1. Colligative Properties of Solutions
Chapter 12 (continued)
Colligative Properties of Solutions

2. Key Idea: Having solute particles present in solution (with a liquid solvent) ______
decreases the “escaping tendency” of solvent molecules
Liquid molecules are less likely to “leave” the solution to:
Turn into a gas (i.e., evaporate or boil)
Turn into a solid (i.e., freeze)
Travel across a semi-permeable membrane
“stabilizes” the liquid state of the solvent (over the gaseous or solid states)
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3. As a result, it becomes ________
Harder to escape to the gas phase
Vapor pressure “lowers”
VP of solution is lower than that of pure solvent
Harder to boil
Boiling point “elevates”
Bp of solution is higher than that of pure solvent
Harder to freeze
Freezing point “depresses”
Fp of solution is lower than that of pure solvent
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4. Okay, so how much harder does it become?
It depends on how many particles are dissolved in a given amount of solute:
It depends on the concentration of dissolved particles (“Colligative” properties)
Greater concentration means:
More VP lowering
More bp elevation
More fp depression
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5. Colligative Properties (of solutions)
Dictionary.com:
“(of the properties of a substance) depending on the number of molecules or atoms rather than on their nature.”
Clarification:
(regarding properties of a solution)
depending on the concentration of dissolved particles rather on what the particles are (i.e., doesn’t depend on their size, mass, number of atoms/per particle, etc.)
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6. http://www. chem. iastate
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7. Figure 11.10 The Presence of a Nonvolatile Solute Lowers the Vapor Pressure of the Solvent
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8. Figure Phase Diagrams for Pure Water (Red) and for an Aqueous Solution Containing a Nonvolatile Solute (Blues)
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9. Sugar Dissolved in Water to Make Candy Causes the Boiling Point to be Elevated
Adding Salt to Roads Prevents Ice Build-up by Lowering the Freezing Point of Water
The Addition of Antifreeze Lowers the Freezing Point of Water in a Car's Radiator
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10. Figure (a) Ice in Equilibrium with Liquid Water (b) Ice in Equilibrium with Liquid Water Containing a Dissolved Solute
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11. Table Molal Boiling-Point Elevation Constants (Kb) and Freezing-Point Depression Constants (Kf) for Several Solvents
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12. Table Expected and Observed Values of the van't Hoff Factor for 0.05 m Solutions of Several Electrolytes
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13. Figure 11.16 A Tube with a Bulb on the End that is Covered by a Semipermeable Membrane
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14. Figure 11.17 Osmosis can be Prevented by Applying Pressure to the Solution
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15. Figure 11.18 Osmotic Pressure
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16. Red Blood Cells in Three Environments
Isotonic (environment)
hypertonic (environment)
hypotonic (environment)
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17. Tro’s “thirsty water” idea (Why you would dehydrate if you drank seawater)
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18. Figure 11.19 Functioning of the Artificial Kidney
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19. Figure 11.20 Reverse Osmosis
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20. Figure 11.21 (b) Machinery in the desalination plant for Catalina Island
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21. Chapter 13, Unnumbered Figure 1, Page 593

22. Chapter 13, Figure 13.14

23. Chapter 13, Unnumbered Figure 2, Page 593

24. Chapter 13, Unnumbered Figure 1, Page 594

25. Chapter 13, Unnumbered Figure 2, Page 594

26. Chapter 13, Unnumbered Figure 3, Page 594

27. Chapter 13, Unnumbered Figure 4, Page 594

28. Chapter 13, Unnumbered Figure 1, Page 600

29. Chapter 13, Unnumbered Figure 2, Page 600

30. Chapter 13, Table 13.8

31. Chapter 13, Unnumbered Figure, Page 601

32. Chapter 13, Unnumbered Figure, Page 602

33. Chapter 13, Chemistry In Your Day Figure, Page 603

34. Chapter 13, Figure 13.16, An Osmosis Cell

35. Chapter 13, Table 13.9

36. Chapter 13, Figure 13.17, Ion Pairing

37. Chapter 13, Figure 13.18, Red Blood Cells and Osmosis