$20 \ g$ of a binary electrolyte (molar mass = $100 \ g \ mol^{-1}$) is dissolved in $500 \ g$ of water. The freezing point of the solution is $-0.74 \ ^oC$. Given $K_f = 1.86 \ K \ kg \ mol^{-1}$,the degree of dissociation of the electrolyte is ......... $\%$.
- A$50$
- B$75$
- C$100$
- D$0$
Explore More
Similar Questions
If $\alpha$ is the degree of dissociation of $Na_2SO_4$,the Van't Hoff factor $(i)$ used for calculating the molecular mass is
MediumAIEEE 2005
View SolutionThe degree of dissociation $(\alpha)$ of a weak electrolyte,$A_xB_y$ is related to van't Hoff factor $(i)$ by the expression
DifficultAIEEE 2011
View SolutionThe van't Hoff factor $i$ for a compound which undergoes dissociation in one solvent and association in other solvent is respectively
Easy
View SolutionIn a solution with molality $m$,if the solute exists as a trimer,what would be the depression in the freezing point of the solution?
Medium
View SolutionThe van't Hoff factor $(i)$ is .....
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