The dissociation constant of a base $BOH$ at $25^{\circ} C$ is $1.0 \times 10^{-12}$. The concentration of $OH^{-}$ in a $0.01 \ M$ aqueous solution is .......
- A$1.0 \times 10^{-5} \ M$
- B$1.0 \times 10^{-7} \ M$
- C$2.0 \times 10^{-6} \ M$
- D$1.0 \times 10^{-14} \ M$
Explore More
Similar Questions
Which of the following formulae is used to find the $[OH^{-}]$ ion concentration of a weak monoacidic base?
The ionization constant of acetic acid is $1.74 \times 10^{-5}$. Calculate the degree of dissociation of acetic acid in its $0.05 \ M$ solution. Calculate the concentration of acetate ion in the solution and its $pH$.
Difficult
View SolutionThe dissociation constant of an acid $HA$ is $1 \times 10^{-5}$. The $pH$ of $0.1 \ M$ solution of the acid will be
Medium
View SolutionCalculate the value of the dissociation constant $(K_b)$ of a weak monoacidic base if it dissociates to $2 \%$ in a $0.1 \ M$ solution.
What will be the hydrogen ion concentration of $0.006 \ M$ benzoic acid? $(K_a = 6 \times 10^{-5})$
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