1. Ch. 15 – 4 What is titration? p. 571-578

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

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

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

5. Titration
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
MVn = MVn
M(50.0mL)(2)
=(1.3M)(42.5mL)(1)
M = 0.55M H2SO4

6. Learning Check
Write a balanced equation and calculate the mL of 2.00 M H2SO4 required to neutralize 50.0 mL of 1.00 M KOH?
__H2SO4 + __KOH __K2SO4 + __ H2O
12.5 mL 2) mL 3) mL
Answer: 12.5 mL

7. Learning Check
A 25 mL sample of phosphoric acid is neutralized by 40. mL of 1.5 M NaOH. What is the molarity of the phosphoric acid solution?
3NaOH + H3PO Na3PO H2O
1) M 2) 0.80 M 3) 7.2 M
Answer : 2) 0.80 M