This study investigates the effect of pH on the hydrolysis of acetylsalicylic acid (C9H8O4) to salicylic acid (C7H6O3) and acetic acid (C2H4O2) at a temperature of 333.15 K (60°C). The hydrolysis reaction was systematically analyzed by measuring the concentration of salicylic acid using spectrophotometry across a range of pH levels (2.0, 4.0, 6.0, 8.0, and 10.0). The results reveal a clear trend: as the pH increases, the concentration of salicylic acid also increases. This observation indicates that acetylsalicylic acid exhibits reduced stability in more basic conditions, leading to a higher rate of hydrolysis in alkaline environments.

The findings support the hypothesis that the hydrolysis rate of acetylsalicylic acid is indeed pH-dependent, with higher pH levels significantly accelerating the reaction. This conclusion is consistent with previous research and enhances our understanding of the chemical behavior of aspirin under varying pH conditions. Specifically, the data suggest that the stability of acetylsalicylic acid decreases as the environment becomes more alkaline, resulting in increased formation of salicylic acid.

These results have important implications for pharmaceutical sciences and medicine. The pH-dependent hydrolysis of acetylsalicylic acid highlights the necessity of considering the pH of the gastrointestinal tract when evaluating the stability and absorption of aspirin. In the acidic environment of the stomach, aspirin remains relatively stable, while in the more basic conditions of the small intestine, it is more prone to hydrolysis. This understanding is crucial for optimizing the therapeutic efficacy of aspirin and minimizing potential gastrointestinal side effects.