Review For Unit Test 3 (Acids and Bases)
Review Topics:
 Dissociation of Ionic Compounds
 Separation of Molecular Compounds
 Ionization of Acids
 Diagnostic Testing of Solutions (conductivity, litmus)
 Solubility
 Solubility Equilibrium
 Percent By Mass Concentration
 Parts Per Million Concentration
 Molar Concentration
 Concentration of Individual Ions
 Dilution
 Preparing Standard Solutions
 Arrhenius Theory
 Modified Arrhenius Theory and the Hydronium Ion
 Strong and Weak Acids
 Strong and Weak Bases
 Monoprotic and Polyprotic Acids and Bases
 pH, [H3O+(aq)], pOH, and [OH-(aq)] Calculations
 Determining pH with Acid-Base Indicators
Remaining of Period To Work on Questions from Review Package
Chem 20
Chapter 3 Review Questions
1. Is a saturated solution always a concentrated solution? Give an example to illustrate your
answer.
2. Define the term “solubility”. What factors affect the solubility of solids, liquids and gases in
other liquids?
3. Iron concentration of 0.2 to 0.3 ppm in water causes fabric staining when washing clothes. A
typical wash uses 12.0 L of water. What is the maximum mass of iron that can be present
without staining the clothes?
4. What are the concentrations of each ion in the following solutions?
a. 4.12 mol/L ammonium chloride
b. 0.275 mol/L barium hydroxide
c. 0.543 mol/L ammonium phosphate
5. Calculate the new concentration when the following dilutions are performed:
a. 25.0 mL of 1.50 mol/L hydrochloric acid is diluted to 150 mL of solution
b. 1.3 L of 1.2 mol/L sodium nitrate diluted to 7.3 L of solution
c. 500 mL of 3.75 mol/L ammonium phosphate, with 2.75 L of water added
6. A sample of lemon juice has a pH of 2. A sample of club soda has a pH of 5. How much
more concentrated is the hydronium ion in the lemon juice than in the club soda?
7. The pH of pure water is 7.00. Explain why.
8. Which of the solutions in each pair has a higher pH? Explain why.
a. 0.10 mol/L solution of a weak acid; 0.010 mol/L solution of the same acid
b. 0.10 mol/L solution of an acid; 0.10 mol/L solution of a base
c. a solution with a pOH of 7.0; a solution with a pOH of 8.0
d. 0.10 mol/L solution of a strong acid; 0.10 mol/L solution of a weak acid
e. 0.10 mol/L solution of a strong base; 0.10 mol/L solution of a weak base
f. 0.10 mol/L solution of H2SO4; 0.10 mol/L solution of HSO4-
9. Fill in the table with the appropriate information:
Solution
[H3O+(aq)]
[OH-(aq)]
(mol/L)
(mol/L)
-8
3.11 x 10
1
2
3
pH
pOH
4.45 x 10-11
5.92
4
14.62
10. Which of the solutions in #9 is the most acidic? The most basic?
11. A student tests 4 unknown solutions with the following observations:
Solution A: doesn’t conduct electricity, blue litmus stays blue, red litmus stays red
Solution B: does conduct electricity, blue litmus stays blue, red litmus turns blue
Solution C: does conduct electricity, blue litmus stays blue, red litmus stays red
Solution D: does conduct electricity, blue litmus turns red, red litmus stays red
Identify the type of compound that could cause each of these observations.
12. Acid-base indicators are used to identify the possible pH of 3 unknown solutions. The
following observations are made:
Indicator
Solution A
Solution B
Solution C
methyl red
red
yellow
yellow
phenol red
yellow
red
orange
phenolphthalein
colourless
pink
colourless
bromothymol blue
yellow
blue
blue
possible pH range: