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Synthesis of aspirin lab
Synthesis of aspirin lab
Synthesis of aspirin lab
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In the beginning of our experiment of the synthesis of aspirin, we believed that if the catalyst increases in Ka value, i.e. acidity, and the conjugate base(s) do not react, then the percent yield of aspirin will increase when percent yield is a function of the acidity of the catalyst. While performing the experiment, we discovered that the sulfuric acid dissociated the most, which allowed the substance to have the greatest percent yield. This is due to the fact that the increased dissociation allows for more hydrogen protons to be donated. The sulfuric acid had the highest percent yield with a value of 69.7%. In addition, the phosphoric acid dissociated less than the sulfuric acid due to its lower Ka value.
The experimental Fischer esterification of 8.92g of acetic acid with 5.0g of isopentyl alcohol using concentrated sulfuric acid as a catalyst yielded 4.83g (65.3% yield) of isopentyl acetate. The product being isopentyl acetate was confirmed when the boiling point during distillation had similar characteristics to that of the literature boiling points2. Physical characteristics like color and smell also concluded a match of our product with what was intended. 1H-NMR spectroscopy analysis supported this claim due to the fact that the integration values and chemical shifts were comparable to isopentyl acetate. Lastly, infrared spectroscopy (IR) showed similar key characteristics of our product’s wavelengths to that of pure isopentyl acetate5.
Aspirin contains the substance acetylsalicylic acid (ASA), which can relieve inflammation, fever, pain, and known as a “blood thinner”. Aspirin was not officially trademarked until March 6, 1899 when the Imperial Office of Berlin made it official. It has been used for the last 110 years, but its natural form, salicylic acid has been around for thousands by Egyptians, Greeks, and Romans. Aspirin is available in over 80 countries and known as the best non-prescription drug. The most common use of aspirin is to cure headaches and use it as a pain reliever, but aspirin is known to prevent heart attack and strokes. It was first proposed in 1940, but wasn’t confirmed until 1970 when doctors would recommend taking aspirin daily [1].
Ninhydrin test is performed to detect the presence of free α-amino group (-NH2) which presents in all amino acids, proteins or peptides. It is an endothermic process involving redox reaction. Ninhydrin is a powerful oxidizing agent which also known as triketohydrindene hydrate. First, an oxidative deamination reaction occurs as the α-amino acid reacts with ninhydrin. Two hydrogens from the α-amino acid are elicited to produce an alpha-imino acid. On the same time, the ninhydrin itself undergoes reduction by losing an oxygen atom to form reduced ninhydrin, hydrindantin. Next, hydrolysis reaction happens. The amine group in the alpha-imino acid reacts with the water molecule to form an alpha-keto acid with an ammonia molecule. The alpha-keto acid then undergoes decarboxylation to form an aldehyde with a carboxyl group (CO2). The net result includes hydrindantin, aldehyde, ammonia, and CO2. The hydrindantin and ammonia produced are responsible for the colour formation. The process is continuing as ninhydrin condenses with ammonia and hydrindantin to produce an intensely blue or purple pigment, Ruhemann's purple. This reaction provides an extremely sensitive test for amino acids. Ninhydrin which is originally yellow reacts with amino acid and turns deep purple. The colour intensity produced is directly proportional to the amino acid
This experiment is based on being able to properly isolate/purify trimyristin from nutmeg and synthesize myristic acid from trimyristin. Liquid-solid extraction and recrystallization are the techniques used to isolate/purify the trimyristin from nutmeg. Base hydrolysis is the technique used to synthesize the myristic acid from trimyristin. Isolating trimyristin from nutmeg is considered natural product chemistry. Natural product chemistry involves isolating organic compounds from living things, such as plants (Weldegirma 2016). Usually, natural product chemistry is complicated, intensive, and tedious. However, the isolation of trimyristin is not very difficult because a large portion of nutmeg is made up of trimyristin. Trimyristin is a unique triglyceride, as all three of its fatty acid groups are identical.
Extraction is a separation method that is often used in the laboratory to separate one or more components from a mixture. Sucrose was separated at the beginning because it is the most immiscible and it’s strongly insoluble. Next Acetylsalicylic Acid was separated which left Acetanilide alone. Variety steps could have led to errors occurring. For example the step of separation, when dichloromethane layer was supposed to be drained out, it could be possible some aqueous layer was drained with it. Which could make the end result not as accurate. Also errors could have occurred if possibly some dichloromethane was not drained out. Both way could interfere with end result of figuring the amount of each component in the mixture. The solids percentage were 22.1% more than the original. That suggests that solids weren’t separated completely which clarifies the reason the melting points that were recorded were a slightly lower than the actual component’s melting point. The melting point for Acetylsalicylic Acid is 136 C but that range that was recorded during the experiment was around 105 C to 118 C. The melting points were slightly lower than the literature value. Sucrose was the purest among all component due to its higher melting point which follows the chemical rule that the higher the melting point the more pure the component
This experiment synthesized luminol (5-Amino-2,3-dihydro-1,4-phthalazinedione) and used the product to observe how chemiluminescence would work. The starting material was 5-nitro-2,3-dihydrophthalazine-1,4-dione, which was, after addition of reaction agents, refluxed and vacuum filtered to retrieve luminol. Using two stock solutions, we missed our precipitated luminol with sodium hydroxide, potassium ferricyanide, and hydrogen peroxide, in their respective solutions, in a dark room, to observe the blue light
Isolating Keratin protein is done through oxidation and reduction. Keratin can be converted into soluble proteins in acid and be digestible by trypsin or pepsin when oxidized. After oxidation, reduction occurs in an alkaline reaction (basic solutions) with optimum pH of 10-13. Reduction also considered as hydrolysis dissolves disulfide groups, which then starts unravelling the fibrous keratin structures. Reductants such as thioglycolic acid, potassium cyanide and sodium sulfide/sulfite can be used to dissolve the disulfide groups.
Abstract: This week we experimentally determined the rate constant k for the reaction 2HCl (aq) +Na2S2O3 (aq) → S (s) + SO2 (aq) + H2O (l) + 2NaCl (aq). In order to do this the average reaction time was recorded in seconds during two trials. The data from the experiment shows this reaction is in the first order overall: rate=.47s-1 [HCl]0 [Na2S2O3]1. These findings seem to be consistent with the expected results
In this lab, it was determined how the rate of an enzyme-catalyzed reaction is affected by physical factors such as enzyme concentration, temperature, and substrate concentration affect. The question of what factors influence enzyme activity can be answered by the results of peroxidase activity and its relation to temperature and whether or not hydroxylamine causes a reaction change with enzyme activity. An enzyme is a protein produced by a living organism that serves as a biological catalyst. A catalyst is a substance that speeds up the rate of a chemical reaction and does so by lowering the activation energy of a reaction. With that energy reactants are brought together so that products can be formed.
Background Information Aspirin is an analgesic (pain relieving) and an antipyretic drug (a drug that lowers body temperature). The main constituent of aspirin is 2 - ethanoythydroxybenzoic acid, also known as acetylsalicyclic acid (shown below right). It was originally made from just salicylic acid (which is found in the bark of a willow tree) when used by the Ancient Greeks to counter fever and pain, but its bitterness and tendency to irritate the stomach caused problems. These were resolved by the German chemist Felix Hoffman, who made the acetyl derivative of salicylic acid in the
Compared to the 0.5 M hydrochloric acid that was less concentrated, the more concentrated 2 M hydrochloric acid c...
Hydrolysis of aspartame under acidic or basic conditions results in aspartic acid, phenylalanine and methanol. Several solutions can be prepared in order to study the amino acids of aspartame. With TLC analysis, we were able to observe the polarity of each of the solutions prepared. Out of all the solutions, aspartic acid has the lowest Rf value because it is a charged amino acid, therefore it is polar. The solution with the highest Rf is phenylalanine because it is a hydrophobic amino acid.
·Aspirin (salicylic acid acetate) is an anti-inflammatory (decreases swelling and inflammation), anti-pyretic (fever reducing), and anti-platelet (decreases platelets in the body to thin blood). Many heart treatment patients take an aspirin a day to prevent blood clotting. However, if aspirin is taken in large quantities over long periods of time, it may cause gastric ulcers or other internal damage. The molecular formula of aspirin is C9H8O4. Some examples of Aspirin are Bayer, Ecotrin, and Aspergum.
His second book “Sirr al Asrar” is about chemical operations regarding pharmacology such as the instruments used in laboratory and chemical reactions. “Sirr al Asrar” gained special recognition in the West and was translated to Latin.
Sulphuric acid is considered to be one of the strongest acids. It was first discovered in the 800A.D by an Islamic chemist by the name of Jābir ibn Hayyān. It is also the world’s most important industrial chemical, often called the “oil of vitrol”. It is a diprotic acid and is very corrosive and it able to eat through many organic substances and the acid is soluble in water at all concentrations. One of the reason as to why sulphuric Acid is important to the chemical industry because it has many different uses examples of this include lead-acid vehicles battery, oil refining and over 50% of sulphuric acid is used as fertilisers.