The saponification of ethyl acetate and sodium hydroxide
is related to the reaction between esters and bases. Now, the saponification of ethyl acetate and sodium hydroxide is the secret of its kinetics.

1. Experimental rationale
Ethyl acetate ($CH_3COOC_2H_5 $) meets sodium hydroxide ($NaOH $), and the saponification reaction is caused by sodium acetate ($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 secondary reaction. In the constant volume environment, the reaction rate is proportional to the concentration of ethyl acetate and sodium hydroxide. Assuming that the concentration of ethyl acetate and sodium hydroxide is $a $at the beginning, and the concentration of both is $x $at a certain time, the speed equation is: $v = k (a - x) ^ 2 $, $k $, the rate constant is also.

Second, the experimental method
1. ** Preparation **: Take pure ethyl acetate, sodium hydroxide, phenolphthalein test solution, distilled water, etc., and prepare graduated volumetric bottles, pipettes, conical bottles, thermostatic water baths, magnetic stirrers, stopwatches, etc.
2. ** Liquid preparation **: Use volumetric bottles to accurately prepare a certain concentration of ethyl acetate solution and sodium hydroxide solution.
3. ** It should be noted **: The two solutions are placed in a constant temperature water bath. After reaching a predetermined temperature, take an appropriate amount of sodium hydroxide solution and inject it into a conical bottle containing ethyl acetate solution. At the same time, start the stopwatch and use a magnetic stirrer to homogenize it so that it should be homogenized.
4. ** Concentration measurement **: After a certain period of time, take the solution and titrate the remaining sodium hydroxide with a standard acid solution. With phenolphthalein as an indicator, the solution changes from red to colorless as the titration end point. Remember the amount of acid consumed, push the concentration of the remaining sodium hydroxide, and then know the concentration of each substance in the reaction process.

III. Analysis of data
1. ** Number of records **: Remember the volume of acid consumed by each titration, when it should be, etc.
2. ** Calculate concentration **: According to the principle of titration, calculate the concentration of sodium hydroxide at each time, and the concentration of ethyl acetate is the same from the formula.
3. ** Find the value of $k $**: Substitute the concentration data at different times into the second-order reaction rate equation integral formula $\ frac {1} {a - x} -\ frac {1} {a} = kt $, plot $\ frac {1} {a - x} $against $t $, and get a straight line with a slope that is the rate constant $k $.

4. Conclusion
Through this experiment, the kinetic characteristics of the saponification reaction of ethyl acetate and sodium hydroxide are known, and the method of calculating the rate constant is known. The procedure of the experiment must abide by the rules of operation, so as to obtain the exact number, which is essential for the research and work of the chemical industry.