1. TOPICS TO BE COVERED 1.WHAT ARE SOLUTIONS? 2.SOLVENTS AND SOLUTES 3.SOLUBILITY AND ITS FACTORS 4.CONCENTRATIONS 5.SOLUTION STOICHIOMETRY 6.COLLIGATIVE PROPERTIES

2. SOLUTIONS CHEMICALS + WATER

5. 1. WHAT ARE SOLUTIONS OBJECTIVE: WHAT ARE THEY?

6. SOLUTIONS IMPORTANCE OF STUDYING SOLUTIONS BECAUSE MANY REACTIONS TAKE PLACE IN SOLUTIONS BECAUSE MIXING REACTANTS IN SOLID FORM OFTEN DO NOT RESULT IN REACTIONS. REACTIONS REQUIRE COLLISIONS AT THE ATOMIC/MOLECULAR LEVEL, AND IN THE SOLID STATE, THIS DOES NOT OCCUR AT A SIGNIFICANT RATE.

7. 1. WHAT ARE SOLUTIONS? SOLUTIONS ARE… HOMOGENOUS MIXTURES HOMOGENOUS VS. HETEROGENEOUS MIXTURE VS. COMPOUND

8. 1. WHAT ARE SOLUTIONS? HOMOGENEOUS EVEN DISTRIBUTION HETEROGENEOUS UNEVEN DISTRIBUTION

9. 1. WHAT ARE SOLUTIONS? MIXTURES PHYSICALLY MIXED COMPOUND CHEMICALLY JOINED

10. SOLUTIONS

11. 1. WHAT ARE SOLUTIONS? MIXTURES CAN BE SEPARATED COMPOUND CANNOT BE SEPARATED

12. 1. WHAT ARE SOLUTIONS? MIXTURES CAN BE SEPARATED COMPOUND CANNOT BE SEPARATED

13. 1. WHAT ARE SOLUTIONS? SOLUTIONS ARE… HOMOGENOUS MIXTURES SOLUTIONS = TWO OR MORE THINGS EVENLY MIXED TOGETHER SOLUTIONS = THINGS MIXED INTO WATER

14. 1. WHAT ARE SOLUTIONS? HETEROGENEOUS MIXTURES: SUSPENSIONS & COLLOIDS Suspensions Separates and Settles Colloids do not Jello or Milk

15. 2. SOLUTES AND SOLVENTS OBJECTIVE: CLASSIFYING INGREDIENTS IN SOLUTIONS

16. 2. SOLVENT AND SOLUTE All solutions have at least TWO ingredients Ingredients can be classified as either a SOLVENT SOLUTE

17. 2. SOLVENT AND SOLUTE SOLVENT -PRESENT IN GREATER AMOUNT -DOES THE “DISSOLVING” WATER IS THE UNIVERSAL SOLVENT SOLUTE -PRESENT IN LESSER AMOUNT -IS THE ONE “DISSOLVED”

19. 2. SOLVENT AND SOLUTE Does not always involve liquids

22. 2. SOLVENT AND SOLUTE CAN THERE BE MORE THAN ONE SOLUTE IN A SOLUTION? CAN THERE BE MORE THAN ONE SOLVENT IN A SOLUTION? IF A SOLUTION IS A MIXTURE, DO THE SOLUTES AND THE SOLVENTS CHEMICALLY REACT OR PHYSICALLY MIX?

23. 3. SOLUBILITY OBJECTIVE: IF SOMETHING DOES OR DOES NOT DISSOLVE

24. 3. SOLUBILITY Why do some things dissolve while others do not? What does it mean for something to “dissolve?”

25. 3. SOLUBILITY Why do some things dissolve while others do not? “Like dissolves Like”

27. 3. SOLUBILITY “Like dissolves Like” Polar Solvent will dissolve… Non-Polar Solvent will dissolve

28. 3. SOLUBILITY Miscible vs. Immiscible Miscible = dissolves Immiscible = does NOT dissolve

29. 3. SOLUBILITY What does it mean for something to “dissolve?” It means to “ dissociate ”

30. Dissociation Separating dipoles

31. 3. SOLUBILITY Now we know why some things dissolve and others do not. We also know what it means for something to dissolve.

32. 3. SOLUBILITY How much of some thing can be dissolved? Solubility THE MAXIMUM AMOUNT OF A SOLUTE THAT CAN DISSOLVE AT A SPECIFIED TEMPERATURE AND PRESSURE

33. 3. SOLUBILITY Increasing/Decreasing Solubility 1.Temperature 2.Pressure

34. 3. SOLUBILITY WHAT IS THE TREND?

35. SO AS TEMPERATURE _______, SOLUBILITY ______

43. 3. SOLUBILITY Increasing Solubility with Temperature

44. Unsaturated Solutions more solute can be dissolved no heat necessary

45. Saturated Solutions no more solute can be dissolved no heat necessary

46. Super-Saturated Solutions more solute than normal heat necessary

47. Super-Saturated Solutions Rock Candy

49. GAS SOLUTE AS TEMPERATURE _____ THE SOLUBILITY OF GAS _______. SO TEMPERATURE AND SOLUBILITY OF A GAS HAVE A(N) ____. RECALLING HEAT AS KINETIC ENERGY, WE CAN EXPLAIN THIS BY…

50. SOLUBILITY OF SOLIDS SOLUBILITY OF GASES

51. 1.EXPLAIN WHY THERE MIGHT BE MORE MINERAL FORMATION SURROUNDING THERMAL SPRINGS THAN COOL MOUNTAIN SPRINGS. 2.WHY DOES WARM SODA FLATTEN FASTER THAN COLD SODA? 3.ON SAME SHEET, ANSWER QUESTIONS #67-72 ON PG 491. 4.TURN IN

52. 4. CONCENTRATIONS OBJECTIVE: MEASURING SOLUBILITY

53. 4. CONCENTRATION Concentration = how much solute in the solution 2 methods

54. 4. CONCENTRATION MolarityMOLALITY Symbol Formula Units Example

55. 4. CONCENTRATION MolarityMOLALITY Symbol M Formula M = mol L Units mol = mol of SOLUTE L = liters of solution Example 5 M, or 5 molar

56. 4. CONCENTRATION 1.23 mol of HCl in solution With volume of 5.00 L. What is molartiy?

57. 4. CONCENTRATION 3.45 M solution of AgCl is made with 2. 45 mol of AgCl. What is volume?

58. 4. CONCENTRATION 3.45 M solution of AgCl is made with 2.45 L. What is mol of AgCl?

59. 4. CONCENTRATION What are some signs that a chemical change has taken place?

60. 4. CONCENTRATION Precipitate = a solid that forms

61. 4. CONCENTRATION Solution Stoichiometry 2 types 1.Molarity, then stoichiometry 2.Stoichiometry, then Molarity

62. 4. CONCENTRATION Solution Stoichiometry Molarity  mol  mole ratio  mol  answer

63. 4. CONCENTRATION 0.125 L of 0.100 M HCl is added to Zn. What mass of ZnCl 2 is formed? Zn + 2HCl → ZnCl 2 + H 2

64. 4. CONCENTRATION Solution Stoichiometry grams  mol  mole ratio  mol  Molarity

65. 4. CONCENTRATION 11.0 g of Cu are needed. What volume of a 0.500 M solution of CuSO 4 is needed to result in 11.0 g of copper? 3CuSO 4 + 2Al  3Cu + Al 2 (SO 4 ) 3

66. BA(NO 3 ) 2(AQ) + NA 2 SO 4(AQ)  BA(SO 4 ) (S) + 2NANO 3(AQ) 25ML OF 0.5M BA(NO3)2 SOLUTION IS COMBINED WITH EXCESS NA2SO4. HOW MANY GRAMS OF PRECIPITATE ARE FORMED?

67. CACL 2(AQ) + 2NH 4 OH (AQ)  CA(OH) 2(S) + 2NH 4 CL (AQ) HOW MANY ML OF A 0.2M NH 4 OH SOLUTION WOULD BE REQUIRED TO PRECIPITATE ALL OF THE CA 2+ IONS IN 50ML OF A 0.15M CACL 2 SOLUTION?

68. SOLUBILITY OF GASES HENRY’S LAW AT A GIVEN TEMPERATURE, THE SOLUBILITY OF A GAS IN A LIQUID (S) IS DIRECTLY PROPORTIONAL TO THE PRESSURE OF THE GAS ABOVE THE LIQUID (P).

69. PB(NO 3 ) 2(AQ) + 2NACL (AQ)  PBCL 2(S) + 2NANO 3(AQ) HOW MANY GRAMS OF PRECIPITATE WOULD FORM IF 30ML OF A 0.25M PB(NO 3 ) 2 SOLUTION WAS ADDED TO 20ML OF A 0.50M NACL SOLUTION? HOW MANY MOLES OF THE EXCESS REACTANT ARE LEFT OVER AFTER THE REACTION? WHAT IS THE MOLARITY OF THE EXCESS REACTANT AFTER THE REACTION?

71. CAN A SOLUTION WITH UNDISSOLVED SOLUTE BE SUPERSATURATED?

72. SOLUBILITY OF GASES HENRY’S LAW IF THE SOLUBILITY OF A GAS IN WATER IS 0.77G/L AT 350KPA OF PRESSURE, WHAT IS ITS SOLUBILITY, IN UNITS OF GRAMS/LITER, AT 100KPA?

73. SOLUBILITY OF GASES HENRY’S LAW A GAS HAS A SOLUBILITY OF 3.6G/L AT A PRESSURE OF 100KPA. WHAT PRESSURE IS NEEDED TO PRODUCE AN AQUEOUS SOLUTION CONTAINING 9.5G/L OF THE SAME GAS? THE SOLUBILITY OF METHANE IN WATER AT 100KPA IS 0.026G/L, WHAT WILL THE SOLUBILITY BE AT A PRESSURE OF 180KPA?

74. SOLUBILITY OF LIQUIDS LIKE DISSOLVES LIKE MISCIBLE – DESCRIBES TWO OR MORE LIQUIDS THAT ARE ABLE TO DISSOLVE INTO EACH OTHER IMMISCIBLE – DESCRIBES TWO OR MORE LIQUIDS THAT DO NOT MIX WITH EACH OTHER

75. SOLUBILITY OF LIQUIDS LIKE DISSOLVES LIKE MISCIBLE NON-POLAR AND NON-POLAR = MISCIBLE POLAR + POLAR = MISCIBLE IMMISCIBLE NON-POLAR + POLAR = IMMISCIBLE

76. PERCENT SOLUTIONS SIMILAR TO PPM

77. PERCENT SOLUTIONS WHAT IS THE PERCENT BY VOLUME OF ETHANOL (C 2 H 6 O) WHEN 75ML OF ETHANOL IS DILUTED TO A VOLUME OF 250ML WITH WATER? A SOLUTION CONTAINS 2.7G OF CUSO4 IN 75ML OF SOLUTION. WHAT IS THE PERCENT BY MASS OF THE SOLUTION?

78. CONCENTRATION OF IONS CALCULATE THE NUMBER OF MOLES OF CL- IN 2.75 L OF 1.0X10-3M ZNCL2 HOW MANY GRAMS OF SULFATE ION ARE PRESENT IN 500ML OF A 2M AL2(SO4)3 SOLUTION?

79. 5. COLLIGATIVE PROPERTIES OBJECTIVE: CHANGING BOILING AND FREEZING POINTS

80. COLLIGATIVE PROPERTIES THE PHYSICAL PROPERTIES OF A SOLUTION ARE DIFFERENT FROM THOSE OF A PURE SOLVENT. SOME OF THESE DIFFERENCES ARE DUE TO THE PRESENCE OF SOLUTE PARTICLES IN THE SOLUTION.

81. COLLIGATIVE PROPERTIES COLLIGATIVE PROPERTIES – A PROPERTY OF A SOLUTION THAT DEPENDS ON THE CONCENTRATION OF THE SOLUTE PARTICLES. THE WORD COLLIGATIVE IS DERIVED FROM THE LATIN COLLIGATUS MEANING BOUND TOGETHER, SINCE THESE PROPERTIES ARE BOUND TOGETHER BY THE FACT THAT THEY ALL DEPEND ON THE NUMBER OF SOLUTE PARTICLES.

82. COLLIGATIVE PROPERTIES BOILING POINT ELEVATION – THE DIFFERENCE IN TEMPERATURE BETWEEN THE BOILING POINTS OF A SOLUTION AND OF THE PURE SOLVENT. FREEZING POINT DEPRESSION – IS THE DIFFERENCE IN TEMPERATURE BETWEEN THE FREEZING POINTS OF A SOLUTION AND OF THE PURE SOLVENT.

83. COLLIGATIVE PROPERTIES THE MAGNITUDE OF BP ELEVATION AND FP DEPRESSIONS IS PROPORTIONAL TO THE NUMBER OF SOLUTE PARTICLES DISSOLVED IN THE SOLVENT.

84. COLLIGATIVE PROPERTIES WOULD A DILUTE OR CONCENTRATED SODIUM FLUORIDE SOLUTION HAVE A HIGHER BOILING POINT? IF EQUAL NUMBER OF MOLES OF KI AND MGF 2 ARE DISSOLVED IN EQUAL AMOUNTS OF WATER, WHICH SOLUTION WOULD HAVE THE HIGHEST: BOILING POINT FREEZING POINT

85. MOLARITY MOLALITY VOLUME OF SOLUTE + VOLUME OF SOLVENT UNIT = M BOTH MOLARITY AND MOLALITY MEASURE CONCENTRATION MASS OF SOLVENT IN KILOGRAMS UNIT = M (ITALICIZED)

86. CALCULATING MOLALITY CALCULATE THE MOLALITY AND TOTAL MOLALITY (IF APPLICABLE) OF A SOLUTION PREPARED BY DISSOLIVING 10.0G OF NACL IN 600 G OF WATER. CALCULATE THE MOLALITY AND TOTAL MOLALITY (IF APPLICABLE) OF A SOLUTION PREPARED BY DISSOLIVING 10.0G C 12 H 22 O 11 OF IN 600 G OF WATER.

87. CALCULATING MOLALITY HOW MANY GRAMS OF POTASSIUM IODIDE MUST BE DISSOLVED IN 500G OF WATER TO PRODUCE A 0.060 MOLAL KI SOLUTION?

88. CALCULATING MOLALITY WHAT IS THE DIFFERENCE BETWEEN A 1M AND A 1M SOLUTION? A 4 G SUGAR CUBE (C 12 H 22 O 11 ) IS DISSOLVED IN A 350 ML TEACUP OF 80 °C WATER. WHAT IS THE MOLALITY OF THE SUGAR SOLUTION IF THE DENSITY OF WATER AT 80° = 0.975 G/ML

89. CALCULATING BP AND FP CHANGES BP Δ T B = K B * M FP Δ T F = K F * M

90. CALCULATING BP AND FP CHANGES K B, K F = THE MOLAL BP/FP CONSTANT, WHICH IS EQUAL TO THE CHANGE IN BP/FP TEMPERATURE FOR A 1 MOLAL SOLUTION.

91. CALCULATING BP AND FP CHANGES WHAT IS THE BOILING POINT OF A 1.5 MOL SOLUTION THAT IN 800G OF WATER?

92. CALCULATING BP AND FP CHANGES WHAT IS THE BOILING POINT OF A 1.2 MOL SOLUTION OF NACL IN 800G OF WATER?

93. CALCULATING BP AND FP CHANGES WHAT IS THE BP AND FP OF A 1.40 MOL SOLUTION OF NA 2 SO 4 IN 1750G OF WATER?

94. DETERMINING MOLAR MASS FROM Δ T B AND Δ T F M OLAR MASS = 7.5 G OF SOLUTE IS ADDED TO 22.60 G OF WATER. THE WATER BOILS AT 100.78 DEGREES C. WHAT IS THE MOLAR MASS OF THE SOLUTE?