Calculate the degree of hydrolysis of a salt | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) For a salt of a weak acid and a weak base,the degree of hydrolysis $(h)$ is independent of the concentration of the salt solution.The formula for

Vedclass · Accepted Answer

$10^{-2}$

Vedclass · Answer

(A) For a salt of a weak acid and a weak base,the degree of hydrolysis $(h)$ is independent of the concentration of the salt solution.The formula for the degree of hydrolysis is given by: $h = \sqrt{\frac{K_w}{K_a 	imes K_b}}$Given values: $K_w = 10^{-14}$,$K_a = 10^{-5}$,$K_b = 10^{-5}$.Substituting the values: $h = \sqrt{\frac{10^{-14}}{10^{-5} 	imes 10^{-5}}} = \sqrt{\frac{10^{-14}}{10^{-10}}} = \sqrt{10^{-4}} = 10^{-2}$.

Calculate the degree of hydrolysis of a salt formed from $0.1 \ N$ $NH_4OH$ and $0.1 \ N$ $HCN$. Given $K_a = 10^{-5}$ and $K_b = 10^{-5}$.

Similar Questions

The $pH$ of ammonium phosphate solution,if $pK_a$ of phosphoric acid and $pK_b$ of ammonium hydroxide are $5.23$ and $4.75$ respectively,is ..... .

The aqueous solution of $FeCl_3$ is acidic due to

Calculate the $pH$ of a $0.5 \ M$ aqueous solution of $KCN$. Given that $pK_{b}$ for $CN^{-} = 4.70$. (in $.5$)

$A$ solution of $MgCl_2$ in water has $pH$:

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

Vedclass Test Series

Exam Paper Generator

Online Exam Module