Creating and Testing Aspirin
Introduction
Aspirin is created when salicylic acid and acetic anhydride react together (French et al. 82). However, phosphoric acid is needed as a catalyst, and acetic acid is released as a by-product (French et al. 82). The reaction of aspirin is as shown below: Figure 1. Structures Found in Aspirin Synthesis (French et al. 82
The limiting reagent controls how much product can be produced (French et al. 83). The reagent that is the first to be completely used is the limiting reagent, and by using calculations to discover which reagent produces the smallest amount of the product (French et al. 83).
Theoretical yield is the maximum amount of product that can be produced during a reaction (French et al. 83). The numbers used to find theoretical yield must be those of the limiting reagent (French et al. 83). Because parts of the material used are inevitably lost during experiments, the actual yield will be smaller than the theoretical yield (French et al. 83). To test the efficiency of the reaction, calculate the percent yield as shown below:
% yield= (actual yield)/(theoretical yield) ×100
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83) Recrystallization helps to purify products and remove contaminants (French et al. 83). To do this, the product is dissolved in a hot substance and then reforms as crystals when the substance cools; the crystals are the filtered out of the solution so that they are separated from any impurities dissolved in the substance (French et al. 83). The proper solvent used for recrystallization should not react with the desired product (French et al. 84). Instead, it should dissolve the desired product at warm temperatures, but not dissolve it at cool temperatures (French et al.
The experiment was not a success, there was percent yield of 1,423%. With a percent yield that is relatively high at 1,423% did not conclude a successful experiment, because impurities added to the mass of the actual product. There were many errors in this lab due to the product being transferred on numerous occasions as well, as spillage and splattering of the solution. Overall, learning how to take one product and chemically create something else as well as how working with others effectively turned out to be a
The purpose of this experiment was to learn and preform an acid-base extraction technique to separate organic compounds successfully and obtaining amounts of each component in the mixture. In this experiment, the separation will be done by separatory funnel preforming on two liquids that are immiscible from two layers when added together. The individual components of Phensuprin (Acetylsalicylic acid, Acetanilide, and Sucrose as a filler) was separated based upon their solubility and reactivity, and the amount of each component in the mixture was obtained. Also, the purity of each component will be determined by the melting point of the component.
The question that was proposed for investigation was: Can the theoretical, actual, and percent yields be determined accurately (Lab Guide pg. 83)?
The most important concept that should be taken from this lab is that the limiting reactant restricts the amount of product possible from a reaction. Increasing the amounts of other reactants will not increase the amount of product, but increasing the amount of the limiting reactant will.
The solvent should be easily removed from the purified product, not react with the target substances, and should only dissolve the target substance near it’s boiling point, but none at freezing. A successful recrystallization uses minimum amount of solvent, and cools the solution slowly, if done to fast, many impurities will be left in the crystals. Using the correct solvent, in this case ice water and ethyl acetate, the impurities in the compound can be dissolved to obtain just the pure compound. A mixed solvent was used to control the solubility of the product. The product is soluble in ethanol an insoluble in water. Adding water reduced solubility and saturates the solution and then the crystals
The general objective of this experiment was for the students to familiarise with the preparation of a simple organic compound and to purify the compound by recrystallization. This experiment allows the students to conduct synthesis of aspirin, reinforcing the skills of recrystallization and the technique of melting point determination.
The purpose of the experiment is to study the rate of reaction through varying of concentrations of a catalyst or temperatures with a constant pH, and through the data obtained the rate law, constants, and activation energies can be experimentally determined. The rate law determines how the speed of a reaction occurs thus allowing the study of the overall mechanism formation in reactions. In the general form of the rate law it is A + B C or r=k[A]x[B]y. The rate of reaction can be affected by the concentration such as A and B in the previous equation, order of reactions, and the rate constant with each species in an overall chemical reaction. As a result, the rate law must be determined experimentally. In general, in a multi-step reac...
Acetaminophen is a replacement pain reliever for children, due to aspirin side effects. The redox of acetaminophen is an irreversible, however, this under conditions where the pH is acidic. Acetaminophen is reduced to N-acetyl-4-quinoneimine. Due to acidic conditions, it is rapidly hydrolyzed to N-acetyl-4-quinoneimine hydrate, which cannot be forced back to acetaminophen. In order to overcome this, the analysis is done in a neutral or basic buffer. This prevents N-acetyl-4-quinoneimine from being hydrolyzed and allows it to be oxidized back to acetaminophen1. Acetaminophen under a neutral environment becomes a quasi-reversible system. Since not all of the N-acetyl-4-quinoneimine can be prevented from forming the hydrate, the data will contain errors. The amount of acetaminophen stated on the children’s Tylenol was 160 mg per 5
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].
All the bond types in this molecule are covalent bonds because all the elements involved are non-metals. There are three carbon rings in the molecule and each carbon ring is connected with an oxygen. The inactive ingredients alcohol, camphor, castor oil, collodion, ether, ethylcellulose, hypophosphorous acid, menthol, and polysorbate 80. The active ingredient in Compound W is salicylic acid. Salicylic acid, also called ortho-hydroxybenzoic acid, is mainly used for pharmaceutical products such as aspirin and Compound W. The chemical formula for salicylic acid is C7H6O3. In 1838, an Italian chemist Raffaele Piria created salicylic acid from salicylaldehyde. This was the first time salicylic acid was ever prepared. Later on in 1860, two German chemists discovered an synthesis based on phenol and carbon dioxide. However, today salicylic acid is not made either of these ways. It is made from dry sodium phenoxide and carbon dioxide which is then followed by treatment with acid. Even though salicylic acid is prepared, it can be found in small quantities in plants of the genus
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
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
Once we know all the values of the ingredients, the value can be multiplied by the
Pyrrole synthesis can be achieved by a vast number of methods. Some of the most common processes used in today’s laboratory include the Hantzch pyrrole method, Paal-Knoor Knorr synthesis and the Knoorr synthesis; the latter which will be studied in this experiment. Other complex methods explored include Robinson’s utilization of the reaction between an aldehyde and a hydrazine . However, this method requires high temperatures which are not economically favourable to maintain and so the other classic methods are gene...
This is a set of instructions that will teach high school or undergraduate chemistry students how to determine the limiting reagent in a chemical reaction. Finding the limiting reagent in a chemical reaction will show which element or compound will run out first and be limited. These instructions will help to determine how much product will be produced in the chemical reaction. Any high school or undergraduate chemistry student with basic knowledge of chemistry and stoichiometry will be able to complete these instructions.