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Calculate the mole fraction of solute in...

Calculate the mole fraction of solute in a dilute aqueous solution from which ice begins to separate out at `-46^(@)C`. (`K_(f)` of `H_(2)O` =`1.86 K m^(-1)`)

Text Solution

Verified by Experts

`DeltaT_(f)=K_(f) xx m rArr m=(DeltaT_(f))/K_(f)=(0-(0-0.46))/1.86 = 0.46/1.86=0.247 m`
Use the relation,
`m=(n_(2)xx1000)/(n_(1)xxMw_(1))`
`:.n_(2)/n_(1)=chi_(2)=(m xx Mw_(1))/1000`
=`(0.247 xx 18)/1000`
`=0.004`
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Knowledge Check

  • Mole fraction of solute in 1 mole aqueous solution is

    A
    1.77
    B
    0.177
    C
    0.0177
    D
    0.0344

  • What is the molality of ethy alcohol ( mol. wt. = 46) in aqueous solution which freezes at - 10^(@) C ? ( K_(f) for water 1.86 K molality ^(-1) )

    A
    3.504
    B
    4.567
    C
    5.376
    D
    6.315

  • What would be the freezing point of aqueous solution containing 17 g of C_(2)H_(5)OH in 100 g of water (K_(f) H_(2)O = 1.86 K mol^(-1)kg) :

    A
    `-6.8^(@)C`
    B
    `-0.34^(@)C`
    C
    `0.0^(@)C`
    D
    `0.34^(@)C`

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