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The Compounding Medicine Controversy
explanatory essay
Pharmacy is a booming field when it comes to medicine, but it certainly has controversial issues such as compounding drugs. While the practice of making drugs customized to a patient seems ethical, there are problems that come along with it. Drug compounding was the norm in the past, but over time consumers began to see issues with it. Drug compounding still occurs to this day because some patients do need medicine specifically tailored to their needs. Compounding has also been the focus of recent disasters, some of which occurred less than two years ago. Whatever side one may take on this issue, it is clear that compounding medicine will be a polarizing issue for years to come.
In this essay, the author
- Opines that compounding medicine is a polarizing issue for years to come. it is ethical, but there are problems that come along with it.
- Explains that the professional compounding centers of america defines compounding as the art and science of preparing personalized medications for patients.
- Explains that compounding is needed if a patient wants to change something about the medicine such as flavor or strength. it is also important for allergy needs.
- Opines that compounding medicine is a polarizing issue for years to come. it is ethical, but there are problems that come along with it.
- Explains that the professional compounding centers of america defines compounding as the art and science of preparing personalized medications for patients.
- Explains that compounding is needed if a patient wants to change something about the medicine such as flavor or strength. it is also important for allergy needs.
- Explains that compounding is heavily regulated by the fda and state boards of pharmacy. the united states pharmacopeia (usp) has standards used every day that are "mandated by law."
- Explains that the new england compounding center was at the center of a 2012 outbreak of fungal meningitis, which led to the filing of chapter 11 bankruptcy by the necc.
- Opines that the fda cannot have full control over the local compounding pharmacies, which is what pharmacists like stephen bernardi used to defend.
- Opines that not all compounding pharmacies are against stricter regulation from the fda. leiter's compounding pharmacy in san jose, california, is fine with more fda regulation if it meant safety for the customers.
- Explains that compounding has been around for many years and is still practiced to this day. for it to become a failsafe practice, all-encompassing regulations must be imposed by the fda and u.s. congress.
- Cites university compounding pharmacy's history of compounding.
- Explains that compounding pharmaceuticalists face a fungal meningitis outbreak. nbc news. 21 dec.2012. web. 3 apr. 2014.
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Synthesis Of Aspirin Synthesis Essay
explanatory essay
4.00 mL of acetic anhydride was then added to the salicylic acid inside the Erlenmeyer flask. 5 drops of concentrated sulfuric acid (H2SO4) was added to the cloudy solution. Concentrated sulfuric acid acted as a catalytic agent which sped up the reaction. Prior to weighing and preparing the solution, a water bath was placed on top of a hot plate and allowed to heat up until only 80 °C. An increase in temperature would cause the solution to polymerize into a different substance. Once the desired temperature of the water bath was achieved, the Erlenmeyer flask containing the solution was floated in it and swirled until the salicylic acid dissolved and the solution became clear. Ten minutes was the maximum allotted amount of time for the reaction. After the dissolution of the salicylic acid and acetic anhydride, 20 mL of distilled ice water was added to the solution and was subjected to an ice bath. The water would destroy any unreacted acetic anhydride and will cause the insoluble aspirin to precipitate (Bettleheim, 2001). The flask was swirled to initiate and speed up the crystallization of acetylsalicylic acid and to allow the oily layer to disperse. Once the oily layer disappeared, Buchner funnel was prepared. The funnel was placed on top of an Erlenmeyer flask subjected to vacuum suction. The purpose of the vacuum suction was to dry the crystals as much
In this essay, the author
- Explains how the synthesis of aspirin was remodeled and revised for a small scale experiment.
- Explains that aspirin is a non-steroidal anti-inflammatory drug (nsaid) that blocks the synthesis of prostaglandins and induces fever.
- Describes how aspirin was developed by felix hoffman, who was working for a dye company named bayer.
- Explains how the synthesis of aspirin was remodeled and revised for a small scale experiment.
- Explains that aspirin is a non-steroidal anti-inflammatory drug (nsaid) that blocks the synthesis of prostaglandins and induces fever.
- Describes how aspirin was developed by felix hoffman, who was working for a dye company named bayer.
- Explains that the active ingredient in aspirin is salicylic acid. the purity of the drug could be tested by recrystallization or through the use of ferric chloride.
- Explains that the main objectives of the experiment are to synthesize, isolate and purify from a one-step reaction of salicylic and acetic anhydride and to characterize aspirin's molecular structure.
- Describes how the experiment used a buchner funnel, erlenmeyer flask, vacuum suction, 400-ml beaker, and thermometer.
- Describes how a 125-ml erlenmeyer flask was weighed on an electronic gram balance, and 5 drops of concentrated sulfuric acid (h2so4) added to the cloudy solution.
- Explains the two methods used to purify crude aspirin: single and mixed solvents. the first solvent was ethyl acetate and the second was petroleum benzene.
- Explains that the purified aspirin was weighed after it was dried and subjected to ir spectrum analysis to verify the purity of the product.
- Explains the general rule of polarity "like dissolves like" applies in the results obtained. since aspirin has four oxygen atoms that form hydrogen bonds, it is more soluble in hydroxylic solvents such as water or methanol.
- Describes the esterification reaction of salicylic acid with acetic anhydride to produce aspirin.
- Explains that the crystals that form in the ice bath are much purer than the crude one because most of the impurities would have failed to dissolve in hot solution due to a higher melting point.
- Compares the ir spectrum analysis of pure aspirin with that of acetylsalicylic acid, where the two peaks are the same.
- Explains that the solubility test could have had discrepancies regarding the temperature of the solvent. careful transfer and keen observation could lead to a higher percent yield.
- Cites references from chem.latech.edu/deddy/chem104/104aspirin.htm.
- Explains lehman, kriz, and engel's introduction to organic laboratory techniques.
- Describes the results of the macroscale and microscale organic experiments.
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Hypertension
explanatory essay
The discovery of captopril as a potent inhibitor of ACE led to the recent development of many series of novel structures with similar biological activity [9]. To date a wide variety of ACE inhibitors from various land and marine food sources have been reported such as milk [10], cheese [11], egg white [12], canola [13], peanut [14], rapeseed [15], antler [16], fish muscle [17], seaweeds [18] and tuna [2].
In this essay, the author
- Explains that phlorotannin components are responsible for the biological activities of ecklonia.
- Explains that hypertension is one of the major risk factors for the development of cardiovascular diseases including stroke. angiotensin i-converting enzyme (ace) is a carboxyl-terminal dipeptidyl exopeptidase.
- Explains that the ethanol extract of e. cava enhances ace inhibition making them superior to the water extract.
- Explains that phlorotannin components are responsible for the biological activities of ecklonia.
- Explains that hypertension is one of the major risk factors for the development of cardiovascular diseases including stroke. angiotensin i-converting enzyme (ace) is a carboxyl-terminal dipeptidyl exopeptidase.
- Explains that the ethanol extract of e. cava enhances ace inhibition making them superior to the water extract.
- Explains that phlorotannins form covalent bonds with proteins and inhibit ace activity. nitric oxide is an important messenger molecule involved in many physiological and pathological processes within the mammalian body.
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(Video) Lab 11 - Synthesis of Aspirin PrelabIbuprofen Research Paper
explanatory essay
Ibuprofen or more commonly known as Advil or Motrin, is a nonsteroidal anti-inflammatory drug (NSAID) that works by reducing the chemical level of prostaglandins that causes inflammation and pain in the body. In 1974, the U.S. Food and Drug Administration or FDA, approved ibuprofen production. In the classic route of Ibuprofen the starting material is isobutylbenzene. With the starting material, acetic anhydride and aluminum trichloride are reacted together creating an intermediate. Hydrochloric acid, aluminum, and acetic alcohol are created also but go unused as essentially waste products. Acetic alcohol and hydrochloric acid are each created separately during the next two intermediate steps. Ammonia is released during the last immediate step before the intermediate turns into isobutylphenylpropanoic acid or more commonly known as Ibuprofen. This process takes six full steps in order to create the desired product with only a 40% atom efficiency or economy. Atom economy is defined as the mass of the wanted product (Ibuprofen) divided by the total mass of products (Ibuprofen + waste). Having only a 40% atom economy means that 60% of the mass created is waste and isn’t reused within the intermediate steps in this
In this essay, the author
- Explains that ibuprofen is a nonsteroidal anti-inflammatory drug that works by reducing the chemical level of prostaglandins that causes inflammation and pain in the body.
- Describes the new green chemistry route of ibuprofen, which utilizes atom economy, less hazardous chemical synthesis, catalysis, and other principles.
- Explains that ibuprofen is the most popular nsaid agent, but its piccolo derivative has found application as a topical anti-inflammatory agent in acne treatment.
- Explains that ibuprofen is a nonsteroidal anti-inflammatory drug that works by reducing the chemical level of prostaglandins that causes inflammation and pain in the body.
- Describes the new green chemistry route of ibuprofen, which utilizes atom economy, less hazardous chemical synthesis, catalysis, and other principles.
- Explains that ibuprofen is the most popular nsaid agent, but its piccolo derivative has found application as a topical anti-inflammatory agent in acne treatment.
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Lab Report Esterification Lab
explanatory essay
The esterification procedure was performed first. To begin the lab, the heating mantle was set at the 6 setting, and the hot plate heat was turned on to low. In a round bottom flask, 6.1 g of benzoic acid and 21 mL of MeOH were added into the flask. Once this was added to the flask, 2 mL of sulfuric acid was added and poured carefully down the side of the flask. It was noted that after the addition of the sulfuric acid there was heat production in the flask. The contents were swirled and a boiling chip was added into the flask. The flask was connected to the hood by a clamp. Water was then ran through the condenser and connected to the round bottom flask to begin refluxing the contents in the flask. The mixture was gently heated at reflux for one hour.
In this essay, the author
- Describes how the lab begins with reflux of the reaction to form an ester followed by several extractions from an organic layer.
- Describes the esterification procedure in which benzoic acid and meoh were added to a round bottom flask, followed by sulfuric acids. the mixture was heated at reflux for one hour.
- Describes how the aldol condensation procedure was performed while the esterification reaction was under reflux. the mixture was cooled in an ice water bath and the crystals were collected via vacuum filtration.
- Describes how the lab begins with reflux of the reaction to form an ester followed by several extractions from an organic layer.
- Describes the esterification procedure in which benzoic acid and meoh were added to a round bottom flask, followed by sulfuric acids. the mixture was heated at reflux for one hour.
- Describes how the aldol condensation procedure was performed while the esterification reaction was under reflux. the mixture was cooled in an ice water bath and the crystals were collected via vacuum filtration.
- Describes how the esterification reflux setup was left to cool down and the sand bath was turned down to the three setting.
- Describes how the dichloromethane layer was dried with anhydrous mgso4 and the drying agent was removed by gravity filtration. the filtrate and boiling chip were placed into a 100 ml round bottom flask.
- Explains the process of recovery of benzoic acid from the sodium bicarbonate wash by acidification with concentrated hcl until the solution tested acidic to litmus paper.
- Describes how the dichloromethane setup was taken down and the crude methyl benzoate was transferred into a 50 ml round bottom flask. the ester was distilled in an air-cooled condenser wrapped with tin foil.
- Analyzes the properties of benzoate and trans-p-anisalacetophenone. the extraction during esterification was important to ensure that no aqueous layer remained in the organic layer.
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The Synthesis Of Aspirin
explanatory essay
The hydroxyl group present on the salicylic acid is corrosive. As a result, salicylic acid cannot be easily ingested. This property is present in many other compounds that have free phenolic groups. Therefore, an acetyl group, is added to salicylic acid to create acetylsalicylic acid (ASA). So
In this essay, the author
- Explains that salicin, salicylic acid, and aspirin belong to a family of medicinally useful compounds.
- Explains that the crude salicylic acid is collected by vacuum filtration and its purity is measured by melting point determination. the acid catalysed reaction uses sulfuric acid as catalyst.
- Explains how the crude aspirin is collected by vacuum filtration and recrystallized, and analysed by thin layer chromatography, ferric chloride test and infrared spectroscopy.
- Explains that salicin, salicylic acid, and aspirin belong to a family of medicinally useful compounds.
- Explains that the crude salicylic acid is collected by vacuum filtration and its purity is measured by melting point determination. the acid catalysed reaction uses sulfuric acid as catalyst.
- Explains how the crude aspirin is collected by vacuum filtration and recrystallized, and analysed by thin layer chromatography, ferric chloride test and infrared spectroscopy.
- Describes how the reaction mixture was heated, cooled, and filtered. the crystals were collected by vacuum filtration.
- Describes the process of preparation of warm water by heating 100ml of distilled water and boiling chips to 45-50 °c, weighing 3.0g of salicylic acid and adding 5 drops of concentrated sulphuric acid to the beaker.
(Video) Aspirin Percent Yield Math1399 words
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Summary Of Phensuprin
explanatory essay
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.
In this essay, the author
- Explains that the 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.
- Explains how they mixed phensuprin and dichloromethane in a 125 ml erlenmeyer flask until the solid dissolved. sucrose was washed with 5 ml of dichlormethan.
- Describes the process of removing the acetylsalicylic acid from the solution.
- Explains that the 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.
- Explains how they mixed phensuprin and dichloromethane in a 125 ml erlenmeyer flask until the solid dissolved. sucrose was washed with 5 ml of dichlormethan.
- Describes the process of removing the acetylsalicylic acid from the solution.
- Describes the process of extracting the phensuprin from the acetylsalicylic acid, methylene chloride, and sucrose.
- Explains that extraction was used to separate a mixture of three solids to their individual components based on their acid-base properties.
- Explains that acetanilide remained in the organic layer and acetylsalicylic acid transferred to the aqueous layer.
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Synthesis Of Aspirin
explanatory essay
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:
In this essay, the author
- Explains that aspirin is created when salicylic acid and acetic anhydride react together.
- Explains the objective of the experiment is to synthesise aspirin using salicylic acid and acetic anhydride using a phosphoric acid catalyst. all reactants should react completely and any impurities should be filtered out during recrystallization.
- Opines that no changes were made to the procedure found in the lab manual.
- Explains that aspirin is created when salicylic acid and acetic anhydride react together.
- Explains the objective of the experiment is to synthesise aspirin using salicylic acid and acetic anhydride using a phosphoric acid catalyst. all reactants should react completely and any impurities should be filtered out during recrystallization.
- Opines that no changes were made to the procedure found in the lab manual.
- Explains that the experiment was correct in predicting that pure aspirin would be produced if salicylic acid and acetic anhydride were combined using a phosphoric acid catalyst.
- Explains that the result could have been caused by several potential errors, such as the loss of material on the filter paper and the jostling off of the material during the experiment.
- Explains that some of the reagents may have remained unreacted during the recrystallization period, which would have caused the yield to be lower.
- Explains that the limiting reagent controls how much product can be produced. the theoretical yield is the maximum amount of product produced during a reaction.
- Explains that recrystallization helps to purify products and remove contaminants. the purity of the aspirin created will be tested by using the phenol group.
1012 words
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Aspirin Research Paper
explanatory essay
Regarded as the most successful non-prescription drug of all time, aspirin has enjoyed commercial popularity since its inception in the mid-18th century. Aspirin is found in a natural form as salicylic acid, traditionally used for the treatment of pain and fevers. This was refined in 1853, when scientist Charles Fredric Gerhardt added an acetyl chemical to the plant-derived pain-reliever. However, this preliminary form of acetylsalicylic acid was deemed unstable, and it wasn’t until 1897 that the compound commercially known today was formed. Felix Hoffman, a young chemist in the pharmaceutical laboratory of German company Friedrich Bayer and Co., worked independently at home experimenting with the addition of various chemical compounds to salicylic acid. Hoffman was searching for an effective, palatable pain-reliever in order to aid his rheumatic father after he complained that the sodium salicylate he had previously used was inedible and harsh. On the 10th of August 1897, Hoffman prepared the first sample of pure acetylsalicylic acid – a pure, stable and extraordinarily efficacious ...
In this essay, the author
- Explains that aspirin is the most successful non-prescription drug of all time. it is found in a natural form as salicylic acid, traditionally used for pain and fevers.
- Explains that aspirin acts as an anti-prostaglandin and antiplatelet agent because of its effect on the cyclooxygenase enzyme.
- Explains that aspirin is used to treat a variety of symptoms, including pain, inflammation, and bleeding. however, acetylsalicylic acid can be used widely and fairly generally, but users may experience some side effects.
- Explains that aspirin is the most successful non-prescription drug of all time. it is found in a natural form as salicylic acid, traditionally used for pain and fevers.
- Explains that aspirin acts as an anti-prostaglandin and antiplatelet agent because of its effect on the cyclooxygenase enzyme.
- Explains that aspirin is used to treat a variety of symptoms, including pain, inflammation, and bleeding. however, acetylsalicylic acid can be used widely and fairly generally, but users may experience some side effects.
- Explains that aspirin is 200 times more effective in the thinning of blood than it is in discouraging inflammation, due to the level of its effect on the specific enzymes.
(Video) isolation of aspirin from tablets - laboratory experiment517 words
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Chemical Reaction Lab Report
explanatory essay
Before any chemical reactions occurred, there was 0.46 grams of elemental copper metal. After the copper was added to the 250 milliliter beaker containing the 5.0 milliliters of nitric acid, nitrogen dioxide gas came out. The gas color was a light brown color, and the clear nitric acid within the beaker became a green-brown color. Once the chemical reaction concluded and nitrogen dioxide gas stopped releasing from the beaker, 20 milliliters of distilled water was added to the solution, and the color within the beaker turned to a neon blue. This was the chemical equation for the first chemical reaction, 4 HNO3 (aq) + Cu (s) → Cu(NO3)2 (aq) + H2O (l) + 2 NO2 (g).
In this essay, the author
- Explains the chemical equation for the first chemical reaction, where 0.46 grams of elemental copper metal was added to a 250 milliliter beaker containing nitric acid.
- Describes the reaction where copper (ii) nitrate reacts with sodium hydroxide in a precipitation reaction. when 20 milliliters of 6.0 m naoh was added to the neon blue beaker, the extremely light blue color darkened.
- Describes how the copper (ii) hydroxide was heated, taking advantage of how it is thermally unstable, forming copper oxide. once the beaker was placed on a hot plate, the dark blue changed to black in color.
- Explains the chemical equation for the first chemical reaction, where 0.46 grams of elemental copper metal was added to a 250 milliliter beaker containing nitric acid.
- Describes the reaction where copper (ii) nitrate reacts with sodium hydroxide in a precipitation reaction. when 20 milliliters of 6.0 m naoh was added to the neon blue beaker, the extremely light blue color darkened.
- Describes how the copper (ii) hydroxide was heated, taking advantage of how it is thermally unstable, forming copper oxide. once the beaker was placed on a hot plate, the dark blue changed to black in color.
- Explains that the next reaction consisted of reacting the copper (ii) oxide with sulfuric acid in a double-displacement reaction, to form copper sulfate. once the 5 milliliters of 6.0 m h2so4 was added to the beaker, all the black coffee-sand substance within the solution dissolved.
- Explains that 1.26 grams of solid zinc was added to the copper (ii) sulfate, forming a reddish-brown solid and solid, elemental copper, via oxidation-reduction reaction.
- Explains that the copper was washed 3 times with 5 milliliters of distilled water each time, and the water was decanted after each wash. after the final wash, the beaker was heated on a hot plate to remove any excess water.
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Preparing and Observing the Properties of Esthers
explanatory essay
The purpose of this experiment is to prepare and observe the properties of esters. The ester that will be synthesized in this methyl Salicylate
In this essay, the author
- Explains that the purpose of this experiment is to prepare and observe the properties of esters.
- Explains the process of esterification, which is a mixture of esters and other molecules like alcohol. carboxylic acid contains the –cooh group
- Explains that if salicylic acid reacts with methanol, the result will be an ester and water.
- Explains that the purpose of this experiment is to prepare and observe the properties of esters.
- Explains the process of esterification, which is a mixture of esters and other molecules like alcohol. carboxylic acid contains the –cooh group
- Explains that if salicylic acid reacts with methanol, the result will be an ester and water.
- Explains that 4 drops of concentrated sulphuric acid were added to the solution in the test tube.
- Describes how the test tube was placed in a beaker filled with water and placed on the hot plate.
- Explains that the test tube was removed from the beaker after and was allowed to cool for 2-3 minutes.
- Explains that the content in the test tube was poured into an evaporating dish that was half filled with water to identify the smell.
- Explains that the result of the reaction mainly depends on how much time the mixture is on the boiling water. the methyl salicylate had a wintergreen fragrance.
- Explains that sulphuric acid acts as a catalyst in the creation of methyl salicylate. it speeds up the reaction rate and prevents it from going backward.
- Explains that the waxy layer on the top of the solution was due to the carboxylic acid not being soluble in water.
- Explains that when the salicylic acid reacted with methanol an ester was produced which means the hypothesis is accepted. the main role of the sulphuric acid was to prevent the reaction from going backward and also to absorb the water.
- Explains that the cork used to cover the test tube was made of rubber. after being heated, the smell of the rubber made it impossible to identify the scent.
- Describes how they prepared an ester with a wintergreen scent by pouring the mixture from the reaction between methanol, sulphuric acid and salicylic acid into an evaporating dish with water.
- Explains that methyl salicylate is an organic ester with a wintergreen scent and can be used in chewing gum, candy, body spray, and drugs. both natural and artificial flavours are made in the lab.
930 words
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Acetamidophenol
explanatory essay
With the knowledge of the melting point, the potential name of the compound could be identified. In this specific experiment, the compound of acetamidophenol was discovered as the unknown numbered 32. Errors encountered in acquiring this information included mistakenly adding more water than was necessary during the filtering process of the macroscale recrystallization. The error reinforced the importance of being precise in these various lab experiments. As a result, we did the macroscale recrystallization over in order to attain crystals. Another error encountered throughout this process occurred when dealing with the Melting Point station. The Melting Point station caused my partner and I trouble when we were trying to acquire 2 degrees per minute rise on the timer. However, once attained completing the experiment in acquiring the melting of these crystals produced in both the macro- and micro- recrystallization went perfectly
In this essay, the author
- Explains that the melting point of unknown #32 was 168.8 to 170.2 degrees celsius. the initial weight of the compound is.505 g.
- Explains the significance of recrystallizing an unknown substance in order to determine its melting point. errors encountered in acquiring this information included mistakenly adding more water than was necessary during the filtering process.
- Defines melting point range as the degree from when crystals first begin to liquefy to the point where the entire sample has melted.
- Explains that the melting point of unknown #32 was 168.8 to 170.2 degrees celsius. the initial weight of the compound is.505 g.
- Explains the significance of recrystallizing an unknown substance in order to determine its melting point. errors encountered in acquiring this information included mistakenly adding more water than was necessary during the filtering process.
- Defines melting point range as the degree from when crystals first begin to liquefy to the point where the entire sample has melted.
- Explains the proper heating rate used to determine a compound’s melting point range 1 to 2 degrees celsius.
- Explains that in the first case, it is possible that the compound is not pure, or that it was denatured forming an undesired compound.
- Describes the melting point values of ferrocene, acetylferocène, and adipic acid, respectively, at 173-176 degrees celsius.
- Explains that to differentiate between citric acid and adipic acid, one would calculate their phs by using the concentration of elements, and then use the ph equation to determine this.
- Explains that the minimum amount of ethanol needed to recrystallize a 2.0-gram sample compound x is (2.0 grams/1.4 grams) * 10 ml = 14.3
- Explains that it is important to use only the minimal amount of hot solvent needed to achieve a recrystallization because it would negatively impact your percent yield of your final crystals.
- Explains the importance of a pre-heated filter during the "hot" gravity filtration step because it helps to remove insoluble impurities.
- Opines that benzyl alcohol would be a poor choice because the fluorenol would not recrystallize if it is melting.
- Explains that colored organic contaminants would be filtered through the addition of charcoal, which would absorb the contaminants through filtration.
- Explains that acetone is a popular solvent because it can remove almost every organic compound and remove impurities from glassware. it is also flammable, which can lead to fires and safety hazards.
846 words
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(Video) CHEM111L: Aspirin Pre-Lab VideoMultistep Synthesis Lab Report
comparative essay
First, the reaction between acetanilide and chlorosulfonic acid was performed. This reaction resulted in a white powder which was confirmed through IR and 1H NMR to be 4-acetamidobenezenesulfonyl chloride. The IR spectrum, RM-12-Ai, shows an amine group at 3316 cm-1 and 1585 cm-1, a carbonyl at 1679 cm-1, an aromatic carbon-carbon stretch at 1533 cm-1, a sulfone 1372 cm-1 and 1166 cm-1, and a para-substituted ring at 836 cm-1. All of these functional groups are represented in this compound,
In this essay, the author
- Explains that a multistep synthesis, electrophilic aromatic substitution, and protecting group were used to obtain the compound sulfaniliamide.
- Explains that the reaction between acetanilide and chlorosulfonic acid resulted in a white powder which was confirmed by ir and 1h nmr.
- Explains that concentrated ammonium hydroxide was added to 4-acetamidobenezenesulfonyl chloride to produce the next product.
- Explains that a multistep synthesis, electrophilic aromatic substitution, and protecting group were used to obtain the compound sulfaniliamide.
- Explains that the reaction between acetanilide and chlorosulfonic acid resulted in a white powder which was confirmed by ir and 1h nmr.
- Explains that concentrated ammonium hydroxide was added to 4-acetamidobenezenesulfonyl chloride to produce the next product.
- Compares the ir spectrums of 4-acetamidobenezenesulfonamide with those of rm-12-ai.
- Explains that 4-acetamidobenezenesulfonamide was reacted with diluted hydrochloric acid and resulted in the synthesis of tan, shiny crystals and weighed 0.916 g.
- Concludes that the multistep synthesis and the experiment were successful.
1140 words
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History and Uses of Aspirin
explanatory essay
In terms of production, aspirin can be produced either manually or industrially. Aspirin also known as acetylsalicylic acid to chemists can be obtained from willow bark. In terms of making aspirin industrially, phenol, sodium hydroxide, carbon dioxide, and acid are needed. Firstly, phenol is mixed with concentrated sodium hydroxide to get sodium phenoxide. Then, reacted with carbon dioxide, sodium salicylate is generated. After that, in acidic solvent, sodium ions are substituted by H+ ions. In this way, salicylic acid is produced. To make hard aspirin tablets, corn starch and water need to be added to salicylic acid. Finally, the chemical mixture is compressed into tablets by tablet machines.
In this essay, the author
- Explains that aspirin is one of the world's most widely used medicines due to its fever-reducing and anti-inflammatory effects. it was invented by a german scientist to cure his father’s pain.
- Explains that the first chemically pure and stable acetylsalicylic acid was synthesized by a german chemist called felix hoffmann, in 1897. aspirin was first taken by his father in order to reduce his arthritis pain.
- Explains that the invention of aspirin, a medical-breakthrough, belongs to the knowledge of chemistry and pharmacology knowledge.
- Explains that aspirin is one of the world's most widely used medicines due to its fever-reducing and anti-inflammatory effects. it was invented by a german scientist to cure his father’s pain.
- Explains that the first chemically pure and stable acetylsalicylic acid was synthesized by a german chemist called felix hoffmann, in 1897. aspirin was first taken by his father in order to reduce his arthritis pain.
- Explains that the invention of aspirin, a medical-breakthrough, belongs to the knowledge of chemistry and pharmacology knowledge.
- Explains that aspirin appeals to patients due to its unique chemically pain easing. millions of patients owe their happiness and wellbeing to the invention of it.
- Explains how aspirin can be produced either manually or industrially, using phenol, sodium hydroxide, carbon dioxide, and acid.
495 words
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TLC Analysis Of Analgesics
explanatory essay
The components of an analgesic will be determined by noting the separation between the solid and liquid (or mobile) phases and comparing it to these predicted reference values.
In this essay, the author
- Explains that thin layer chromatography is one of the most widely used techniques in laboratories today. the main applications of tlc are to detect the presence of a particular compound in urine or blood.
- Explains where the sample ends up after the separation phase and its location in comparison to the pre-existing compounds determines its composition. the components of an analgesic will be determined by noting separation between the solid and liquid phases and comparing it to predicted reference values.
- Explains that the eluting solvent mixture also affects the rf value and separation between the mobile/liquid phase and solid phases.
- Explains that thin layer chromatography is one of the most widely used techniques in laboratories today. the main applications of tlc are to detect the presence of a particular compound in urine or blood.
- Explains where the sample ends up after the separation phase and its location in comparison to the pre-existing compounds determines its composition. the components of an analgesic will be determined by noting separation between the solid and liquid phases and comparing it to predicted reference values.
- Explains that the eluting solvent mixture also affects the rf value and separation between the mobile/liquid phase and solid phases.
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FAQs
What is the conclusion of the aspirin synthesis lab report? ›
Conclusion: A total of 2.169 grams of pure aspirin was synthesize out of a possible yield of 2.52 grams. Thus, there was 86.07% product yield. Acetylation of salicylic acid makes aspirin less acidic and therefore less damaging to the digestive system of the human body.
How is aspirin prepared lab answers? ›To prepare aspirin, salicylic acid is reacted with an excess of acetic anhydride. A small amount of a strong acid is used as a catalyst which speeds up the reaction. In this experiment, sulfuric acid will be used as the catalyst. The excess acetic anhydride will be quenched (reacted) with the addition of water.
What is the summary of synthesis of aspirin? ›Aspirin is prepared by chemical synthesis from salicylic acid, through acetylation with acetic anhydride. The molecular weight of aspirin is 180.16g/mol. It is odourless, colourless to white crystals or crystalline powder.
How is aspirin synthesized in lab report reference? ›Synthesis of aspirin was produced using esterification of salicylic acid in acetic anhydride in the presence of an acid catalyst, which is 85% phosphoric acid and heat by means of nucleophilic acyl substitution. After heating, water was added to hydrolyze excess acetic anhydride into acetic acid.
How would you describe the end point of aspirin? ›The only base remaining in each flask will be excess base that has not reacted with the aspirin. Using your burette with your ~0.1 M HCl solution, titrate the excess base in each flask with HCl until the pink colour just disappears. The endpoint is best described as “cloudy white”.
What was the purpose of the aspirin experiment? ›Your two primary objectives in this experiment will be to synthesize and analyze aspirin. There is more than one way to synthesize aspirin; in this experiment, you will react acetic anhydride with salicylic acid in the presence of phosphoric acid (which acts as a catalyst). The reaction equation is shown below.
What are the lab results for aspirin? ›If your healthcare provider prescribed aspirin for inflammation or arthritis, the typical level of aspirin is between 10 to 30 milligrams per deciliter (mg/dL) of blood. Any concentration above 40 mg/dL can be toxic. In adults, taking 10 to 30 grams of aspirin can be fatal.
What are the key points in the synthesis of aspirin? ›The synthesis of aspirin is known in organic chemistry as an esterification reaction. This is a substitution reaction in which an alcohol (the –OH group in salicylic acid) reacts with acetic anhydride to form an ester, aspirin.
What were the lab errors in the synthesis of aspirin? ›The possible sources of error in the experiment were: (1) the collected crude aspirin was not dried and immediately subjected to another recrystallization; (2) the Erlenmeyer flask used was not clean, and; (3) the solution did not heat in a steam bath for 15 minutes.
What is the hypothesis of the aspirin synthesis? ›Hypothesis: I hypothesize that salicylic acid will react with acetic anhydride to produce acetylsalicylic acid (aspirin) and acetic acid (vinegar). Variables: Independent and controlled variables: The amount of sulfuric acid used for catalysis and the amount of salicylic acid and acetic anhydride.
What is the melting point of aspirin in a lab report? ›
Melting point of purified aspirin is 135-136 °C.
How do you determine the amount of acetylsalicylic acid in an aspirin lab report? ›To determine the amount of acetylsalicylic acid present in an aspirin tablet, the easiest process would be to dissolve a tablet and titrate it with a base. Titration uses a solution of known concentration to react completely with an analyte to determine its concentration or amount.
How did you determine the purity of your synthesized aspirin? ›The purity and amount of acetylsalicylic acid in aspirin can be measured using a Visual Spectrophotometer. Here's why: when iron is added to aspirin, it produces violet tetraaquosalicylatroiron complex. To put it simply there is a visible violet color reaction.
What is the product of aspirin synthesis? ›Answer and Explanation: The byproduct of the synthesis of aspirin is acetic acid. During the reaction of salicylic acid with acetic anhydride for the synthesis of aspirin, acetic acid comes out to be the byproduct with formula CH3 COOH.
What is the purpose of adding water at the end of aspirin synthesis? ›After the reaction takes place, water is added to destroy the excess acetic anhydride and cause the product to crystallize. The aspirin is then collected, purified by recrystallization, and its melting temperature measured.
What is aspirin describe its action and effect? ›Aspirin, an acetylated salicylate (acetylsalicylic acid), is classified among the nonsteroidal antiinflammatory drugs (NSAIDs). These agents reduce the signs and symptoms of inflammation and exhibit a broad range of pharmacologic activities, including analgesic, antipyretic, and antiplatelet properties.
How is aspirin structure described? ›Aspirin Formula and Structure
The chemical formula for Acetylsalicylic Acid is C9H8O4. Similarly, the extended formula for the same is said to be CH3COOC6H4COOH. Further, the molecular mass of it is around 180.159 g mol-1.
The aspirin causes blood pH to drop, and in response hyperventilation kicks in to raise the pH. An influx of an acid such as aspirin, or of a large dose of an alkaline substance like baking soda, can affect blood pH, but the effect is temporary due to the blood's rapid buffering action.
What does the chemical analysis of aspirin indicate? ›The chemical analysis of aspirin indicates that the molecule is 60.00% carbon, 4.44% hydrogen, and 35.56% oxygen.
What is the main impurity in aspirin synthesis? ›Salicylic acid is a major hydrolytic degradation product of aspirin, responsible especially for gastric irritation during oral aspirin administration. This impurity was investigated in 12 different brands of aspirin formulation readily available in our locality.
What were possible sources of error in this lab? ›
Physical and chemical laboratory experiments include three primary sources of error: systematic error, random error and human error. These sources of errors in lab should be studied well before any further action.
What are the sources of error in synthesis lab? ›- Spilling.
- Dropping equipment.
- Not cleaning equipment.
- Ignoring directions.
- Writing an incorrect number.
- Hitting the wrong key on a calculator.
- Not paying attention to units/labels.
He proved that aspirin and other non-steroid anti-inflammatory drugs (NSAIDs) inhibit the activity of the enzyme now called cyclooxygenase (COX) which leads to the formation of prostaglandins (PGs) that cause inflammation, swelling, pain and fever.
What is the format of a lab report? ›A lab report is broken down into eight sections: title, abstract, introduction, methods and materials, results, discussion, conclusion, and references. The title of the lab report should be descriptive of the experiment and reflect what the experiment analyzed.
How does temperature affect the rate of reaction of aspirin? ›The breakage of Aspirin, characterised by single particle impact tests, was found to increase with temperature. Additionally, the breakage propensity of Aspirin as a function of temperature was found to be well described by the Arrhenius equation.
What is the balanced equation for the synthesis of aspirin? ›The balanced equation is: C4H6O3 + C7H6O3¡C9H8O4 + C2H4O2 In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g/mL) and 1.25 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin.
What is the percent purity of aspirin lab? ›Standards for medications are defined by the United States Pharmacopeia (USP) (6). Aspirin tab- lets must contain not less than 95 percent and not more than 105 percent of the labeled amount of CgH8O4 (acetylsalicylic acid). The same percentage applies for CgH9NO2 (acetaminophen).
How do you calculate the percent yield of aspirin lab? ›- Actual Yield of Aspirin in lab after filtered/dried (mock value) = 370 g.
- Mass of Theoretical Yield of Aspirin (mock value) = 360.3 g.
- Percent Yield = (Actual ÷ Theoretical) x 100 = (370 ÷ 360.3) x 100 = 103 %
mg. Generally, one tablet of aspirin contains about 75 mg to 150 mg depending upon the requirement. Aspirin tablet is used to provide relief from pain and is also used for reducing fever. So, the commonly used unit to measure the mass of aspirin in one tablet is mg (milligrams).
What are the most likely impurities present in the sample of aspirin? ›The main impurity in our crystallized aspirin will be salicylic acid. Salicylic acid will co-precipitate with the aspirin if the procedure is done too quickly. The first method we can use to determine the purity of our sample is the determination of its melting point.
Why is it important to determine the purity of aspirin? ›
Significance of Determining Aspirin Purity
The purity of the product is essential for its use as a drug, thus necessitating students to measure the purity of their products. Thin layer chromatography (TLC) is normally used for this purpose.
The salicyclic acid will be the limiting reagent. As far as the calculation of the theoretical yield is concerned, we assume that every mole of salicylic acid will be converted to aspirin or acetylsalicylic acid.
What is the overall reaction of synthesis of aspirin? ›*The chemical equation corresponding to the synthesis reaction is: C7H6O3 + (CH3CO)2O → C9H804 + CH3COOH.
What conclusions can you draw about your aspirin based on the FeCl3 test? ›Aspirin does not contain a phenolic group (rather a carboxylic acid -COOH) so if the sample is pure it should not result in a color change. Therefore, when the FeCl3 F e C l 3 is added, the color will remain yellow (which is the color of the iron solution).
What is the main reaction in the synthesis of aspirin? ›The synthesis of aspirin is known in organic chemistry as an esterification reaction. This is a substitution reaction in which an alcohol (the –OH group in salicylic acid) reacts with acetic anhydride to form an ester, aspirin.
How to increase the reaction rate of the aspirin synthesis reaction? ›Making aspirin
This reaction would be very slow without a catalyst. In this case just a few drops of sulphuric acid added to the mixture means that there are some free positive hydrogen ions in the solution which can bind to the ethanoic anhydride. This makes it more active and speeds up the reaction.
The therapeutic range of salicylate is 15-30 mg/dL. Patients are often symptomatic at salicylate concentrations higher than 40-50 mg/dL. Patients with salicylate concentrations approaching or exceeding 100 mg/dL usually have serious or life-threatening toxicity.
What is a high salicylate level? ›Salicylate levels greater than 100 mg/dL are considered severe toxicity and occur 12 to 24 hours after ingestion. Damage to the basement membranes will cause cerebral and pulmonary edema. Patients may become obtunded and develop seizures.
What tests can be performed to determine the purity of the synthesized aspirin? ›Because today's aspirin is mass produced in tablet form, Spectrophotometers are a reliable and economical way to keep the purity of Aspirin consistent throughout the manufacturing process. The purity and amount of acetylsalicylic acid in aspirin can be measured using a Visual Spectrophotometer.
What are the sources of error in the aspirin synthesis lab? ›The possible sources of error in the experiment were: (1) the collected crude aspirin was not dried and immediately subjected to another recrystallization; (2) the Erlenmeyer flask used was not clean, and; (3) the solution did not heat in a steam bath for 15 minutes.
How do you determine the purity of aspirin by titration? ›
One way to determine the purity of aspirin is to hydrolyze it with a NaOH solution and titrate the remaining NaOH. The reaction between aspirin and NaOH is: C9H8O4(s)+2OH−(aq)→C7H5O−3(aq)+C2H3O−2(aq)+H2O(l) C 9 H 8 O 4 ( s ) + 2 O H − ( a q ) → C 7 H 5 O 3 − ( a q ) + C 2 H 3 O 2 − ( a q ) + H 2 O ( l ) .
What is the purpose of the FeCl3 in this aspirin test? ›Iron (III) ion reacts with phenols to form a purple complex. Salicylic acid contains a phenol group, but acetylsalicylic acid does not. Therefore, if you add FeCl3 to an aspirin sample and you see a purple color, it means that there is still some salicylic acid present and the sample is impure.
Which product is produced by the aspirin synthesis reaction? ›The byproduct of the synthesis of aspirin is acetic acid. During the reaction of salicylic acid with acetic anhydride for the synthesis of aspirin, acetic acid comes out to be the byproduct with formula CH3 COOH. Therefore, the correct answer is e. acetic acid.