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Calculate the freezing point of a soluti...

Calculate the freezing point of a solution containing `0.5 ` g KCl (Molar mass = `74.5 ` g/mol) dissolved in 100 g water, assuming KCl to be 92% ionized.
`K_(f)` of water = 1.86 K kg/mol.

Text Solution

Verified by Experts

`KCl to K^(+) + Cl^(-)`
n = 2
` i = 1 - alpha + nalpha`
` i = 1 + alpha`
`Delta T_(f) = iK_(f) m`
` = (1+ 0.92) x 1.86 x(0.5x 1000)/(74.5 x 100)`
` DeltaT_(f) = 0. 24`
` Delta T _(f) = 0.24`
` DeltaT_(f)=T_(f)^(0) - T_(f)`
` T'_(f) =- 0.24^(@) C`
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Calculate the freezing point of a solution containing 8.1 g of HBr in 100g of water, assuming the acid to be 90% ionized. [Given : Molar mass Br = 80 g/mol, K_(f) water = 1.86 K kg/mol].

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Calculate the freezing point of a solution when 3 g of CaCI_(2) (M=111 g mol^(-1)) was dissolved in 100g of water assuming that CaCI_(2) undergoes complete ionisation (K_(f) "for water"=1.86 K kg mol^(-1)) .

Knowledge Check

  • What is the freezing point of a solution containing 8.1g HBr in 100 g water assuming the acid to be 90% ionised ? ( K_f for water =1.86 K kg "mol"^(-1) ) :

    A
    `0.85^@K`
    B
    `-3.53^@K`
    C
    `0^@K`
    D
    `-0.35^@K`

  • What is the freezing point of a solution containing 8.1 g HBr in 100g water assuming the acid to be 90% ionised ( K_(f) for water = 1.86 "Kg mole"^(-1) )

    A
    `0.85^(@)C`
    B
    `-3.53^(@)C`
    C
    `0^(@)C`
    D
    `-0.35^(@)C`