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1. What is the name of the major component of a solution?

2. What are the units of molarity?

3. What are the units of molality?

4. What are the units of mole fraction?

5. What are the units of normality?

6. What is the normality of a 1.5 M solution of H2SO4?

7. What is the molarity of a solution prepared from 10.0 g NaCl with a final solution volume of 286 mL?

8. What is the molality of a solution prepared from 10.0 g NaCl and 255 g of water?

9. What is the mole fraction of water in a solution prepared from 10.0 g NaCl and 255 g of water?

10. What is the mass percent of NaCl in a solution prepared from 10.0 g NaCl and 255 g of water?

11. What happens to the mass percent of argon in a solution of 1 mole of argon dissolved in 2 moles of NO2 when the volume of the container is tripled?

12. When the half of the water in a 1.0 m solution of sucrose is boiled off, what happens to the concentration of sucrose?

13. When the half of the water in a 1.0 M solution of sucrose is boiled off, what happens to the concentration of sucrose?

14. What is the maximum mole fraction for a component of a solution?

15. Why is it essential that the denominator for the mass percent calculation must be the total mass of the solution?

16. Between which two of the following will a solution form?

17. Between which of the following phases can a solution not form?

18. Which of the following observations indicates that the mixture you possess is not a solution?

19. What happens to the solubility of carbon dioxide in water when the surface area of the solution-gas interface is doubled?

20. Why does a bottle of soda "fizz" when it is first opened?

21. What would happen to the solubility of a gas in water if the volume of the water were decreased but the volume of the gas remained constant?

22. Scuba divers who ascend too quickly experience a paralyzing disorder known as the bends. Given that the divers breathe a mixture of oxygen and nitrogen gas (compressed air), which of the following explanations is the most reasonable cause of the bends?

23. In most lakes, there exists a temperature gradient. The warmest water is near the surface and the coldest is at the bottom. However, certain situations can cause a lake to "turn over" placing the coldest layers on top. Such an event is extremely dangerous to the nearby inhabitants because it can cause suffocation. Which of the following best explains why a lake turning over can cause the suffocation of nearby inhabitants?

24. Which of the following does not increase its solubility in water with increasing temperature?

25. Which of the following will increase the solubility of BaSO4 in water?

26. When power plants release water that was boiled to turn steam engines, fish throughout the area die of asphyxiation. Which of the following best explain why that is so?

27. What intermolecular forces are present in pure PH3?

28. What intermolecular force is weaker in H 2S than in H2O?

29. Which of the following will form a solution together?

30. Which of the following will not form a solution together?

31. Which of the following is not a colligative property?

32. Which of the following will produce an aqueous solution with the lowest vapor pressure?

33. If the vapor pressure of water at 25 oC is 23 mmHg, which of the following vapor pressures could not exist for an aqueous solution at that temperature?

34. Frequently, the experimentally determined van't Hoff factor is less than the one calculated from the number of particles that should be released upon dissolution. However, the value of i is never greater than that the calculated value. Which of the following best explains that observation?

35. How can we rationalize a situation where the vapor pressure of a solution is greater than that of the pure solvent despite Raoult's law that predicts a lower vapor pressure?

36. If the vapor pressure of acetone (CH3COCH3) at 25 oC is 58 mmHg, what is the vapor pressure of a 1.0 m solution of sucrose in acetone?

37. What is the mole fraction of solute in a solution that has a vapor pressure of 26 mmHg when the pure solvent has a pressure of 28 mmHg?

38. Which of the following aqueous solutions has the lowest vapor pressure?

39. The normal freezing point of benzene is 5.5 oC. If a solution of 0.1 mole of sucrose in 1500 g of benzene freezes at 5.16 oC, what is the molal freezing point depression constant, Kf?

40. Why do we use CaCl2 to remove ice from our driveways instead of NaCl?

41. Which of the following is not true about freezing points?

42. What is the change in freezing point for a 1.0 m solution of glucose in camphor? The value of Kf for camphor is 40 oC kg / mol.

43. Which colligative property predicts the boiling point elevation phenomenon?

44. What is the boiling point of a 1.2 m aqueous solution of a nonelectrolyte? The Kb of water is 0.51 oC kg / mol.

45. Which of the following would explain a higher than expected boiling point elevation?

46. Which of the following best explains a lower than expected boiling point?

47. A careless experimenter placed a permeable membrane that allows the flow of both solute and solvent molecules through the membrane in the osmotic pressure measuring setup? Which of the following would be the result of his experiment?

48. What is the molar mass of a nonelectrolyte solute that causes an osmotic pressure of 15 torr at 25 oC when 0.1 g of the unknown are dissolved in water to form a total volume of 125 mL?

49. What is the osmotic pressure of a 0.01 M solution of NaCl at 305 K?

50. What happens to the osmotic pressure of a solution when a different solute is added?

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