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Cryoscopic constant of a liquid is:...

Cryoscopic constant of a liquid is:

A

decreases in freezing point when 1 gram of solute is dissolved per kg of the solvent

B

decreases in the dreezing point when 1 mole of solute is dissolved per kg of the solvent

C

the elevation for 1 molar solution

D

a factor used for calculation of elevation in boiling point

Text Solution

Verified by Experts

The correct Answer is:
B
`DeltaT_(f) = K_(f), m`
If `m = 1, DeltaT_(f) = K_(f)`
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Given below are two statements labelled as Assertion (A) and Reason (R) Assertion (A):Cryoscopic constant depends on nature of solvent. Reason(R):Cryoscopic constant is a universal constant. Select the most appropriate answer from the options given below:

A weak electrolyte XY is 5% dissociated in water. What is the freezing point of a 0.01 molal aqueous solution of XY ? The cryoscopic constant of water is 1.86 K/m.

Knowledge Check

  • Cryoscopic constant of a liquid depends on :

    A
    the latent heat of fusion of solvent
    B
    the freezing point of solvent
    C
    the concentration of solution
    D
    the melting point of solute

  • The molal cryoscopic constant for water is

    A
    `1.86 K "molality"^(-1)`
    B
    5.26 K `molality_(-1)`
    C
    `55.5 K "molality"^(-1)`
    D
    `0.52 K "molality"^(1)`

  • 0.1 molal solution of Hg(NO_(3))_(2) freezes at -.558^(@) C. The cryoscopic constant for water is 1.86 KKg mol^(-1) then what will be the percentage ionisation of salt ?

    A
    `33.33%`
    B
    `50%`
    C
    `75%`
    D
    `100%`

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    An aqueous solution freezes at 271.5 K. Determine its boiling point and vapour pressure at 298 K. The cryoscopic constant of water is 1.86^@ , its ebullioscopic constant is 0.516o and the water vapour pressure at 298 K is 3168 Pa.

    A solution is prepared by dissolveing 26.3g of CdSO_(4) in 1000g water. The depression in freezing point of solution was found to be 0.284K. Calculate the Van't Hoff factor. The cryoscopic constant of water is 1.86K kg solvent "mol"^(-1)-"solute" .

    The cryoscopic constant for acetic acid is 3.6 K kg/mol. A solution of 1g of a hydrocarbon in 100 g of acetic acid freeze at 16.14^(@)"C" instead of the usual 16.60^(@)"C" . The hydrocarbon contains 92.3% carbon. What is the molecular formula?

    Freezing point of benzene is 278.4K and heat of fusion of benzene is 10.042 KJ/mol. Acetic acid exists partly as dimer in benzene solution. The freezing point of 0.02mol fraction of acetic acid in benzene is 277.4K. The molal cryoscopic constant of benzene in K "molality"^(-1) is

    The cryoscopic constant value depends upon

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