Titration Lecture Notes

Introduction to Titration

• Definition: A technique to determine the concentration of an unknown solution using a solution with a known concentration.
• Process: Add the known solution to a set volume of the unknown solution until the reaction completes.
• Purpose: Calculate the concentration of the unknown solution.
• Indicator Use: May be needed to signal the end of the reaction.

Apparatus Needed for Titration

• Pipette: Accurately measures a specific volume of the unknown solution into the flask.
• Burette: Measures and adds the known reactant to the unknown solution with up to 0.05 cubic cm accuracy.

Steps to Carry Out a Titration

1. Add Unknown Solution: Use a pipette to add a set volume to a clean conical flask.
2. Add Indicator: Add a few drops if necessary.
3. Fill Burette: Use it with the known solution.
4. Record Initial Volume: Note the starting volume on the burette.
5. Add Known Solution: Slowly add from the burette to the unknown solution in the flask while swirling the flask or using a stir plate.
6. End Point: Stop adding when the reaction completes and an indicator shows an appropriate color change.
7. Record Final Volume: On the burette.
8. Calculate Volume Added: Subtract the initial volume from the final reading to get the titration volume.
9. Repeat for Accuracy: Repeat the experiment until consistent titration values are obtained.

Indicator Usage

• Gradual vs. Sudden Change:
  • Universal Indicator: Offers a gradual color change, suitable for acid-alkali titrations.
  • Litmus: Provides a sudden color change.
• Variation in Solutions:
  • The acid may be the known solution and the alkali unknown, or vice versa.

Next Steps

• Titration Calculation: To determine the concentration of the unknown solution.
• Summary: Titrations are essential for determining unknown solution concentrations using another solution of known concentration.

Follow-Up

• Watch the next video for titration calculations and further understanding of determining unknown concentrations.