dissociated at $298 \ K$. What is its dissociation constant?