1. III. Titration (p. 493 – 503)
Ch. 15 & 16 – Acids & Bases

2. Neutralization
Neutralization is a chemical reaction between an acid and a base.
The products are a salt (any ionic compound) and water.
Acid + Base Salt + Water
Ex. HCl + NaOH NaCl + H2O

3. Neutralization Continued…
Neutralization does not necessarily mean pH = 7
Salts can be neutral, acidic, or basic depending on the strength of the acid and base involved in the reaction.
Ex. HCl + NaOH NaCl + H2O
strong strong neutral
Ex. HC2H3O2 + NaOH NaC2H3O2 + H2O
weak strong basic

4. Indicators
Acid-base indicators are compounds whose colors are sensitive to pH.
- the color of the indicator changes as pH changes
- indicators are typically made from weak acids or bases
Acid-base indicators are good for determining approximate pH.
If exact pH is needed, a pH meter can be used.

5. Titration
Titration is an analytical method in which a standard solution is used to determine the concentration of an unknown solution.
The equivalence point tells you when equal amounts of H3O+ and OH- are in the solution.
- you know you have reached the equivalence point
when there is a dramatic change in pH or a color
change in the indicator.
The point at which the indicator changes color is called the endpoint.

6. Calculations moles H3O+ = moles OH- M * V * n = M * V * n
M = molarity (moles/L)
V = volume (L)
n = # of H+ ions in the acid OR
# of OH- ions in the base

7. Practice
42.5 mL of 1.3M KOH are required to neutralize 50.0 mL of H2SO4. Find the molarity of H2SO4.
H3O+
M = ?
V = 50.0 mL
n = 2
OH-
M = 1.3M
V = 42.5 mL
n = 1
MV# = MV#
M(50.0mL)(2) = (1.3M)(42.5mL)(1)
M = 0.55M H2SO4