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The amount of urea to be dissolved in 50...

The amount of urea to be dissolved in 500mL of water (K=18.6 K `mol^-1` 100 g solvent) to produce a depression of `0.186^@C` in freezing point is:

A

0.3 g

B

3 g

C

6 g

D

9 g

Text Solution

Verified by Experts

The correct Answer is:
B
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15 gm of a substance dissolved in 450 gms of water produces a depression of -0.34^@ C in the freezing point . Calulation the Mol. Wt. of the solid ( K_f for water is 1.86 K kg mol ^(-1) )

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Knowledge Check

  • A solution containing 1 mole of ethylene glycol dissolved in 1000 g of water (K_t = 18.6 K molality^-1 ) will freez at:

    A
    `-5.2^@C`
    B
    `-0.52^@C`
    C
    `-18.6^@C`
    D
    `-1.86^@C`

  • A solution containing 1 mole of ethylene glycol dissolved in 1000 g of water (K_f = 1.86 K molality^-1 ) will freez at:

    A
    `-5.2^@C`
    B
    `-0.52^@C`
    C
    `-18.6^@C`
    D
    `-1.86^@C`

  • 20 g of a binary electrolyte (mol. Wt. = 100) are dissolved in 500 g of water. The freezing point of the solution is -0.74^@C , K = 1.86 k molality^-1. The degree of ionization of the electrolyte is:

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

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    Calculate the boiling points of a solution prepared by dissolving 15g NaCl to 250g of water. ( K_b of water = 0.512 K kg mol^(-1) , molar mass of NaCl = 58.5) (Hints: triangle T_b = iK_bm )

    20 g of a binary electrolyte (mol. Wt. = 100) are dissolved in 500 g of water. The freezing point of the solution is -0.74^@C , K = 1.86 k molality^-1. The degree of ionization of the electrolyte is:

    Molal depression of freezing point of water is 1.86^@C per 1000 g of water. 0.02 mole of urea dissolved in 100 g of water will produce a lowering of temperature of:

    Molal depression of freezing point of water is 1.86^@C per 1000 g of water. 0.02 mole of urea dissolved in 100 g of water will produce a lowering of temperature of:

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