$pH$ of $0.05 \ M$ aqueous solution of diethyl amine is $10$. The value of equilibrium constant $(K_b)$ is:

The degree of ionization of $0.10 \ M$ lactic acid is $4.0 \%$. The value of $K_a$ is:

What is the percent ionization $(\alpha)$ of a $0.01 \ M \ HA$ solution? $......\%$ $(K_a = 10^{-6})$

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.]

The $K_a$ of monobasic acid $A, B$ and $C$ are $10^{-6}, 10^{-8}$ and $10^{-10}$ respectively. The concentrations of $A, B$ and $C$ are respectively $0.1 \ M, 0.01 \ M$ and $0.001 \ M$. Which of the following is correct for $pOH$ of $A, B$ and $C$?

For a $0.1 \ M$ solution of a weak acid $HQ$,the $pH$ is $3$. The ionization constant $K_a$ of the acid is: