1. Titrations & their CALCULATIONS

2. Titrations
A titration is a laboratory technique used to find the concentration of a solution
Titrations are used to measure the molarity of a solution using a standard solution.
A Standard Solution is one with a precisely known concentration

3. Titration
During a titration, the standard solution and solution with an unknown concentration
A Burette is used to add on solution to another
A burette can add a solution to another while carefully measuring the volume added
If we know the volume added AND the concentration (from the standard solution) we can calculate the moles of reactant added

4. Titration
We will only talk about acid-base titrations (mixing and acid and base)
During an acid-base titration, an acid reacts with a base (a compound with OH-) in a double replacement reaction to form water

5. Titration Before titrating, an indicator is added to the solution.
An Indicator changes colour when a reaction is neutralized
Neutralized means the moles of acid and base are equal
When the solution is neutralized, we call that the endpoint of the titration
Since we can calculate the moles added and the moles of acid and base are equal, we can calculate the unknown.

6. Titration
When performing a titration, it is important to reach the proper endpoint
If you add too much, the moles you calculate will be wrong and you did a whole experiment for NOTHING!

7. Titration Calculations
A titration calculation is a simple stoichiometric calculation. Follow the 4 steps:
Balance the equation
Go to moles
Rebalance
Go where it asks

8. Example 1:
What volume of 0.32 M nitric acid is needed to neutralize 26 mL of 0.22 M calcium hydroxide solution?

9. Example 2:
What volume of 0.80 mol/L KOH is needed to neutralize 15.0 mL of 0.65 M H2SO4?