Preparation of aspirin experiment. CHM457 LAB REPORT 4 Preparation of Acetylsalicylic Acid (Aspirin) 2022-12-12

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Aspirin, also known as acetylsalicylic acid, is a common pain reliever and fever reducer. It is widely used in both over-the-counter and prescription medications. The preparation of aspirin involves a chemical reaction called esterification, which involves the reaction of an acid and an alcohol. In this experiment, salicylic acid will be used as the acid and methanol as the alcohol.

Before starting the experiment, it is important to gather all necessary materials and equipment. These may include:

It is also important to wear appropriate personal protective equipment, such as goggles and lab coat, to ensure the safety of the experimenter.

To begin the experiment, the round bottom flask should be placed on the stir plate and the stir bar should be added to the flask. Next, add 5.0 grams of salicylic acid and 5.0 mL of methanol to the flask. The mixture should be stirred until the salicylic acid is fully dissolved.

Next, add 5 drops of sulfuric acid to the mixture and continue stirring. The sulfuric acid acts as a catalyst in the esterification reaction and helps to increase the reaction rate. The mixture should be heated to a temperature of around 70-80°C, using a heating mantle or hot water bath. It is important to monitor the temperature using the thermometer and to maintain the temperature within this range throughout the reaction.

Once the mixture has reached the desired temperature, the reflux condenser should be attached to the round bottom flask. The reflux condenser helps to prevent the loss of volatile reactants and products during the reaction. The reaction should be allowed to proceed for approximately 2-3 hours, or until the theoretical yield of aspirin is obtained.

After the reaction is complete, the mixture should be cooled to room temperature and then filtered using a vacuum filtration setup. To do this, the vacuum pump should be connected to the vacuum hose, which is then connected to the vacuum filter flask. The vacuum filter flask should be placed on the vacuum filtration flask stand and secured using the vacuum filtration flask clamp. The vacuum filtration paper should be placed on the Buchner funnel, which is then placed in the neck of the vacuum filter flask.

The mixture should be carefully poured onto the vacuum filtration paper, using a funnel if necessary. The vacuum pump should be turned on, which will create a vacuum in the vacuum filter flask. This will cause the mixture to be drawn through the vacuum filtration paper and into the vacuum filter flask. Once all of the mixture has been filtered, the vacuum pump should be turned off and the vacuum filtration setup should be disassembled.

The aspirin should be washed with a small amount of distilled water to remove any impurities, and then allowed to dry. The dried aspirin can be weighed and the yield calculated by comparing it to the theoretical yield.

In conclusion, the preparation of aspirin involves the chemical reaction of salicylic acid and methanol, catalyzed by sulfuric acid. Careful attention must be paid to the materials, equipment, and safety precautions used during the experiment. By following these steps,

Experiment No. 5 Preparation of Aspirin (final).pdf

preparation of aspirin experiment

Aceticanhydride is a lachrymator its vapor irritates the eyes causing tears to flow. A small amount of a strong acid is used as a catalyst which speeds up the reaction. The volume of the NaOH solution does not have to be known too accurately because this solu- tion will be titrated to determine the exact concentration. Thus, at the equivalence point, the moles of NaOH equals the moles of KHP. Organic chemistry encompasses a large number of molecules with many different properties, characteristics, and reactivities. Swirl the flask to dissolve the aspirin. Pour the mixture into a vacuum filtration and rinse the flask with water.

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Experiment_614_Synthesis of Aspirin_1_1_2

preparation of aspirin experiment

For example, bananas contain 3-methylbutyl acetate, CH 3 COOCH 2 CH CH 3 2 and oranges contain octyl acetate, CH 3 COOCHCH 3 C 6 H 13. Three at once may be difficult to observe. The active ingredient in willow bark was later found to be salicylic acid. Refer to the grad- ing rubric to help you write your discussion. Although salicylic acid was effective at reducing pain and fever, it also had some unpleasant side effects. If the temperature is increased at a faster rate the melting point range will be too wide because the crystals will not be able to reach thermal equilibrium.

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Experiment 9 Preparation of blog.sigma-systems.com

preparation of aspirin experiment

An important characteristic of salicylic acid is its bifunctionality, meaning it has two different functional groups. It also contains information about safety precautions put in place to ensure the safety of the team who carried out the experiment. We will synthesize aspirin by mixing salicylic acid with acetic anhydride. Molar absorptivity of the Fe Sa 3 complex is determined by adding 5. Remove all the liquid from the crystals by pressing with a clean stopper or cork.

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(PDF) Experiment 8

preparation of aspirin experiment

The polar oxygen accepts the electrons from now positively charged hydrogen. Within this table, find salicylic acid some old editions may list it as 2-hydroxybenzoic acid. The two compounds we will be preparing, aspirin acetylsalicylic acid and oil of wintergreen methyl salicylate , are both organic esters. This is a good example of the reactivities and properties of different functional groups. In case of contact with skin, rinse immediately with copious amounts of water. The Merck Index is an extremely valuable reference that can be found in the Reference Section of the Fintel Library as well as several reading rooms on 5th floor Trexler.

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PREPARATION OF ASPIRIN

preparation of aspirin experiment

Aspirin is not very soluble in water so the aspirin product will precipitate when water is added. Look up aspirin in The Merck Index. When finished with the experiment, place your aspirin product in a test tube and stopper it. Use a hot plate for heating throughout this experiment. Add 50 mL of DI water to each flask. The isolated product yield is calculated to be 86%.

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1: Synthesis of Aspirin (Experiment)

preparation of aspirin experiment

References Exp: Synthesis of Aspirin ChemSkills. Something else that can improve the experiment is allowing more than fifteen minutes for the Acetyl Salicylic acid to sit in the ice bath; this will allow for more product to crystallize out from solution and will allow for a higher percent yield. NOTE: The aspirin you will make is impure and must not be taken internally! Be sure to determine the limiting reagent, either salicylic acid or acetic anhydride. Before starting the reaction, a hot bath is set up in a 400 mL beaker and the temperature is regulated around 50 °C. In preparing the NaOH solution, accurately weighing solid NaOH is difficult because it absorbs water from the air. All results obtained have been included as well as a detailed analysis of what they represent alongside any improvements to the method used. Salicylates are organic acids from plants that people for hundreds of years have been used for pain reducing.

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CHM457 LAB REPORT 4 Preparation of Acetylsalicylic Acid (Aspirin)

preparation of aspirin experiment

These quizzes are available free to Teach Chemistry schools. What is the theoretical yield of aspirin in two significant figures. Therefore, the final product can be tested with ferric acid to detect any presence of salicylic acid in the sample. Add a minimum amount of hot acetyl acetate into the flask and gently heat the mixture on a steam bath. From the results obtained, the experimental mass of the product is 2 g while the actual mass is 2 g. Aspirin is made when Acetic Anhydride reacting with Salicylic acid to produce Acetylsalicylic acid and Acetic acid diluted vinegar.


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Exp. 18 Synthesis of Aspirin and Oil of Wintergreen S20

preparation of aspirin experiment

At what frequency in the spectrum would you look for evidence of this contamination? Briefly describe the source of each compound. The ethanol should be around 60°C. Write a structure for the ester formed from acetic acid and ethanol. This compound, which has a familiar odor is used as a flavoring agent and in rubbing ointments. Polyesters are often made from dicarboxylic acids and diols. For this reaction, the crude product's percent yield will be determined. The actual yield of pure aspirin was 2.

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