The K_a of a weak acid HA is 1.00 times 10^{- | vedclass

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

Question

(B) For a weak acid,the dissociation constant $K_a$ is related to the degree of dissociation $\alpha$ and concentration $C$ by the formula: $K_a = C\a

Vedclass · Accepted Answer

$1$

Vedclass · Answer

(B) For a weak acid,the dissociation constant $K_a$ is related to the degree of dissociation $\alpha$ and concentration $C$ by the formula: $K_a = C\alpha^2$ (assuming $\alpha Given $K_a = 1.00 	imes 10^{-5}$ and $C = 0.100 \ M$.$\alpha = \sqrt{\frac{K_a}{C}} = \sqrt{\frac{1.00 	imes 10^{-5}}{0.100}} = \sqrt{1.00 	imes 10^{-4}} = 1.00 	imes 10^{-2}$.Percentage dissociation = $\alpha 	imes 100 = (1.00 	imes 10^{-2}) 	imes 100 = 1\%$.

The $K_a$ of a weak acid $HA$ is $1.00 \times 10^{-5}$. If $0.100 \ mol$ of this acid is dissolved in $1 \ L$ of water,what is the percentage dissociation of the acid at equilibrium?

Similar Questions

Calculate the $pH$ of $0.02 \ M$ monobasic acid having $2 \%$ dissociation.

$0.2 \ M$ solution of formic acid is ionized $3.2 \%$. Its ionization constant is:

The dissociation constant of an acid $HA$ is $1 \times 10^{-5}$. The $pH$ of $0.1 \ M$ solution of the acid will be

For a $10^{-2} \ M \ Ca(OH)_2$ solution with a degree of dissociation $\alpha = 10\%$,what are the values of $pOH$ and $pH$ respectively?

The $pH$ of a $0.1 \ M$ solution of the acid $HA$ is $3$. The value of the ionization constant,$K_a$ of this acid is

Vedclass Test Series

Exam Paper Generator

Online Exam Module