Determine whether each of the following statements concerning the titrations in Problem 17.35 is true or false. (b) The titration curves will both be essentially the same after passing the equivalence point.

Verified step by step guidance

1. Identify the acids involved in the titration: chloric acid (HClO3) and formic acid (HCOOH).
2. Recognize that chloric acid is a strong acid and formic acid is a weak acid.
3. Understand that after the equivalence point, the titration curve is determined by the excess titrant, which is typically a strong base.
4. Note that the behavior of the solution after the equivalence point is dominated by the excess strong base, making the titration curves similar.
5. Conclude that the statement is true because the titration curves will both be essentially the same after passing the equivalence point due to the presence of excess strong base.

Key Concepts

Titration Curves

Titration curves graphically represent the pH 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 at the equivalence point, while weak acids and bases exhibit a more gradual change. Understanding these curves is essential for predicting the behavior of the solutions after the equivalence point.

Equivalence Point

The equivalence point in a titration occurs when the amount of titrant added is stoichiometrically equivalent to the amount of substance in the solution being titrated. At this point, the reaction between the acid and base is complete, and the pH can change dramatically depending on the strengths of the acids and bases involved. Recognizing the equivalence point is crucial for interpreting titration curves and determining the outcome of the titration.

Strength of Acids

Acids can be classified as strong or weak based on their ability to dissociate in water. Strong acids, like chloric acid, completely ionize in solution, leading to a higher concentration of hydrogen ions. Weak acids, such as formic acid, only partially dissociate, resulting in a lower concentration of hydrogen ions. This distinction affects the shape of the titration curve and the pH after the equivalence point, making it vital for understanding the comparison between the two solutions in the question.