1. D’ CHEMISTRY OF SOLUTIONS

2. SOME DEFINITIONS A solution is a _______________ mixture of 2 or more substances in a single phase. One constituent is usually regarded as the SOLVENTand the others as SOLUTES.

6. 1.0 g of sugar dissolved in 100 g of water.

7. 50 mL of water mixed with 20 mL isopropyl alcohol

8. A tincture of Iodine is prepared with 0.10 g I2 and 10.0 mL of ethyl alcohol.

9. 40 % ethanol a rubbing alcohol.

10. Sugar is the smaller quantity that is dissolving. Therefore it the solute and water is the solvent.

11. Since both water and isopropyl alcohol are liquids, the one smaller volume, is the solute and water is the solvent.

12. Iodine is the solute and ethyl alcohol is the solvent.

14. 10 g NaCl and 100 g of water.

15. 50 mL ethanol and 10 mL H2O

16. 2.0 L oxygen and 8.0 L nitrogen.

17. 100 g silver and 40 g mercury.

19. Liquid

21. D’ UNIVERSAL SOLVENT WATER H2O

22. HOW SOLUTIONS ARE FORMED?

26. The intermolecular forces.How Does a Solution Form?

32. What ‘drives’ the dissolution process?

34. DISSOLUTION PROCESS IN SOLIDS… In solids this can be explained as the breakdown of the crystal lattice into individual ions, atoms or molecules and their transport into the solvent.

35. DISSOLUTION PROCESS IN LIQUIDS & GASES… For liquids and gases, the molecules must be compatible with those of the solvent for a solution to form.

36. dry Dissolution vs Reaction NiCl2(s) Ni(s) + HCl (aq) NiCl2(aq) + H2(g) Dissolution is a physical change—you can get back the original solute by evaporating the solvent. If you can’t, the substance didn’t dissolve, it reacted.

37. DEFINE SOLUBILITY?

38. What is Solubility? refers to the maximum amount of solute, expressed in grams, that can be dissolved in 100 g of water at a specific temperature & pressure.

40. LABORATORY ACTIVITY 2.7SOLUBILITY IN WATER INSOLUBLE INSOLUBLE SOLUBLE S/SOLUBLE INSOLUBLE INSOLUBLE SOLUBLE S/SOLUBLE INSOLUBLE INSOLUBLE SOLUBLE S/SOLUBLE INSOLUBLE INSOLUBLE SOLUBLE S/SOLUBLE SOLUBLE SOLUBLE INSOLUBLE S/SOLUBLE SOLUBLE SOLUBLE INSOLUBLE S/SOLUBLE INSOLUBLE INSOLUBLE SOLUBLE S/SOLUBLE INSOLUBLE INSOLUBLE SOLUBLE S/SOLUBLE

43. Solvent holds as much solute as is possible at that temperature.

44. Undissolved solid remains in flask.

45. Dissolved solute is in dynamic equilibrium with solid solute particles.Degree of Saturation

47. Less than the maximum amount of solute for that temperature is dissolved in the solvent.

49. Solvent holds more solute than is normally possible at that temperature.

53. Temperature Generally, the solubility of solid solutes in liquid solvents increases with increasing temperature.

54. LABORATORY ACTIVITY 2.8FACTORS SOLUBILITY TAKES TIME TO DISSOLVE EASILY DISSOLVED TAKES TIME TO DISSOLVE EASILY DISSOLVED TAKES TIME TO DISSOLVE EASILY DISSOLVED

57. It is more difficult it is for solvent molecules to surround bigger molecules.

58. If all of the above mentioned factors all excluded, a general rule can be found that larger particles are generally less soluble.

62. Factors Affecting Solubility The stronger the intermolecular attractions between solute and solvent, the more likely the solute will dissolve. Example: ethanol in water Ethanol = CH3CH2OH Intermolecular forces = H-bonds; dipole-dipole; dispersion Ions in water also have ion-dipole forces.

64. Factors Affecting Solubility Vitamin A is soluble in nonpolar compounds (like fats). Vitamin C is soluble in water.

65. Which vitamin is water soluble and which is fat soluble? HEALTHAPPLICATION

66. Gases in Solution In general, the solubility of gases in water increases with increasing mass. Why? Larger molecules have stronger dispersion forces.

67. Gases in Solution The solubility of liquids and solids does not change appreciably with pressure. But, the solubility of a gas in a liquid is directly proportional to its pressure. Increasing pressure above solution forces more gas to dissolve.

68. Henry’s Law States that:

69. Henry’s Law Sg = kPg Where: Sg is the solubility of the gas; k is the Henry’s law constant for that gas in that solvent; Pgis the partial pressure of the gas above the liquid.