In this lab, the kinetics of a solvolysis reaction was analyzed. The reactions rate was also investigated during this lab to understand the affects a solvents polarity has on the reaction. To achieve this, two titrations were performed, one for solution 1 and one for solution 2. For the first titration, a buret with 49mL of stock NaOH was use to titrate solution 1. Solution 1 consisted of 25mL of absolute ethanol, 25mL of water and five drops of bromthymol blue. The solution changed from clear to yellow when the bromthymol blue was added. When the initial volume of 49 mL of NaOH and the initial time of zero was recorded, about 2mL of alkyl chloride was added. The timer was started at this point and 2mL of NaOH was added to solution 1. It instantly turned blue when the base was added, but after 184 seconds, the solution turned green.…show more content… After this, 2mL of NaOH was added again. Once the solution was green, the time was recorded. This was done a total of 6 times. The solution turned green at 184 seconds, 440 seconds, 650 seconds, 855 seconds, 1032 seconds, and 1235seconds. The table below shows the buret readings and the time in which each part turned to green. There is an extra data point in this run, because on the sixth addition of NaOH, the solution was not allowed to go all the way to yellow and the time was recorded. For V∞, time should not be recorded. This extra data point can be a source of error because it dose effect the slope of this run. Ideally with this extra data point, the slope will be more precise for this run, but this slope is not equal to the slope if only five data points were used. This error can be prevented by allowing the solution after the sixth addition to proceed all the way to yellow. Once the solution did proceed to yellow, it was heated for 15 minutes. The whole time it was heated, and throughout to titration, the solution was being