On the Solubility of Aspirin in Ethyl Acetate
Introduction
The dissolution characteristics of substances are of key significance in chemical exploration and practical application. Aspirin, a commonly used drug, its solubility in different solvents affects its preparation, dosage form development and efficacy. Ethyl acetate, as a common organic solvent, studies the solubility of aspirin in it, which may provide important basis for related fields.

Experimental Preparation
1. ** Materials **: Pure aspirin samples to ensure that their purity is up to standard and no impurities interfere with the experiment; analysis of pure ethyl acetate to ensure the quality of the solvent.
2. ** Instrument **: Accurate balance, used to accurately weigh the quality of aspirin; several corked conical bottles for dissolution experiments; constant temperature water bath device to maintain a stable temperature environment; stirring utensils to accelerate the dissolution process.

Experimental process
1. In a series of corked conical bottles, add quantitative ethyl acetate respectively. Use the balance to accurately weigh different quality aspirin, and add each conical bottle in turn.
2. Place the conical bottle in a constant temperature water bath device, set a specific temperature, and turn on stirring to fully dissolve the aspirin. During the process, closely observe and record the dissolution.
3. Continue stirring until the aspirin dissolves in equilibrium, that is, there is no obvious dissolution change over a period of time.

Results and analysis
1. The solubility of aspirin in ethyl acetate is different at different temperatures. With the increase of temperature, the solubility shows an upward trend. This is due to the increase of temperature, the thermal movement of molecules intensifies, and the interaction between aspirin and ethyl acetate molecules is enhanced, which is conducive to dissolution.
2. The data are recorded in detail in the table below (the temperature-solubility correspondence table can be listed here according to the hypothetical data). Through data analytics, the relationship between solubility and temperature can be fitted, providing an intuitive reference for subsequent related studies.

Conclusion
This experiment explores the solubility of aspirin in ethyl acetate, and clarifies the effect of temperature on its solubility. This research result may provide theoretical support for the research and development of aspirin-related preparations, solvent selection and process optimization in the production process. Future research can be further expanded to consider the role of more influencing factors, such as pressure, impurities, etc. on the solubility, in order to improve the understanding of this field.