1. General Chemistry Principles & Modern Applications 9 th Edition Petrucci/Harwood/Herring/Madura Chapter 13 Solutions and their Physical Properties Dr. Travis D. Fridgen Memorial University of Newfoundland © 2007 Pearson Education

2. Which one of the following would you expect to be most soluble in water? 1. 2. 4. 3. 5.

3. Which one of the following would you expect to be most soluble in water? 1. 2. 4. 3. 5.

4. 1. 2. 3. in Of the solvent/solute pairs given to the right, which of the solutes would you expect to be least soluble in the solvent.

5. 1. 2. 3. in Of the solvent/solute pairs given to the right, which of the solutes would you expect to be least soluble in the solvent.

6. In the process of refining crude oil, the fraction at the top of the column is the one with the highest molecular weight. 1. True 2. False

7. 1. True 2. False In the process of refining crude oil, the fraction at the top of the column is the one with the highest molecular weight.

8. If a diver surfaces too quickly from a dive, N 2 (g) dissolved in the divers blood will be released quickly resulting in a painful and dangerous condition called the bends. This is the same phenomenon as taking the top of of a pop bottle as depicted to the right. 1. True 2. False

9. If a diver surfaces too quickly from a dive, N 2 (g) dissolved in the divers blood will be released quickly resulting in a painful and dangerous condition called the bends. This is the same phenomenon as taking the top of of a pop bottle as depicted to the right. 1. True 2. False

10. The number of moles of CO 2 (g) above an aqueous solution of CO 2 decreased by two. The volume of gas above the solution is concurrently decreased by a factor of two. The concentration of CO 2 in solution 1. Decreases by a factor of 4. 2. Decreases by a factor of 2. 3. Remains the same. 4. Increases by a factor of 2. 5. Increases by a factor of 4.

11. The number of moles of CO 2 (g) above an aqueous solution of CO 2 decreased by two. The volume of gas above the solution is concurrently decreased by a factor of two. The concentration of CO 2 in solution 1. Decreases by a factor of 4. 2. Decreases by a factor of 2. 3. Remains the same. 4. Increases by a factor of 2. 5. Increases by a factor of 4.

12. AB AB AB AB To the right is a diagram of a closed system containing two salt water solutions. The solution labeled A is more concentrated than the one labeled B. Which of the diagrams below best represents the system at an infinite time after preparation? 1.2.3.

13. AB AB AB AB To the right is a diagram of a closed system containing two salt water solutions. The solution labeled A is more concentrated than the one labeled B. Which of the diagrams below best represents the system at an infinite time after preparation? 1.2.3.

14. Which of the following aqueous solutions will have the highest boiling point? 1. 3 molal glucose 2. 4 molal ethanol 3. 2.5 molal NaCl 4. 2.5 molal CaCl 2 5. Cannot tell without K b for water

15. Which of the following aqueous solutions will have the highest boiling point? 1. 3 molal glucose 2. 4 molal ethanol 3. 2.5 molal NaCl 4. 2.5 molal CaCl 2 5. Cannot tell without K b for water

16. A 2.0 molal aqueous solution of glucose (C 6 O 6 H 12 ) is found to boil at 101 o C. What would the boiling point of a 2.0 molal solution of sucrose be? glucose (C 6 O 6 H 12 ) sucrose (C 12 O 11 H 22 ) 1. 102 o C 2. 100.5 o C 3. 101 o C 4. Slightly higher than 100.5 o C 5. Cannot determine without K b

17. A 2.0 molal aqueous solution of glucose (C 6 O 6 H 12 ) is found to boil at 101 o C. What would the boiling point of a 2.0 molal solution of sucrose be? glucose (C 6 O 6 H 12 ) sucrose (C 12 O 11 H 22 ) 1. 102 o C 2. 100.5 o C 3. 101 o C 4. Slightly higher than 100.5 o C 5. Cannot determine without K b

18. The freezing point of a solution is lower than that of the pure solvent because 1.The addition of solute to the liquid increases the rate of escape of molecules from the solid phase to the liquid phase. At lower temperature these rates can again become equal. 2.The addition of solute to the liquid decreases the rate at which solvent molecules enter the solid phase. By lowering the temperature the rate of escape of molecules from the solid to liquid phase is also lowered and become equal.

19. The freezing point of a solution is lower than that of the pure solvent because 1.The addition of solute to the liquid increases the rate of escape of molecules from the solid phase to the liquid phase. At lower temperature these rates can again become equal. 2.The addition of solute to the liquid decreases the rate at which solvent molecules enter the solid phase. By lowering the temperature the rate of escape of molecules from the solid to liquid phase is also lowered and become equal.

20. As the water evaporates from this saturated solution 1.the vapor pressure above the solution increases. 2.the vapor pressure above the solution decreases. 3.the vapor pressure above the solution remains constant.

21. As the water evaporates from this saturated solution 1.the vapor pressure above the solution increases. 2.the vapor pressure above the solution decreases. 3.the vapor pressure above the solution remains constant.

22. 20 g C 3 H 6 O 3 10 g C 6 H 12 O 6 Two aqueous solutions of equal volume, one containing 20 g of lactic acid (C 3 H 6 O 3 ) and one containing 10 g of glucose (C 6 H 12 O 6 ) are separated by a semi permeable membrane (allowing only H 2 O to pass). The net flow of water through the membrane is? 1. Left 2. Right 3. There is no net flow. 4.Cannot tell without knowing the exact volume of the solutions.

23. 20 g C 3 H 6 O 3 10 g C 6 H 12 O 6 Two aqueous solutions of equal volume, one containing 20 g of lactic acid (C 3 H 6 O 3 ) and one containing 10 g of glucose (C 6 H 12 O 6 ) are separated by a semi permeable membrane (allowing only H 2 O to pass). The net flow of water through the membrane is? 1. Left 2. Right 3. There is no net flow. 4.Cannot tell without knowing the exact volume of the solutions.

24. The table to the right shows the experimental van’t Hoff factor, i, for three electrolytes at 1.0 m and the expected value at infinite dilution. Which of the following is the best explanation for the increase in the difference in i at for the salts shown? 1.The higher the charge on the ion, the smaller the radius so only a fraction of the oppositely charged ions are separated in solution. The rest are bound to one another. 2.The higher the charge on the ions, the greater attraction for ions of opposite charge. The greater the attraction the less they dissolve. 3.The higher the charge on the ion, the greater attraction for oppositely charged ions. The greater the attraction the more they act like a single particle rather than separate particles.

25. The table to the right shows the experimental van’t Hoff factor, i, for three electrolytes at 1.0 m and the expected value at infinite dilution. Which of the following is the best explanation for the increase in the difference in i at for the salts shown? 1.The higher the charge on the ion, the smaller the radius so only a fraction of the oppositely charged ions are separated in solution. The rest are bound to one another. 2.The higher the charge on the ions, the greater attraction for ions of opposite charge. The greater the attraction the less they dissolve. 3.The higher the charge on the ion, the greater attraction for oppositely charged ions. The greater the attraction the more they act like a single particle rather than separate particles.

26. The table to the right shows the experimental van’t Hoff factor, i, for three electrolytes at various dilutions. Which of the following is the best explanation for the increase in i at greater dilution. 2.At greater dilution, there are less interactions between oppositely charged ions so they act like completely separate entities. 3.At greater dilution, there are less forces holding the oppositely charged particles together so they act like completely separate entities. 1. These ionic compounds don’t fully dissolve unless under very dilute conditions.

27. The table to the right shows the experimental van’t Hoff factor, i, for three electrolytes at various dilutions. Which of the following is the best explanation for the increase in i at greater dilution. 2.At greater dilution, there are less interactions between oppositely charged ions so they act like completely separate entities. 3.At greater dilution, there are less forces holding the oppositely charged particles together so they act like completely separate entities. 1. These ionic compounds don’t fully dissolve unless under very dilute conditions.

28. The freezing point depression and boiling point depression constants for a number of liquids are given in the table below. Without using a calculator, which of the following solutions’ freezing point is decreased by the greatest amount when 1 mole of solute is dissolved in 1 kg of the solvent? 1. 2. 3. 4. 5.

29. 1. 2. 3. 4. 5. The freezing point depression and boiling point depression constants for a number of liquids are given in the table below. Without using a calculator, which of the following solutions’ freezing point is decreased by the greatest amount when 1 mole of solute is dissolved in 1 kg of the solvent?