Acetylsalicylic Acid Lab

Only available on StudyMode
  • Download(s) : 749
  • Published : November 21, 2005
Open Document
Text Preview
Acetylsalicylic Acid
September 15, 2005
September 23, 2005

The objective of this lab experiment is to prepare aspirin (acetylsalicylic acid) by reacting salicylic acid and acetic anhydride.

This purpose of this lab was to prepare aspirin using its basic components: salicylic acid and acetic anhydride. Salicylic acid and acetic anhydride, along with an acid catalyst, react to form acetylsalicylic acid (aspirin) and acetic acid. In this reaction, the hydroxyl group on the benzene ring in salicylic acid reacts with acetic anhydride to form an ester functional group. The acetylsalicylic acid crystallizes as the solution cools and begins to come out of the solution. The acetylsalicylic acid is further purified through recrystallization with ethyl acetate.

Test TubesPasteur Pipette
Salicylic acidacetic anhydride
Sulfuric acid125 mL Erlenmeyer flask
ScaleWaterHot water bath
Ice BathBuchner Fünnel
1% Ferric Chloride
Ethyl acetateGlass Rod
Iodine Aspirin Tablet
Commercial Aspirin tablet

Part A
1.2.0 g of salicylic acid was placed in a 125 mL Erlenmeyer flask. 2.5.0 mL of acetic anhydride was added to the flask and five drops of concentrated sulfuric acid was also added. 3.The flask was swirled to dissolve the salicylic acid.

4.The flask was placed in a hot water bath for ten minutes. 5.The flask had to be placed in an ice bath briefly and the sides were scratched with a glass rod until crystallization occurred. 6.50 mL of water was added and the flask was returned to the ice bath for another five minutes. This allowed for more crystallization to occur. 7.The solution was placed in vacuum filtration using a büchner funnel for five minutes. Distilled water was added to the flask to flush solution off the sides of the flask to be poured into funnel for filtration. 8.The remaining product was allowed to air dry and was weighed. The product weight was 2.88 g. 9.The percentage yield of the product was 11.02 percent.

Part B
This experiment was performed to determine if their was any salicylic acid left in the product. 1.Three test tubes were filed with .5 mL of water.
2.Small portions of the product were added to two test tubes, while the third was filled with water to act as the control. 3.One drop of Ferric Chloride solution was added to each tube. 4.The test tubes containing product turned into a tan/peach color while the control remained yellow. The concluded that the product had little to no salicylic acid present.

Part C
1.3 mL of hot ethyl acetate was added to a small Erlenmeyer flask. 2.Product from the previous experiments was added to the flask. 3.The solution was placed in a hot water bath until dissolved and then placed in an ice bath and scraped with a glass rod until crystallized. 4.The solution was vacuum filtered until dry.

5.The ferric chloride purity test was performed on the new product. The same results from Part B occurred, further proving that the previous solution had little to no salicylic acid. 6.The melting point was determined by using a "melting point apparatus"(?) The melting point of the product was 131°C.

Part D
1.The purified product, ¼ an aspirin tablet, and ¼ a commercial aspirin tablet were each placed in separated test tubes. 2.2 mL of water was added to each tube and each tube was boiled in a hot water bath. 3.A drop of iodine solution was added to each test tube to test the presence of starch. Starch was only present in the regular aspirin tablet, which turned into a violet blue color after having the iodine added to it.

Part A
•2.0g Salicylic acid(s) + 5.0 mL acetic anhydride(aq) + 5 drops sulfuric acid  2.88g acetylsalicylic acid + acetic acid Percentage yield= 11.02%

Part B
Test Tubes w/ ferric chlorideProduct Added?Result
Tube #1YesSolution turned tan/peach color (pure)
Tube #2YesSolution...
tracking img