1. Solutions

2. Matter
Pure Substances
Elements
From Periodic Table
Compounds
Can write formulas for
Mixtures

3. What is a mixture?
A combination of 2 or more pure substances that can be separated.

4. How many kinds of mixtures are there?2

5. What is a heterogeneous mixture?
Heterogeneous do not blend smoothly throughout

6. Examples? Pepperoni pizza Pulpy orange juice Oatmeal raisin cookies
Ranch salad dressing

7. What is a homogeneous mixture?
A mixture that looks the same throughout. It is all in the same phase.

8. What are some examples?
Salt water
Tea
Coffee
Air
Sterling silver

9. What do all mixtures have in common?
They can all be separated.

10. What are some methods to separate mixtures?
Filtration- using a filter to separate solid chunks
Distillation- using boiling to separate a liquid
Crystallization- allowing a liquid to evaporate and leave behind a solid
Decantation- Pouring a liquid off of a solid.
Physical- separating with hands, magnets, tweezers, etc
Chromatography- allowing a liquid to rise up a piece of paper, separating by mass

11. FILTRATION

12. DISTILLATION

13. CRYSTALLIZATION
Evaporated water away to leave the crystal

14. DECANTATION

15. PHYSICAL

16. CHROMATOGRAPHY

17. What is another term for homogeneous mixture?
A solution

18. What are some examples of solutions?
Sterling silver, salt water, Kool-Aid, smog, 14 karat gold

19. How many properties of solutions are there?3

20. What is the first property?
The particles in a solution are very small.

21. And the second?
The particles are evenly distributed.

22. And the third?
The particles in the solution will not separate just by sitting.

23. What are the 2 parts to a solution?
Solute and solvent

24. What does it mean that something is soluble?
It can be dissolved
(Insoluble can not
be dissolved)

25. What is the solute?
The dissolved

26. What is the solvent?
The dissolver

27. How can you tell what the solute is and what the solvent is in a mixture?
Most of the time, the one that changes state is the solute.
You always have more solvent than solute
The solute is ADDED to the solvent.

28. Ocean water - Salt and water Kool-Aid - Powder, sugar, and water
Identify the solute(s) and solvent in each solution. Underline the solutes and circle the solvents.
Ocean water - Salt and water
Kool-Aid - Powder, sugar, and water
Antifreeze – 10% Water and 90% ethylene glycol
Steel- 98.5% Iron and 1.5% Carbon
Soda Pop - Syrup, water, and CO2 gas
Air – N2, O2, and other gases
18K Gold jewelry – 75% Gold and 25% Cu, Zn, Ag, Co

29. What is the universal solvent?
Water is usually the solvent.

30. Why?
It has odd characteristics because it is polar and has hydrogen bonds.

31. What are the three types of solutions?
Solid, Liquid and Gas

32. How do you make a solid solution?
The solids are usually mixed in the liquid state and then solidify.

33. What is a mixture of 2 metals called?
An Alloy

34. What is the air we breathe an example of?
A gaseous solution

35. Why is there so much nitrogen in the air?
To dilute the oxygen, it is toxic to humans and the air would combust.

36. Why can fish breathe under water?
There is oxygen dissolved in the water (a liquid solution). They are able to separate the gas from the water through their gills.

37. What is the most common type of solution?
Liquid solutions

38. What is a suspension?
A heterogeneous mixture that unless it is continuously stirred, the particles will settle out.

39. What is an example of a suspension?
Muddy water

40. What is the key to know that you have a suspension?
You have to shake well.

41. What is a colloid?
Mixtures with small particles that do not settle out when sitting, and cannot be separated by filtration.

42. What do most colloids appear to be?
Homogeneous

43. What are some examples of colloids?
Milk, gelatin, shaving cream, fog

44. How can you tell the difference between a colloid and a solution?
By using the Tyndall effect

45. What is the Tyndall effect?
When light is scattered by the larger particles in a colloid, but light is not scattered by a solution.

46. What are solutions called in which water is the solvent?
Aqueous Solutions

47. What is an aqueous solution that can conduct electricity called?
An electrolyte

48. Why do they conduct electricity?
They have polar molecules or the solute is ionic

49. What are the factors that affect dissolving?
Heat, surface area, and stirring

50. How does surface area affect dissolving?
If you increase the surface area, then things will dissolve faster.

51. How do you increase the surface area of something?
You crush it into smaller pieces.

52. How does stirring something affect dissolving?
When you stir something, it will cause the particles to break up faster.

53. Why is that?
When you stir, then you increase the number of times solute comes into contact with the solvent.

54. How does adding heat affect dissolving?
The particles are moving faster, which helps to separate the solute.

55. If you have a solution that heats when being made, what is it called?
Exothermic
Heat is released, making you feel warmer

56. If you have a solution that feels cool when being made, what is it called?
Endothermic
Heat is absorbed, making you feel cooler

57. Why can you only dissolve so much sugar into a glass of tea?
There is only so much room for the solute to dissolve in the solvent.

58. If there is still room to dissolve solute in the solvent, what is it called?
Unsaturated

59. What happens when there is no more room for solute to dissolve?
The solution becomes saturated.

60. What do saturated solutions usually look like?
Unsaturated or there might be solute crystallized at the bottom of the solution.

61. What is a supersaturated solution?
A solution that contains more solute than a saturated solution under the same conditions.

62. How do you make a supersaturated solution?
Usually you heat it, add more solute, then let it cool.

63. Are supersaturated solutions stable or unstable?
Very unstable.

64. Why?
They contain “too many” solute particles, so if they are disturbed, they will crystallize.

65. Super Saturated Sodium Acetate
And Another...

66. What is solubility?
How much solute that is required to form a saturated solution at certain temperatures.

67. How does temperature affect solubility?
Usually, increasing the temperature increase solubility.

68. By the “like dissolves like” rule.
How can you tell if two things are going to dissolve in one another or not?
By the “like dissolves like” rule.

69. What is that?
If two substances are polar they will dissolve, if one is polar and one is non polar, they will not dissolve.

70. What is the rapid escape of a gas from a liquid called?
Effervescence

71. What is a solubility curve?
A graph that shows solubility of different substances.

72. What specifically does it tell you?
The amount of solute dissolved into 100.0g of H2O by a certain temperature.
See how this is written? Write it this way ALWAYS from the graph for sigfigs!

73. Why do some lines go backwards from others?
They are gases
Gases decrease
solubility at higher
temps

74. For sigfigs write the solubility and temperature numbers from the graph with a decimal after. Assume they are there. 20 is 20.

75. If you are on the line, what type of solution do you have?
Saturated

76. If you are below the line, what type of solution do you have?
Unsaturated

77. If you are above the line, what type of solution do you have?
Super Saturated

78. What is the solubility of potassium chlorate at 60°C?
Means where is it saturated?

79. How many grams of potassium nitrate is needed to make 400
How many grams of potassium nitrate is needed to make 400.g of solution at 45°C?

80. How many grams of water is needed to make a saturated solution using 87.0g of K2Cr2O7 at 45°C?

81. What is concentration?
It is how much solute is in the solvent.

82. Can things be more or less concentrated than others?
Yes, you could have very concentrated orange juice or not so concentrated orange juice.

83. What term do we use the most for concentration of solutions?
Molarity (M) M

84. How do we solve for molarity?
Moles of solute
Molarity= Liters of solvent

85. What unit do we use for molarity?
Moles/liter or just M

86. What does molarity mean?
It means how much solute do we add to a certain amount of solvent.

87. Molarity Problems
You Tube Video

88. A student dissolves 2.75 g of sodium hydroxide in water to make 250 mL of solution. What is the molarity of the solution?

89. You need 1. 75L of a 3M sodium hydroxide solution
You need 1.75L of a 3M sodium hydroxide solution. How many grams of sodium hydroxide do you need?

90. What is molality?
Another measure of concentration. It tells you how many moles of solute in kg of solvent m

91. What is the equation used for molality?
Moles of solute
Molality= kg of solvent

92. What units are used for molality?
Mol/kg or just m

93. How to do the math:

94. You have 4g of sugar (C12H22O11) dissolved into 342. 11g of water
You have 4g of sugar (C12H22O11) dissolved into g of water. What is the molality of the solution?

96. What is a colligative property?
A property that modifies a state of matter change temperature

97. What do colligative properties depend on?
The amount of solute added to a solution.
Solute gets in the way and blocks solvent from changing state

98. What are 2 colligative properties?
Freezing point depression and boiling point elevation

99. What is boiling point elevation?
The temperature difference between a pure solvent’s boiling point and a solution’s boiling point.

100. What is freezing point depression?
The temperature difference between a pure solvent’s freezing point and a solution’s freezing point.

101. How do we solve for freezing point depression?
ΔTf=Kfm
ΔTf Change in temperature
Kf Constant (Given in question)
m molality
∆ means “change in”

102. How do we solve for boiling point elevation?
ΔTb=Kbm
ΔTb Change in temperature
Kb Constant (Given in question)
m molality

103. What do the answers tell us?
ΔTf or ΔTb tell us how much the original temperature changes.
ΔTf subtracts from freezing point
ΔTb adds to boiling point

104. While antifreeze protects a car from freezing, it also protects it from overheating. Calculate the freezing point depression of a solution of 100. g of ethylene glycol, C2H6O2, in kg of water. (Kf = 1.86 oC/m)
What is the new freezing point of water, if the original freezing point was 0.0°C?

105. Water with sugar added to it will boil at a higher temperature than pure water. By how much will the boiling point of water be elevated if 100. g of sucrose, C12H22O11, is added to 500. g of water?
(Kb = 0.52 oC/m)
What is the new boiling point of water, if the original was 100.0°C?

106. How many grams of iodine would have to be dissolved into 1620g of ethanol to lower the freezing point by 0.25°C? Kf for ethanol is 1.99°C/m.