1. Name & describe each of the 7 crystal structures

2. Solutions

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

4. Solute Substance being dissolved Portion in lesser molar amount

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

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

9. Suspension Even larger particles Particles block or reflect light

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

11. Size Comparison Solution < Colloid Colloid < Suspension

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

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

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

15. Concentration The amount of solute dissolved into solution

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

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

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

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

20. Solution Measures Concentration Molarity Molality Mole Fraction

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

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

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

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

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

26. Drill: Calculate: mass of NaCl required to make 1.5 L of 2.0 M NaCl:

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

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

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

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

31. Examples Vapor pressure Boiling & Freezing points Osmotic pressure

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

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

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

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

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

38. 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

39. Calculate the osmotic pressure of a solution containing 120 g of NaOH dissolved in 250 mL solution at 27 o C

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

41. Calculate the osmotic pressure of a solution containing 12 g of C 4 H 8 O 4 dissolved in 750 mL solution at 27 o C

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

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

44. Drill: Calculate BP & FP of 88 g of CO 2 in 750 mL water K BP = 0.512 o C/mo K FP = -1.86 o C/mo

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

46. 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.

47. 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.

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

49. 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.

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

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

52. 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