1. Aim: What is titration?
Write the completed neutralization reaction for the following reactants.
1. Carbonic acid and potassium hydroxide
2. Phosphoric acid and sodium hydroxide
3. Nitric acid and calcium hydroxide

2. Mono, Diprotic, and Triprotic
Monoprotic acids (produce 1 H+ ions)  acids that ionize in 1 STEP
Ex: HCl  ____ + ____
Diprotic acids (produce 2 H+ ions) acids that ionize in 2 STEPS
Ex: H2SO4  ____ + ______
HSO4-  ____ + ______
Triprotic acids (produce 3 H+ ions) acids that ionize in 3 STEPS
Ex: H3PO4  ____ + ______
H2PO4- ____ + ______
HPO42- ____ + ______

3. Titration
chang_7e_esp/crm3s5_5.swf

4. Titration: Is used to find the molarity of an acid or a base
Is adding measured volumes of an acid or base of known molarity to a base or acid of unknown molarity until neutralization occurs (when # of H+ = # of OH-) and pH of the solution is 7 (called equivalence point)

5. Endpoint of Titration
An acid-base indicator can be used to show when an neutralization has occurred.
The point of neutralization is the endpoint of the titration.

7. Titration formula Titration formula (Table T): MA VA = MB VB
Where: MA = molarity of acid (H+)
VA = volume of acid
MB = molarity of base (OH-)
VB = volume of base

8. 1 M of HCl gives off 1 mole H+/liter
1 M H2SO4 gives off 2 mole H+/liter
2 M H2SO4 gives off ____ mole H+/liter
1 M NaOH gives off 1 mole OH-/liter
2 M NaOH gives off _____ mole OH-/liter
1 M Ca(OH)2 gives off 2 mole OH-/liter
2 M Ca(OH)2 gives off ____ mole OH-/liter

9. Sample Problem 1: What is the concentration of a solution of HI if 0
Sample Problem 1: What is the concentration of a solution of HI if 0.3 L is neutralized by 0.6 L of 0.2 M solution of KOH?
Sample Problem 2: What is the concentration of a hydrochloric acid solution if 50.0 mL of a M KOH solution are needed to neutralize 20.0 mL of the HCl solution of unknown concentration?

10. Sample Problem 3: A particular acid has an H+ concentration of 0
Sample Problem 3: A particular acid has an H+ concentration of 0.1 M and a volume of 100 mL. What volume of a base with a 0.5 M [OH-] will be required to neutralize the reaction?
**Sample Problem 4: You have 50 mL of 1.0 M H2SO4(aq). What volume of 0.5 M NaOH would be required to neutralize the acid? Remember Diprotic Acids yield 2 H+ ions in solution!