At $27^{\circ} C$,the degree of dissociation of a weak acid $(HA)$ in its $0.5 \ M$ aqueous solution is $1 \%$. Its $K_{a}$ value is approximately:
- A$5 \times 10^{-4}$
- B$5 \times 10^{-5}$
- C$5 \times 10^{-6}$
- D$5 \times 10^{-8}$
Explore More
Similar Questions
An acid solution of $pH=6$ is diluted $1000$ times,the $pH$ of the final solution becomes
DifficultMHT CET 2011
View SolutionSulphurous acid $(H_{2}SO_{3})$ has $Ka_{1} = 1.7 \times 10^{-2}$ and $Ka_{2} = 6.4 \times 10^{-8}$. The $pH$ of $0.588 \ M \ H_{2}SO_{3}$ is ..... . (Round off to the Nearest Integer)
DifficultJEE MAIN 2021
View SolutionWhat is the value of $pH$ of a $NaOH$ solution that dissociates $2 \%$ in its $0.01 \ M$ solution?
$A$ weak monobasic acid dissociates to $0.001 \%$ in its $0.01 \ M$ solution. What is its dissociation constant?
The degree of dissociation of $0.1 \, M \, HCN$ solution is $0.01 \%$. Its ionisation constant would be
Easy
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo