Home
Class 12
CHEMISTRY
An aqueous solution containing 0.2g of c...

An aqueous solution containing 0.2g of compound A in 21.7g of water freezes at 272.814 K. If the value of `K_(f)` for water is 1.86K kg `mol"^(-1)`, calculate molecular weight of compound A.

Text Solution

AI Generated Solution

To find the molecular weight of compound A, we will follow these steps: ### Step 1: Calculate the depression in freezing point (ΔTf) The depression in freezing point can be calculated using the formula: \[ \Delta T_f = T_{f0} - T_f \] Where: ...
Promotional Banner

Topper's Solved these Questions

  • SOLUTIONS

    ICSE|Exercise Follow up Problems |58 Videos

  • SOLUTIONS

    ICSE|Exercise EXERCISE (PART-I Objective Questions)|26 Videos

  • SOLID STATE

    ICSE|Exercise ISC EXAMINATION QUESTIONS PART-I (Numerical Problems)|6 Videos

  • SOME IMPORTANT ORGANIC NAME REACTIONS

    ICSE|Exercise Questions |278 Videos

Similar Questions

Explore conceptually related problems

An aqueous solution of glucose containing 12 g in 100 g of water was found to boil at 100.34^(@)C . Calculate of K_(b) for water in K mol^(-1)Kg .

Assuming 100% polymerization of an organic compound in its aqueous solution, the number of moles of organic compound undergoing polymerization containing 9.4g of organic compound per 100g of the solvent is ……….Freezing point depression is 0.93K, K_(f) of water is 1.86K kg"mol"^(-1) and molecular weight of organic compound is 94u

When a solution w g of urea in 1 Kg of water is cooled to -0.372^(@)C,200g of ice is separated .If K_(f) for water is 1.86K Kgmol^(-1) ,w is

A solution containing 0.85 g of ZnCl_(2) in 125.0g of water freezes at -0.23^(@)C . The apparent degree of dissociation of the salt is: (k_(f) for water = 1.86 K kg mol^(-1) , atomic mass, Zn = 65.3 and Cl = 35.5)

A solution containing 62 g ethylene glycol in 250 g water is cooled to -10^(@)C . If K_(f) for water is 1.86 K mol^(-1) , the amount of water (in g) separated as ice is :

A solution containing 62g ethylene glycol in 276g water is cooled to -10^(@)C . If K_(f) for water is 1.86 kg mol^(-1) , the amount of water (in moles) separated as ice is ________.

What should be the freezing point of aqueous solution containing 17g of C_(2)H(5)OH is 1000g of water ( K_(f) for water = 1.86 deg kg mol^(-1) )?

A solution containing 0.5 g of KCI dissolved in 100 g of water and freezes at -0.24^(@)C . Calculate the degree of dissociation of the salt. ( K_(f) for water = 1.86^(@)C . [Atomic weight K = 39, Cl = 35.5]

An aqueous solution contains 5% by weight of urea and 10% by weight of glucose. What will be its freezing point ? ( K_(f) for water =1.86^(@)" mol"^(-) kg)

Calculate the temperature at which a solution containing 54g of glucose, (C_(6)H_(12)O_(6)) in 250g of water will freeze. ( K_(f) for water = 1.86 K mol^(-1) kg)