Question 1

A 75 mg sample of a natural product isolated from alfalfa hay was dissolved in water to make 100.0 mL of solution. The solution did not conduct electricity and had an osmotic pressure of 0.246 atm at 27°C. What is the molar mass of this compound?

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Question 2

Ethylene glycol is used commonly as an antifreeze in automobile radiators. Automobile temperatures in the U.S. are commonly measured in degrees Fahrenheit. What is the freezing point in °F of a 50:50 mixture of ethylene glycol and water by volume? (C₂H₆O₂, 62.07 g/mol, 1.1132 g/mL, K_f = 3.35°F/m).

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Question 3

A solution of 5.00 g of lithium chloride in 1.00 kg of water has a freezing point of -0.410°C. What is the actual van 't Hoff factor for this salt at this concentration? K_f(water) = 1.86°C/m

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Question 4

The arrow in the diagram below indicates the direction of solvent flow through a membrane in osmosis. Which solution, A or B, is more concentrated? Explain your reasoning.

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Question 5

The molal concentration of ions in seawater is 1.17 m, and the molar concentration is 1.15 M. What is the minimum pressure that must be applied to produce pure water from seawater through reverse osmosis at 25°C?

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Question 6

Describe how the data obtained by a measurement of osmotic pressure can be used to determine the molar mass of a compound.

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Question 7

Suppose 100.0 mL of a 2.50 mM NaCl solution were mixed with 100.0 mL of a 3.40 mM MgCl₂ solution at 25°C. Assuming the volumes are additive and using the ideal van 't Hoff factors, what would be the osmotic pressure of the resulting solution?

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Question 8

Ethylene glycol is used commonly as an antifreeze in automobile radiators. Automobile temperatures in the U.S. are commonly measured in degrees Fahrenheit. A 50:50 mixture of ethylene glycol and water by volume protects down to about -30°F. What is the boiling point in °F of this 50:50 mixture? (C₂H₆O₂, 62.07 g/mol, 1.1132 g/mL, K_b = 0.94°F/m).

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Question 9

Determine the molarity of an aspirin solution that produces an osmotic pressure of 0.0555 atm at 25°C (i = 1).

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Question 10

Describe how the molar mass of a compound can be determined from data obtained in two experiments: (1) measurements of the freezing point, and (2) measurements of the boiling point of a solution of the compound.

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Quiz 11: Solutions: Properties and Behavior