Synthesis Of Aspirin And Oil Biology Essay

Synthesis Of Aspirin And Oil Biology striveEsterification is the reaction mingled with carboxylic acerbs and alcohols to produce esters. Aspirin or acetylsalicylic erosive was organize by reacting salicylic biting and acetic anhydride age Methylsalicylate was formed from salicylic harsh and methanol, both in the front line of H2SO4 responsible for the removal of -OH to form an ester and donates H+ to protonate the salicylic corrosive. The reaction motley in the synthesis of acetylsalicylic mordant should be heat up in temperature between 70-90C for the formation of acetylsalicylic sulfurous crystals that was boost self- hoard using vacuum filtration with cold wet to wash out the impurities and further produced a 57% sire product. The synthesized methylsalicylate moderateed to a minty olfactory sensation that is used generally as ointment or cream for get acrossing muscle pains and sprains. exam using FeCl3 to verify the purity of the synthesized acetylsalicyl ic panelling resulted to a violet-colored solution in acetylsalicylic loony toons qualification it an im exquisite product because of the charge phenol radicaling that must not be present in the structure. However, positive result in methylsalicylate turned the solution from clear to dark-green and further to a purple solution ascribable to the presence of phenol collection. The results of the experiment are therefore accurate and useful in knowing the importance and uses of native products and knowing the process of esterification involving carboxylic virulents and alcohols.__________________________________________________________________________INTRODUCTIONAspirin or acetylsalicylic unpleasant from a family of chemicals known as salicylates is known to be an anti-inflammatory medicine and used as a pain reliever (1). On the former(a) hand, anoint of wintergreen or methylsalicylate is an external analgesic used to treat muscle aches, sprain, and strains having anti-in flammatory and pain-relieving effects as well (4). Both the acetylsalicylic acid and methylsalicylate can be produced from salicylic acid, a natural surpassring chemical in plants, consisting of twain functional groups carboxylic acid and phenol. The synthesis of acetylsalicylic acid and methylsalicylate from salicylic acid results in the formation of ester in the process called esterification where an acid reacts with an alcohol (2). The purity of the synthesized aspirin will be tested by using FeCl3 test where a purple color will determine the presence of the phenol group where the -OH group in the benzene ring will form a complex with Fe+3 (3).MATERIALS AND METHODSFor the making of aspirin, a piss system lavatorytub with temperature ranging from 70-90C was prepared while weighing 0.150 g of salicylic acid and dropped 85% H2SO4. Then, 0.3 ml of acetic anhydride was added to the reaction mixture and heated with the prepared water bath until it dissolved. Then, it was recrys tallized in an ice bath after adding 0.2 ml deionized water. The formed aspirin was collected using vacuum filtration, washed with cold water, allowed to ironical overnight and weighed again to calculate for the percentage yield. For the making of the Methylsalicylate, 0.25 g of salicylic acid was used and added 2.0 ml methanol until it dissolved. Then, 10 drops of H2SO4 was added and heated in the water bath for 15 minutes followed by allowing it to cool down in running water. The odor of the product formed was then determined. For the FeCl3, the synthesized aspirin and methylsalicylate were added 5 ml of distilled water and a drop of 1% FeCl3 to the test tubes for observations.RESULTS AND DISCUSSIONSEsterification involving salicylic acid and methanol will produce methylsalicylate that has pain-relieving and anti-inflammatory effects while salicylic acid and acetic anhydride in excess will form acetylsalicylic acid in the presence of H2SO4. The results and observations gathered i n the experiment involving the FeCl3 test are summarized in Table 1.Table 1. Data and Results for the rejoin of Aspirin and FeCl3 TestA. Yield of AspirinMass of Salicylic Acid0.150 gMass of acetyl salicylic acid0.114 g% Yield57 %B. FeCl3 TestSampleObservationAcetylsalicylic acidViolet-coloredMethylsalicylateLiquid From clear to dark-green solution Addition of cold water turned into dark purpleThe aspirin or the acetyl salicylic acid was formed by reacting 0.150 g of salicylic acid with acetic anhydride with the presence of acid catalyst which is H2SO4 to speed up the reaction as well as being responsible in removing the -OH to form an ester. The acid catalyst donates H+ and protonates the salicylic acid as shown in strain 1. material body 1. Reaction of salicylic acid with acetic anhydrideAcetic anhydride was used for the reaction will be often faster and will produce a higher percentage yield (5). The reaction mixture was heated in the water bath with temperature between 70-90C to aid in the formation of acetylsalicylic acid crystals and thus making the acetic acid as a byproduct. The salicylic acid dissolved while in the water bath due to the change magnitude heat and increased solubility that made the solution colorless and allowed the salicylic acid white crystals to dissolve. The growth of water after removing the reaction mixture in the water bath aid in destroying the excess acetic anhydride that is unreactive. Then, recrystallization was performed in an ice bath since cooling of the mixture forms white crystals by decreasing its solubility. The aspirin was collected using vacuum filtration while washing it with cold water to remove the solid crystals as well as the removal of impurities in the crystals. after drying, 0.114 g of acetylsalicylic acid was obtained with a yield of 57% with calculations shown in Figure 2.Thoretical yield = 0.150 g x x x = 0.20 g substantial yield (Mass of acetyl salicylic acid) = 0.114 g57%% Yield = x one C = x 100 = Figure 2. Calculations for the % Yield of the Synthesized AspirinThe methylsalicylate or oil of wintergreen was also formed from salicylic acid where it reacted with methanol in the presence of H2SO4 again for the removal the -OH to form an ester in the reaction called esterification as shown in Figure 3. The sulfuric acid as a catalyst protonates the ester group while the methanol attacks the carbonyl group. As the carbonyl group was deprotonated, methylsalicylate formed.Figure 3. Reaction of salicylic acid with MethanolThe product formed a minty odor that is used in food, perfumery, toothpaste, and candies or used as pain-reliever. The purity of the synthesized aspirin and methylsalicylate were tested using FeCl3 to test for the presence of phenol. The acetylsalicylic acid resulted to a violet-colored mixture indicating that the product formed has impurities since the synthesized aspirin or acetylsalicylic acid does not give birth an OH group, however, it turned violet or dark pu rple due to the presence of salicylic acid that didnt react purely in the process. On the other hand, methylsalicylate in FeCl3 gave a positive result where it turned dark-green and further into dark-purple due to the presence of phenol thus making the methylsalicylate as a pure product. Over all, the results of the experiment are accurate and useful in appreciating products that occur naturally as well as knowing how to synthesize aspirin and oil of wintergreen from salicylic acid.