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2. Vocab
Colligative
Properties
Molarity &
Dilutions
Solubility
Curves
Properties of
Solutions
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3. A solution that contains a relatively small amount of solute in a solvent

4. dilute solution

5. A substance that dissolves in water to give a solution that conducts electric current

6. electrolyte

7. A type of colloid in which a solid is dispersed throughout a liquid.

8. sol

9. The particles in a solvent are so large that they settle out unless the mixture is constantly stirred or agitated

10. suspension

11. The rapid escape of a gas from a liquid in which it is dissolved

12. effervescence

13. Colligative properties depend, NOT on the identity of the solute, but on the ___________.

14. Concentration of solute dissolved in the solution

15. Pure, unsweetened tea boils at 99. 5°C
Pure, unsweetened tea boils at 99.5°C. If 5 grams of sugar were dissolved in that tea and then the solution was brought to a boil, would the new boiling point be equal to, greater than, or less than 99. 5°C?

16. colligative property = boiling point elevation
greater than 99.5°C
colligative property =
boiling point elevation

17. In the winter, when trucks add salt to icy streets, which of the 4 colligative property is being displayed?

18. freezing point depression

19. What happens to the vapor pressure above a saltwater solution if an additional 25 grams of NaCl are dissolved into the solution?

20. colligative property = vapor pressure lowering
The vapor pressure
decreases
colligative property =
vapor pressure lowering

21. If a red blood cell is placed in a hypertonic solution, it will begin to shrivel. Which solution is MORE concentrated, the one inside of the cell or the one outside of the cell?

22. outside of the cell
according to osmosis, the water (solvent) moves from lower concentration to higher concentration so it leaves the less concentrated blood cell and enters the more concentrated outside solution, causing the cell to shrivel

23. Give the formulas for finding both molarity and dilutions.

24. Molarity (M) = moles solute
liters solution
Dilutions = MCVC = MDVD

25. The molarity of a solution in which 48
The molarity of a solution in which 48.5 grams of NaCl (molar mass = g/mol) are dissolved in 0.50 liters of solution.

26. 48.5 g 1 mol = mols
58.5 g
M = mols = M
0.5 L

27. If you dilute 49.8 mL of 1.35 M sodium chloride to a new volume of 300 mL, what is the concentration of this new solution?

28. (49.8 mL)(1.35 M) = (MD)(300 mL)
MD = M

29. The number of moles in 300 mL of 2.5 M lithium chloride.

30. 2.5 M = x mols
0.300 L
x = mols

31. A 3. 88 M solution contains 4. 1 moles of KNO3
A 3.88 M solution contains 4.1 moles of KNO3. What is the volume (in mL) of KNO3 solution?

32. 3.88 M = 4.1 mols
x L
x = L = mL

33. The number of grams of KNO3 soluble in 100 grams of water at 60⁰C.

34. 100 grams

35. The least soluble compound at 70⁰C.

36. Ce2(SO4)3

37. The type of solution found at 40⁰C, when 110 grams of NaNO3 is dissolved in 100 grams of water.

38. supersaturated

39. The amount of NH4Cl that can be dissolved in 300 grams of water at 20⁰C.

40. 111 grams

41. The amount of precipitate formed when a saturated solution of KNO3 is cooled from 60⁰C to 30⁰C.

42. 100°C = 100 g KNO3
30°C = 45 g KNO3 =
55 grams precipitate

43. Which would dissolve faster in coffee: granulated sugar or cubes of sugar?

44. = more surface area of each particle is exposed
granulated sugar
= more surface area of each particle is exposed

45. As the temperature of a gas increases, the solubility of the gas will ____.

46. decrease

47. As the pressure of a gas increases, its solubility will ____.

48. increase

49. As the lower the molar mass of a gas, the ____ the gas’s solubility.

50. lower

51. In addition to surface area/particle size, what are the 3 other factors that affect the solubility of a solid in a liquid?

52. the nature of the solute/solvent (like dissolves like), temperature,
and stirring/agitation