Lecture on Acid-Base Titration

Introduction to Titration

• Acid-Base Titration: A method to determine the concentration of an acid or base in a solution.
• Process: Involves measuring the volume of a titrant (acid or base) needed to completely react with the solution.
• Comparison to Stoichiometry: Similar concept, involving precise measurements and calculations.

Titration Curve

• Plot: pH is plotted against the volume of titrant added.
• Behavior of pH:
  • Initially rises slowly as base is added.
  • Sharp rise near the equivalence point.
• Equivalence Point: The point where the amount of titrant added exactly neutralizes the acid in the solution.

Indicators

• Function: Substances used to signal the equivalence point by changing color.
• Example: Sharp color change indicates that the equivalence point has been reached.

Equivalence Point Details

• Strong Acid with Strong Base: Equivalence point at pH 7.
• Weak Acids/Bases: Equivalence point will differ from 7.

Example Problem

• Given: A sodium hydroxide solution of unknown concentration.
• Reactants: 3.0M sulfuric acid used to titrate 25 mL of sodium hydroxide.
• Result: 11.6 mL of acid required to reach equivalence point.
• Calculation:
  • Convert volumes to liters.
  • Use conversion factors and stoichiometric ratios to determine reactant concentrations.

Conclusion

• Purpose: Understanding the process and calculation in titration helps determine unknown concentrations.
• Next Steps: Practice with various examples to solidify understanding.

Remember to subscribe for more tutorials and feel free to reach out via email with questions.