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Phenacetin Synthesis

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The main objective of this experiment was the formation of phenacetin from the synthesis of acetaminophen. This was done through a chemical reaction known as the Williamson ether synthesis using techniques of refluxing, vacuum filtration and recrystallization incorporating a mixed solvent system. A further objective of this experiment was to study the formation of the product (phenacetin). Such validation was completed by using techniques for determining the melting point, calculating percent yield, and IR (infrared spectroscopy) of the resultant product. Our reaction yielded 3.696% of phenacetin product. Hence, the formation of phenacetin via acetaminophen synthesis was not a success. In addition, the poor amount of product formed was not white colored crystals, instead the crystals were of black appearance. A main reason to suggest for the unsuccessful completion of phenacetin could be due to the usage of 2 mL 2.5M sodium hydroxide solution (NaOH)/H2O, instead of the recommended ethanolic sodium hydroxide solution, which was mainly recommended because of the stability and …show more content…

The results were an indicative for expected IR spectrum of pure phenacetin. The IR spectrum showed peaks at (3281.67 cm-1) which indicate the presence of the N=H stretch, (3131.40 cm-1 and 3073.97 cm-1) representing the Sp2 C-H stretches, (2982.26 cm-1, 2927.60 cm-1 and 2885.53 cm-1) expressing the Sp3 C-H stretches, also (1656.82 cm-1) indicating the C=O amide stretch, and finally a wavelength at (1603.51 cm-1) representing the aromatic C=C stretch of the phenacetin molecule, respectively. Such IR spectrum results from phenacetin in comparison with an acetaminophen IR spectrum clearly showed the elimination of the hydroxide (OH) bond present at the acetaminophen molecular structure, which resulted in the IR spectrum not indicating the presence of a strong and broad (alcohol-phenol) band at about 3500 cm-1

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The purpose of this experiment was to identify the two components of an unknown mixture through diverse experimental techniques such as recrystallization, extraction, melting point, and acid-base reactions. From this, the group to which these two compounds belong to had to be determined. These groups are: Carboxylic Acids, phenols, and neutrals. By determining the melting points of the two unknown compounds, these values were compared to the values of melting points in the chart and the proper compound was selected. For the case of this experiment, the unknown mixture contained, 4-methylbenzoic acid.

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After finding the Rf values of the four known compounds, solvent 1 (99.5% ethyl acetate/0.5% acetic acid) was chosen, due to the wide range of results, for the remaining experiments. Ibuprofen, our known tablet, gave a similar Rf value to our previous results for Ibuprofen. For Anadin extra, there were three compounds identified as Caffeine, Paracetamol and Aspirin as the Rf values of the drug were close to the values of these three compounds in the first part of the practical. For both of these known drugs, the Rf values acquired were close to my predictions before the experiment. For the unknown powder, we obtained Rf values of 0.52 and 0.76 so we believe that the unknown powder contains Aspirin and Ibuprofen.

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Lab Report 5: Acetylsalicylic Acid (Aspirin) Synthesis Name: Divya Mehta Student #: 139006548 Date Conducted: November 19th 2014 Date Submitted: November 26th 2014 Partner’s Name: Kirsten Matthews Lab Section: Wednesday 2:30 L9 IAs Name: Brittany Doerr Procedure: For the procedure, see lab manual (CH110 Lab Manual, Fall 2014) pages 96-98. Wilfrid Laurier University Chemistry Department. Fall 2014. Acetylsalicylic Acid (Aspirin) Synthesis.

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The difference in this chemical and physical properties will aid in their separation. Processes like solubility, gravitational filtration and recrystallization will be used to separate the substances present in Panacetin. The melting and boiling point of the substances will help in concluding on which of these compounds will be presented at the end of experiment. Procedure and observation The Panacetin content was weighed approximately 3.0493g and transferred to the Erlenmeyer flask; 75ml of dichloromethane (CH¬2CL2) was added to the content. The dichloromethane (CH2Cl2) dissolved the sucrose, leaving the active unknown agent and aspirin behind.

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The purpose of this experiment was to understand the pharmacokinetics of the drug acetaminophen within the body, specifically focusing on its partition coefficient, drug protein interaction and its bioavailability through various form of administration. The bioavailability of the drug was determined to be 100% for IV because the drug is injected directly into the systemic circulation in its active form and this is also visible on Figure 4, where the initial concentration of drug is much higher than in PO and IP. For PO and IP administration, the bioavailability was determined to be 72.6% and 39.1%, respectively. This makes sense because both of these type of administration involve the first-pass effect where a portion of the drug is metabolized by peripheral organs, especially the liver in this case, and therefore the amount of active drug reaching the circulation is less. PO administration, however has a much higher content reaching the circulation than IP, because the IP route involves passing through the whole gastrointestinal tract before being absorbed in the liver while the IP route injects the drug into the

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Structural Features Acetaminophen is a molecule that is made of twenty atoms; its bonds consist of fourteen single bonds and four double bonds. Acetaminophen is also composed of clusters atoms with groups with names. First of all, part of an acetaminophen atom is a benzene ring. A benzene ring is a ring of six carbon atoms that are connected to each other by three double bonds and three single bonds and unusually all the bond are the same size. In addition, to make sure all the electrons in the outer valence are used the there are hydrogen atoms bonded to stabilize the carbon atoms.

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Inducing Prodigiosin Transposon mutagenesis in Serratia Marcescens Introduction Serratia Marcescens is an opportunistic pathogen, mainly of healthcare facilities but can also be found in many diverse environments. Serratia is a gram negative bacteria which can give it innate resistance to certain antibiotics, especially those that target peptidoglycan cell wall synthesis, due to its outer membrane. In an environment with different microorganisms competing for food Serratia holds a component that gives it another selective advantage. The bacteria contains a red pigment called prodigiosin, that has antibacterial, antifungal, and even antiprotozoal activity.

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If this were to happen, the reaction mixture would produce a completely different reaction or a certain component would have been missing (dissolved) within the reaction mixture. Throughout the heating process, we observed the solid being dissolved, precipitated, and, redissolved. This was able to happen because paracetamol and acetic acid are the byproducts of the primary reaction that occurs when p-aminophenol and acetic anhydride react. This response is completed in three unique solvents; iso-amyl alcohol, water, and 2-propanol. In addition, the reaction can be carried out with or without impurities.

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[3] Tadelech Atomssa and A.V. Gholap. "Characterization of caffeine and determination of caffeine in tea leaves using uv-visible spectrometer." African Journal of Pure and Applied Chemistry 5.1 (2011): 1-8. [4] O'Neil, M.J. (ed.). The Merck Index - An Encyclopedia of Chemicals, Drugs, and Biologicals.

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It is helpful to reduce pains like headache. It is also included in many other active medicines like Tylenol and Midol as an ingredient, because acetaminophen compound is a coal tar derivative which can act on the synthesis of prostaglandins and other compounds for the transmission of pain impulse but the higher rate of use will lead to liver failure. Different methods were used in this lab for the preparation of acetaminophen. This experiment and the related researches that I have

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The reason for this is due to the alcohol functional group present in the salicylic acid starting material, as it has a higher Rf value when TLC is run on the compound in which it is contained at the start of the reaction. TLC of the Aspirin product contained an ester functional group, which was expected to have a lower Rf due to residual hydrogen bonding which occurred between the hydroxyl group of the carboxylic acid and adjacent carbonyl of the ester. Experimental results followed this expected outcome, indicating the successful synthesis of the experimental aspirin product, which maintained a lower Rf value than the reaction starting material (Rf Data Figure 1). Experimental IR results indicated the presence if characteristic wavelength peak values that are found in a successfully synthesized Acetylsalicylic Acid (2-acetoxybenzoic acid) or Aspirin product. The IR spectra revealed the presence of the ester functional group via a peak at 1760cm-1 indicating C=O carbonyl bonding of an ester.

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APOMORPHINE AND PARKINSON’S DISEASE History of apomorphine The early reported synthesis of apomorphine was by Arppe in 1845 and later by Matthiesen and Wright in 1869 which involved reacting morphine with hydrochloric acid or sulfuric acid respectively ((Art 2 from 218). Thereafter, apomorphine had found its use in veterinary therapeutics to treat problems associated with behavior of farmyard animals. By 1874, it was known that apomorphine led to emetic effects along with various effects influencing the central nervous system. In medicine, it was recommended as emetic, sedative, as well as treatment for narcotic and alcohol addiction.

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The hydrolysis formed salicylic concentration which was mixed with iron(III) solution to form a purple complex. This was then use to study under the UV/Visible absorption spectroscopy which gave absorbance values recorded at 525nm to determine the concentration of salicylic acid using the Beer Lambert’s Law and later corrected to find the actual concentrations. The concentrations of aspirin at various intervals was found from salicylic concentrations. Upon plotting a graph of ln(aspirin) vs time, it produced a linear equation from which the gradient gave the rate constant of 0.0083min-1 and the overall shape of the graph concluding this reaction to be pseudo first order with respect to the concentration of aspirin with the deviations and improvements as

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536 Words | 3 Pages

The reaction to synthesize benzocaine was known as a Fisher esterification reaction. The Fisher esterification was reaction between alcohol and carboxylic acid in the presence of acid. The reaction was used to form an ester. In the experiment, sulfuric acid acted as a catalyst and necessary for this reaction to occur. There was a change between the –OH group of carboxylic acid to an –OCH2CH3 group in the reaction.

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In this process,phenolic compounds such as caffeic acid and tannin are extracted from a water fern called azolla mycrophylla, this plant does not have seed or flowers. Both these acids have immense potenial roles Caffeic acid as an antioxidant,anticarcinogenic as well as anti-inflammatory while tannin has been used to treat various diseases along with acting as a shield from external attackers like predators in plants. The extraction procedure started from the crushing of the dried azolla plant material converting it into powderous form so as to mix it with a solvent such as petroleum ether instead of ethanol for further mixing and then it is placed inside a UV sonicator before filteration using a funnel and filter papaer for removal of the plant debris,after using a seperating funnel for seperation it is placed in a rotary evaporator so that the solute and solvent gets seperated as the solvent that had been initially used is seperated out along with drying of the rest of the material which can be further used for the analysis of caffeic acid as well as tannin and for their further analysis using aspectrophotometer. Spectrophotometer analysis gave the exact peaks at the particular wavelengths. These acids have olso

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