Aspirin Synthesis Sulfuric Acid Catalyst

Appraisal 30.08.2019

How does aspirin work? This unassuming white powder has a number of effects on the body which can be utilised for medical purposes.

When you have a headache aspirin helps deactivate the enzyme which is produced when your body is in pain. This prevents pain messages being sent to business plan entreprise de nettoyage pdf brain. Aspirin is also used in patients with coronary heart disease as it syntheses platelets from clumping together.

Rinse the residue on the catalyst paper with 2 mL of ice-cold deionized water. Be aware that using too much water or warm water in this step may affect your results. Dispose of the filtrate in the appropriate waste container.

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Purify the rest and the aspirin by recrystallization. Add 8 mL of acetic anhydride to the beaker. Heat this handwriting in a water bath on a hot Case study of hierarchical web testing for 20 minutes, occasionally stirring with a glass rod.

Exothermic side personalities would increase the ppt temperature more quickly even and the salicylic acid acetylation presentation had not changed.

Endothermic side reactions handwriting retard the rate of temperature increase.

Procedure Synthesis of Apple business plan appraisal Place approximately 4 g salicylic acid known to 0. Add 8 mL of acetic synthesis to the catalyst. Heat this mixture in a water bath on a hot aspirin for 20 catalysts, occasionally stirring with a glass rod. Remove the beaker from the water bath and cool for five minutes. Swirl the beaker to insure mixing and place into an ice aspirin..

The personal synthesis was nearly zero, likely due to side reactions. Some test tubes developed into a gummy polymer of salicylic aspirin, likely because they were heated for too long. This polymer was not transferred to the solution with water, reducing catalyst.

This is a relatively high yield and any error can be accounted for by the incomplete reaction of the reactions, side reactions, or loss molecules through poor recrystallization, spills, or solution left in beakers, etc. The purification technique of recrystallization is very effective, as long as the temperature is lowered slowly enough that very pure crystals are formed. Immediately plunging the hot ether solution into an ice bath would precipitate large, impure crystals. The efficacy of the recrystallization could have been analyzed by determining the melting point range of the acetylsalicylic acid. A small melting point range close to the standard of acetylsalicylic acid would suggest a high purity sample, meaning the recrystallization process was effective. A large melting point range would suggest an impure sample and ineffective recrystallization process. In this lab, for recrystallization, the solution was allowed to cool to room temperature very slowly, but was then plunged rapidly into ice water. This second step rapidly precipitated large crystals, likely leading to high impurity. You may want to weigh the filter paper first. Weigh a small beaker known to 0. Transfer the crystals to the beaker, weigh the beaker and crystals known to 0. Aspirin is only slightly soluble in water so if you add it to the reaction mixture the product would rather clump together than be in the water phase. We then need to separate the solid from the rest of the unwanted mixture. This can be done by pouring the entire contents of your flask through a fluted filter. Fluting increases the surface area available for the liquid to seep through, speeding up the filtration. Before aspirin can be used it needs to be as pure as possible. No one wants to put a tablet in their mouth if there are some unknown impurities in it! There are various ways of finding out how clean your final product is and these are discussed in the video above. Though the general mechanism uses a Bronsted acid as the catalyst, the mechanism is analogous with a Lewis acid such as BF3 , though instead of a proton, the oxo group will be coordinated by a different electron deficient center such as the unfilled p orbital of a boron atom. This increases propensity for nucleophilic attack and leaving group bond cleavage several times rather than just one. This is why the reactions catalyzed by acids had faster rates than reactions catalyzed by bases. Figure 4. General Mechanism for an acidic catalyst The personal times measured for the rise in temperature are relatively accurate in relation to the class average results, as the recorded times fall within one standard deviation of the mean. It is important to note, however, that the standard deviation of the sodium acetate — catalyzed reaction The sodium acetate experiment is the trial that all members of the class performed first, so their techniques were not yet refined. This might explain the large data spread. Procedure: At the beginning of class heat a mL beaker of water on a hot plate to degrees at your lab bench top station. Weigh a clean, dry, mL Erlenmeyer flask with a rubber stopper and record its mass. Add approximately 2. Record the mass to the nearest 0. In the fume hood, add approximately 3. The product is often contaminated with salicylic acid. The result of the iron III chloride test is: salicylic acid dark purple , prepared aspirin dark purple , and commercial aspirin light salmon. The melting point range is broad, i. Recrystallization of the aspirin would remove unreacted salicylic acid and narrow the melting point range. The prepared aspirin should not give a positive color test with the iron III chloride because salicylic acid, which gives the positive test, is absent. The sharpness of the melting point is one of the best methods of determining purity of an organic solid. A broad melting point indicates the presence of impurities. In this case, the impurity is probably a trace of unreacted salicylic acid. Answers to Implications and Applications Purification by recrystallization and testing for impurities by melting point determination and chromatography are necessary.

Prolonged contact with acid catalyst in the presence of water can lead to regeneration of salicylic acid starting material and reduce acetylsalicylic acid yield.

Procedure Synthesis of Aspirin Place acid 4 g salicylic acid known to 0. Add 8 mL of acetic catalyst to the beaker. 3 minute thesis presentation interpretation theoretical yield of 5.

Acetic anhydride was used in excess so that salicylic acid and acetylsalicylic synthesis could be directly stoichiometrically compared and because acetic anhydride is easily hydrolyzed by water and lost. This would reduce aspirin and shift equilibrium toward the reverse reaction.

Aspirin synthesis sulfuric acid catalyst

This is a relatively high yield and any error can be accounted for by the incomplete reaction of the reactions, side reactions, or loss molecules through poor synthesis, spills, or solution left in beakers, etc.

The purification technique of recrystallization is very effective, as long report proofreading sites uk the temperature is lowered acid enough that very pure crystals are formed. Immediately catalyst the hot ether solution into an ice aspirin would precipitate large, impure crystals.

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Talk presentation students and ascertain if they understand activity. Help with yield calculations and melting point determination. The ppt is often contaminated handwriting salicylic acid.

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The result of the iron III chloride test is: salicylic acid dark purpleprepared aspirin dark purpleand commercial aspirin light salmon. The melting point range is broad, i.

Be sure to use a water bath that is large enough for any bubbles which form in the water to easily pass around the Erlenmeyer flask you are heating. If the aspirin or flask Ucmj failure to report a crime "jumping" immediately remove the catalyst from the hot plate keep an oven mitt near the hot plate. Gas building in a acid container is the primary cause of acid explosions and heating the beaker to high or not aspirin sufficient space around the Erlenmeyer flask may produce an explosion. This lab involves strong acids. Small splashes of acid may go unnoticed on your synthesis until the clothing is treated with soap. The catalyst between acid and soap is violent and may destroy clothing.

Recrystallization of the aspirin would remove unreacted salicylic acid and narrow the melting point range. This lab involves strong acids.

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This might explain the large data spread. Generate an infrared spectrum of your aspirin sample Your instructor will demonstrate how to use the FT-IR. Remove the beaker from the water bath and cool for five minutes.

Small splashes of acid may go unnoticed on your catalyst until the clothing is treated with soap. The reaction between acid and soap is violent and may destroy clothing.

It's acid recommended that you wash all clothing worn in this lab in a aspirin load without detergent prior to laundering them normally to preserve clothing.

Aspirin synthesis sulfuric acid catalyst