What will be the $pH$ of a $0.1 \ M$ $NH_3$ solution?

$A$ weak monoacidic base dissociates to $1.5 \%$ in $0.001 \ M$ solution at $298 \ K$. Calculate the dissociation constant of the weak base.

What is the $pH$ of acetic acid at equilibrium, given that acetic acid concentration is $0.1 \ M$ and it is $30 \%$ dissociated at equilibrium? $(\log 3=0.47)$

At $298 \ K$,$0.1 \ M$ solution of acetic acid is $1.34 \ \%$ ionized. What is the dissociation constant of acetic acid?

At $25 \, ^\circ C$,the dissociation constant of a base $BOH$ is $1.0 \times 10^{-12}$. The concentration of hydroxyl ions in $0.01 \, M$ aqueous solution of the base would be:

An organic monobasic acid has a dissociation constant of $2.25 \times 10^{-6}$. What is the percent dissociation in its $0.01 \ M$ solution (in $\%$)?