Kinetics of alkaline hydrolysis of ethyl acetate

I. INTRODUCTION
Chemical kinetics The study of chemical reaction rate and its influencing factors is essential for in-depth understanding of chemical reaction mechanism. As a typical organic reaction, alkaline hydrolysis of ethyl acetate is of great significance in the field of chemistry.

II. EXPERIMENTAL PRINCIPLE
Ethyl acetate ($CH_3COOC_2H_5 $) reacts with sodium hydroxide ($NaOH $) to form sodium acetate ($CH_3COONa $) and ethanol ($C_2H_5OH $). The reaction formula is: $CH_3COOC_2H_5 + NaOH\ longrightarrow CH_3COONa + C_2H_5OH $. This reaction is a second-order reaction, and the reaction rate is proportional to the product of the concentration of ethyl acetate and sodium hydroxide. The reaction rate constant can be determined by monitoring the concentration of a reactant or product over time during the reaction.

III. Experimental Materials and Methods
(I) Experimental Materials
1. ** Pharmaceuticals **: ethyl acetate, sodium hydroxide, phenolphthalein indicator, distilled water.
2. ** Instruments **: thermostatic tank, magnetic stirrer, conical flask, pipette, alkaline burette.

(II) Experimental Steps
1. ** Preparation of Solution **: Accurately prepare a certain concentration of ethyl acetate and sodium hydroxide solution.
2. ** Constant Temperature Treatment **: Adjust the thermostatic tank to the set temperature, and place the conical bottle containing the reactant solution into the thermostatic tank at constant temperature for a period of time.
3. ** Reaction Start **: Quickly pour the ethyl acetate solution into the sodium hydroxide solution, turn on the magnetic stirrer and stopwatch at the same time, and start recording the reaction time.
4. ** Sampling Titration **: At different reaction times, take out a certain amount of the reaction solution accurately with a pipette, quickly add excess hydrochloric acid to stop the reaction, use phenolphthalein as an indicator, titrate the remaining hydrochloric acid with the sodium hydroxide standard solution, and record the volume of the sodium hydroxide solution consumed by titration.

IV. Experimental Results and Analysis
1. ** DATA RECORD **: Record the different reaction times $t $and the corresponding titration consumption of sodium hydroxide solution volume $V $.
2. ** DATA PROCESSION **: According to the reaction principle and titration data, calculate the concentration of the reactants at different times, and plot with 1 dollar/c $vs. $t $ ($c $is the concentration of the reactants). A straight line can be obtained. The slope of the straight line is the reaction rate constant $k $.
3. ** RESULTS ANALYSIS **: Analyze the influence of factors such as temperature and the initial concentration of the reactants on the reaction rate constant, compare with theoretical expectations, and explore the source of error.

5. CONCLUSION
The alkaline hydrolysis kinetics of ethyl acetate was studied experimentally, and the reaction rate constants were successfully determined to understand the influence of various factors on the reaction rate. This experiment provides important data support for the optimization of related chemical processes and theoretical research, and is of great value for in-depth understanding of the kinetic mechanism of organic reactions.