3. 7moles of Ba(NO3)2 is dissolved in 75kg of distilled water. What is the boiling point of this solution? Hint: Find molality first.<

Question

3. 7moles of Ba(NO3)2 is dissolved in 75kg of distilled water.
What is the boiling point of this solution? Hint: Find molality first.

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Maris 5 months 2021-08-13T09:32:56+00:00 1 Answers 0 views 0

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    2021-08-13T09:34:47+00:00

    Answer:

    100.14°C

    Explanation:

    The boling point elevation is a colligative property that describes the increasing in boiling point of a solution regard to the boiling point of the pure solvent. The equation is:

    ΔT = Kf*m*i

    Where ΔT is boiling point elevation

    Kf is boiling point elevation (0.51°C/m for water)

    m is molality of the solution (7moles Ba(NO3)2 / 75kg = 0.09333m

    i is Van’t Hoff factor = 3 for Ba(NO3)2 (Because its dissolution produce 3 ions = Ba²⁺ and 2 NO₃⁻

    Replacing:

    ΔT = 0.51°C/m*0.09333m*3

    ΔT = 0.14°C is the boiling point elevation

    As the boiling point of water is 100°C, the boiling point of the solution is:

    100°C + 0.14°C =

    100.14°C

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