Home
Class 11
CHEMISTRY
Calculate the freezing point of an aqueo...

Calculate the freezing point of an aqueous solution of a non-electrolyte having an osmotic pressure 2.0 atm at `"300 K. Kf = 1.86 k.kg.mol"^(-1.)" R = 0.0821 lit.atm.k"^(-1)" mol"^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
`[-0.151^(@)C]`
Promotional Banner

Topper's Solved these Questions

  • COLLIGATIVE PROPERTIES

    NCERT BANGLISH|Exercise Questions(D. Explain briefly on the following)|2 Videos

  • COLLIGATIVE PROPERTIES

    NCERT BANGLISH|Exercise Questions(C. Answer the following in one (or) two sentences)|10 Videos

  • CHEMICAL KINETICS - I

    NCERT BANGLISH|Exercise Questions(E. Explain briefly on the following)|6 Videos

  • DETECTION AND ESTIMATION OF ELEMENTS

    NCERT BANGLISH|Exercise Problems (Estimation of halogens)|5 Videos

Similar Questions

Explore conceptually related problems

Calculate the depression of freezing point of 0.1 (M) aqueous soln. of an weak acid for 20% dissociation given Kf = 1.86 k//hg mol^-1 .

Calculate the osmotic pressure of a 10%. Solution of glucose at 18^@C . R = 0.082 lit atm K^-1 mol^-1 .

An aqueous solution of 0.1 molal concentration of sucrose should have freezing point (k_f = 1.86 k mol^(-1) kg)

What is meant by the molarity of a solution ? What would be the osmotic pressure of a 0.02 molar aqueous solution of urea at 27^(@)C ? (R = 0.082 L.atm.K^(-1). Mol^(-1) )

An aqueous solution of urea has a freezing point of -0.515^@C . Predict the osmotic pressure (in atm) of the same solution at 37^@C . k_f = 1.86 k kg (mol)^(-1)

Calculate the freezing point of a solution of a non-volatile solute in a unknown solvent of molar mass 30 g/mol having mole fraction of solvent equal to 0.8. Given that latent heat of fusion of solid solvent = 2.7 kcal mol(-1)k^(-1) , freezing point of solvent = 27^@C and R = 2 cal mol^(-1) k^(-1)

6gm of urea and 9gm of glucose are dissolved in 1 Litre aqueous solution. Calculate the osmotic pressure of the solution at 300K.

An aqueous solution freezes at - 0. 186^@C then elevation in boiling point is (K_b = 0.512, K_f = 1.86)

A 0.2 molal aqueous solution of weak acid HX is 20% ionized. The freezing point of solution is ( K_f =1.86 )

Calculate elevation in boiling point for 2 molal aqueous solution of glucose. (Given : k_b(H_2O) = 0.5 K kg. mol^(-1))