why is glacial acetic acid used in this reaction_why is glacial acetic acid used in this reaction

Glacial acetic acid, also known as ethanoic acid, is a colorless liquid with a sharp, pungent odor. It is widely used in various industrial and laboratory applications, including food preservation, the manufacture of plastics and synthetic fibers, and as a solvent in chemical reactions. However, despite its versatility, it is essential to acknowledge the hazards associated with glacial acetic acid. Understanding these risks is crucial for ensuring safety in its use and handling.

The boiling point of glacial acetic acid is approximately 118.1°C (244.58°F). This relatively high boiling point can be attributed to the strong intermolecular forces present in the liquid. Specifically, glacial acetic acid molecules engage in hydrogen bonding with one another, resulting in a more stable liquid structure that requires more energy (in the form of heat) to break these bonds and transition into the gaseous state. Hydrogen bonding arises because of the presence of a hydroxyl (–OH) group in acetic acid, which allows for the interaction between the hydrogen atom of one molecule and the oxygen atom of another.

Both glacial acetic acid and ethyl acetate can be found in many commercial products, but their applications differ slightly due to their unique properties. While glacial acetic acid serves as a chemical precursor and a reagent, ethyl acetate primarily functions as a solvent. In laboratories, glacial acetic acid is often used in titrations and for purposes requiring acidity, while ethyl acetate is regularly employed for extraction and purification processes.

Apart from purity, temperature significantly influences the density of glacial acetic acid. As temperature increases, most liquids expand and their density decreases. Consequently, it is crucial to maintain consistent temperature conditions when measuring the density of glacial acetic acid to ensure accurate results. For instance, at higher temperatures, the density may decrease to approximately 1.04 g/mL, while at lower temperatures, it can increase. This temperature dependence highlights the importance of calibrating measurement devices accordingly.