How do you perform a titration with a weak base and strong acid?

To perform a titration with a weak base and strong acid, you add the strong acid to the weak base gradually while monitoring the pH.

In a titration involving a weak base and a strong acid, the weak base is usually placed in the burette and the strong acid in the conical flask. The process begins by adding a few drops of a suitable indicator into the conical flask. Phenolphthalein is often used as it changes colour at around pH 7, which is the endpoint of the titration.

The strong acid is then added drop by drop to the weak base. As the strong acid is added, it reacts with the weak base to form a salt and water. This reaction is exothermic, meaning it releases heat. The heat released can be measured using a thermometer, and this can give an indication of the progress of the reaction.

The pH of the solution in the conical flask is monitored throughout the titration using a pH meter. At the start of the titration, the pH is relatively high because the weak base is in excess. As the strong acid is added, the pH decreases. The point at which the pH changes rapidly is known as the equivalence point. This is the point at which all the weak base has reacted with the strong acid.

The titration is stopped when the indicator changes colour, indicating that the pH has reached around 7. The volume of strong acid added to reach this point is noted. This volume can be used to calculate the concentration of the weak base, using the equation for the reaction and the known concentration of the strong acid.

Remember, safety is paramount when performing a titration. Always wear safety goggles and a lab coat to protect your eyes and clothing from any potential spills or splashes.