Part 3: Preparation and Standardization of HCl Procedure Part 4: Quantitative Analysis of Aspirin Further Analysis Conclusion The overall objectives of
Section VI – Post-lab: Give a source of error in this experiment. https://phdessay.com/synthesis-of-aspirin/, Synthesis of Cinnamaldehyde from Benzaldehyde. Purify the rest of the aspirin by recrystallization. Büchner Funnel (1)
A precipitate formed as the solution cooled.
The accuracy of this lab could be improved with more precise equipment, allowing the experimenter to be more confident in the accuracy of the measurements obtained. Weigh a piece of filter paper and vacuum filter the product. 7. a. Polar what are the types of gas leak detection system? Rubber Stopper (1) Sample Calculations . It let's us know not just the composition of reactants and products but their structure as well.
81. Another source of error could have been due to the transport of the aspirin from the Erlenmeyer flask after cooling to the funnel to be filtered. Be careful not to heat the water bath above 85 ˚C.
Safety goggles must be warn at all times in this lab. Remove the flask from the water bath and slowly add ten drops of deionized water to convert any excess acetic anhydride to acetic acid. In the presence of moisture, aspirin may decompose (hydrolysis) into salicylic acid and acetic acid. The purity of the aspirin is determined by melting point determination and infrared spectroscopy.
After heating, then cooling and scratching the solution, a white precipitate formed. Assemble a Büchner funnel and filter flask as shown in the figure. Weighed the piece of filter paper with the aspirin on it. Q2: If 0.150 moles of salicylic acid and excess acetic acid are used during a synthesis of aspirin, how many grams of aspirin will be obtained if the reaction gives a 38% yield?
Weighed out 1.5g of salicylic acid on a piece of filter paper. Compare the literature melting point and infrared spectrum to the experimental and comment on the purity of your aspirin. The boiling chips (calcium carbonate) were white, opaque crystals.
It has been present for over one hundred years and is one of the most widely used medications in the world. If crystals do not appear scratch the walls of the flask with a stirring rod to induce crystallization. Gas building in a sealed container is the primary cause of laboratory explosions and heating the beaker to high or not providing sufficient space around the Erlenmeyer flask may produce an explosion. 1.51g C7H6O3 x 1 mole C7H6O3 x 1 mole C9H8O4 x 180.154 g C9H8O4 138.118 g C7H6O3 1 mol C7H6O31 mol C9H8O4 When your aspirin is dry, record the mass of the filter paper + aspirin. First, convert both masses to moles. Answer the following post-lab question: If 0.150 moles of salicylic acid and excess acetic acid are used during a synthesis of aspirin, how many grams of aspirin will be obtained if the reaction gives a 38% yield? 1,2-dibromo-1,2-diphenylmethane Learn. STUDY.
2.Sometimes When You Open An Old Bottle Of Aspirin You Can Detect A "vinegar-like" Smell. The limiting reactant of the equation was salicylic acid.
Recrystallization is a common method of purifying organic substances through the differences in solubility at different temperature. 60. Hot Plate Poured the acetic anhydride into the 50 mL Erlenmeyer flask containing the salicylic acid.
C3 - Knowing the maximum theoretical yield, and your actual yield, for this reaction calculate the percent yield for your experiment.
95% Ethanol In this experiment, acetanilide was produced by acetylation of aniline with acetic anhydride.. After the solid dissolved, added about 15 mL of distilled water. From that structure we can begin to understand why and how chemical reactions occur. Inaccurate calibrations of the hot plate or balance could have shown higher or lower quantitative data which would have affected the results by producing either a higher or lower percent yield. The active metabolite ingredient in acetylsalicylic acid (aspirin) is salicylic acid (Wikipedia, Salicylic acid, 2013), which was first discovered by Edward Stone in 1763 (Wikipedia, Aspirin, 2013).
custom paper from our expert writers, Synthesis of Aspirin. Rinsed the dirty apparatus thoroughly with lots of water. This is accomplished by dissolving the acid in warm ethyl alcohol, adding cold water, and then allowing it to recrystallize in an ice bath. Section I – Procedure: summarize the procedure using a flow chart format.
Other than being used in the production of aspirin, acetic anhydride is used to convert cellulose to cellulose acetate, a key component in photographic film and other coated materials (Wikipedia, Acetic anhydride, 2013). Results.
15. The main objective of the synthesis of aspirin lab was so produce aspirin (acetylsalicylic acid) through the reaction of salicylic acid and acetic anhydride. It has become very common as an antiplatelet to prevent blood clot formation and is used to prevent heart attacks and strokes.
The aspirin formed will be contaminated with acetic acid and must be purified by recrystallization. Heat it for fifteen minutes with occasional stirring. In this experiment, you will prepare aspirin from salicylic acid and acetic anhydride using sulfuric acid as a catalyst.
It is necessary to consider resonance forms of intermediate structures.
Aspirin: yellow/orange. we did a lab at school where we made aspirin (ASA) i couldn't figure this one out Why did you add hot water to the crystals, and then cool the mixture?
1 mole is equal to the molar mass of a substance; therefore, the grams of acetic anhydride and grams of salicylic acid must be divided by their molar masses respectively. Sulfuric acid has many applications, such as pigments, explosives, lubricants, batteries, antifreeze, and detergents. Theoretical yield1.969566168g. In the fume hood, add approximately 3.5 - 4.0 mL of acetic anhydride to the flask containing the salicylic acid and stopper it. Q1: Give a source of error in this experiment. This is just a sample. The salicylic acid was a find, white solid powder. Measured out 5.0 mL of acetic anhydride in a graduated cylinder from the fume hood.
; Heat the flask gently on the steam bath for at least 10 minutes.
Water is LIGHTEST in what region?
Preparing esters from an alcohol and a carboxylic acid using an acid as catalyst is one of the most useful reactions in an organic chemists toolbox. 2. Don't use plagiarized sources. A contamination of the substances used or the glassware could have caused the substances to react differently with each other, again causing the percent yield to change depending on how the contamination affected the substances by producing a higher or lower percent yield. Stir to dissolve it completely, and then add 5 mL of warm (70°C) deionized water. 58.
Molar mass of acetic anhydride = 4(12.01) + 6(1.008) + 3(16) = 102.088g Molar mass of salicylic acid = 7(12.01) + 6(1.008) + 3(16) = 138.118 g, Acetic anhydride: 5.4g C4H6O3 x 1 mole C4H6O3 l= 0.052895541 moles C4H6O3, Salicylic acid:1.51g C7H6O3 x 1 mole C7H6O3 = 0.01093268 moles C7H6O3138.118 g C7H6O3. Placed a few boiling chips in the beaker to prevent bumping if the water began to boil. Section V – Results: Comment on how well the reaction worked based on the percent yield. It is a pain reliever and a non-steroidal anti-inflammatory (NSAID). Acetylsalicylic acid is commonly used to alleviate minor aches and pains (Wikipedia, Aspirin, 2013).
These resonance forms will help you understand why a partial positive charge appears on the carbon atom in acetic anhydride and how this results in a new bond forming at that carbon. PLAY.
S Oil Dependence and how it could be fixed and changed for the best interest of the. Created by. How can one prepare aspirin through a reaction between salicylic acid and acetic anhydride? You will determine the percent yield of aspirin and you will confirm it's identity with FT-IR spectroscopic anaylsis. When the salicylic acid and acetic anhydride were mixed, a white, powdery solution formed. 13. 1. Percent error of melting point Exam 2013, Questions and Answers OChem Cheat Sheet- Alcohols and epoxides handout Lab 5 Base Extraction of Benzoic Acid from Acetanilide Long report 3 - Experiment 8: Thermochemistry and Hess Law Post-Lab 2 Organic Chemistry 3rd ed. Meltemp, Salicylic acid C2 - Using the limiting reagent calculate the maximum theoretical yield for your reaction.
The mechanism of this reaction can be understood by examining the Lewis structures of each reagent. It is effective in reducing pain (it is an analgesic), reducing inflammation (anti-inflammatory), reducing fever (antipyretic), and thinning blood (anti-coagulant).
0. Vidallon, Mark Louis P. Date Performed: February 20, 2012 CHEM44. 400 mL Beaker (2) 2.
Salicylic acid is toxic in large quantities but in small doses can be useful for food preservatives and as an antiseptic.
Recorded the volume of acetic anhydride used on the data sheet.
When the sulfuric acid was added, a clear solution formed that produced heat.
Acetic anhydride and salicylic acid are mixed together, and then acidified by the addition of a few drops of concentrated sulfuric acid, which catalyzed the reaction.
Theoretical yield c. Tropical Therefore, salicylic acid is the limiting reactant of the reaction.
It's strongly recommended that you wash all clothing worn in this lab in a single load without detergent prior to laundering them normally to preserve clothing.
The complete lab report must be typed (this includes the calculations), Prepare a cover page. 9. Add 5 mL (0.05 mole) of acetic anhydride, followed by 5 drops of conc. I don't know how you made your aspirin), side products or impurities that were present in your reagents. The moisture in the precipitate was filtered overnight and what was left over was the desired product, aspirin. aspirin product as well as a commercial aspirin tablet will be compared to a standard 0.15% ferric-salicylate solution.