The solution of sodium carbonate has $pH$

$pK_a$ of acetic acid is $4.74$. The concentration of $CH_3COONa$ is $0.01 \ M$. The $pH$ of $CH_3COONa$ is

Calculate the $pH$ of a $1.0 \, M$ ammonium formate solution,given that $K_a = 1 \times 10^{-4}$ and $K_b = 1 \times 10^{-5}$.

$A$ $100 \ L$ solution of $KCN$ undergoes $3.7\%$ hydrolysis. If the dissociation constant of $HCN$ is $7.2 \times 10^{-10}$,find the value of $K_w$.

The salt that forms a neutral solution in water is

Identify the weak acid-weak base salt from the following.