Ask Questions, Get Answers

Want to ask us a question? Click here
Browse Questions
Home  >>  AIMS  >>  Class12  >>  Chemistry  >>  Liquid Solutions
0 votes

A solution containing 8.6g per $dm^3$ of urea (molar mass = 60g $mol^{–1}$) was found to be isotonic with a 5 percent solution of an organic non-volatile solute. Calculate the molar mass of the latter (solute).

Can you answer this question?

1 Answer

0 votes
According to the van’t Hoff theory, isotonic solutions have the same osmotic pressure at the same temperature and the same molar concentration
Let $M_2$ be the molar mass of the unknown solute
Molar concentration of urea solution =$\large\frac{50gdm^{-3}}{M_2}$
Since both the solutions are isotonic, hence, by definition, their molar concentrations are equal.
Thus $\large\frac{50g\;dm^{-3}}{M_2}=\frac{8.6g dm^{-3}}{60g mol^{-1}}$
Hence (A) is the correct answer.
answered Jun 11, 2014 by sreemathi.v

Related questions

Ask Question
student study plans
JEE MAIN, CBSE, NEET Mobile and Tablet App
The ultimate mobile app to help you crack your examinations
Get the Android App