Hydrolysis of Salts

The $\mathrm{pH}$ of an aqueous solution of $0.01 \mathrm{M} {\mathrm{CH}}_3{\mathrm{COONH}}_4$ at $25 °\mathrm{C}$ is:

$\left({\mathrm{K}}_{\mathrm{a}}\left({\mathrm{CH}}_3\mathrm{COOH}\right)={\mathrm{K}}_{\mathrm{b}}\left({\mathrm{NH}}_4\mathrm{OH}\right)=1.8\times {10}^{-5}\right)$

If a salt of a strong acid and a weak base hydrolyses appreciably, which of the following formulae is to be used to calculate the degree of hydrolysis ${}^{\text{'}}\mathrm{X}^{\text{'}}$?

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

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

The process of hydrolysis is

Calculate the $\mathrm{pH}$ of each of the following solutions:

$100 \mathrm{mL}$ of $0.1 \mathrm{M} {\mathrm{CH}}_3\mathrm{COOH}$ mixed with $50 \mathrm{mL}$ of $0.1 \mathrm{M} \mathrm{NaOH}$

$\left({\mathrm{K}}_{\mathrm{a}}\left({\mathrm{CH}}_3\mathrm{COOH}\right)=1.8\times {10}^{-5}, {\mathrm{K}}_{\mathrm{w}}=1\times {10}^{-14}\right)$

Calculate the $\mathrm{pH}$ of each of the following solution:

$100 \mathrm{mL} 0.1 \mathrm{M} {\mathrm{CH}}_3\mathrm{COOH}$ mixed with $100 \mathrm{mL}$ of $0.1 \mathrm{M} \mathrm{NaOH}$

Calculate the hydrolysis constant of the reaction

${\mathrm{HCO}}_2^{-}+{\mathrm{H}}_2\mathrm{O}\rightleftharpoons {\mathrm{HCO}}_2\mathrm{H}+{\mathrm{OH}}^{-}$

${\mathrm{K}}_{\mathrm{a}}\left(\mathrm{HCOOH}\right)=1.8\times {10}^{-4}$

(Report your answer in multiples of ${10}^{-11}$)

A $0.02 \mathrm{M}$ solution of ${\mathrm{CH}}_3\mathrm{COONa}$ in water at $25°\mathrm{C}$ is found to have an ${\mathrm{H}}^{+}$ concentration of $3\times {10}^{-9} \mathrm{g}$ ionic weight per litre. What is the hydrolysis constant of the salt? ${\mathrm{K}}_{\mathrm{w}}=1.01\times {10}^{-14}, {\mathrm{K}}_{\mathrm{a}}\left({\mathrm{CH}}_3\mathrm{COOH}\right)=1.75\times {10}^{-5}$

(Report your answer in multiple of ${10}^{-10}$ and upto two decimal points)

Calculate the hydrolysis constant of ${\mathrm{NH}}_4\mathrm{Cl}$: determine the degree of hydrolysis of this salt in $0.01 \mathrm{M}$ solution and the $\mathrm{pH}$ of the solution.

${\mathrm{K}}_{\mathrm{b}}\left({\mathrm{NH}}_4\mathrm{OH}\right)=1.8\times {10}^{-5}$

Calculate the degree of hydrolysis of ${\mathrm{CH}}_3\mathrm{COOK}$ in $0.1 \mathrm{M}$ and the $\mathrm{pH}$ of the solution.

${\mathrm{K}}_{\mathrm{a}}^{}\left({\mathrm{CH}}_3\mathrm{COOH}\right)=1.8\times {10}^{-5}$

Calculate the degree of hydrolysis of an $\mathrm{N}/10$ $\mathrm{KCN}$solution at $25°\mathrm{C}$. ${\mathrm{K}}_{\mathrm{a}}\left(\mathrm{HCN}\right)=7.2\times {10}^{-10}; {\mathrm{K}}_{\mathrm{w}}=1\times {10}^{-14}$.

The dissociation constant of $\mathrm{HCN}$is $4.8\times {10}^{-10}$. What is the concentration of ${\mathrm{OH}}^{-}$ and $\mathrm{HCN}$ in a solution prepared by dissolving $0.16 \mathrm{mole}$ of $\mathrm{NaCN}$ in $450 \mathrm{mL}$ of water at $25°\mathrm{C}?$