1. Acids & Bases
Titration

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

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
Neutralization does not mean pH = 7

4. ACID + BASE  SALT + WATER
A. Neutralization
ACID + BASE  SALT + WATER
Double replacement reaction
Can predict products – ex. antacids in your stomach
HCl + Ca(OH)2  2
CaCl2 + H2O 2
strong
strong
neutral

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

6. B. Titration Stoichiometry Provides basis for titration Examples:
1 mol HCl will neutralize 1 mol NaOH
2 mol HCl will neutralize 1 mol Mg(OH)2
HCl + NaOH  NaCl + H2O
2HCl + Mg(OH)2  MgCl2 + 2H2O

7. B. Titration Equivalence point
Point at which equal number of moles of H3O+ and OH- are in solution
Determined by…
indicator color change
dramatic change in pH

8. B. Titration
Strong acid, strong base
Weak acid, strong base

9. B. Titration Endpoint Point at which indicator color changes
Should be close to equivalence point if correct indicator is chosen

10. moles H3O+ = moles OH- MAVA nA = MBVB nB B. Titration M: Molarity
V: volume
n: # of H+ ions in the acid or OH- ions in the base

11. B. Titration
50.0 mL of an unknown solution of NaOH are titrated with M HCl. Find the molarity of the NaOH solution if 52.5 mL of acid are required to reach the equivalence point.

12. B. Titration
42.5 mL of 1.3M KOH are required to neutralize 50.0 mL of H2SO4. Find the molarity of H2SO4.