1. Here’s the plan: Pre-activity Strong/Weak Acids/Bases
Writing equilibrium reactions for weak acids and weak bases
Writing Acid/Base Reactions
Titration calculations (weak/strong)

2. “Pre-Activity”
According to the Bronsted-Lowry definition, an acid is something that will _________ __ ______ while a base will __________ __ _______ . According to the Arrhenius definition, an acid has ____ while a base has _____ . The strong acids are: __________ . The strong bases are: __________ . Conjugates are _____________ . Placing a conjugate acid and base in the same solution will create a _________ which resists ________ in ___.

3. 1. Separate the cards given into 4 piles: Strong Acid Weak Acid Strong Base Weak Base
HBr
CuOH
Ca(OH)2
NH4+
HCOOH (which H is the one?)
KOH
HC2H3O2
H2SO4
OH-1
NH3
NaC2H3O2 HF
NO2-1
CH3COOH (this is identical to which card?)
HNO3
CH3NH2 + H2O  CH3NH3+ + OH-1
NaOH HA
KClO
H+1

4. 2. Write the equilibrium reactions each would form when dissolved in water.
HA (a general formula for a weak acid)
B (a general formula for a weak base)
HNO2
NH3
H2CO3
NH4+
CH3COO-1

5. 3. Write NET IONIC EQUATIONS for the following reactants
3. Write NET IONIC EQUATIONS for the following reactants. If no reaction occurs, write the reactants and “No Reaction” for the products
Formic acid (HCOOH) and KOH
Ammonia and ammonium
Pyradine (a base, C5H5N) and perchloric acid
Propanoic acid (C3H5COOH) and ammonia
The underlined H is the H+ that would be donated.

6. 4. Perform the calculations below and sketch the titration curve
80. mL of 0.28 M chlorous acid (Ka=1.2 x 10-2) is titrated with 0.35 M potassium hydroxide.
Calculate the pH at each point in the titration:
0 mL KOH has been added
32 mL KOH has been added
64 mL KOH has been added
96 mL KOH has been added
Use a dashed line to sketch the titration curve if 0.35 M barium hydroxide had been used instead.