If two acids of equimolar concentration are taken,then which option is correct?
- A$\alpha_1^2 K_{a_1} = \alpha_2^2 K_{a_2}$
- B$\alpha_1 K_{a_1}^2 = \alpha_2 K_{a_2}^2$
- C$\alpha_1^2 K_{a_2} = \alpha_2^2 K_{a_1}$
- D$\alpha_1 K_{a_2}^2 = \alpha_2 K_{a_1}^2$
Explore More
Similar Questions
Calculate the molar concentration of a weak monobasic acid if the acid dissociation constant $K_a = 1.8 \times 10^{-5}$ and the degree of dissociation $\alpha = 0.01$.
DifficultMHT CET 2026
View SolutionCalculate the pH of a centimolar solution of a monoacidic weak base which is $10 \%$ dissociated in its aqueous solution.
Calculate the value of the dissociation constant $(K_a)$ of a weak acid,which dissociates to $0.01 \%$ in its $0.1 \ M$ solution.
The percent dissociation of a weak monobasic acid is $3 \%$ in its $0.02 \ M$ solution. What is the dissociation constant of the acid?
For a diprotic organic acid in aqueous solution,the ionization constants are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. For a $0.034 \ M$ solution of this acid,select the correct statement.
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