Question

0.5molal solution is prepared the freezing point depressed by 9k, find depression in freezing point constant (kb)?​

Answer 1

Answer:

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Answer 2

Answer:

The freezing point depression ∆T = KF·m where KF is the molal freezing point depression constant and m is the molality of the solute. Rearrangement gives: mol solute = (m) x (kg solvent) where kg of solvent is the mass of the solvent (lauric acid) in the mixture. This gives the moles of the solute.

Kf is the molal freezing point depression constant of the solvent (1.86 °C/m for water).

Explanation:

When a pure solvent freezes, its particles become more ordered as the intermolecular forces that operate between the molecules become permanent. ... As a result, more energy must be removed from the solution in order to freeze it, and the freezing point of the solution is lower than that of the pure solvent.

To calculate the freezing point depression constant, or Kf, you'll need the equation: delta Tf = Kfcm where cm is the molal concentration of the solution. Write down what you know. Since Kf is a constant, or a number that is always the same, it is often provided in a chart or table in chemistry books.

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