If the $K_a$ for cyanoacetic acid is $3.5 \times 10^{-3}$,what is the degree of hydrolysis for a $0.05 \ M$ solution of sodium cyanoacetate?

The percentage degree of hydrolysis of a salt of weak acid $(HA)$ and weak base $(BOH)$ in its $0.1 \ M$ solution is found to be $10 \%$. If the molarity of the solution is $0.05 \ M$,the percentage hydrolysis of the salt should be ....... $\%$.

An aqueous solution of $CH_3COONa$ will be

At $25\,^oC$,the dissociation constant for acetic acid is $K_a = 1.8 \times 10^{-5}$ and for $NH_4OH$ is $K_b = 1.8 \times 10^{-5}$. Determine the nature of an aqueous solution of ammonium acetate.

It is found that at $25\,\text{°C}$,$0.1\,M$ solutions of four sodium salts $NaA$,$NaB$,$NaC$,and $NaD$ have the $pH$ values $7$,$9$,$10$,and $11$ respectively. Which one of the corresponding acids is the strongest?

The degree of hydrolysis in hydrolytic equilibrium $A^{-} + H_2O \rightleftharpoons HA + OH^{-}$ at salt concentration of $0.001 \ M$ is $(K_a = 1 \times 10^{-5})$