What is the $pH$ of a solution containing $7 \ g$ of $NH_4OH$ per $500 \ mL$? (Given: $K_b$ of $NH_4OH = 1.8 \times 10^{-5}$,Molar mass of $NH_4OH = 35 \ g \ mol^{-1}$)

The $pH$ of a monoacidic weak base is $10.9$. Calculate the percent dissociation in a $0.02 \ M$ solution. (in $\%$)

Calculate the $pH$ of $0.02 \ M$ monobasic acid having $2 \%$ dissociation.

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 $C$?

When a $1$ deci-normal solution of acetic acid is $1.3\%$ ionized,what is the value of the ionization constant $(K_a)$?

The amount of acetic acid in $1 \ L$ of solution having $\alpha = 1\%$ and $K_a = 1.8 \times 10^{-5}$ is ............. $g$.