1. Titrations

2. Learning outcomes You should be able to:
be able to carry out titrations and the associated calculations

4. Titration
Titration using a known concentration to find the concentration of an unknown
Today we will the concentration of an UNKNOWN acid by titrating it with a known base concentration:
NaOH = 0.50 mol . dm-3

5. Stoichiometry
The stoichiometry of an acid-base neutralization reaction is the same as that of any other reaction For example, in the reaction: NaOH (aq) + HCl (aq)  NaCl (aq) + H2O (l) 1 mol of NaOH neutralizes 1 mol of HCl:

6. The pH meter measures the pH of the acid solution in the beaker as a solution of a base with a known concentration is added from the buret.

7. pH curve for Strong Acids and Bases
This abrupt change in pH occurs at the equivalence point

8. Boardworks GCSE Separate Sciences 2009 Titrations
Titration equipment
NaOH
Base in Burette
Titrant
safety filler
burette
stand
pipette
conical flask
beaker
Acid in flask
Analyte
Acid in flask
Analyte

9. Titration with an Indicator

10. What’s the Point of a Titration Again?
To find the unknown concentration of an acid or a base.
Note the volume you started with and how much volume of the titrant you added

11. Practical Set up equipment
Put one spatula of metal oxide and one spatula of carbon into your crucible and mix well.
Heat in a blue Bunsen flame until you see a change.
Leave your crucible to cool.
SAFETY: Wear safety goggles. Wash hands after practical.