The graphs labeled (a) and (b) show the titration curves for two equal-volume samples of bases, one weak and one strong. Both titrations were carried out with the same concentration of strong acid.
(ii) Which graph corresponds to the titration of the strong base and which one to the weak base?

Key Concepts

Titration Curves

Titration curves graphically represent the pH change of a solution as a titrant is added. The shape of the curve is influenced by the strength of the acid and base involved. Strong acids and bases typically show a steep rise in pH near the equivalence point, while weak acids and bases exhibit a more gradual change due to their incomplete dissociation.

Strong vs. Weak Bases

Strong bases, such as sodium hydroxide, completely dissociate in solution, leading to a rapid increase in pH when titrated with a strong acid. In contrast, weak bases, like ammonia, only partially dissociate, resulting in a slower pH change. This fundamental difference affects the shape and steepness of the titration curve.

Equivalence Point

The equivalence point in a titration is reached when the amount of titrant added is stoichiometrically equivalent to the amount of substance in the solution being titrated. At this point, the pH of the solution can vary significantly depending on whether a strong or weak base is involved, influencing the overall shape of the titration curve.