For a $10^{-2} \ M \ Ca(OH)_2$ solution with a degree of dissociation $\alpha = 10\%$,what are the values of $pOH$ and $pH$ respectively?

At what concentration of $0.2 \ M$ $CH_3COOH$ will its degree of dissociation become double (in $M$)? (Given: $K_a = 1.8 \times 10^{-5}$ for $CH_3COOH$)

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.]

Calculate the value of the dissociation constant $(K_b)$ of a weak monoacidic base if it dissociates to $2 \%$ in a $0.1 \ M$ solution.

Calculate the ionisation constant of $0.08 \ mol \ dm^{-3}$ of a monobasic acid having $pH = 2$.

Determine the degree of ionization and $pH$ of a $0.05 \, M$ ammonia solution. The ionization constant of ammonia $(K_{b})$ is $1.77 \times 10^{-5}$. Also,calculate the ionization constant of the conjugate acid of ammonia.