1. Properties of Solutions!
SALT!
WATER!

3. Solution: a homogenous mixture (s, l, g) -solute: the substance that is dissolved in the solution (lesser amount) -solvent: the substance that dissolves the solute ( greater amount)

5. are homogenous mixtures.
Liquid Solutions:
are homogenous mixtures.
do not disperse light.
may have color.
will not settle.
pass through a filter.

6. Solubility Factors Nature of Solute and Solvent:
Polar dissolves polar and ionic.
Non-polar dissolves non-polar.
Temperature:
Liquid & Solid: The higher the temperature, the more soluble.
Gas: Opposite
Pressure:
Has no effect on liquids & solids.
As the pressure increases, the solubility of gas increases.

7. A solution is saturated when it contains the maximum amount of solute it is able to dissolve at a given Temp.
It’s unsaturated when it has less than the maximum amount of solute.
It’s supersaturated when it has more than the maximum amount of solute. Crystals may form, unstable, given Temp.

9. Solubility Curve
Solution A is unsaturated because it falls below the line.
Solutions B and D are saturated because it falls on the line.
Solution C is supersaturated because it falls above the line.
Solubility B C A D
Temperature

10. To figure out which ions are soluble in water!
Use Reference Table F
To figure out which ions are soluble in water!

12. Molarity Mol solute L solution =2.5 mol/L M =
The relationship between the moles of solute and the volume of solution.
Mol solute
M =
L solution
Ex: What is the molarity of a 10.0 L solution containing 25 moles of solute?
25 mol
10.O L M=
=2.5 mol/L

13. The relationship between moles of solute to kilograms of solvent.
molality
The relationship between moles of solute to kilograms of solvent.
Mol solute m=
kg solvent
Ex: What is the molality of a solution containing 25 moles of solute and 10 grams of solvent?
25 m
0.010O Kg m=
m=250.0 molal

14. Parts Per Million grams of solute grams of solution X 10^6 ppm =
The relationship between the mass of solute and the total mass for very dilute solutions.
grams of solute
grams of solution
(whole)
X 10^6
ppm =

15. response must include both oxygen and water. [1]
June 2007.
Part C
Answer all questions in this part.
Directions (64–82): Record your answers in the spaces provided in your answer booklet. Some questions may require the use of the Reference Tables for Physical Setting/Chemistry.
Base your answers to questions 64 through 66 on the information below.
Scientists who study aquatic ecosystems are often interested in the concentration of
dissolved oxygen in water. Oxygen, O2, has a very low solubility in water, and therefore
its solubility is usually expressed in units of milligrams per grams of water at
atmosphere. The graph below shows a solubility curve of oxygen in water.
64 A student determines that 8.2 milligrams of oxygen is dissolved in a gram sample
of water at 15°C and 1.0 atmosphere. In terms of saturation, what type of solution is
this sample? [1]
65 Explain, in terms of molecular polarity, why oxygen gas has low solubility in water. Your
response must include both oxygen and water. [1]
66 An aqueous solution has gram of oxygen dissolved in grams of water. In
the space in your answer booklet, calculate the dissolved oxygen concentration of this
solution in parts per million. Your response must include both a correct numerical
setup and the calculated result. [2]

16. The percent of solute present in a solution.
Percent by Mass
The percent of solute present in a solution.
Mass of part
Mass of whole
% Mass=
X 100

17.
PartC #66

18. Base your answers to questions 65 through 68 on the information below.
In a laboratory, a student makes a solution by completely dissolving 80.0 grams of KNO3(s) in grams of hot water. The resulting solution has a temperature of 60.°C The room temperature in the laboratory is 22°C.
65 Classify, in terms of saturation, the type of solution made by the student. [1]
66 Compare the boiling point of the solution at standard pressure to the boiling point of water at standard pressure. [1]
67 Describe the direction of heat flow between the solution made by the student and the air in the laboratory. [1]
68 Describe a laboratory procedure that can be used to recover the solid solute from the aqueous solution
June 2010.

19. Icy Road

21.
#70-71