Aim The aim of this experiment was to use the Spectrophotometer to determine the milligrams of acetylsalicylic acid (aspirin) in a commercial aspirin product and to compare the mass of acetylsalicylic acid in various commercial aspirin products. 0.04g of synthesised aspirin and transfer it to a 25ml beaker. Swirl to dissolve. TLC analysis showed that Add 15ml of distilled water to the beaker. 1. Before humans had the luxury of pain relievers and pharmaceutical drugs, many relied on the curing effects of willow tree bark, which was either chewed or boiled and used to relieve fevers and inflammation. In order to determine the purity of the aspirin, it must be characterized through various techniques based on an understanding of the energy of the system on the microscopic and atomic scale. The theoretical yield was 2.520 grams. This experiment clearly verified that you can make aspirin via esterification, and that we were able to determine a percent yield as a lab group. Clearly, acetic anhydride (alcohol) reacts with salicylic acid (acid) to yield the ester (aspirin), as was shown by the crystals that formed and dried over a week that measured in at 2.28g. The aspirin will be characterized by three methods: melting point analysis, Fourier transform infrared spectroscopy (FTIR), and Fourier transform Erlenmeyer flask. Titration of Aspirin Tablets. In the following experiment, Aspirin was synthesized and analyz… Reactions: Procedure and Results: Aspirin Synthesis Tap water was heated on a steam bath in a 250 mL beaker. The amount of crude aspirin synthesized was 3.029 grams and the amount of pure aspirin synthesized was 2.169. determine if pure aspirin was synthesized. be done by weighing 0.5g of the aspirin prepared in the previous experiment into a clean. In this lab, you will determine the percent purity of two commercially available aspiring tablets using an acid-base titration. Add 1ml of Ethanol to the beaker of aspirin. Prepare the synthesized aspirin sample for testing. Purpose: To determine which of four catalysts yields the fastest reaction rate in the acetylation of salicylic acid (1) to form acetylsalicylic acid (2). This can. Complete this step quickly; Measure approx. Mix the solution. Record the mass of aspirin weighed to the nearest 0.001g. Thus, there was a percent error of 13.93 % and percent yield of 86.07%. Then, the aspirin product was dissolved in water and titrated with both solutions to find the percent purity of the aspirin, which was found to be 99.6% pure. 25ml of alcohol is then added into the flask to dissolve the aspirin and two. This is an extremely high purity, which coincides with the quantitative analysis done in Part 1. The temperature of an alcohol thermometer was equilibrated in a beaker of room temperature tap water. Aspirin, acetylsalicylic acid, is a familiar drug, used for relieving cold and flu symptoms, fevers, and general aches and pains in the body, and, as made clear by its chemical formula, contains salicin a chemical found in willow bark. In general, an acid and a base react to produce a salt and water by transferring a proton (H+): HA (aq)+ NaOH (aq) H2O (l)+ NaA (aq)(1) Thus, it is doubtful that there are very many sources of error. The purity of aspirin or acetylsalicylic acid can be analyzed by using acid-base titration. Synthesis of Aspirin By: Jon Torre.