Home
Class 11
CHEMISTRY
Depression in freezing point is 6K for N...

Depression in freezing point is 6K for NaCl solution. If `K_(f)` for water is `1.86 "K kg mol"^(-1)`, amount of NaCl dissolved in 1kg water is :

A

3.42

B

1.62

C

3.24

D

1.71

Text Solution

Verified by Experts

The correct Answer is:
B
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • SOLUTIONS (GENERAL AND COLLIGATIVE PROPERTIES)

    OP TANDON|Exercise Set-2 (Level-A)|22 Videos

  • SOLUTIONS (GENERAL AND COLLIGATIVE PROPERTIES)

    OP TANDON|Exercise Level-B|53 Videos

  • SOLUTIONS (GENERAL AND COLLIGATIVE PROPERTIES)

    OP TANDON|Exercise Practice Problem|66 Videos

  • PROBLEMS BASED UPON STRUCTURES AND REACTIONS OF ORGANIC COMPOUNDS

    OP TANDON|Exercise Some Solved Problems|21 Videos

  • STATES OF MATTER (GASES AND LIQUIDS)

    OP TANDON|Exercise Self Assess,ent|28 Videos

Similar Questions

Explore conceptually related problems

45 g of ethylene glycol (C_(2)H_(6)O_(2)) is mixed with 600 g water. Calculate (a) freezing point depression (b) freezing point of the solution (K_(f)" for water = 1.86 K kg mol"^(-1)," Atomic masses : C = 12, H = 1, O = 16 amu") .

What do you understand by the term that K_(f) for water is 1.86 K kg mol^(-1) ?

Knowledge Check

  • A solution of sucross (molar mass = 342 g "mol"^(-1) ) has been prepared by dissolving 68.4 g of sucrose in one kg of water. K_(f) for water is "1.86 K kg mol"^(-1) and vapour pressure of water at 298 K is 0.024 atm. If on dissolving the above amount of NaCl in 1 kg of water, the freezing point is found to be -0.344^(@)C , the percentage dissociation of NaCl in the solution is

    A
    `75%`
    B
    `80%`
    C
    `85%`
    D
    `90%`

  • A solution of sucross (molar mass = 342 g "mol"^(-1) ) has been prepared by dissolving 68.4 g of sucrose in one kg of water. K_(f) for water is "1.86 K kg mol"^(-1) and vapour pressure of water at 298 K is 0.024 atm. The freezing point of the solution will be

    A
    `-0.684^(@)C`
    B
    `-0.342^(@)C`
    C
    `-0.372^(@)C`
    D
    `-0.186^(@)C`

  • The freezing point of 0.05 molal solution of non- electrolyte in water is _____. (K_(f) = 1.86 K Kg mol ^(-1))

    A
    `271.3 K`
    B
    `0.93K`
    C
    `272.907 K`
    D
    `-0.0093K`

    • Similar Questions

    Explore conceptually related problems

    The creysopic constant (K_(f)) for water is 1.86 K mol^(-1)kg^(-1) . What does it signift ?

    What mass of NaCl (molar mass "58.5 g mol"^(-1) ) must be dissolved in 65 g of water to lower the freezing point by 7.5^(@)C ? The freezing point depression constant, K_(f) for water is "1.86 K kg mol"^(-1) . Assume that van't Hoff factor for NaCl is 1.87.

    What is osmotic pressure of the aq. Solution of the given solute at 27^(@)C if depression in freezing point is 0.93^(@)C ? Molal depression constant of water is 1.86K mol^(-1) kg ? Assume molality as molarity.

    A solution of urea in water has boiling point of 100.15^(@)C . Calculate the freezing point of the same solution if K_(f) and K_(b) for water are 1.87 K kg mol^(-1) and 0.52 K kg mol^(-1) , respectively.

    0.05 m urea solution will have freezing point ( K_(f) = 1.86 K kg "mol"^(-1) )

    Home
    Profile