1. Chemistry 16.3

2. Colligative Properties of Solutions
16.3
The wood frog is a remarkable creature because it can survive being frozen. Scientists believe that a substance in the cells of this frog acts as a natural antifreeze, which prevents the cells from freezing. You will discover how a solute can change the freezing point of a solution.

3. Vapor-Pressure Lowering
16.3
Vapor-Pressure Lowering
Vapor-Pressure Lowering
What are three colligative properties of solutions?

4. Vapor-Pressure Lowering
16.3
Vapor-Pressure Lowering
A property that depends only upon the number of solute particles, and not upon their identity, is called a colligative property.

5. Vapor-Pressure Lowering
16.3
Vapor-Pressure Lowering
Three important colligative properties of solutions are
vapor-pressure lowering
boiling-point elevation
freezing-point depression

6. Vapor-Pressure Lowering
16.3
Vapor-Pressure Lowering
In a pure solvent, equilibrium is established between the liquid and the vapor.
The vapor pressure of a solution of a nonvolatile solute is less than the vapor pressure of a pure solvent. a) In a pure solvent, equilibrium is established between the liquid and the vapor. b) In a solution, solute particles reduce the number of free solvent particles able to escape the liquid. Equilibrium is established at a lower vapor pressure. Interpreting Diagrams How is decreased vapor pressure represented in the diagram?

7. Vapor-Pressure Lowering
16.3
Vapor-Pressure Lowering
In a solution, solute particles reduce the number of free solvent particles able to escape the liquid. Equilibrium is established at a lower vapor pressure.
The vapor pressure of a solution of a nonvolatile solute is less than the vapor pressure of a pure solvent. a) In a pure solvent, equilibrium is established between the liquid and the vapor. b) In a solution, solute particles reduce the number of free solvent particles able to escape the liquid. Equilibrium is established at a lower vapor pressure. Interpreting Diagrams How is decreased vapor pressure represented in the diagram?

8. Vapor-Pressure Lowering
16.3
Vapor-Pressure Lowering
The decrease in a solution’s vapor pressure is proportional to the number of particles the solute makes in solution.

9. Vapor-Pressure Lowering
16.3
Vapor-Pressure Lowering
Three moles of glucose dissolved in water produce 3 mol of particles because glucose does not dissociate.
Particle concentrations differ for dissolved covalent and ionic compounds in water. a) Three moles of glucose dissolved in water produce 3 mol of particles because glucose does not dissociate. b) Three moles of sodium chloride dissolved in water produce 6 mol of particles because each formula unit of NaCl dissociates into two ions. c) Three moles of calcium chloride dissolved in water produce 9 mol of particles because each formula unit of CaCl2 dissociates into three ions.

10. Vapor-Pressure Lowering
16.3
Vapor-Pressure Lowering
Three moles of sodium chloride dissolved in water produce 6 mol of particles because each formula unit of NaCl dissociates into two ions.
Particle concentrations differ for dissolved covalent and ionic compounds in water. a) Three moles of glucose dissolved in water produce 3 mol of particles because glucose does not dissociate. b) Three moles of sodium chloride dissolved in water produce 6 mol of particles because each formula unit of NaCl dissociates into two ions. c) Three moles of calcium chloride dissolved in water produce 9 mol of particles because each formula unit of CaCl2 dissociates into three ions.

11. Vapor-Pressure Lowering
16.3
Vapor-Pressure Lowering
Three moles of calcium chloride dissolved in water produce 9 mol of particles because each formula unit of CaCl2 dissociates into three ions.
Particle concentrations differ for dissolved covalent and ionic compounds in water. a) Three moles of glucose dissolved in water produce 3 mol of particles because glucose does not dissociate. b) Three moles of sodium chloride dissolved in water produce 6 mol of particles because each formula unit of NaCl dissociates into two ions. c) Three moles of calcium chloride dissolved in water produce 9 mol of particles because each formula unit of CaCl2 dissociates into three ions.

12. Freezing-Point Depression
16.3
Freezing-Point Depression
Freezing-Point Depression
What factor determines the amount by which a solution’s vapor pressure, freezing point, and boiling point differ from those properties of the solvent?

13. Freezing-Point Depression
16.3
Freezing-Point Depression
The difference in temperature between the freezing point of a solution and the freezing point of the pure solvent is the freezing-point depression.

14. Freezing-Point Depression
16.3
Freezing-Point Depression
The magnitude of the freezing-point depression is proportional to the number of solute particles dissolved in the solvent and does not depend upon their identity.

15. Freezing-Point Depression
16.3
Freezing-Point Depression
The freezing-point depression of aqueous solutions makes walks and driveways safer when people sprinkle salt on icy surfaces to make ice melt. The melted ice forms a solution with a lower freezing point than that of pure water.
Surfaces can be free of ice even at temperatures below freezing if salt is applied. Inferring Why would calcium chloride (CaCl2) be a better salt for this purpose than sodium chloride (NaCl)?

16. Boiling-Point Elevation
16.3
Boiling-Point Elevation
Boiling-Point Elevation
The difference in temperature between the boiling point of a solution and the boiling point of the pure solvent is the boiling-point elevation.
The same antifreeze added to automobile engines to prevent freeze-ups in winter, protects the engine from boiling over in summer.

17. Boiling-Point Elevation
16.3
Boiling-Point Elevation
The magnitude of the boiling-point elevation is proportional to the number of solute particles dissolved in the solvent.
The boiling point of water increases by °C for every mole of particles that the solute forms when dissolved in 1000 g of water.

18. 16.3 Section Quiz.
16.3.

19. 16.3 Section Quiz.
1. Which of the following is NOT a colligative property of
vapor-pressure lowering
freezing-point depression
boiling-point elevation
solubility elevation

20. 16.3 Section Quiz.
2. Choose the correct word for the space: The magnitude of each colligative property of solutions is proportional to the __________ solute dissolved in the solution.
type of
number of particles of
molar volume of
particle size of the

21. 16.3 Section Quiz.
3. The decrease in vapor pressure when a solute is added to a liquid is due to
attractive forces between solvent particles.
repulsion of the solute particles by the solvent particles.
dissociation of the solvent particles.
attractive forces between solvent and solute particles.

22. 16.3 Section Quiz.
4. You have 500 mL of 1M solutions of NaCl, Na2SO4, Na3PO4, and Al2(SO4)3. Which solution will have the highest boiling point?
NaCl(aq)
Na2SO4(aq)
Na3PO4(aq)
Al2(SO4)3(aq)

23. END OF SHOW