Drill: Draw LDDs for:

1. Drill: Draw LDDs for: BF3 NH3 C3H6 C3H7NO

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

6. Colloid • Slightly larger particles • Light passes & particles stay suspended

7. Suspension • Even larger particles • Particles block or reflect light

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

9. Size Comparison • Solution < Colloid • Colloid < Suspension

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

11. Solubility • The max amount of one substance (solute) dissolved in another (solvent)

12. Concentration • The amount of solute dissolved into solution

13. ConcentratedSolution • A solution with a relatively large amount of solute dissolved

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

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

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

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

18. Drill: Draw LDDs for: C4H8 HNO3 C4H6O

19. Solution Chemistry

20. Solution Measures • Concentration: % soln • Molarity • Molality • Mole Fraction

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

22. Molarity • Moles of solute per liter of solution • M = molessolute/Lsoln

23. Molality • Moles of solute per kilogram of solvent • mo = molessolute/kgsolvent

24. Mole Fraction • Moles of one portion per total number of moles in the solution • X = molesa/molessoln

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

26. Calculate the molality of 69 g of C2H5OH dissolved in 500.0 mL of water

27. Calculate the mole fraction of each portion when 92 g of C2H5OH dissolved in 144 mL of water

28. Calculate the molality & mole fraction of a solution containing 46 g of C2H5OH dissolved in 1782 mL of water

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

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

31. Examples • Vapor pressure • Boiling & Freezing points • Osmotic pressure

33. Vapor Pressure • VPsolution = (VPsolvent)(Xsolvent) • X = mole fraction • VP = vapor pressure

34. Boiling & Freezing DT = imoK DT = change in BP or FP i = ionic activity K = BP or FP constant

35. Osmotic Pressure p = iMRT p = osmotic pressure i = ionic activity M = Molarity

36. Calculate the vapor pressure of a solution containing 150 g C5H10O5 in 162 mL of water at 30oC

37. Calculate BP & FP of 60.0 g of NaOH in 250 mL waterKBP = 0.512oC/moKFP = -1.86oC/mo

38. Calculate the osmotic pressure of a solution containing 12 g of NaOH dissolved in 250 mL solution at 27oC

39. Drill: • Calculate the VP of a solution containing 36 % m/m glucose (C6H12O6) in water at 29oC: • (VPwater = 30.0 mm Hg)

40. Drill: Draw LDDs for: BF3 NH3 C3H6 C3H7NO

41. Are there any questions on previous material?

42. Solutions

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

44. Solute • Substance being dissolved • Portion in lesser molar amount

45. Solvent • Substance doing the dissolving • Portion in greatest molar amount

46. Colloid • Slightly larger particles • Light passes & particles stay suspended

47. Suspension • Even larger particles • Particles block or reflect light

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

49. Size Comparison • Solution < Colloid • Colloid < Suspension

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