1. Acid Base Titrations
Chm 3.2.3

2. Titration
The controlled addition and measurement of the amount of a solution with a known concentration required to react completely with a measured amount of a solution with an unknown concentration

3. H+ + Cl- + Na+ + OH-  H2O + Na+ + Cl-
Acid Base Reaction
HCl + NaOH  H2O + NaCl
H+ + Cl- + Na+ + OH-  H2O + Na+ + Cl-
H+ + OH-  H2O
In an acid base neutralization reaction H+ in being neutralized by OH- to form H2O

4. Acid Base Stoichiomety
What concentration of 100 mL of an NaOH is needed to neutralize 200 mL of a 0.5 M HCl solution.
200 mL of 0.5 M HCl
= 0.10 mole HCl = 0.1 moles H+
H+ + OH-  H2O
0.1 moles OH- = 0.1 mole NaOH
in 100 mL = 1.0 M solution of NaOH

5. When H+ and OH- are 1:1 mole ratio
For a neutralization reaction
MAVA = MBVB
Proven by previous example:
(0.5 M HCl x 200 mL) = (1.0 M NaOH x 100 mL)

6. Example
What volume of a 0.3 M HCl solution will be needed to neutralize 500 mL of a 0.1 M KOH solution?