1. v. Neutralization reactions
Acid + Base  Salt + water
Salt – ionic compounds (except oxides)
Salts can be
Neutral – when both the acid and base are strong
Acidic – when a strong acid reacts with a weak base
Basic – when a strong base reacts with a weak acid

2. v. Neutralization reactions
Examples

3. standard solution
unknown solution
VII. Titration
Concept: analytical method used to determine the concentration of an unknown substance. Often an acid-base reaction.
Equivalence point: point at which moles of H+ = moles of OH-; can use this fact (and the volumes involved) to calculate the molarity of the unknown (similar to dilution formula)
The equivalence point can be determined by measuring the pH at regular intervals and graphing the data or
Estimate the equivalence point by using an indicator

4. c) End Point: the point at which an indicator changes color
vii. titration
c) End Point: the point at which an indicator changes color
This will be close to (but not exactly) the equivalence point. For example – phenolphthalein changes from colorless to pink at a pH of about 8. If you are doing a strong acid/strong base titration, the equivalence point is at a pH of 7. The difference is only a mL or so, so it gives a very close approximation of the equivalence point

5. vii. titration

8. VII. titration
d) Titration Calculation Formula MaVana = MbVbnb M = molarity V = volume n = number of moles of OH- (for the base) or H+ (for the acid) -use the subscript a refers to the acid, b refers to the base

9. vii. titration
d. Titration Calculation i. example: 42.5mL of 1.3M KOH are required to neutralize 50.0mL of H2SO4. Find the molarity of the sulfuric acid