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What is the freezing point of a solution...

What is the freezing point of a solution containing `8.1g Br `in `100g` water assuming the acid to be `90%`ionised(`K_(f)`for water =`1.8K "mole"^(-1))`

Text Solution

Verified by Experts

`HBr to H^(+) + Br^(-)`
`i = 1-alpha+mx`
n=2
`i=1+alpha`
`DeltaT_(f) = iK_(f)m`
`DeltaT_(f) = (1-alpha)1.86 xx (8.1)/(81) xx (1000)/(100)`
`rArr DeltaT_(f) = (1+0.9) xx 1.86 xx (8.1)/(81) xx 10`
`DeltaT_(f) = 3.53`
`T_(f)^(@) = 0^(@)C`
`DeltaT_(f) = T_(f)^(@) - T_(f)`
`T_(f) = -3.534^(@)C`
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Knowledge Check

  • 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`

  • 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 should be the freezing point of aqueous solution containing 17g of C_(2)H(5)OH is 1000g of water ( K_(f) for water = 1.86 deg kg mol^(-1) )?

    A
    `-0.69^(@)C`
    B
    `0.34^(@)C`
    C
    `0.0^(@)C`
    D
    `-0.34^(@)C`

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    The freezing point of a solution that contains 10 g urea in 100 g water is ( K_1 for H_2O = 1.86°C m ^(-1) )

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