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Will the depression in freezing point be...

Will the depression in freezing point be same or different if 0.1 mole of sugar or 0.1 mole of glucose is dissolved in one litre of water ?

Text Solution

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The depression in freezing point will be same in both the solutions because both are non-electrolytes and give same number of solute particles.
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Knowledge Check

  • Mole fraction of sugar, if 34.2 g of sugar is dissolved in 180 g of water is

    A
    `0.0099`
    B
    `0.099`
    C
    `0.99`
    D
    `9.90`

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

    A
    `0.186^(@)`
    B
    `0.372^(@)`
    C
    `1.86^(@)`
    D
    `3.72^(@)`

  • When 0.01 mole of sugar is dissolved in 100 g of a solvent the despersion is frezzing point is 0.40^(@)C . When 0.03 mole of glucose is dissolved in 50 g of the same solvent , the depression in freezing point will be __________.

    A
    `0.60 ^(@)C`
    B
    `0.80^(@)C`
    C
    `1.60^(@)C`
    D
    `2.40^(@)C`

    • Similar Questions

    Explore conceptually related problems

    0.1 mole of NaCI has lesser elevation in boiling point than 0.1 mole BaCI_(2) dissolved in one litre of water. Why?

    If solution sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point water (Delta T_(f)) , when 0.01 mole of solution sulphate is dissolved in 1 kg of water, is: (K'_(f) = 1.86 kg mol^(-1))

    The depression in freezing point for 1 m urea, 1 m glucose and 1 m NaCl are in the ratio

    The molal boiling point constant of water is 0.573^(@)C kg "mole"^(-1) . When 0.1 mole of glucose is dissolved in 1000g of water, the solution boils under atmospheric pressure at:

    The depressions in freezing point for 1 M urea, 1 M glucose and 1M NaCl are in the ration :

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