Characteristics 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

Separation and Purification of the Components of an Analgesic Tablet. Cora Bruno, Lab Section E. Aspirin, Caffeine and Acetaminophen were separated from four analgesic tablets of Excedrin using extraction techniques. 5% wt/vol NaHCO3, 4M HCL, ethyl acetate and deionized water were used to separate the three active components. MgSO4 was used to dry each extraction. Aspirin was isolated using a hot water bath and weighed to determine the percent theoretical recovery and the actual percent recovery of aspirin. After separation, Aspirin (ASA), Caffeine (CAF), and Acetaminophen (ACE) were purified and identified using Thin Layer Chromatography (TLC). Standards and purified ASA, CAF, and ACE were spotted on the silica gel (stationary phase) of the

In this experiment the concentration of acetyl salicylic acid (ASA) in an aspirin tablet will be determined. This can be done by dissolving a tablet in a strong base, NaOH, and titration it with a strong acid, HCl. The quantity was found to be about 75.5% of the weight of the tablet, or about 318 mg per tablet. This value tells the pharmaceutical companies how much to state the recommended dosage as based on how much ASA is needed to feel the headache and pain resistant effects. Also it can be used to state precautions for the customers based on the known LD50 value (200 mg/kg).

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.

This experiment involved three steps: synthesis of aspirin, isolation and purification, and the estimation of purity of the final product. The synthesis involved the reaction of salicylic acid and acetic anhydride in the presence of a catalyst, phosphoric acid, H3PO4. When the aspirin was prepared, it was isolated and filtered. The percentage yield of the synthesis was calculated to be 78.42%. The experimental melting point range of aspirin was determined to be 122 -132°C. Due to its wide range, and lower value than that of the theoretical melting point of 136°C, it was

The goal of this experiment was to synthesize aspirin. In this experiment aspirin, also known as acetylsalicylic acid, was synthesized from salicylic acid and acetic anhydride. In the reaction the hydroxyl group on the benzene ring in salicylic acid reacted with acetic anhydride to form an ester functional group. This method of forming acetylsalicylic acid is an esterification reaction. Since this esterification reaction is not spontaneous, sulfuric acid was used as a catalyst to initiate the reaction. After the reaction was complete some unreacted acetic anhydride and salicylic acid was still be present in the solution as well as some sulfuric acid, aspirin, and acetic acid. Crystallization, which uses the principle of

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

Both Aspirin and the Unknown are soluble in dichloromethane, due to their non-polar characteristics. To separate the two components, sodium bicarbonate was added (see figure 3). Sodium bicarbonate reacted with aspirin and converted it to a salt, also forming water and carbon dioxide. It was observed that the solution "fizzed" when this reaction took place, showing the release of carbon dioxide. The newly formed salt then traveled to an aqueous layer where it was soluble, while the unknown remained in the dichloromethane layer. The two layers were then separated. To collect an aspirin solid, the combination of the addition of HCl and the process of vacuum filtration helped to break down the salt and form a solid. Then the solid was placed in the Fisher Scientific Biotemp Oven to dry it to a constant mass of 0.091 g, 32.97% of the total composition. The

Industrial production of Aspirin is dependent on the company producing the drug; however the general method of production is known as slugging or dry-granulation. In this method, corn starch is mixed with pure water and is then heated and

The purpose of this lab was to synthesize aspirin, determine the theoretical yield, compare the percent yield to the theoretical yield and test the purity of aspirin by adding Iron (III) chloride to the product.

The purpose of the lab was to synthesize aspirin and oil of wintergreen, and to determine its purity using recrystallization process, determining its melting point and using back-titration. To synthesize aspirin, salicylic acid and anhydride was used to drive the reaction to completion. In the synthesis of oil of wintergreen we reacted salicylic acid and methanol to produce methyl salicylate. This reaction is an example of a condensation reaction where the carboxylic acid and alcohol group combine to form an ester. In producing aspirin, we wanted to obtain the purest form, so we removed impurities such as unreacted salicylic acid and acetic acid. Acetic acid was removed by rinsing the sample in water because acetic acid is soluble in water. Salicylic, however, was removed by using the recrystallization process because it is insoluble in water. To recrystallize, we dissolved a sample of crude aspirin in warm ethanol and let it cool. Because aspirin is less soluble in ethanol than salicylic acid, it will crystallize out of the solution. To obtain the purified aspirin sample, we then filtered the solution to separate it from the impurities. To determine qualitatively the purity of the recrystallized aspirin, we determined its melting point using a melting point apparatus. Using the idea of freezing point depression, the presence of impurities will lower the melting point of the substance. Thus, by comparing the melting point to the actual

Acetaminophen is also found in combination with other active ingredients, otherwise known as combination medicines, which can treat conditions such as flu or cold symptoms, allergy, and sleeplessness. Medicines that contain this pain relieving drug can come in many physical forms including drops, syrups, and pills. It is easy for a person to not be able to recognize how much acetaminophen they are ingesting because of the many forms and medications it can be found in, therefore all people should be cautious and monitor their medicinal intake (U.S. Food and Drug Administration 2015).

Although the mechanism of action of acetaminophen is unclear, it is generally believed to work the same was as ibuprofen. Ibuprofen and acetaminophen produce therapeutic effects by reversibly inhibiting cyclooxygenase and thus blocking the synthesis of proinflammatory prostaglandins, prostacyclins and thromboxanes from arachidonic acid. The effects of these prostanoids include lowering the pain threshold thereby exaggerating pain perception. Inhibiting the synthesis of these prostanoids increases the pain

Its chemical formula is C9H8O4, meaning it has 9 carbon (C), 8 hydrogen (H), and 4 oxygen (O) ions. Aspirin is avaliable OTC (over-the-counter, meaning you don't need a perscription to buy it) and treats mild pain, fever, and can also help prevent arterial and venous thrombosis (blood clots). In dry air it's quite stable, allowing it to be stored for long periods of time in medicine cabinets so it can be available whenever you need it. Acetylsalicylic acid binds to the serine in cyclooxygenases, which is how it can prevent inflammation and platelet accumulation- which can lead to blood

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.