Masterton Practice for Acids and Bases
1. Classify each of the following as a strong or weak base:
a. LiOH
b. CH3CH2NH2
c. Ca(OH)2
d. F-
2. Show how these weak bases react with water in an equation and Kb expressions.
a. BO3b. CH3NH2
c. CN3. Classify each of the following as a strong or weak acid:
a. HNO3
b. HNO2
c. HC2H3O2
d. H3PO4
4. For each acid in question #3, show the appropriate dissociation and equilibrium
expression.
5.
a.
b.
c.
Label the following as the acid, base, conjugate acid or conjugate base.
HNO2 + H2O  H3O+ + NO2H2O + S-2  HS- + OHCN- + HC2H3O2  C2H3O2- + HCN
6. For each of the equations in #5 list the conjugate acid-base pairs.
7. For hypobromous acid (Ka = 2.1 x 10-9), calculate the [H+] and pH in solutions
prepared by adding the following number of moles of HBrO to water make one liter
of solution.
a. 1.0 mole
b. 0.20 mole
8. Calculate the pH of solutions of acetic acid (Ka= 1.8 x 10-5) prepared by adding
the following number of moles of acetic acid to 2.50L of water:
a. 3.75 mol
b. 0.700 mol
9. Lactic acid (Ka = 1.4 x 10-4) is present in sore muscles after vigorous exercise.
For a 1.5M solution of lactic acid, calculate:
a. [H+]
b. [OH-]
c. pH
d. % dissoc
10. For a 0.10M solution of benzoic acid (Ka=6.6 x 10-5), calculate:
a. [H+]
b. [OH-]
c. pH
d. % dissoc
11. The pH of a solution prepared by dissolving0.150 mol of formic acid, HCHO2 to
form 0.500L of solution is 2.14. Calculate the Ka of formic acid.
12. The percent dissociation of a certain weak acid in 0.10 M solution is 0.025%.
Calculate the Ka of the weak acid.
13. Calculate the [OH-] and pH in a solution prepared by dissolving 0.20 mol NH3
(Kb= 1.8 x 10-5) in one liter of water.
14. Calculate the [OH-], [H+] and the pH of 0.20M solutions of each of the following
amines.
a. triethyamine, [(C2H5)3N, Kb=4.0 x 10-4]
b. hydroxylamine (HONH2, Kb=1.1 x 10-8]
15. Calculate the pH of a 0.20 M C2H5NH2 solution (Kb = 5.6 x 10-4)
16. Calculate the percent dissociation of 0.10 M pyridine, C5H5N, Kb = 1.7 x 10-9.
17. The pH of a 0.01 M HCOOH (formic acid) is approximately
a. 1
b. 3
c. 7
d. 11
e. 13
18. The pH of a 0.05 M solution of ammonia is approximately
a. 1
b. 3
c. 7
d. 11
e. 13
19. The ionization constant of water at 45°C is 4.0 x 10-14. What is the pH of water
at this temperature?
20. Which is the strongest acid?
a. Ascorbic acid, Ka=8.0 x 10-5
b. Benzoic acid, Ka=6.5 x 10-5
c. 3-chlorobenzoic acid, Ka=1.5 x 10-4
d. 2-hydroxybenzoic acid, Ka=1.1 x 10-3
e. Chloroacetic acid, Ka=1.4 x 10-3
21. Which of the following acids has the strongest conjugate base?
a. Ascorbic acid, Ka=8.0 x 10-5
b. Benzoic acid, Ka=6.5 x 10-5
c. 3-chlorobenzoic acid, Ka=1.5 x 10-4
d. 2-hydroxybenzoic acid, Ka=1.1 x 10-3
e. Chloroacetic acid, Ka=1.4 x 10-3