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Tert-Butyl Chloride Investigation

648 Words3 Pages

Objective
The objective of the experiment was to measure and analyze the reaction rate of tert-butyl chloride with sodium hydroxide, and plot it in a graph in order to observe the rate.

Procedure Part A- Measurement of the SN1 Reaction Rate of Tert-Butyl Chloride
• 100 mL of a solution of propan-2-ol and water (1:1 ratio) were collected from a container provided by the instructor, and they were placed in a 250 mL Erlenmeyer flask, which was subsequently cork-stoppered. Afterwards, 150 mL of NaOH were acquired and placed in a beaker, and in turn this 150 mL sample of NaOH was used to fill a 50 mL buret to the highest mark, and this buret was attached to a butterfly clamp attached to a ring stand in preparation for a future step. In a 100 mL …show more content…

After 2.5 mL of NaOH had been added to the solution, the color of the solution remained blue for an acceptable amount of time. It was imperative for the experiment to be as fats as possible when performing this procedure, since there were times at which samples had to be collected. After completing this process the content of the Erlenmeyer falsk were disposed of in the halogenated waste container, and the Erlenmeyer flask was cleaned and prepared for the next steps. This same process of treating with acetone and titrating the solution was repeated at the 20, 35, and 50 minute mark, and the amounts of NaOH added to had to be recorded as well. Table 1.A was constructed in order to represent the resultant amounts of NaOH that were used and their respective time that they were added, as well as the amounts of sample and acetone that were mixed, and Calculations 1.A shows the calculations used to find the concentrations of HCl at different times, which is needed for the calculation of the rate constant. Graph 1.A represents the plot of kinetic data from the recorded results seen in this experiment, and this graph also includes the calculated slope, which is used

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3. Upon adding 20 drops of NaOH, a white precipitate was formed signifying acidic impurity. In the second NaOH mixture, about 20 drops were administered and no precipitate formed indicating that the ample is more pure than before. Data: Weight of flask = 75.10 grams Weight of the flask with solids =

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In the first part of the experiment, Part A, the standard solutions were prepared. As a whole, the experiment was conducted by four people, however, for Part A, the group was split in two to prepare the two different solutions. Calibrations curves were created for the standard solutions of both Red 40 and Blue 1. Each solution was treated with a serial 2-fold dilution to gain different concentrations of each solution.

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Conclusion: Based on the results of molarity from Trials 1, 2, and 3, it is concluded that our experimental for each trial is .410M NaOH, .410M NaOH, and .450M NaOH. The actual molarity of the NaOH concentration used was found to be 1.5M NaOH. The percent error of the results resulted in 72%. The large error may have occurred due to over titration of the NaOH, as the color of the solution in the flask was a darker pink in comparison for the needed faint pink. Discussion of Theory:

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In addition, phenolphthalein was added as an indicator. The aliquots were titrated against sodium hydroxide (NaOH) solution until end point was reached, after which volume of NaOH consumed was recorded. The value of the rate constant, k, obtained was 0.0002 s-1. The experiment was then repeated with 40/60 V/V isopropanol/water mixture and a larger value of k = 0.0007 s-1 was obtained. We concluded that the rate of hydrolysis of (CH3)3CCl is directly proportional to water content in the solvent mixture.

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