The $pH$ of a $0.1 \ M$ solution of a monobasic acid is $2.34$. Calculate the degree of dissociation of the acid.
- A$3.1 \times 10^{-2}$
- B$4.57 \times 10^{-2}$
- C$2.18 \times 10^{-2}$
- D$2.5 \times 10^{-3}$
Explore More
Similar Questions
$A$ weak monoacidic base is $1.2 \%$ dissociated in its $0.2 \ M$ solution. What is the value of dissociation constant?
Derive the equation for the ionization constant $K_a$ of a weak acid $HX$.
Calculate the value of the dissociation constant $(K_b)$ of a weak monoacidic base if it dissociates to $2 \%$ in a $0.1 \ M$ solution.
The ionization constant of $0.1$ $M$ weak acid is $1.74 \times 10^{-5}$ at $298$ $K$ temperature. Calculate the $pH$ of its $0.1$ $M$ solution. (in $.88$)
Difficult
View Solution$0.01 \ M \ HA_{(aq)}$ is $2\%$ ionized; $[OH^{-}]$ of solution is
Medium
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