The hydrogen ion concentration of a 0.006 M | vedclass

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

Question

(B) For a weak acid,the dissociation is given by: $C_6H_5COOH \rightleftharpoons C_6H_5COO^- + H^+$The dissociation constant $K_a$ is given by $K_a =

Vedclass · Accepted Answer

$6 	imes 10^{-4}$

Vedclass · Answer

(B) For a weak acid,the dissociation is given by: $C_6H_5COOH ightleftharpoons C_6H_5COO^- + H^+$The dissociation constant $K_a$ is given by $K_a = \frac{[H^+][C_6H_5COO^-]}{[C_6H_5COOH]} \approx C\alpha^2$.Given $C = 0.006 \ M$ and $K_a = 6 	imes 10^{-5}$.The degree of dissociation $\alpha = \sqrt{\frac{K_a}{C}} = \sqrt{\frac{6 	imes 10^{-5}}{0.006}} = \sqrt{10^{-2}} = 0.1$.The hydrogen ion concentration $[H^+] = C\alpha = 0.006 	imes 0.1 = 6 	imes 10^{-4} \ M$.

The hydrogen ion concentration of a $0.006 \ M$ benzoic acid solution is $(K_a = 6 \times 10^{-5})$

Similar Questions

Which of the following compounds has the maximum $K_{a}$ value?

For a weak base $BOH$ at $25\,^oC$,the dissociation constant $K_b$ is $1.0 \times 10^{-12}$. The concentration of hydroxyl ions in its $0.01\,M$ aqueous solution will be:

The $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.

The degree of dissociation of $0.1 \ M$ acid $HA$ is $5 \%$. The value of $K_c$ of $HA$ is

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?

Vedclass Test Series

Exam Paper Generator

Online Exam Module