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A 0.561 m solution of an unknown elecro...

A 0.561 m solution of an unknown elecrolyte depresses the freezing point of water by `2.93^(@)C`. What is van't Hoff factor for the electrooyte ? The freezing point depression constant `(K_(f))` for water is 1.86 kg `mol^(-1)`.

Text Solution

Verified by Experts

The correct Answer is:
2.81
`i=(DeltaT_(f))/(K_(f)xxm)`
`DeltaT_(f)=2.93^(@)C, 2.93 K, m = 0.561 " mol kg"^(-1)`
`K_(f)=1.86^(@)C" kg mol"^(-1)=1.86" K kg mol"^(-1)`
`i=((2.93K))/((1.86" K kg mol"^(-1))xx(0.561" mol kg"^(-1)))=2.81`
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Knowledge Check

  • 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

  • How much amount of NaCl solution be added to 600 g of water (rho=1.00 g/mL) to decrease the freezing point of water to -0.2^(@)C ? (The freezing point depression constant for water =2 K kg mol^(-1) )

    A
    2.14 g
    B
    0.88 g
    C
    1.96 g
    D
    1.76 g

  • The freezing point of 0.2 molal K_(2)SO_(4) is -1.1^(@)C . Calculate van't Hoff factor and percentage degree of dissociation of K_(2)SO_(4).K_(f) for water is 1.86^(@)

    A
    `97.5`
    B
    `90.75`
    C
    `105.5`
    D
    `85.75`

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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)) .

    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) ).

    The freezing point of an aqueous solutions is 272 .93 K . Calculate the molality of the solution if molal depression constant for water is 1.86 Kg mol^(-1)

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

    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.

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