Chapter 17: Q6DQ (page 733)
You drop an ice cube (made from pure water) into a saltwater solution at . Explain what happens and why.
The ice cube would melt, when it is dropped (made from pure water) into a saltwater solution at
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The normal boiling point of methanol is . A solution containing a non-volatile solute dissolved in methanol has a vapor pressure of 556.0 torr atrole="math" localid="1663821787160" . What is the mole fraction of methanol in this solution?
Use the data in the following table for three different aqueous solutions of CaCl2 to calculate the apparent value of the Van’t Hoff factor.
Molality
Freezing-Point
Depression
(8˚C)
0.0225 0.110
0.0910 0.440
0.278 1.330
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?
If a solution shows positive deviations from Raoult’s law, would you expect it to have a higher or lower boiling point than if it were ideal? Explain.
Consider Fig. 17.8. Suppose that instead of having a nonvolatile solute in the solvent in one beaker, the two beakers have different volatile liquids. That is, suppose one beaker contains liquid torr ) and the other beaker contains liquid B torr ). Explain what happens as time passes. How is this similar to the first case shown in the figure? How is it different?
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