Aspirin Lab Report

Aspirin, Caffeine and Salicylamide were extracted from an over-the-counter pain reliever (BC Powder). These components were separated by manipulating their solubilities by adjusting the acidity and basicity of the solution. By doing this, the three components were forced into conjugate acid (or base) forms, causing selective solubility in either an aqueous or organic solvent. These layers were then separated by use of a separation funnel. Once separated, the components extracted were characterized by measuring the melting point and performing a TLC analysis. Also, the recovered aspirin from the first part of the experiment was recrystallized and compared to that of the

The synthesis of acetaminophen involves the attraction of the electrophilic carbonyl group of acetic anhydride to the nucleophilic NH2

Aspirin was synthesized by reacting salicylic acid with acetic anhydride in the presence of phosphoric acid, H3PO4, as a catalyst:

The goal of this experiment was to synthesize aspirin. In this experiment aspirin, also known as acetylsalicylic acid, was synthesized from salicylic acid and acetic anhydride. In the reaction the hydroxyl group on the benzene ring in salicylic acid reacted with acetic anhydride to form an ester functional group. This method of forming acetylsalicylic acid is an esterification reaction. Since this esterification reaction is not spontaneous, sulfuric acid was used as a catalyst to initiate the reaction. After the reaction was complete some unreacted acetic anhydride and salicylic acid was still be present in the solution as well as some sulfuric acid, aspirin, and acetic acid. Crystallization, which uses the principle of

24) Separate the formed crystals (benzoin) and allow them to dry, then take the MP.

Ever wonder about the chemical makeup of tablets that people take for pain relief? Before a tablet can be successfully made, the limiting and excess reactants must be considered. The limiting reactant will affect the amount of the product that can be made. Another reason why the starting reactants must be determined carefully is to make reduce the amount of the reactant in excess so that reactants are not wasted. This experiment uses an Alka-Seltzer tablet. Alka-Seltzer dissolves in water and is an antacid and a pain reliever1. The Alka-Seltzer tablet has many uses such as relief of headaches, ingestion, heart burns, or even upset stomachs2. The active ingredients in an Alka-Seltzer tablet is aspirin, also known as acetyl-salicylic acid (C8H12O4), citric acid (C6H8O7), and sodium bicarbonate (NaHCO3)2. The aspirin in the Alka-Seltzer tablet helps with pain relief. Because of the acid-base chemistry (Brønsted-Lowry), citric acid and sodium bicarbonate produce O2, which makes the tablet fizz when it is dropped in liquid. The Brønsted-Lowry theory shows how the Brønsted-Lowry acid donates a hydrogen ion while the Brønsted-Lowry base accepts the hydrogen ions3. The remaining NaHCO3 that is in excess post reaction with the citric acid is what is used to neutralize stomach acid which helps relief heart burn2. The problem in

Industrial production of Aspirin is dependent on the company producing the drug; however the general method of production is known as slugging or dry-granulation. In this method, corn starch is mixed with pure water and is then heated and

The aspirin crystals were washed by pouring 10 mL of water over them through the funnel.

The purpose of the lab was to synthesize aspirin and oil of wintergreen, and to determine its purity using recrystallization process, determining its melting point and using back-titration. To synthesize aspirin, salicylic acid and anhydride was used to drive the reaction to completion. In the synthesis of oil of wintergreen we reacted salicylic acid and methanol to produce methyl salicylate. This reaction is an example of a condensation reaction where the carboxylic acid and alcohol group combine to form an ester. In producing aspirin, we wanted to obtain the purest form, so we removed impurities such as unreacted salicylic acid and acetic acid. Acetic acid was removed by rinsing the sample in water because acetic acid is soluble in water. Salicylic, however, was removed by using the recrystallization process because it is insoluble in water. To recrystallize, we dissolved a sample of crude aspirin in warm ethanol and let it cool. Because aspirin is less soluble in ethanol than salicylic acid, it will crystallize out of the solution. To obtain the purified aspirin sample, we then filtered the solution to separate it from the impurities. To determine qualitatively the purity of the recrystallized aspirin, we determined its melting point using a melting point apparatus. Using the idea of freezing point depression, the presence of impurities will lower the melting point of the substance. Thus, by comparing the melting point to the actual

Aspirin also known as acetylsalicylic acid is a salicylate drug, often used as an analgesic to relieve minor aches and pains, as an antipyretic to reduce fever, and as an

1. Fill up a 200ml beaker with tap water and then pour it into the designated jar

Place 100 ml of distilled water in a 250-ml (or 400-ml) beaker. Add 1.26g of oxalic acid dihydrate (H2C2O4.2H2O) and 1 ml of concentrated ammonia. Stir the mixture until the solid has dissolved completely.

2) Rinse the solid with about 30 mL of distilled water and decant the liquid from the solid. It is critical that as little solid as possible is lost during this process. Repeat the rinsing two or three times.

2. Add about 20 mL of distilled water and stir the mixture with a glass stirring rod to dissolve the sample. There may be a small amount of insoluble residue. If your sample does not dissolve completely, remove the insoluble material by filtration.

This report presents the synthesis of Aspirin (acetylsalicylic acid), as the product of the reaction of salicylic acid with ethanoic anhydride under acidic conditions. Aspirin was purified through recrystallisation by vacuum filtration, followed by desiccation of the Aspirin crystal over silica gel. The percentage yield was calculated as 44.89% and a sample of Aspirin was analysed using infra-red spectroscopy and compared to the spectrum of pure Aspirin, this served as an introduction to the identification of functional groups in organic compounds. The melting point was calculated using an IA9000M apparatus and recorded to be 35.2°C, which was slightly below the melting point of pure Aspirin; known to be between 138-140°C. Both IR spectroscopy and melting point measurement were used verify the purity of synthetic Aspirin made, which proved to be fairly pure under these laboratory conditions.