An organic monobasic acid has a dissociation constant of $1.96 \times 10^{-8}$. What is its percentage dissociation in a $0.01 \text{ M}$ solution (in $\%$)?

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.

Calculate the dissociation constant of a weak monobasic acid if it is $0.05 \%$ dissociated in a $0.02 \ M$ solution.

The $pH$ of a monoacidic base is $10$. Calculate its percentage dissociation in $0.01 \ M$ solution at $298 \ K$. (in $\%$)

Which of the following has the highest $pH$?

The ionization constant of $0.1$ $M$ weak acid is $1.74 \times 10^{-5}$ at $298$ $K$ temperature. Calculate the $pH$ of its $0.1$ $M$ solution. (in $.88$)