1. Drill: Name & describe each of the 7 crystal structures

2. Drill: Draw LDDs for: BF 3 NH 3 BeCl 3 C 3 H 6 H 3 PO 4 H 2 CO 3

3. Drill: Draw LDDs for: C6H8C6H8

4. Drill: Draw LDD for: C 3 H 5 NO

5. CHM II Test Friday

6. CHM II HW Read: Chapter 14 Work Problems 25 & 29 on page 585

7. Solutions

8. Solution Homogeneous mixture made up of at least one solute dissolved in the solvent

9. Solute Substance being dissolved Portion in lesser molar amount

10. Solvent Substance doing the dissolving Portion in greatest molar amount

13. Colloid Slightly larger particles Light passes & particles stay suspended

14. Suspension Even larger particles Particles block or reflect light

15. Tyndall Effect Because light reflects off suspended particles, the light ray can be seen from the side

16. Size Comparison Solution < Colloid Colloid < Suspension

17. Soluble When one substance (solute) dissolves in another (solvent)

18. Solubility The amount of one substance (solute) dissolved in another (solvent)

19. Concentration The amount of solute dissolved into solution

20. Concentrated Solution A solution with a relatively large amount of solute dissolved

21. Dilute Solution A solution with a relatively small amount of solute dissolved

22. Saturated Solution A solution with the maximum amount of solute dissolved in the solution

23. Unsaturated Solution A solution with less than the maximum amount of solute dissolved in solution

24. Supersaturated Solution A solution with greater than the maximum amount of solute dissolved in solution

25. Solution Measures Concentration –Molarity –Molality –Mole Fraction

26. Percent Solution Mass of one portion per the total mass, all times 100 % % soln = m a /m total x 100 %

27. Drill: Define & give units for: –Molarity –Molality –Mole Fraction

28. Molarity Moles of solute per liter of solution M = moles solute /L soln

29. Molality Moles of solute per kilogram of solvent mo = moles solute /kg solvent

30. Mole Fraction Moles of one portion per total number of moles in the solution X = moles a /moles soln

31. Calculate the molarity of a 250 mL solution containing 5.0 g NaOH dissolved in water

32. Calculate the molality of 69 g of C 2 H 5 OH dissolved in 500.0 mL of water

33. Calculate the mole fraction of each portion when 92 g of C 2 H 5 OH dissolved in 144 mL of water

34. Drill: Calculate the mass of KI required to make 250 mL of 0.500 M KI.

35. Review Drill Review HW

36. Calculate the molality & mole fraction of a solution containing 46 g of C 2 H 5 OH dissolved in 1782 mL of water

37. Chm II Homework: Problems: 31 & 38 Page: 585 & 586

38. AP Chm HW: Problems: Page:

39. Colligative Properties Properties dependent only on the concentration of particles in solution

40. Examples Vapor pressure Boiling & Freezing points Osmotic pressure

42. Vapor Pressure VP solution = (VP solvent )(X solvent ) X = mole fraction VP = vapor pressure

43. Boiling & Freezing  T = i moK  T = change in BP or FP i = ionic activity K = BP or FP constant

44. Osmotic Pressure  = i MRT  = osmotic pressure i = ionic activity M = Molarity

45. Calculate the vapor pressure of a solution containing 150 g C 5 H 10 O 5 in 162 mL of water at 30 o C

46. Drill: Calculate the VP of a solution containing 36 % m/m glucose (C 6 H 12 O 6 ) in water at 29 o C: (VP water = 30.0 mm Hg )

47. Calculate BP & FP of 60.0 g of NaOH in 250 mL water K BP = 0.512 o C/mo K FP = -1.86 o C/mo

48. Calculate the osmotic pressure of a solution containing 12 g of NaOH dissolved in 250 mL solution at 27 o C

49. Chm II Homework: Problems: 47 & 87 Page: 585 - 587

50. AP Chm HW: Problems: 31, 35, & 39 Page: 298

51. Calculate the vapor pressure of a solution containing 120 g C 3 H 7 OH in 144 mL of water at its BP.

52. Drill: Calculate the mass of lead(II)nitrate required to make 250 mL of 0.40 M Pb(NO 3 ) 2

53. Test on Monday on Bonding, Lewis Dot Diagrams, & Solution Chemistry

54. Draw LDDs for: BH 3 NCl 3 CF 4 C 3 H 6 SO 3 SO 3 -2

55. Calculate the osmotic pressure of a solution containing 12 g of C 4 H 8 O 4 dissolved in 50.0 mL solution at 27 o C (VP = 26.7 mmHg)

56. Clausius-Claperon Eq H v = R ln (T 2 )(T 1 ) P 2 (T 2 – T 1 ) P 1

57. VP benzene Temp ( o C) 24.5 27 73.5 127 Calculate H v for benzene:

58. Calculate the osmotic pressure of a solution containing 29.9 g of CoBr 3 dissolved in 7500 mL solution at 27 o C

59. Calculate the vapor pressure of a solution containing 12.0 g C 3 H 8 O in 14.4 mL of water at its BP. VP solvent = 1.0 Atm

60. Calculate the molality of a solution that is 33.1 % by mass Pb(NO 3 ) 2 in water

61. Drill: Calculate the osmotic pressure of 0.88 g of CO 2 in 750 mL of soln at 27 o C

62. Test Tomorrow

63. 300 g C 3 H 6 NF was dissolved in 500 g C 6 H 12 O at 27 o C making a 0.800 g/mL solution. Calculate X, mo, M, , VP, BP, & FP.

64. 180 g C 3 H 8 O was dissolved in 180 mL H 2 O at 27 o C making a 1.5 g/mL solution. Calculate X, mo, M, , VP, BP, & FP.

65. A 1.2 g/cm 3 aqueous solution is 20.0 % by mass NaOH at 27 o C. Calculate: X, mo, M, , & MP

66. Calculate the molecular mass of a covalent compound dissolved in an aqueous solution to make it 25 % by mass when it boils at 102.048 o C

67. AP Homework: Read: Chapter 11 Power Point: 19

68. Chm II Homework: Read: Chapter 15 Power Point: 16