Honors Chemistry
Unit 7 – Stoichiometry
Lesson 6 – Titrations
Book Section: 15-2
Objective: SWBAT use molarity and
stoichiometry to solve titration problems.
Agenda: Experimental Setup, Lesson,
Guided Practice, HW
A titration is a lab
technique – it is one of the
most common quantitative
 A titration is a measured
reaction between two
solutions – one you know
the concentration of, and
one you don’t.
 The use of a color-changing
indicator tells us when the
reaction has reached
Solving Titration Problems
 Titration
problems are solution stoichiometry
problems – plain and simple. They just refer
specifically to the lab technique of titration.
 Example: A 25 mL solution of 0.5 M NaOH is
titrated until neutralized into a 50 mL of HCl. What
was the concentration of the HCl?
Harder Example
 Titration
reveals that 11.6 mL of 3.0 M
sulfuric acid are required to neutralize the
sodium hydroxide in 25.00 mL of NaOH
solution. What is the molarity of the NaOH
You Try
 When
34.2 mL of a 1.02 M NaOH solution is added
from a buret to 25.00 mL of a phosphoric acid
solution that contains the indicator phenolphthalein,
the solution changes from colorless to red. What is
the molarity of the phosphoric acid?
HW: #27-30, Read 15-2
Next Week
Monday: Stoichiometry Review, Quiz 7-7
 Tuesday: Stoichiometry Exam
 Wednesday: Begin Unit 8: The Periodic
Table – History of the Periodic Table (5-1)
 Thursday: Electron Configurations and the
Periodic Table (5-2), Quiz 8-1
 Friday: Atomic & Ionic Radius (5-3), Quiz 8-2