Exploring the Equivalence Point of Acetic Acid Titration

What is the equivalence point when the weak acid acetic acid is titrated with NaOH?

A) 4.3 B) 7 C) 8.7 D) 14

Final Answer:

The equivalence point when acetic acid is titrated with NaOH is pH 8.7

When conducting a titration of acetic acid with NaOH, it is essential to determine the equivalence point. In this case, the equivalence point can be determined by understanding the properties of the weak acid, acetic acid, and the strong base, NaOH.

The final answer for the equivalence point is pH 8.7. This means that when the acetic acid is completely neutralized by the NaOH, the resulting solution will have a pH of 8.7. This is slightly basic, indicating that the solution becomes more basic as the titration progresses.

The reason for the pH of 8.7 at the equivalence point can be explained by the reaction between acetic acid and NaOH. Acetic acid is a weak acid, so it does not completely ionize in solution. At the equivalence point, the acetate ions formed by the reaction between acetic acid and NaOH react with water to produce hydroxide ions (OH-), which results in a basic solution. This shift towards basicity causes the pH to be greater than 7, landing at 8.7 in this specific titration.

Understanding the equivalence point in titrations is crucial for determining the concentration of solutions and identifying the stoichiometry of the reaction. By recognizing the pH at the equivalence point, chemists can accurately calculate the amount of acid or base present in the solution and make informed decisions about chemical processes.