SCH3U
Review– Chapter 8
McGraw Hill
Define:
1.Solution:_______________________________________________________________
________________________________________________________________________
2.Solvent:_______________________________________________________________
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3.Solute_________________________________________________________________
________________________________________________________________________
4.Solubility:______________________________________________________________
_______________________________________________________________________
 A solute is described as soluble if ______________________________________
 A solute is described as slightly soluble if ________________________________
 A solute is described as insoluble if _____________________________________
5. Saturated solution:______________________________________________________
_______________________________________________________________________
6. Unsaturated solutions: ___________________________________________________
_______________________________________________________________________
7. Supersaturated solutions:_________________________________________________
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Factors that effect solubility and rate of dissolving.
1.What are the forces that determine the formation of a solution??
2. What is hydrogen bonding?
3. What is hydration?
4. Why ionic compounds are dissolved in water?
5. Why polar molecular compounds are dissolved in water?
6. Why non-polar molecular compound are not dissolved in water?
10. “Like Dissolve Like”. Complete the chart.
Polar or Ionic
Solvent
Solute
Non-polar
Polar
Non-polar
11. Does CH3OH dissolves in PH3 gas? Explain.
12. A solution of NaCl is produced by dissolving 2g of the substance in 100mL of water.
Sodium chloride is classified as:
a. soluble
b. slightly soluble
c. insoluble
Answer: A
13. A solution of NaCl is classified as a saturated solution at room temperature. If a
spoon of solute is added to the solution, it decants at the bottom of the container. Is the
final solution consider a supersaturated solution?
______NO _________________
14. Explain why stainless steel, seawater, and air are
all considered solutions.
They are mixtures. They are homogenous.
15. Which solution will contain the higher concentration of nitrate ions? (Answer: b)
0.452 mol/L sodium nitrate
or 0.228 mol/L aluminum nitrate
a. sodium nitrate
b. aluminum nitrate
c. They contain the same concentration of nitrate ions.
d. This must be determined experimentally.
16. Which of the following is a liquid in gas type of solution? (answer: B)
a. carbon dioxide in water
b. water in air
c. methanol in water
d. oil in water
17. Which of the following does not dissolve very well in water? (answer : D)
a. sodium chloride
b. sugar
c. ethanol
d. gasoline
18. A solution that has a relatively large quantity of solute dissolved in the solvent is
(Answer: C)
a. homogenous
b. dilute
c. concentrated
d. saturated
19. Which of the following contains 1 mol of dissolved copper(II) nitrate? (Answer: C)
a. 500 mL of a 0.5 mol/L solution
b. 750 mL of a 0.75 mol/L solution
c. 500 mL of a 2.0 mol/L solution
d. 1 L of a 0.9 mol/L solution
20. Which piece of lab equipment is used to obtain a small, accurate volume from a stock
solution for a dilution procedure? (answer: B)
a. graduated cylinder
b. pipet
c. beaker
d. volumetric flask
21. In a chemical analysis, 2.2 mg of oxygen was measured in 250 mL of pond water.
What is the concentration of oxygen, in ppm?
mO2 = 2.2mg
vH2O=250ml=0.25L
cO2=?
mO2
2.2mg
C = ------------ = ------------ = 8.8 ppm
vH2O
0.25L