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Calculate the freezing point depression ...

Calculate the freezing point depression expected for `0.0711` m aqueous solution of `Na_(2)SO_(4)` . If this solution actually freezes at `-0.320 ^(@)C` , what would be the value of Van't Hoff factor ?
(`K_(f)` for water is `1.86 ^(@)C mol^(-1)`) .

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To solve the problem, we need to calculate the freezing point depression for a 0.0711 M aqueous solution of Na₂SO₄ and then determine the Van't Hoff factor (i) based on the actual freezing point of the solution. ### Step-by-Step Solution: 1. **Identify the given values:** - Molarity (M) of Na₂SO₄ = 0.0711 M - Actual freezing point of the solution = -0.320 °C - Freezing point of pure water = 0 °C ...
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Calculate the freezing point depression expected for 0.0711M aqueous solution of Na_(2) SO_(4) . If this solution actually freezes at -0.320^(@) C , what would be the value of van't Hoff factor ? (K_(f) = 1.86^(@) C mol^(-1))

What would be the value of Van't Hoff factor for a dilute solution of K_(2)SO_(4) in water ?

Knowledge Check

  • The depression in freezing point of 0.1M aqueous solution of HCL,CuSO_(4)andK_(2)SO_(4) are in the ratio.

    A
    `1:1:1.5`
    B
    `1:2:3`
    C
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  • An aqueous solution containing an ionic salt having molality equal to 0.19 freezes at -0.704^(@)C . The Van't Hoff factor of the ionic salt is ( K_(f) for water= 1.86 K m^(-1) )

    A
    3
    B
    2
    C
    4
    D
    5

  • The ratio of freezing point depression values of 0.01 M solutions of urea, common salt, and Na_(2)SO_(4) are

    A
    `1:1:1`
    B
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    C
    `1:2:3`
    D
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