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(i) Prove that depression in freezing p...

(i) Prove that depression in freezing point is a colligative property.
(ii) 45 g of ethylene glycol `(C_(2)H_(6)O_(2))` is mixed with 600g of water . Calculate the freezing point depression. (`K_(f)` for water = 1.86 k kg `mol^(-1)`)

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### Step-by-Step Solution #### Part (i): Proving that Depression in Freezing Point is a Colligative Property 1. **Definition of Colligative Properties**: - Colligative properties are properties that depend on the number of solute particles in a solution and not on the nature or identity of the solute. 2. **Understanding Freezing Point Depression**: ...
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45 g of ethylene glycol (C_(2)H_(6)O_(2)) is mixed with 650 g of water. The freezing point depression (in K) will be (K_(f)"for water "=1.86 "K kg mol"^(-1)) .

45 g of ethylene glycol C_(2)H_(6)O_(2) is mixed with 600 g of water. Calculate (a) the freezing point depression and (b) the freezing point of solution. Given K_(f)=1.86 K kg mol^(-1) .

Knowledge Check

  • 45 g of ethylene glycol (C_(2) H_(6)O_(2)) is mixed with 600 g of water. The freezing point of the solution is (K_(f) for water is 1.86 K kg mol^(-1) )

    A
    273.95 K
    B
    270.95 K
    C
    370 . 95 K
    D
    373.95 K

  • How much amount of KCl must be added to 1 kg of water so that the freezing point is depressed by 2 K? (K_f "for water" = 1.86 kg mol^(-1))

    A
    40 g
    B
    20 g
    C
    10 g
    D
    60 g

    • 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") .

    An antifreeze solution is prepared by dissolving 31 g of ethylene glycol (Molar mass = 62 "g mol"^(-1) ) in 600 g of water. Calculate the freezing point of the solution. ( K_(f) for water =1.86" K kg mol"^(-1) )

    Calculate the amount of KCl which must be added to 1kg of water so that the freezing point is depressed by 2K . ( K_(f) for water =1.86K kg "mol"^(-1) ).

    Calculate the amount of KCl which must be added to 1 kg of water so that the freezing point is depressed by 3 K. (K for water = 1.86 K "mol"^(-1) ).

    The freezing point of a solution containing 50 cm^(3) of ethylene glycol in 50g of water is found to 34^(@)C . Assuming ideal behaviour calculate the density of ethylene glycol. (K_(b) for water = 1.86 K kg mol^(-1))

    Calcualate the amount of NaCl which must be added to 100 g water so that the freezing point, depressed by 2 K . For water K_(f) = 1.86 K kg mol^(-1) .

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