AP Chemistry 2015-2016
16.1-16.3 Practice
A. Name the following acids and bases:
1) NaOH
Name:
2)
H2SO3
3) H2S
4)
H3PO4
5) NH3
6)
HCN
7) Ca(OH)2
8)
Fe(OH)3
Date:
9) H3P
B. Identify the following as strong or weak acids or bases.
1) NaOH
2)
H2SO3
3) H2S
4)
H3PO4
5) NH3
6)
HCN
7) Ca(OH)2
8)
Fe(OH)3
9) H3P
C. Using your knowledge of the Brønsted-Lowry theory of acids and bases, write equations for the
following acid-base reactions and label each conjugate acid-base pair:
1) HNO3 + OH- 
2) CH3NH2 + H2O 
3) OH- + HPO4-2 
Per:
D. Answer the following in complete sentences.
1) What is meant by autoionization? Write the chemical equation that illustrates the autoionization
of water.
2) Explain why pure water is a poor conductor of electricity.
3) Write the expression for the ion-product constant for water, Kw.
E. Calculate [H+] for each of the following solutions and indicate whether the solution is acidic, basic, or
neutral:
1) [OH-] = 0.00005 M
2) [OH-] = 3.2x10-9 M
3) [OH-] = 0.00005 M
4) [OH-] is 100 times greater than the [H+]
F. Calculate [OH-] for each of the following solutions. Indicate whether the solution is acid, basic, or
neutral:
a) [H+] = 0.0041 M
b) [H+] = 3.5x10-9 M
c) [H+] is 10 times greater than [OH-]
G. At the freezing point of water (0°C), kw = 1.2x10-15. Calculate the [H+] and [OH-] for a neutral solution
at this temperature.
AP Chemistry 2015-2016
16.4-16.5 Practice
Name:
Date:
Per:
1. Consider two solutions, solution A and solution B. [H+] in solution A is 500 times greater than that
in solution B. What is the difference in the pH values of the two solutions?
2. If NaOH is added to water, how does the [H+] change? How does the pH change?
3. Estimate (without a calculator) the pH of a solution in which [H+] = 0.00003M. Is the solution
acidic or basic?
4. If pH = 7.8, calculate the [H+] and [OH-] in the solution.
5. Complete the following table by calculating the missing entries and indicating whether the
solution is acidic or basic:
[H+]
[OH-]
pH
pOH
Acidic or basic?
-3
7.5x10 M
3.6x10-10 M
8.25
5.70
6. A solution is labeled 0.500M HCl. What is the [H+] for the solution?
7. A solution is labeled 0.125M Sr(OH)2. What is the [OH-]?
8. Determine the [H+], [OH-], pH and pOH of each of the following:
a. 0.0575M HNO3
b. 0.723g HClO4 in 2.00 L
c. 0.175M NaOH diluted to 2.00L
d. 0.0050M KOH
e. A solution formed by mixing 10.0mL of 0.015M Ba(OH)2 with 30.0mL of 7.5x10-3M NaOH.
AP Chemistry 2015-2016
Chapter 16 Review Questions
Name:
Date:
Per:
Directions: Answer in complete sentences in your notebook.
1. What are the general physical and chemical properties of acids? Of bases?
2. What is the Arrhenius definition of an acid? Of a base?
3. What is a hydronium ion? Does H+ exist in solution by itself?
4. What is the Brønsted-Lowry definition of an acid? Of a base?
5. Why is there more than one definition of acid-base behavior? Which definition is the right one?
6. Describe amphoteric behavior and give an example.
7. What is a conjugate acid-base pair? Give an example.
8. Explain the difference between a strong acid and a weak acid and list one example of each.
9. What are diprotic and triprotic acids? List an example of each.
10. Define the acid ionization constant and explain its significance.
11. What is the equation for the autoionization of water?
12. What is the equilibrium expression for the autoionization of water?
13. What is this expression equal to at 25°C?
14. What happens to the [OH-] when the [H3O+] is increased? Decreased? Your answer should include
a discussion of equilibrium
15. Define pH. What pH range is acidic? Basic? Neutral?
16. Define pOH. What pOH range is acidic? Basic? Neutral?
17. In most solutions contained a strong or weak acid, the autoionization of water can be neglected
when calculating [H3O+]. Explain why this is the case.
18. When calculating [H3O+] for weak acid solutions, we can often use the x is small approximation.
Explain the nature of this approximation and why it is valid.
19. What is the percent ionization of an acid? Explain what happens to the percent ionization of a
weak acid as a function of the concentration of the weak acid solution.
20. In calculating [H3O+] for a mixture of a strong acid and weak acid, the weak acid can often be
neglected. Explain why this is so.
21. Write a generic equation for how a weak base ionizes in water.
22. How can you determine whether an anion will act as a weak base?
23. What is the relationship between Ka and Kb?
24. What kinds of cations act as weak bases? Include examples.
25. When calculating the [H3O+] for a polyprotic acid, the second ionization step can often be
neglected. Explain why this is so.