1. Titration
Acids & Bases

2. Acid Dissociation Constant (Ka)
The ratio of the concentration of the dissociated form of an acid to the concentration of the undissociated form.
H2CO3(aq) + H2O(l)  H3O+ + HCO3-
Larger Ka, the stronger the acid.

3. Neutralization Chemical reaction between an acid and a base.
Products are a salt (ionic compound) and water.

4. ACID + BASE  SALT + WATER
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.
Neutralization does not mean pH = 7.

5. Titration
standard solution
unknown solution
Titration
Analytical method in which a standard solution is used to determine the concentration of an unknown solution.

6. Titration dramatic change in pH Equivalence point (endpoint)
Point at which equal amounts of H3O+ and OH- have been added.
Determined by…
indicator color change
dramatic change in pH

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

9. Titration H3O+ M = ? V = 50.0 mL n = 2 OH- M = 1.3M V = 42.5 mL n = 1
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

10. Buffer
A solution of a weak acid and a weak base that resists large pH changes when acid or base is added.
Buffer capacity: amount of acid or base that can be added without changing the pH
Buffered Aspirin
Bufferin