The dissociation constant of a monoacidic weak base $MOH$ is $1.8 \times 10^{-5}$. What is the concentration of $OH^{-}$ ions in its $0.1 \, M$ solution?
- A$1.8 \times 10^{-5}$
- B$1.34 \times 10^{-3}$
- C$5 \times 10^{-5}$
- D$4.0 \times 10^{-3}$
Explore More
Similar Questions
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:
For a $0.1 \ M$ solution of a weak acid $HQ$,the $pH$ is $3$. The ionization constant $K_a$ of the acid is:
Medium
View SolutionThe $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.
The $pH$ of a monoacidic base is $10$. Calculate its percentage dissociation in $0.01 \ M$ solution at $298 \ K$. (in $\%$)
The $pH$ of a $0.1 \ M$ solution of the acid $HQ$ is $3$. The value of the ionization constant,$K_a$ of the acid is:
MediumAIEEE 2012
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