If a $0.01 \ M \ NaCN$ solution is $3.37 \%$ hydrolyzed,calculate the value of $K_h$.

When a salt of a weak acid and a weak base is dissolved in water at $25\,^{\circ}C$,the $pH$ of the resulting solution will always :-

The degree of hydrolysis of a salt of weak acid and weak base in its $0.1 \, M$ solution is found to be $50 \%$. If the molarity of the solution is $0.2 \, M$,the percentage hydrolysis of the salt should be $...... \%$.

The dissociation constants of $CH_3COOH$ and $HCN$ are $1.8 \times 10^{-5}$ and $7.2 \times 10^{-10}$ respectively. What is the relationship between the degree of hydrolysis of $KCN$ $(x_1)$ and $CH_3COOK$ $(x_2)$?

Calculate the hydrolysis constant $(K_h)$ for a salt containing $NO_2^-$. Given that the dissociation constant $(K_a)$ for $HNO_2$ is $4.5 \times 10^{-4}$ and the ionic product of water $(K_w)$ is $1.0 \times 10^{-14}$.

An aqueous solution of $CuSO_4$ will be: