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13 Dec 2019

Discuss why the freezing point of a solution is typically lower than the freezing point of pure solvent?

why molality is used as the unit of concentration in colligative property calculation?

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Bunny Greenfelder
Bunny GreenfelderLv2
17 Dec 2019

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Related questions

1. Explain/Discuss what a colligative property is. Provide at least 2 examples of colligative properties.

2. Provide at least one real-life application of freezing point depression.

3. Define the concentration term molality (m). Under what conditions are Molarity and molality approximately the same?

4. Discuss/Explain why the temperature of a substance remains relatively constant during the freezing of liquid to solid.

Discuss why the freesing point of a solution is typically lower than the freezing poiunt of pure solvent

Vapor-pressure lowering is a colligative property, as are freezing-point depression and boiling-point elevation. What is a colligative property? Why is the freezing point depressed for a solution as compared to the pure solvent? Why is the boiling point elevated for a solution as compared to the pure solvent? Explain how to calculate āˆ†T for a freezing-point depression problem or a boiling-point elevation problem. Of the solvents, which would have the largest freezing-point depression for a 0.50 molal solution? Which would have the smallest boiling-point elevation for a 0.50 molal solution? A common application of freezing-point depression and boiling-point elevation experiments is to provide a means to calculate the molar mass of a nonvolatile solute. What data are needed to calculate the molar mass of a nonvolatile solute? Explain how you would manipulate these data to calculate the molar mass of the nonvolatile solute.

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