1. Ch. 15 & 16 - Acids & Bases
III. Titration (p )

2. A. Neutralization Chemical reaction between an acid and a base.
Products are a salt (ionic compound) and water.
Neutralization occurs when hydronium ions and hydroxide ions are supplied in equal numbers by reactants.

3. ACID + BASE  SALT + WATER
A. Neutralization
ACID + BASE  SALT + WATER
HCl + NaOH  NaCl + H2O
strong
strong
neutral
HC2H3O2 + NaOH  NaC2H3O2 + H2O
weak
strong
basic
Salts can be neutral, acidic, or basic.

4. B. Titration
standard solution
unknown solution
Because acids and bases react, the progressive addition of an acid to a base can be used to compare the concentrations of the acid and base.

5. Titration
Titration: analytical method in which a standard solution is used to determine the concentration of another solution.
Standard solution: one for which the concentration is known

6. B. Titration Equivalence point (endpoint)
Point at which equal amounts of H3O+ and OH- have been added.
End point
Point in a titration at which
an indicator changes color.

7. moles H3O+ = moles OH- MV n = MV n B. Titration M: Molarity
V: volume
n: # of H+ ions in the acid or OH- ions in the base

8. B. Titration
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

9. A 15. 5 mL sample of 0. 215 M KOH solution is mixed with
A 15.5 mL sample of M KOH solution is mixed with .645 M HCl, in a titration experiment. Calculate the volume of the hydrochloric acid solution.
Answer: L