Ch 7 Solutions Review Worksheet p. 224–243
Name
Section 7.1 – Solutions and Other Mixtures
1. What are the two types of mixtures? Define each and give an example of a solid,
liquid and gas for each.
a.
b.
2. What is a suspension? Give 3 examples.
a.
b.
c.
3. How can you separate a suspension?
4. What is the particle size of a suspension?
5. What is immiscible?
6. How can you separate immiscible substances?
7. What is miscible?
8. How can you separate miscible substances?
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Ch 7 Solutions Review Worksheet p. 224–243
Name
9. What is a colloid? Give 3 examples.
a.
b.
c.
10. What is the particle size of a colloid?
11. Explain the Tyndall effect. Does this happen for every colloid?
12. What is an emulsion? Give two examples.
a.
b.
13. What is a solution? Give 3 examples.
a.
b.
c.
14. What are the 2 parts of a solution? Give an example of each.
a.
b.
15. What states of matter can form solutions?
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Ch 7 Solutions Review Worksheet p. 224–243
Name
16. What is an alloy?
17. Why would you want to use an alloy? Give at least one example.
18. Classify each of the following as a heterogeneous mixture or a homogeneous
mixture.
a. Salad
b. Tap water
c. Muddy water
Section 7.2 – How Substances Dissolve
1. What is considered to be the universal solvent?
2. Describe (in detail) the 3 steps in solution formation.
3. Explain hydrogen bonding.
4. What is an example of a polar molecule? What does this mean?
5. What is an example of a nonpolar molecule? What does this mean?
6. What does “like dissolves like” mean?
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Ch 7 Solutions Review Worksheet p. 224–243
Name
7. What are 3 factors that affect solubility?
a.
b.
c.
Section 7.3 – Solubility and Concentration
1. What is solubility? Give 2 examples that are soluble in water.
a.
b.
2. Give 2 examples that are insoluble in water.
a.
b.
3. Define concentration of a solution.
4. What is an unsaturated solution? How can you tell?
5. What is a saturated solution? How can you tell?
6. What is a supersaturated solution? What would happen if pressure or temperature
decreases in a supersaturated solution?
7. What factors affect solubility of gases?
8. What is the equation for the calculation of the concentration of a solution?
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Ch 7 Solutions Review Worksheet p. 224–243
Name
9. What is this quantity called?
10. Which solution is the most concentrated H2SO4?
a. 1.0 M H2SO4
b. 2.0 M H2SO4
c. 3.0 M H2SO4
d. 4.0 M H2SO4
11. Determine the molarity of the following solutions:
a. 2 mol of calcium chloride dissolved in 1 L of solution.
b. 0.75 mol of copper (II) sulfate, dissolved in 1.5 L of solution.
c. 2.25 mol of sulfuric acid dissolved in 725 mL of solution.
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