Station 1: Ionization Reactions
Directions: For each of the following acids, write the ionization
reaction that displays what happens to the acid in water.
Ionization should include only 1 of the hydrogen atoms.
Remember that the charges on both sides of the equation must
balance.
Example: H2SO3:
H2SO3(aq) + H2O(l)  H3O+(aq) + HSO3-(aq)
1. H3PO4:
2. H2SO4 :
3. HF:
4. HBr:
Directions: For each of the following bases, write the ionization
reaction that displays what happens to the base in water.
Assume that all bases start as solids. Remember that the
charges and atoms on both sides of the equation must balance.
Example: NaOH:
5. LiOH:
6. Ca(OH)2:
7. Ba(OH)2:
8. Fe(OH)3:
NaOH (s)  Na+ (aq) + OH- (aq)
Station 2: Identifying Arrhenius Acids and Bases
1. Complete the following neutralization equations. Make
sure each equation is balanced, and circle the salt
produced.
a. CH3COOH + LiOH 
b. Mg(OH)2 + H3PO4 
c. Sulphuric acid reacting with iron(III) hydroxide
2. Write the formula and the name for the parent acid and
the parent base that react to form each salt listed:
Parent Acid
a. KNO2
b. NH4Cl
c. CuC2O4
Parent Base
Station 3: Identifying Conjugate Acid-Base Pairs
1. In the following equilibrium, identify the acids and bases,
and the two conjugate acid-base pairs:
HF(aq) + CN-(aq) ⇌ HCN(aq) + F-(aq)
2. Complete the following table:
Conjugate Acid
H2C2O4
Conjugate Base
SO32-
HCO3H2O
3. Complete the following equilibrium, which represents the
reaction of a Bronsted-Lowry acid and base. Circle the
substances that make up one of the conjugate acid base
pairs.
NO2-(aq) + H2CO3(aq) ⇌
4. Write the Bronsted-Lowry acid-base equilibria which
occurs when the following pairs of substances are mixed
in solution.
a. HPO42- and SO42-
b. HIO3 and C2O42-
Station 4: Amphiprotic Species
1. Write an equation for a reaction between HCO3- and CNwhere HCO3- acts as an acid.
2. Write an equation for a reaction between HCO3- and H2O
where HCO3- acts as a base.
3.
a. Identify the amphiprotic substances in the following
list:
i. CH3COOH
ii. H2PO4iii. PO43iv. H2C2O4
v. HC2O4b. Explain what an amphiprotic species is and give the
characteristics it must possess.
ANSWER KEY
Station 1
1.
H3PO4(aq) + H2O  H3O+ + H2PO4-
2.
H2SO4(aq) + H2O  H3O+ + HSO4-
3.
HF(aq) + H2O  H3O+ + F-
4.
HBraq) + H2O  H3O+ + Br-
5.
LiOH(s)  Li+(aq) + OH-(aq)
6.
Ca(OH)2(s)  Ca2+(aq) + 2 OH-(aq)
7.
Ba(OH)2(s)  Ba2+(aq) + 2 OH-(aq)
8.
Fe(OH)3(s)  Fe3+(aq) + 3 OH-(aq)
1.
a. CH3COOH(aq)
Station 2
+ LiOH(aq)  H2O(l) + LiCH3COO(aq)
b. 3 Mg(OH)2 (aq) + 2 H3PO4(aq)  6 H2O(l) + Mg3(PO4)2(aq)
c. 3 H2SO4(aq) + 2 Fe(OH)3(aq)  6 H2O(l) + Fe2(SO4)3(aq)
2.
KNO2
Parent Acid: HNO2 – nitrous acid
Parent Base: KOH – potassium hydroxide
NH4Cl
Parent Acid: HCl – hydrochloric acid
Parent Base: NH3 – ammonia or NH4OH – ammonium hydroxide
CuC2O4
Parent Acid: H2C2O4 – oxalic acid
Parent Base: Cu(OH)2 – copper(II) hydroxide
Station 3
1.
2.
3.
HF(aq) + CN-(aq) ⇌ HCN(aq) + F-(aq)
Acid
Base
Acid
Base
Conjugate Acid
H2C2O4
HSO3HCO3H3O+
Conjugate Base
HC2O4SO32CO32H2O
NO2-(aq) + H2CO3(aq) ⇌ HNO2 + HCO3-
4.
a. HPO42- and SO42HPO42- + SO42- ⇌ PO43- + HSO4b. HIO3 and C2O42HIO3 + C2O42- ⇌ IO3- and HC2O4Station 4
1.
HCO3- + CN- ⇌ CO32- + HCN
2.
HCO3- + H2O ⇌ H2CO32- + OH3.
a. H2PO4- , HC2O4b. Can act both as an acid and as a base.
An AMPHIPROTIC species has an easily removed hydrogen, and a
negative charge
Names: _______________________________________________________________________
Station 1
1.
2.
3.
4.
5.
6.
7.
8.
Station 2
1.
a.
b.
c.
2.
KNO2
Parent Acid:
Parent Base:
NH4Cl
Parent Acid:
Parent Base:
CuC2O4
Parent Acid:
Parent Base:
Station 3
HF(aq) + CN-(aq) ⇌ HCN(aq) + F-(aq)
1.
2.
Conjugate Acid
H2C2O4
Conjugate Base
SO32-
HCO3H2O
NO2-(aq) + H2CO3(aq) ⇌
3.
4.
a. HPO42- and SO42-
b. HIO3 and C2O42-
Station 4
1.
2.
3.
a.
b.