1. Solutions Chap. 15

2. I.What is a solution?

3. A. Terms

4. I.What is a solution? A. Terms 1.Solute/solvent The solute is the substance that gets. The solvent does the.

5. I.What is a solution? A. Terms 1.Solute/solvent The solute is the substance that gets dissolved. The solvent does the dissolving. solute solvent

6. I.What is a solution? A. Terms 1.Solute/solvent 2.Soluble/insoluble A substance that is can be dissolved.

7. I.What is a solution? A. Terms 1.Solute/solvent 2.Soluble/insoluble A substance that is soluble can be dissolved.

8. I.What is a solution? A. Terms 1.Solute/solvent 2.Soluble/insoluble 3.Miscible/ immiscible Miscible substances are that will dissolve in each other.

9. I.What is a solution? A. Terms 1.Solute/solvent 2.Soluble/insoluble 3.Miscible/ immiscible Miscible substances are liquids that will dissolve in each other.

10. I.What is a solution? A. Terms 1.Solute/solvent 2.Soluble/insoluble 3.Miscible/ immiscible 4.Electrolytes/non- electrolytes Electrolytes are liquids that are capable of conducting electricity.

11. I.What is a solution? B. Types of solutions

12. I.What is a solution? B. Types of solutions 1.Gaseous solutions Air and other mixtures of gases

13. I.What is a solution? B. Types of solutions 1.Gaseous solutions 2.Liquid solutions In some cases water is the solvent. These are called ( ).

14. I.What is a solution? B. Types of solutions 1.Gaseous solutions 2.Liquid solutions In some cases water is the solvent. These are called (aqueous).

15. I.What is a solution? B. Types of solutions 1.Gaseous solutions 2.Liquid solutions 3.Solid solutions Combinations of solids. Some are homogenous mixtures of metals ( )

16. I.What is a solution? B. Types of solutions 1.Gaseous solutions 2.Liquid solutions 3.Solid solutions Combinations of solids. Some are homogenous mixtures of metals (alloys)

17. I.What is a solution? C. Making a solution

18. I.What is a solution? C. Making a solution 1.Solute/solvent particles are separated.

19. I.What is a solution? C. Making a solution 1.Solute/solvent particles are separated. 2.Solvent particles are attracted to solute particles. This is called solvation. With the solvent this is called hydration

20. I.What is a solution? C. Making a solution 1.Solute/solvent particles are separated. 2.Solvent particles are attracted to solute particles. This is called solvation. With the solvent water this is called hydration

21. I.What is a solution? C. Making a solution 1.Solute/solvent particles are separated. 2.Solvent particles are attracted to solute particles. 3.‘Like dissolves like’

22. Polar/Non-polar Substances PolarNon-polar WaterCarbon tetrachloride MethanolToluene (paint thinner) EthanolHexane, heptane, octane Acetic acidBenzene AcetoneOil Ionic compounds

23. I.What is a solution? 1.Water is polar because it has two oppositely ends D.Dissolving Ionic Compounds in H 2 O

24. I.What is a solution? 1.Water is polar because it has two oppositely charged ends D.Dissolving Ionic Compounds in H 2 O

25. I.What is a solution? 1.Water is polar because it has two oppositely charged ends 2.The end of water is attracted to the anion Anion = negative ion D.Dissolving Ionic Compounds in H 2 O

26. I.What is a solution? 1.Water is polar because it has two oppositely charged ends 2.The positive end of water is attracted to the anion Anion = negative ion D.Dissolving Ionic Compounds in H 2 O

27. I.What is a solution? 3.The combined of water molecules overcomes the attractive force of solute. D.Dissolving Ionic Compounds in H 2 O

28. I.What is a solution? 3.The combined pull of water molecules overcomes the attractive force of solute. D.Dissolving Ionic Compounds in H 2 O

29. I.What is a solution? 3.The combined pull of water molecules overcomes the attractive force of solute. 4.The ionic compound is dissociated into individual ions. Ex. NaCl (s) Na + + Cl - D.Dissolving Ionic Compounds in H 2 O

30. I.What is a solution? E.Dissolving Molecular Compounds in H 2 O.

31. I.What is a solution? 1.Water’s charged ends are attracted to charged portions of solute. E.Dissolving Molecular Compounds in H 2 O.

32. I.What is a solution? 1.Water’s charged ends are attracted to charged portions of solute. 2.The solute is surrounded by water molecules. E.Dissolving Molecular Compounds in H 2 O.

33. I.What is a solution? 1.Water’s charged ends are attracted to charged portions of solute. 2.The solute is surrounded by water molecules. 3.The solute remains intact. E.Dissolving Molecular Compounds in H 2 O.

34. I.What is a solution? F.Rate of Solvation To speed up solvation...

35. I.What is a solution? 1.Stir/shake To speed up solvation... F.Rate of Solvation

36. I.What is a solution? 1.Stir/shake 2.Break apart solute To speed up solvation... F.Rate of Solvation

37. I.What is a solution? 1.Stir/shake 2.Break apart solute 3.Heat the solvent To speed up solvation... F.Rate of Solvation

38. II. Is it soluble?

39. A. Not all ionic compounds dissolve in water.

40. II. Is it soluble? 1.Solubility Table A. Not all ionic compounds dissolve in water.

41. II. Is it soluble? 1.Solubility Table 2.Writing physical states (in equations) A. Not all ionic compounds dissolve in water. Insoluble = (s) for solid Soluble = ______________

42. II. Is it soluble? 1.Solubility Table 2.Writing physical states (in equations) A. Not all ionic compounds dissolve in water. Insoluble = (s) for solid Soluble = (aq) for aqueous

43. II. Is it soluble? 1.Solubility Table 2.Writing physical states (in equations) 3.Solubility Rules A. Not all ionic compounds dissolve in water.

44. Self Check – Ex. 1 Is copper (II) chloride soluble?

45. Self Check – Ex. 2 Is zinc carbonate soluble?

46. Self Check – Ex. 3 Is calcium hydroxide soluble?

47. II. Is it soluble? A. Not all ionic compounds dissolve in water. B. In reality, ionic compounds all dissolve in varying degrees. Some compounds are very soluble while others are slightly soluble

48. II. Is it soluble? A. Not all ionic compounds dissolve in water. B. In reality, ionic compounds all dissolve in varying degrees. 1.Solubility depends on ___________

49. Solubility Curve

50. II. Is it soluble? A. Not all ionic compounds dissolve in water. B. In reality, ionic compounds all dissolve in varying degrees. 1.Solubility depends on temperature 2.Solubility depends on physical state

51. II. Is it soluble? A. Not all ionic compounds dissolve in water. B. In reality, ionic compounds all dissolve in varying degrees. 1.Solubility depends on temperature 2.Solubility depends on physical state 3.Solubility of gas depends on pressure

52. Henry’s Law The solubility (S) of a gas in a liquid is directly proportional to the pressure (P) of the gas S1S1S1S1 P1P1P1P1 S2S2S2S2 P2P2P2P2 =

53. Self Check – Ex. 4 The solubility of O 2 in water is 1.2 g/L when the pressure 2.0 atm. What is the solubility when the pressure is 6.0 atm?

54. III. Heat of solution

55. A. Many reactions warm up when you mix substances Exothermic – heat given off

56. III. Heat of solution A. Many reactions warm up when you mix substances B. Some reactions get colder when you mix substances Endothermic – heat absorbed

57. IV. Concentration

58. A. Terms

59. IV. Concentration 1. Concentrated A. Terms A solution that has a lot of per solvent

60. A solution that has a lot of solute per solvent IV. Concentration 1. Concentrated A. Terms

61. IV. Concentration 1. Concentrated 2. Dilute A. Terms A solution that has a lot of.

62. IV. Concentration 1. Concentrated 2. Dilute A. Terms A solution that has a lot of solvent.

63. IV. Concentration 1. Concentrated 2. Dilute 3. Saturated A. Terms A solution with solute.

64. IV. Concentration 1. Concentrated 2. Dilute 3. Saturated A. Terms A solution with the maximum amount of solute.

65. A solution with. IV. Concentration 1. Concentrated 2. Dilute 3. Saturated 4. Supersaturated A. Terms

66. A solution with more solute than it can hold. IV. Concentration 1. Concentrated 2. Dilute 3. Saturated 4. Supersaturated A. Terms

67. Quantifying concentrations IV. Concentration A. Terms B. Measurements

68. IV. Concentration 1. Percentage A. Terms B. Measurements

69. IV. Concentration 1. Percentage A. Terms B. Measurements a.By mass mass solute mass solution x 100 Solution = solute & solvent Percent by mass =

70. Self Check – Ex. 5 What is the percent by mass when 40 g of salt is added to 200 g of water.

71. IV. Concentration 1. Percentage A. Terms B. Measurements a.By mass b.By volume x 100 Percent by volume =

72. IV. Concentration 1. Percentage A. Terms B. Measurements a.By mass b.By volume volume solute volume solution x 100 Percent by volume =

73. Self Check – Ex. 6 What is the percent by volume when 50 mL of methanol is added to 450 mL of water.

74. IV. Concentration 1. Percentage 2. Molarity A. Terms B. Measurements moles solute volume solution x 100 Molarity =

75. Self Check – Ex. 7 A solution is formed by adding 7.4 g of Ca(OH) 2 to 500 mL of solution. What is the molarity?

76. Self Check – Ex. 8 How many grams of potassium nitrate, KNO 3 are required to make 250 mL solution with a molarity of 0.40 M?

77. IV. Concentration 1. Percentage 2. Molarity 3. Molality A. Terms B. Measurements moles solute volume solution x 100 Molality =

78. Self Check – Ex. 9 What is the molality of a solution of 60 g of NaOH and 2000 g of water?

79. IV. Concentration 1. Percentage 2. Molarity 3. Molality 4. Mole fraction A. Terms B. Measurements moles solute moles solution Mole fraction =

80. IV. Concentration A. Terms B. Measurements C. Diluting solutions M 1 V 1 = M 2 V 2

81. V. Solution Stoichiometry

82. A. Concentrations are ratios, used like conversion factors

83. V. Solution Stoichiometry A. Concentrations are ratios, used like conversion factors B. Remember the rules

84. Stoich. Rules 1. Balance Equation

85. Stoich. Rules 1. Balance Equation 2. ID units of Unknown

86. Stoich. Rules 1. Balance Equation 2. ID units of Unknown 3. Write given

87. Stoich. Rules 1. Balance Equation 2. ID units of Unknown 3. Write given 4. Insert ‘conversion factors’

88. Self Check – Ex. 10 How many grams of AgCl are formed when a 35.5 mL sample 0.12 M AgNO 3 is added to excess NaCl solution?

89. Self Check – Ex. 11 How many milliliters of 0.25 M HCl is required to react with 4.0 g of NaOH?

90. VI. Colligative Properties Properties affected by the number of solute particles, but not the identify of those particles

91. VI. Colligative Properties A. Vapor Pressure: it’s lowered A measure of liquid water’s ability to become a vapor

92. VI. Colligative Properties A. Vapor Pressure: it’s lowered B. Boiling Point: it’s elevated

93. VI. Colligative Properties A. Vapor Pressure: it’s lowered B. Boiling Point: it’s elevated C. Freezing Point: it’s lowered

94. VI. Colligative Properties A. Vapor Pressure: it’s lowered B. Boiling Point: it’s elevated C. Freezing Point: it’s lowered D. Osmotic Pressure: it’s lowered Osmosis is movement of water through a semi- permeable membrane

95. VII. Heterogeneous Mixtures

96. A. Suspensions

97. VII. Heterogeneous Mixtures A. Suspensions B. Colloids

98. The end