Home
Class 12
CHEMISTRY
A solution of 2.8g of Cdl(2) molar mass ...

A solution of `2.8g` of `Cdl_(2)` molar mass `=364g "mol"^(-1)`) in `20g` water has elevation in boiling point of `0.20^(0)`. What is molecular state of `Cdl_(2)` in aqueous solution ? `[K_(b)(H_(2)O)=0.52^(0) "mol"^(-1)kg]`

Text Solution

Verified by Experts

The correct Answer is:
To decide molecular state, determine value of `i` or its molar mass.
(A) If `i=1`, and molar mass `=` calculated molar mass then solute remains without change
(B) If `igt1`, and molar mass `gt` caluclated molar mass then solute is ionised.
(C) If `ilt1`, and molar mass `gt` calculated molar mass then solute is polymerised (dimer, trimer, etc. )
`DeltaT_(b)(1000K_(b)w_(i))/(m_(1)w_(2))(i)`
`i=(DeltaT_(b)m_(1)w_(2))/(1000K_(b)w_(1))=(0.20xx364xx20)/(1000xx0.52xx208)=1.0`
Thus, `Cdl_(2)` remains `Cdl_(2)` (without ionisation) in aqueous solution.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • SOLUTIONS

    RESONANCE|Exercise Advabced Level Problems (PART-1)|71 Videos
  • SOLUTION AND COLLIGATIVE PROPERTIES

    RESONANCE|Exercise PHYSICAL CHEMITRY (SOLUTION & COLLIGATIVE PROPERTIES)|52 Videos
  • STEREOISOMERISM

    RESONANCE|Exercise EXERCISE (PART III : PRACTICE TEST-2 (IIT-JEE (ADVANCED PATTERN))|22 Videos

Similar Questions

Explore conceptually related problems

Calculate elevation in boiling point for 2 molal aqueous solution of glucose. (Given K_b(H_(2)O) = 0.5 kg mol^(-1) )

A solution of glucose (Molar mass = 180 g "mol"^(-1) ) in water has a boiling point of 100.20^@C . Calculate the freezing point of the same solution. Molal constants for water K_f and K_b are 1.86 K kg "mol"^(-1) and 0.512 K kg "mol"^(-1) respectively.

Knowledge Check

  • Calculate elevation in boiling point for 2 molal aqueous solution of glucose - (Given : K_(b(H_(2)O)) =0.5 K kg mol^(-1)).

    A
    1
    B
    4
    C
    3
    D
    2
  • Calculate elevation in boiling point for 2 molal aqueous solution of glucose (Given: K_(b(H_2O) =0.5K kg mol^(-1)))

    A
    `1^@C`
    B
    `4^@C`
    C
    `3^@C`
    D
    `2^@C`
  • To observe an elevation of boiling point of 0.0^(@)C , the amount of th solte (Molar mass 100 g mol^(-1) ) to be added to 100 g of water (K_(b)=0.5 K mol^(-1)) is:

    A
    2.0 g
    B
    0.5 g
    C
    1.0 g
    D
    0.75 g
  • Similar Questions

    Explore conceptually related problems

    A solution of glucose (Molar mass ="180 g mol"^(-1) ) in water has a boiling of 100.20^(@)C . Calculate the freezing point of the same solution. Molal constants for water K_(f) and K_(b) are "1.86 K kg mol"^(-1) and 0.512 K kg "mol"^(-1) respectively.

    A aqueous solution containing 1.248 g of barium chloride (molar mass ="208.34 g mol"^(-1) ) in 100 g of water boids at 100.0832^(@)C . Calculate the degree of dissociation of BaCl_(2)(K_(b)" for water = 0.52 K kg mol"^(-1)) .

    A 2.0 molal solution of sodium chloride in water cuses an elevation in boiling point of water by 1.88 K. What is the vlue of Van't Hoff factor ? What does does it signigy ? ( K_(b) =0.52 K kg mol^(-1) ).

    If 0.5 g of a solute (molar mass 100 g mol^(-1) ) in 25 g of solvent elevates the boiling point by 1 K, the molar boiling point constant of the solvent is

    The elevation in boilng point of a solution of 13.44 g of CuCl_(2) 1 kg of water will be _____. (Molecular mass of CuCl_(2) = 134.4 and K_(b) =0.52 km^(-1))