Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH.
(i) Which acid solution is more concentrated?

Key Concepts

Titration Curves

Titration curves graphically represent the pH of a solution as a function of the volume of titrant added. For weak acids, the curve typically shows a gradual increase in pH, followed by a steep rise at the equivalence point. The shape and position of the curve can provide insights into the concentration and strength of the acids being titrated.

Weak Acids and Their Concentration

Weak acids partially dissociate in solution, meaning that not all acid molecules release protons (H+). The concentration of a weak acid affects the initial pH and the steepness of the titration curve. A more concentrated weak acid will generally have a lower initial pH and a more pronounced change in pH near the equivalence point compared to a less concentrated solution.

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. For weak acids titrated with a strong base like NaOH, the equivalence point is characterized by a rapid increase in pH. Analyzing the position of this point on the titration curve can help determine the concentration of the acid.