# Theoretical yield of aspirin synthesis. Synthesis of Acetyl Salicylic Acid (Aspirin) Essay Example 2022-10-25

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Aspirin, also known as acetylsalicylic acid, is a widely used non-steroidal anti-inflammatory drug (NSAID) that is used to relieve pain, reduce inflammation, and lower the risk of heart attack and stroke. The synthesis of aspirin involves the conversion of salicylic acid into acetylsalicylic acid through the reaction with acetic anhydride. This reaction is known as acetylation and is typically carried out in the presence of an acid catalyst, such as sulfuric acid.

The theoretical yield of aspirin synthesis is the maximum amount of aspirin that can be produced from a given amount of reactants. It is calculated based on the stoichiometry of the reaction, which is the ratio of reactants and products in a chemical reaction. In the case of aspirin synthesis, the stoichiometry is 1 mol of salicylic acid reacting with 1 mol of acetic anhydride to produce 1 mol of acetylsalicylic acid and 1 mol of acetic acid.

The theoretical yield can be calculated by using the following equation:

Theoretical yield = (Reactant mass / Reactant molar mass) x (Product molar mass / Product molar mass)

For example, if we start with 100 grams of salicylic acid and 50 grams of acetic anhydride, the theoretical yield of aspirin can be calculated as follows:

Theoretical yield = (100 g / 138.12 g/mol) x (180.16 g/mol / 180.16 g/mol) = 72.3 g

This means that the maximum amount of aspirin that can be produced from these reactants is 72.3 grams.

However, it is important to note that the actual yield of aspirin synthesis may be less than the theoretical yield due to various factors such as incomplete reactions, side reactions, and losses during purification. These factors can affect the efficiency of the synthesis and reduce the amount of aspirin produced.

In conclusion, the theoretical yield of aspirin synthesis is the maximum amount of aspirin that can be produced from a given amount of reactants based on the stoichiometry of the reaction. The actual yield may be lower due to various factors that can affect the efficiency of the synthesis.

## Lab B

Swirl the mixture to dissolve the solid. A small amount of a strong acid is used as a catalyst which speeds up the reaction. Using these ideas it will be deduced as how the temperature of water affects the solubility of the Aspirin. The ratio of carbon dioxide to glucose is 6:1. Wear gloves when using these chemicals. Aspirin is not very soluble in water so the aspirin product will precipitate when water is added. You can do this either by examining your data points along the curve, or by viewing the data table.

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## Synthesis Of Aspirin Lab Report [vnd5ppm7k5lx]

Iron III nitrate: May intensity fire; oxidizer. However compared to the theoretical yield it is evident that there was a great loss of aspirin that should have been formed. Hold and partially submerge the 50 mL flask and contents in the water bath. Concentration as the Collection Mode. Sulfuricacid H 2SO 4 is highly corrosive. Calculate the precise molar concentration of your stock solution and record it in your data table.

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## Synthesis of Acetyl Salicylic Acid (Aspirin) Essay Example

Remove all the liquid from the crystals by pressing with a clean stopper or cork. The acyl group RCO is deactivating, stopping the reaction cleanly after the addition of one group per aromatic ring. Collect the product by vacuum filtration and rinse out of the flask with a few milliliters of cold petroleum ether. A small amount of the solid will be pushed up into the tube. Bayer's company set up by himself, is generally reckoned to have been the first pharmaceutical company, and the production of aspirin is generally accepted to have laid the foundation of the modern pharmaceutical industry.

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## Chem 1111 Experiment 21

Wait and observe a little longer until all of the aspirin has melted. Dry the crystals by pulling air through them for about 15 minutes. If the absorbance value falls within the range of the salicylic acid standard solutions, record it in your data table. Overall, the reaction takes place between a carboxylic acid and an acid anhydride to form an ester. In modern times,salicylic acid is administered in the form of aspirin which is less irritating to the stomach than salicylic acid. Set up a 150 mL beaker with water to warm up on a hot plate medium heat 2. When you are confident that the reaction has reached completion no vapors appearing , carefully remove the flask from the hot plate and add 20 mL of distilled water.

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## Chemistry 104: Synthesis of Aspirin

From this point on, keep your flask under the hood, because it now contains acetic anhydride the vapors of acetic anhydride are very irritating. Thus, there was 86. Balance:The balance used to calculate the mass of the wet and dry product along with the beaker was considerably outdated. Measure and record the absorbance value of the treated aspirin sample. Based on your percent yield, iron III chloride test, and the measured melting point range, draw a conclusion about the success of your synthesis. Next you will crystallize the aspirin: a.

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## How can I calculate the percent yield of aspirin synthesis?

Carefully observe your sample. The experimentally determined melting temperature of 132. The information on how aspirin is carried out in industry will be established using various text books and internet sources that will be referenced at a later date. Information provided is based on our observations and opinions, not as fact. Repeat the procedure for the remaining salicylic acid solutions that you prepared. Mix the solution thoroughly. This will be the wet weight.

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## 1: Synthesis of Aspirin (Experiment)

Discard all solutions as directed. As soon as this occurs note the temperature. As the yield is produced its melting point will be found, and it will be compared to values of aspirin that have been stated in chemical textbooks. The excess acetic anhydride will be quenched reacted with the addition of water. If the reaction has not fully completed then the Aspirin formed would not be pure, as it would contains unreacted reactants.

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## Experiment_614_Synthesis of Aspirin_1_1_2

One of the compounds used in the synthesis of aspirin is salicylic acid, which is itself a pain reliever that was known to many ancient cultures, including the Native Americans who extracted it from willow tree bark. In other words, work with moles and then convert them to grams. The search for a milder form of this pain reliever led to the successful synthesis of acetylsalicylic acid by the German chemist Felix Hoffmann in 1893. This experiment uses salicylic acid, acetic anhydride and phosphoric acid. As the mixture cools, crystals of aspirin should form in the flask. After heating, turn the bunsen burner off and CAREFULLY remove the flask from the water bath remember it is hot! However, salicylic acid is bitter and irritates the stomach.

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## How do you calculate the theoretical yield of aspirin synthesis?

Visualization of the sample - our result will be viewed under UV light 4. Prepare the synthesized aspirin sample for testing. Use a previously prepared sample in a capillary tube, as described in Step 8, to determine the melting temperature of the sample: a. How do you synthesize ferrocene? CAUTION: Handle the phosphoric acid and acetic anhydride with care. Second, you will use a Spectrophotometer to test the absorbance of salicylic acid impurity in your aspirin sample after it has been complexed with Fe3+ from iron III nitrate solution. This could be reason as for why the there was a great temperature difference in the melting points of aspirin, The solubility of aspirin in water varies with temperature. As the temperature of the water increases, the solubility of aspirin increases due to an increased amount of interactions and collisions.

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## Theoretical Yield Worked Example Problem

Quantitatively transfer the solution from the beaker to a 250 mL volumetric flask. Record the absorbance and concentration values in your data table. Calculate using the following strategy: Convert grams to moles, use the mole ratio to bridge products and reactants, and then convert moles back to grams. This compares reasonably well with the melting temperature test. It is OK to weigh a little extra mass do not return excess salicylic acid to its container as this might contaminate the entire amount if your spatula is not perfectly clean. The report then approaches to the hazards and risk analysis of the chemicals involved in the experiment and how precautions are taken to reduce these risks. Calculate the precise molar concentrations of the five standard solutions in the table above and record them in your data table.

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