$A$ solution containing $0.1050 \ g$ of a substance in $15.84 \ g$ of ether has a boiling point $1 \ ^\circ C$ higher than that of pure ether. What is the molar mass of the substance? [Given: Molar elevation constant for ether per $100 \ g = 21.6$]
- A$144.5$
- B$143.18$
- C$140.28$
- D$146.66$
Explore More
Similar Questions
The boiling point of a $0.1 \ m$ aqueous solution of urea is $100.18 \ ^\circ C$ at $1 \ atm$. The molal elevation constant $(K_b)$ of water is:
Medium
View SolutionWhen $0.01 \ mol$ of nonvolatile solute is dissolved in a certain solvent,calculate the mass of the solvent in $kg$ if $\Delta T_{b} = 0.6 \ K$ and $K_{b}$ for the solvent $= 2 \ K \ kg \ mol^{-1}$. (in $kg$)
Calculate the molar mass of a non-volatile solute when $5 \ g$ of it is dissolved in $50 \ g$ of solvent,which boils at $119.6^{\circ} C$. $[K_{b} = 3.2 \ K \ kg \ mol^{-1}$,boiling point of pure solvent $= 118^{\circ} C]$.
DifficultMHT CET 2024
View SolutionWhich of the following aqueous solutions will exhibit the highest boiling point?
Easy
View SolutionWhich of the following equations correctly represents the molar mass of a solute by knowing the boiling point elevation?
Vedclass 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