Lesson: Cryoscopy and Ebullioscopy Basic Chemistry • Sixth Edition • Chemistry • The Molecular Nature of Matter and Change • Eighth Edition • Introductory Chemistry Essentials • Sixth Edition

Chemistry

In this lesson, we will learn how to calculate the molar mass of a solute based on its effect on the melting or boiling point of the solvent.

Worksheet

Q1:

When 6.29 g of a nonvolatile solute is dissolved in 500 g of water, the freezing point of the resultant aqueous solution is 0.646∘C lower than that of pure water. The cryoscopic constant for water is 𝐾=1.856⋅/Kkgmol and the solute does not dissociate. Estimate the molar mass of the solute.

Q2:

A sample of sulfur weighing 0.201 g was dissolved in 17.8 g of carbon disulfide, CS2 (𝐾=2.43/)b∘Cm. If the boiling point of the carbon disulfide was elevated by 0.107∘C, what is the formula of a sulfur molecule in this solution?

Q3:

Lysozyme is an enzyme that cleaves cell walls. A 0.100 L sample of a solution of lysozyme containing 0.0750 g of the enzyme exhibits an osmotic pressure of 1.32×10 atm at 25∘C. What is the molar mass of lysozyme?
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