1. Conceptual Physical Science 5th Edition Chapter 16: MIXTURES
© 2012 Pearson Education, Inc.

2. This lecture will help you understand:
Most Materials are Mixtures
The Chemist’s Classification of Matter
Solutions
Solubility
Soaps and Detergents
Softening Hard Water
Purifying the Water We Drink
Wastewater Treatment

3. Most Materials are Mixtures
• Pure substance
A material consisting of only one type of element or compound.

4. Most Materials are Mixtures
• Pure substance
A material consisting of only one type of element or compound.
• Mixture
A collection of two or more pure substances.

5. Most Materials are Mixtures
• Pure substance
A material consisting of only one type of element or compound.
• Mixture
A collection of two or more pure substances.
—can be separated by physical means

6. Most Materials are Mixtures

7. The Chemist’s Classification of Matter

8. The Chemist’s Classification of Matter
Pure materials consist of a single element or compound.

9. The Chemist’s Classification of Matter
Pure materials consist of a single element or compound.
Impure materials consist of two or more elements or compounds.

10. The Chemist’s Classification of Matter
Pure materials consist of a single element or compound.
Impure materials consist of two or more elements or compounds.
Mixtures may be heterogeneous or homogeneous.

11. The Chemist’s Classification of Matter
In heterogeneous mixtures, the different components can be seen as individual substances.

12. The Chemist’s Classification of Matter
In heterogeneous mixtures, the different components can be seen as individual substances.
In homogenous mixtures, the composition is the same throughout.

13. The Chemist’s Classification of Matter

14. The Chemist’s Classification of Matter
Homogeneous mixtures

15. The Chemist’s Classification of Matter
Homogeneous mixtures
Solution: all components in the same phase.

16. The Chemist’s Classification of Matter
Homogeneous mixtures
Solution: all components in the same phase.
Suspension: different components in different phases.

17. The Chemist’s Classification of Matter
CHECK YOUR NEIGHBOR
Is the air in your house a homogeneous or a heterogeneous mixture?
A. Homogeneous, because it is mixed very well.
B. Heterogeneous, because of the dust particles it contains.
C. Homogeneous, because it is all at the same temperature.
D. Heterogeneous, because it consists of different types of molecules.
B. Heterogeneous, because of the dust particles it contains.

18. The Chemist’s Classification of Matter
CHECK YOUR ANSWER
Is the air in your house a homogeneous or a heterogeneous mixture?
A. Homogeneous, because it is mixed very well.
B. Heterogeneous, because of the dust particles it contains.
C. Homogeneous, because it is all at the same temperature.
D. Heterogeneous, because it consists of different types of molecules.
B. Heterogeneous, because of the dust particles it contains.

19. Solutions
• Solution: A homogenous mixture consisting of ions or molecules
• Solvent: The major component of a solution.

20. Solutions
• Solution: A homogenous mixture consisting of ions or molecules
• Solvent: The major component of a solution.
• Solute: The minor components of a solution.

21. Solutions
• Solution: A homogenous mixture consisting of ions or molecules
• Solvent: The major component of a solution.
• Solute: The minor components of a solution.
• Saturated: Said of a solution in which no more solute will dissolve.

22. Solutions
• Concentration: A measure of the amount of solute dissolved in solution.

23. Solutions
• Concentration: A measure of the amount of solute dissolved in solution.
Solute
Concentration =
Solution

24. Solutions Solute Concentration =
• Concentration: A measure of the amount of solute dissolved in solution.
Solute
Concentration =
Solution
“concentrated”

25. Solutions
• Concentration: A measure of the amount of solute dissolved in solution.
Solute
Concentration =
Solution

26. Solutions
• Concentration: A measure of the amount of solute dissolved in solution.
Solute
Concentration =
Solution
“dilute”

27. Solutions
• Concentration: A measure of the amount of solute dissolved in solution.
• Mole: A super-large number, 6.02  1023, used to measure numbers of atoms or molecules, a.k.a. Avogadro’s number.

28. Solutions
• Concentration: A measure of the amount of solute dissolved in solution.
• Mole: A super-large number, 6.02  1023, used to measure numbers of atoms or molecules, a.k.a. Avogadro’s number.
The formula mass of a substance expressed in grams contains one mole.

29. Solutions
• Concentration: A measure of the amount of solute dissolved in solution.
• Mole: A super-large number, 6.02  1023, used to measure numbers of atoms or molecules, a.k.a. Avogadro’s number.
Substance Formula Mass
The formula mass of a substance expressed in grams contains one mole.
Carbon, C 12
Oxygen, O2 32
Carbon dioxide, CO2 44
Sucrose, C12H22O11 342

30. Solutions
Sucrose, C12H22O11 = g/mole

31. Solutions CHECK YOUR NEIGHBOR
Water, H2O, has a formula mass of 18. How many moles of water are there in 18 grams of water?
A. 0.5 moles
1 mole
9 moles
18 moles
B 1 mole

32. Solutions CHECK YOUR ANSWER
Water, H2O, has a formula mass of 18. How many moles of water are there in 18 grams of water?
A. 0.5 moles
1 mole
9 moles
18 moles
B 1 mole

33. How many grams of water, H2O, are there in 2 moles of water?
Solutions
CHECK YOUR NEIGHBOR
How many grams of water, H2O, are there in 2 moles of water?
A. 1 gram
9 grams
18 grams
36 grams
D. 36 grams

34. How many grams of water, H2O, are there in 2 moles of water?
Solutions
CHECK YOUR ANSWER
How many grams of water, H2O, are there in 2 moles of water?
A. 1 gram
9 grams
18 grams
36 grams
D. 36 grams

35. Solutions
• Molarity: A unit of concentration expressed in moles solute per liter of solution.

36. Solutions
• Molarity: A unit of concentration expressed in moles solute per liter of solution.
Moles of Solute
Molarity =
Liters of Solution

37. Solutions
• Molarity: A unit of concentration expressed in moles solute per liter of solution.
• ppm: A unit of concentration expressed in milligrams solute in liters of solution.
• Molarity: A unit of concentration expressed in moles solute per liter of solution.
• ppm: A unit of concentration expressed in milligrams solute in liters of solution.

38. Solutions
• Molarity: A unit of concentration expressed in moles solute per liter of solution.
• ppm: A unit of concentration expressed in milligrams solute in liters of solution.
• Molarity: A unit of concentration expressed in moles solute per liter of solution.
• ppm: A unit of concentration expressed in milligrams solute in liters of solution.
1 part solute
1 milligram solute
1 ppm = =
1,000,000 parts solution
1 liter solution

39. Solubility
• Solubility: The ability of a solute to dissolve in a solvent.

40. Solubility
• Solubility: The ability of a solute to dissolve in a solvent.
• Soluble: Said of a solute that has appreciable solubility.

41. Solubility
• Precipitate: Solute that comes out of solution.

42. Solubility CHECK YOUR NEIGHBOR
The amount of oxygen, O2, dissolved in the waters of the arctic ocean is greater, about equal to, or less than the amount of oxygen dissolved in warm tropical waters?
A. Greater than
About equal
Less than
It depends
A. Greater than

43. Solubility CHECK YOUR ANSWER
The amount of oxygen, O2, dissolved in the waters of the Arctic Ocean is greater, about equal to, or less than the amount of oxygen dissolved in warm tropical waters?
A. Greater than
About equal
Less than
It depends
A. Greater than
Explanation:
The solubility of oxygen in water decreases with increasing temperature. As a consequence, cold polar oceans tend to be more fertile than warmer tropical waters.

44. By mass, water is 88.88 percent oxygen. So why can’t we breathe water?
Chapter 12 Review
CHECK YOUR NEIGHBOR
By mass, water is percent oxygen. So why can’t we breathe water?
C. discover the property called inertia.

45. By mass, water is 88.88 percent oxygen. So why can’t we breathe water?
Chapter 12 Review
CHECK YOUR NEIGHBOR
By mass, water is percent oxygen. So why can’t we breathe water?
C. discover the property called inertia.
Hint: What is the elemental formula for the oxygen we breathe and the chemical formula for water?

46. Soaps and Detergents
Soaps and detergents have both polar and nonpolar properties.

47. Soaps and Detergents
Soaps and detergents have both polar and nonpolar properties.
Nonpolar part attracts to the “grime”.

48. Soaps and Detergents
Soaps and detergents have both polar and nonpolar parts.
Nonpolar part attracts to the “grime”.
Polar part attracts to water.

49. Soaps and Detergents

50. Soap and Detergents CHECK YOUR NEIGHBOR
Soap attracts “grime” by which type of molecular interaction?
A. Dipole–dipole.
B. Induced dipole–induced dipole.
C. Hydrogen bonding.
B. Induced dipole–induced dipole.
D. Dipole–induced dipole.

51. Soap and Detergents CHECK YOUR ANSWER
Soap attracts “grime” by which type of molecular interaction?
A. Dipole–dipole.
B. Induced dipole–induced dipole.
C. Hydrogen bonding.
B. Induced dipole–induced dipole.
D. Dipole–induced dipole.

52. Softening Hard Water
Hard water has high concentrations of calcium and magnesium.

53. Softening Hard Water
Hard water has high concentrations of calcium and magnesium.
Undesirable effects

54. Softening Hard Water
Hard water has high concentrations of calcium and magnesium.
Undesirable effects
Clogged pipes

55. Softening Hard Water
Hard water has high concentrations of calcium and magnesium.
Undesirable effects
Clogged pipes
Lower cleaning action of soaps and detergents

56. Softening Hard Water
Hard water has high concentrations of calcium and magnesium.
Undesirable effects
Clogged pipes
Lower cleaning action of soaps and detergents
Soap scum

57. Softening Hard Water
Detergent additives attract the Ca2+ and Mg2+ ions in hard water.

58. Softening Hard Water
Detergent additives attract the Ca2+ and Mg2+ ions in hard water.

59. Softening Hard Water
Some homes contain water softening units.

60. Softening Hard Water
Some homes contain water softening units.

61. Purifying the Water We Drink
The first step to purifying water is removing particles and bacteria.

62. Purifying the Water We Drink
The first step to purifying water is removing particles and bacteria.

63. Purifying the Water We Drink
Water is then aerated to improve the taste and smell.

64. Purifying the Water We Drink
Water is then aerated to improve the taste and smell.
Lastly, the water is disinfected with chlorine gas (or ozone).

65. Purifying the Water We Drink
CHECK YOUR NEIGHBOR
Which of the following is not a method of disinfecting drinking water?
A. Chlorine gas
B. Boiling
C. Aeration
C. Aeration
D. Iodine tablets

66. Purifying the Water We Drink
CHECK YOUR NEIGHBOR
Which of the following is not a method of disinfecting drinking water?
A. Chlorine gas
B. Boiling
C. Aeration
C. Aeration
D. Iodine tablets

67. Purifying the Water We Drink
Sea water can be converted to drinking water through desalination.

68. Purifying the Water We Drink
Sea water can be converted to drinking water through desalination.
Distillation
Reverse osmosis

69. Purifying the Water We Drink

70. Purifying the Water We Drink

71. Purifying the Water We Drink

72. Wastewater Treatment
Screening removes large insoluble items.

73. Wastewater Treatment Screening removes large insoluble items.
Primary treatment allows smaller insolubles to settle to the bottom or rise to the top for removal.

74. Wastewater Treatment Screening removes large insoluble items.
Primary treatment allows smaller insolubles to settle to the bottom or rise to the top for removal.
Secondary treatment aerates the water and allows finer particles to settle for removal.

75. Wastewater Treatment Screening removes large insoluble items.
Primary treatment allows smaller insolubles to settle to the bottom or rise to the top for removal.
Secondary treatment aerates the water and allows finer particles to settle for removal.
Tertiary treatment filters the water.

76. Wastewater Treatment

77. Wastewater Treatment