1. Acid Base Titrations
Lesson 4

2. In a titration the molarity of one chemical is determined by reacting it with another one with known molarity (standard).

3. Special Equipment is used for a titration
Burette
Erlenmeyer Flask
Magnetic Stirrer
Pipette
Pipette Filler

4. Digital Balance
Solid acid to make a standard solution
Volumetric Flask

5. Titration Calculation
mL of M H2C2O4 is required to neutralize 10.0 mL of KOH solution in a titration. Calculate the base concentration.
H2C2O4 + 2KOH  K2C2O H2O L L
0.100 M
? M
L H2C2O4
x mole
x 2 mole KOH
1 L
1 mole H2C2O4
[KOH] = L
= M

6. If you get data in a table, you need to subtract the final burette reading from the initial to get the volume of acid or base added.
If you have multiple trials, average them but reject any volumes that are way off. Use some common sense.
Burette Volume in mL
Initial mL mL mL
Final mL mL mL
Volume Added mL mL mL
reject
average = 8.45 mL 2

7. Now it's your turn to try one!

8. Titration Calculation
mL , 8.46 mL and 8.44 mL of M H2SO4 was required to neutralize 25.0 mL of KOH solution in a titration. Calculate the base concentration.
H2SO4 + 2KOH  K2SO H2O
L L
0.200 M ? M
[KOH] = L H2SO4 x mole x mole KOH L mole H2SO4 L
= M

9. 3. Calculate the mass of H2C2O4. 2H2O required to make 100. 0 mL of a
3. Calculate the mass of H2C2O4.2H2O required to make mL of a M standard solution to use in your titration lab tomorrow.
0.100 L x mol x g = g
1 L mole