Types of Acids and Bases
1. Classify these as an Arrhenius acid or Arrhenius base.
a. Ca(OH)2 _______________________
b. HNO3 _______________________
c. HC2H3O2 _____________________
d. H2SO4 _______________________
e. KOH _______________________
f. HCl _____________________
2. Complete the equations for the Ionization of these Arrhenius acids or bases in water:
ex:
HBr + H2O –––> H3O+ + Brex:
KOH ––––> K+ + OHa. HNO3 + H2O –––>
b. NaOH –––>
c. HCl + H2O –––>
d. Ca(OH)2 –––>
3. Identify the Bronsted-Lowry acid (loses an H+ ion), base (gains an H+ ion), conjugate acid, and the
conjugate base in each of the following.
a. HNO3 + H2O ---> H3O+ + NO3
b. NH3 + H2O <---> NH4+ + OHc. H2SO4 + OH-<---> HSO4- + H2O
d. C2H3O2– + H2O <---> OH- + HC2H3O2
e. H2PO4- OH-<---> HPO4-2 + H2O
f. H2PO4- + H3O+ <---> H3PO4 + H2O
g. HCO3– + H2O <---> H3O+ + CO3-2
h. HCO3– + H2O <---> H2CO3 + OH4. What is the conjugate acid of the following: (particle made by adding an H+ ion)
a. C2H3O2-_________
b. CO3-2 _________
c. Cl- _________
d. HCO3- _________
e. H2PO4- _________
5. What is the conjugate base of the following: (particle made by removing an H+ ion)
a. NH4+ _________
b. H2CO3 _________
c. H2O _________
d. HCO3- _________
f. H2PO4- _________
6. Using your knowledge of the Brønsted-Lowry theory of acids and bases, write equations for the
following acid-base reactions and indicate each conjugate acid-base pair:
a)
HNO3 + OH- 
b)
CH3NH2 + H2O 
c)
OH- + HPO4-2 
7. In the following reactions, construct Lewis structures and identify the Lewis acid and base.
a. Ag+ + 2NH3 --> Ag(NH3)2+
b. B(OH)3 + H2O --> B(OH)4 + H+
8. How do Lewis acids and bases compare to the Arrhenius and Bronsted-Lowry definitions of an acid
and a base?
9. The compound NaOH is a base by all three of the theories we discussed in class. However, each of
the three theories describes what a base is in different terms. Use your knowledge of these three
theories to describe NaOH as an Arrhenius base, a Brønsted-Lowry base, and a Lewis base.