Result Analysis Of Aspirin

Aspirin, Caffeine and Salicylamide were extracted from an over-the-counter pain reliever (BC Powder). These components were separated by manipulating their solubilities by adjusting the acidity and basicity of the solution. By doing this, the three components were forced into conjugate acid (or base) forms, causing selective solubility in either an aqueous or organic solvent. These layers were then separated by use of a separation funnel. Once separated, the components extracted were characterized by measuring the melting point and performing a TLC analysis. Also, the recovered aspirin from the first part of the experiment was recrystallized and compared to that of the

Next, aspirin was extracted from the filtrate. When the filtrate was first mixed with the sodium hydroxide and inverted a couple times, an organic layer formed underneath an aqueous layer in the separatory funnel. Dichloromethane was present in the organic layer because it has a higher density than sodium hydroxide, therefore, it’s in the bottom layer. Aspirin reacts with bases like sodium hydroxide, and it forms the salt sodium acetylsalicylate. The polar salt molecules migrate from the organic layer, where they are insoluble, to the aqueous layer, where they are soluble. After the two layers were separated into two different containers, the aqueous layer, which contained sodium acetylsalicylate, was mixed with hydrochloric acid. A white, cloudy precipitate formed, which was a purer form of the salt. The HCl

Acetic Anhydride and p-Aminophenol were heated in a vial attached to an air condenser to synthesize crude acetaminophen, resulting in 0.097 grams (47.48% yield). The crude acetaminophen was then recrystallized in a solvent of water and methanol over heat resulting in 0.082 grams (39.61% yield) of pure acetaminophen. Melting points of both crude and pure acetaminophen were taken, and found to be 165.9 - 170.9°C and 168.2 - 171.5°C, respectively. The literature melting point of acetaminophen is 169.5 – 171.0°C, indicating that our final product was pure.

Ever wonder about the chemical makeup of tablets that people take for pain relief? Before a tablet can be successfully made, the limiting and excess reactants must be considered. The limiting reactant will affect the amount of the product that can be made. Another reason why the starting reactants must be determined carefully is to make reduce the amount of the reactant in excess so that reactants are not wasted. This experiment uses an Alka-Seltzer tablet. Alka-Seltzer dissolves in water and is an antacid and a pain reliever1. The Alka-Seltzer tablet has many uses such as relief of headaches, ingestion, heart burns, or even upset stomachs2. The active ingredients in an Alka-Seltzer tablet is aspirin, also known as acetyl-salicylic acid (C8H12O4), citric acid (C6H8O7), and sodium bicarbonate (NaHCO3)2. The aspirin in the Alka-Seltzer tablet helps with pain relief. Because of the acid-base chemistry (Brønsted-Lowry), citric acid and sodium bicarbonate produce O2, which makes the tablet fizz when it is dropped in liquid. The Brønsted-Lowry theory shows how the Brønsted-Lowry acid donates a hydrogen ion while the Brønsted-Lowry base accepts the hydrogen ions3. The remaining NaHCO3 that is in excess post reaction with the citric acid is what is used to neutralize stomach acid which helps relief heart burn2. The problem in

The purpose of this lab is to investigate the composition of a compound suspected to be Panacetin, a type of pain-killer. Panacetin is typically made up of sucrose, aspirin, and acetaminophen, but the third component in this experiment is unknown. The unknown component is suspected to be a chemical relative of acetaminophen, either acetanilide or phenacetin. Using techniques such as extraction, evaporation, and filtration, the three components will be isolated based on their solubilities and acid-base properties. Then, the percent composition of Panacetin can be deduced based on the masses of the three dried components. The

Aspirin is one of the most consumed painkillers created up to this date due to its reliability and low expense. It is often used to relieve minor aches and pains, reduce fever and as an anti-inflammatory medication. Due to its wide range of uses, the demand for this pharmaceutical is very high. As a result, manufacturers who produce this drug must be efficient in order to reduce the time taken to produce this drug and produce the in very high quantities.

6. Fe (NO3)3, Ferric nitrate, is much more active than ferrous. It could be identified by its reddish color and when mixed with thiocyanate, it reveals a “bloody” red color.

Working in the hood or a designated work area, add about 1 mL of ethyl alcohol to a clean evaporating dish. Place the evaporating dish on a heat- resistant pad.

Acetaminophen is a worldwide known drug used for aches and pains, but that is all that is thought of when the name is said. Because it is an over the counter medicine, nobody thinks about the effects it can have on you. In fact most people don't even read the warning label. In this paper, it will discuss all of the things nobody even bothers themself to look into. Such as common name/s, what it should be prescribed for, uses, side effects, warnings, drug interactions, and the chemical composition for it. This essay attempts to prove that Acetaminophen is more than just a benign remedy for discomfort.

Five 250mL Erlenmeyer flasks were obtained. Then, 200mL of hydrochloric acid (HCl) was poured into a 600mL beaker. The gelusil

Based on the results of the tests and computations, the experiment did not go completely as what the experimenters want. The crude aspirin obtained was 67% while the percent recovery of the recrystallized aspirin was 50%. It can be concluded that by recrystallizing the crude aspirin, the percent yield decreases. The percent yield was below average and the recrystallized sample was not pure based on the tests that showed positive results of the product being contaminated with salicylic acid. When the product was reacted with ferric chloride, it gave dirty pink complex with undissolved precipitate and in Baeyer’s test, it showed disappearance of the purple complex and formation of brown precipitate after heating, both of which indicates that

This report presents the synthesis of Aspirin (acetylsalicylic acid), as the product of the reaction of salicylic acid with ethanoic anhydride under acidic conditions. Aspirin was purified through recrystallisation by vacuum filtration, followed by desiccation of the Aspirin crystal over silica gel. The percentage yield was calculated as 44.89% and a sample of Aspirin was analysed using infra-red spectroscopy and compared to the spectrum of pure Aspirin, this served as an introduction to the identification of functional groups in organic compounds. The melting point was calculated using an IA9000M apparatus and recorded to be 35.2°C, which was slightly below the melting point of pure Aspirin; known to be between 138-140°C. Both IR spectroscopy and melting point measurement were used verify the purity of synthetic Aspirin made, which proved to be fairly pure under these laboratory conditions.

The purpose of the experiment is to produce common drugs from organic materials. In theory, the experiment tests the idea that the therapeutic drug aspirin can be synthesized from a reaction between salicylic acid and acetic anhydride. Because consuming pure salicylic acid, a derivative of willow bark, can caused stomach pains and be difficult to consumer due to its extremely bitter taste, producing aspirin is of great importance. Aspirin is pleasant to take orally and it only breaks down when it reaches the small intestine, causing little to no damage to the stomach. To meet the primary objective of producing aspirin, a reaction called esterification needs to be undergone. This reaction changes salicylic acid

A historical Development that relates to Aspirin is the father of our modern Medicine Hippocrates, who was a Greek Physician, left records of how they treated headaches, fevers and pains, and to ease child- bearing pains with a powder made of the leaves and bark form a Willow Tree. Also the Ancient Egyptians left a medical text called “Ebers Papyrus” which is also lists willow among a list a plant and animal remedies for pain relief, fever reduction, and as an anti-inflammatory. Also the Roman Celsus recommended Willow extract for treating the symptoms of Inflammations, swollen, red, feverish area, and pain. (Wikipedia “history”) This is relatable as the bark and leaves of the Willow tree are a natural resource of the Salicylic acid, which is found in Aspirin, which made the patients feel better while healing them, similar to the modern Aspirin. Further along in Human history we know that Edward Stone discovered and isolated the key chemical in the Willow bark/leaves called Salicylic Acid. The problem with the Salicylic acid was that it was extremely tough on stomachs and could cause nausea and vomiting, hence the next step in developing Aspirin was to find an effective buffer that would make the Salicylic acid easier for the stomach to handle, a French chemist named Charles Frederic Gerhardt was one of the first to attempt at creating a suitable buffer for Salicylic acid was to combine it with Sodium and Acetyl Chloride,

Headache medicine is a non steroidal mitigating drug,Pain relieving diminishes torment, utilized for the help of migraines and a throbbing painfulness. Calming in higher measurements utilized for the treatment of provocative conditions, for example, joint inflammation.