Analysis of Aspirin

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

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

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

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.

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.

Introduction: The goal or purpose of this experiment was to determine the concentration of Allura Red in red commercially available beverage- Gatorade. Colorimeter are used to shine a LED light through the solution and hit a photocell: it will detect an absorbance or a percent transmittance value. These “value” can be charted and examined as a calibration curve. Calibration curve is a method for determining a substance concentration in an unknown sample

get a cost of $0.40 per ounce for the active ingredients. Finally, to calculate the cost of the active ingredients

The lab checked for neutralization and check if it did not neutralize too much or too little. There were two commonly sold brands examined in this lab which were the Tums and Rolaids. The crushed tablets were dissolved in 0.10 M HCl with a pH indicator bromophenol blue and a solution of KOH was added to it in order to neutralize the solution. The solution turned light blue when it was neutralized. Both the tablets were neutralized and titrated in the same way. From the observations above; Rolaids was better because it had better neutralizing ability per each dollar spent than the Tums. As the Rolaids were 4.07g/$ and the Tums were 4.01g/$ as seen from the observations above. So, the better buy is the Rolaids out of the two as the neutralization ability per dollar spent in the Rolaids is better than the

Is one brand or type any better than another? In this experiment, the purpose was to set out and discover which antacid was the most effective in order to settle these questions once and for all. While every single

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

Aspirin crystals were collected via vacuum filtration with a Hirsch funnel. Then, aspirin crystals were weighted to calculate percent yield and saved to perform TLC

The purpose of the experiment was to compare antacids by the amounts acid they neutralize to find the most effective antacid. Finding the most effective antacid is important because it will help others by allowing them to choose the best product for their heartburn. Titration is the process of which the unknown solutions concentration reacts with a known solution concentration. During the experiment, titration was used to calculate the moles of HCl neutralized by the antacid in this case was gelusil, by knowing the moles of HCl initially added to the flask and moles of HCl neutralized by the NaOH.

The over the counter medication once known only for its ability of easing aches and pains or fighting off fever and inflammation is proving itself to be quite the miracle drug. Aspirin has become part of the protocol for stroke victims as a preventative measure due to its neuro-protective benefits. Stroke can cause lesions in cerebral white matter, which may result in cognitive impairments such as deficits in learning and memory. White matter lesions (WML) have also been linked to increasing the risk of post-stroke dementia. Cerebral white matter damage has been widely overlooked. Comprised of oligodendrocytes that form the insulating myelin in the CNS, white matter is evidentially just as vulnerable to ischemia as gray matter.

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.