$A$ monoprotic acid in $1.00 \ M$ solution is $0.01\%$ ionized. The dissociation constant of this acid is
- A$1 \times 10^{-8}$
- B$1 \times 10^{-4}$
- C$1 \times 10^{-6}$
- D$10^{-5}$
Explore More
Similar Questions
$A$ weak monobasic acid is $3.0 \%$ dissociated in its $0.04 \ M$ solution. What is the dissociation constant of the acid?
The ionization constant of benzoic acid is $6.5 \times 10^{-5}$ at $298 \ K$ temperature. Calculate $pH$ of its $0.15 \ M$ solution. (in $.5$)
Difficult
View SolutionIf the $pH$ of $0.10 \ M$ monobasic acid at $298 \ K$ is $5.0$,the value of $p K_a$ at the same temperature is
The $pH$ of a $1.0 \ M$ monobasic acid $HX$ is $2$. The van't Hoff factor for the aqueous solution of the acid will be ........
Medium
View Solution$A$ weak monoacidic base is $1.2 \%$ dissociated in its $0.2 \ M$ solution. What is the value of dissociation constant?
Vedclass 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