Unit 6
Name _______________________________
# ________
Section 1: Into to Acids and Bases
1. When water self-ionizes, what two ions does it break up into (Give both formula
and name)?
2. Explain why HCl would be classified as both an Arrhenius and a Brønsted-Lowry
acid.
3. Explain why NH3 would be classified as a Brønsted-Lowry base but not an
Arrhenius base.
4. Explain the relationship between the strength of an acid and its conjugate base.
5. For each of the following, label the acid, base, conjugate acid, and conjugate
base.
a. H2PO4- + H2O  H3PO4 + OHb. HCl + H2O  H3O+ + Cl6. List the strong acids and the strong bases. Why are they considered strong?
Section 2: Naming Acids
Write the formula for each of the acids listed below:
1. Nitric acid
2. Chloric acid
3. Acetic acid
4. Hydrobromic acid
5. Sulfurous acid
6. Chlorous acid
7. Hydrochloric acid
8. Phosphoric acid
9. Nitrous acid
10. Hydrofluoric acid
11. Perchloric acid
12. Hydroiodic acid
13. Phosphorous acid
14. Carbonic acid
15. Sulfuric acid
Name each of the following acids:
16. HClO4
17. H3PO4
18. HCl (aq)
19. H2SO4
20. HNO2
21. HI (aq)
22. HC2H3O2
23. HF (aq)
24. H3PO3
25. HClO3
26. H2CO3
27. H2SO3
28. HClO2
29. HNO3
30. HBr (aq)
Section 3: pH and pOH
1. What is the equilibrium expression for water? What is the value for Kw?
2. In neutral water, what is the concentration of H3O+ and OH-?
3. What is the [OH-] if the [H3O+] is 1.0 x 10-9 M?
4. List the range of values for pH. Which values are considered acids? bases?
5. List the range of values for pOH. Which values are considered acids? bases?
6. Complete the table.
Substance Concentration
[H3O+]
1.00 X 10-9
[H3O+]
[H3O+]
1.00 X 10-2
[H3O+]
[H3O+]
[H3O+]
2.00 X 10-4
[H3O+]
[H3O+]
3.50 X 10-10
[H3O+]
5.80 X 10-2
+
[H3O ]
9.50 X 10-11
[OH-]
1.00 X 10-9
[OH ]
[OH-]
1.00 X 10-2
[OH-]
1.00 X 10-11
[OH ]
1.00 X 10-7
[OH-]
[OH-]
5.60 X 10-7
[OH-]
3.50 X 10-10
[OH ]
5.80 X 10-2
[OH-]
9.50 X 10-11
pH
pOH
Acid, base or neutral?
8.00
11.0
neutral
6.25
6.00
10.3
7. What is the pH of an aqueous solution that contains 25 grams of hydrochloric
acid dissolved in 1.5 liters of solution?
8. What is the pH of an aqueous solution that contains 1.2 moles of nitric acid and
1.7 moles of hydrochloric acid dissolved in 1000 liters of solution?
Section 4: Titration
1. Complete and balance the following neutralization reactions.
a. HF + LiOH →
b. HClO3
+
Mg(OH)2
c. HNO3
+
Ba(OH)2
d. HC2H3O2
+
→
→
Sr(OH)2
→
2. What is the purpose of titration?
3. What is an indicator?
4. What is the color of litmus when exposed to basic substances? acidic
substances?
5. What is the color of phenolphthalein in acidic solutions? basic solutions?
6. What is the concentration of the 25 mL of hydrochloric acid that neutralized
30 mL of 0.1 M sodium hydroxide?
7. How many mL of 0.20 M HBr is needed to neutralize 23.45 mL of 0.11 M KOH?
8. In a titration of vinegar (a solution of acetic acid, CH3COOH), you find that it
requires 11.10 mL of 0.748 M NaOH to neutralize a 10.0 mL sample of vinegar.
What is the concentration of acetic acid in the sample of vinegar?