Aspirin is a very well known, versatile, cheap and easy to produce pain reliever available today. Not only can Aspirin be used to treat pain, fever and inflammation, but it can also decrease the risk of heart attacks, strokes and blood clots (Wikipedia, 2017). The world currently consumes an estimated amount of 40,000 tonnes of Aspirin per year and demand is only growing. The first recorded use of Aspirin was over 2,400 years ago, in the form of leaves, bark or flowers from the willow tree (Wikipedia, 2017). The only problem with consuming this organic compound was that it had a large pH level causing irritation to the mouth, throat and stomach, usually causing more harm than good. Salicylic acid was not a viable pain reliever until the synthesis …show more content…
A condensation reaction is a reaction where two molecules react to form a larger and smaller molecule (Boundless 2016). A type of condensation reaction is an esterification reaction generally when an alcohol reacts with a carboxylic acid. However, esters can also be created from phenols but requires a vigorous ethanoylating agent such as an anhydride (York, 2000). In the synthesis of aspirin, the phenol mentioned is salicylic acid. The structure of a basic phenol is shown in figure 3 and figure 4 shows the structure of salicylic acid where the phenol group can easily be seen. The required anhydride for the reaction is acetic anhydride. Similarly, figure 6 shows the general structure of an anhydride and figure 5 shows the structure of acetic anhydride. It can be clearly seen that the basic structure of an anhydride is present in acetic anhydride. Therefore, the phenol molecule of the reaction is salicylic acid and the anhydride is acetic anhydride, reacting together to produce the ester of acetylsalicylic acid. The structure of acetylsalicylic acid is shown in figure 7, a combination of a phenol and one side of the anhydride. The other side of the anhydride is the second product which is acetic acid; a by-product of the …show more content…
In terms of aspirin, the forward reaction is forming Aspirin and the reverse forming the reactants. A system like this will reach a point called chemical equilibria. Temperatures effect on equilibrium can be explained by Le Chatelier’s principle (Wikipedia 2017). Le Chatelier’s principle states that when a system in equilibrium is subjected to a change, the system readjusts itself to counteract the applied change. In terms of Aspirin, when the temperature is changed, the system will adjust itself to counteract the change. Figure 8: Synthesis of aspirin reaction. (Chemskills, 2014) As shown in figure 8, the synthesis of Aspirin reaction contains salicylic acid and acetic anhydride (a phenol and an anhydride) to form acetylsalicylic acid and acetic acid (The product and by-product). The chemical equation for the equation is: C_7 H_6 O_3+C_4 H_6 O_3 + Energy ↔C_9 H_8 O_4+C_2 H_4 O_2 (ΔH =
need is water and an ester and we will end up with an organic acid produced as
acid*1 mol s. Acid/ 138.1g s acid*1 mol aspirin/1 mol s. acid * 180.2 g aspirin/1 mol aspirin = 3.9145 aspirin
In 2015, Doweiko’s research found that ”It is impossible for drugs to travel throughout the body without possible side effects“ (Doweiko, 2015, p.16). ”Prime affects versus side effects have been studied in order to find out how drugs harm but are contributing to healing“ (Doweiko, 2015, p. 16). The primary concern appears to be whether harm has to be the lesser concern in order to heal. Aspirin was used as an example of the healing component versus the side
Esterification was used to synthesize aspirin which was by reacting salicylic acid with acetic anhydride. To speed up the reaction, dehydrating agent and conc. sulphuric acid was present. The purity of a substance, which is the aspirin in this particular experiment, can be determined by the identification of its melting point.
Aspirin contains the substance acetylsalicylic acid (ASA), which can relieve inflammation, fever, pain, and known as a “blood thinner”. Aspirin was not officially trademarked until March 6, 1899 when the Imperial Office of Berlin made it official. It has been used for the last 110 years, but its natural form, salicylic acid has been around for thousands by Egyptians, Greeks, and Romans. Aspirin is available in over 80 countries and known as the best non-prescription drug. The most common use of aspirin is to cure headaches and use it as a pain reliever, but aspirin is known to prevent heart attack and strokes. It was first proposed in 1940, but wasn’t confirmed until 1970 when doctors would recommend taking aspirin daily [1].
In the late 1800’s it was discovered that papa-amino-phenol, could reduce fever, but the drug was too toxic to use. A less toxic extract called phenacetin was later found to be just as effective but also had pain-relieving properties. In 1949, it was learned that phenacetin was metabolized into an active but also less toxic drug, acetaminophen. Since then, acetaminophen has been sold under many over the counter brand names, most popular being Tylenol.
As a final point, the unknown secondary alcohol α-methyl-2-naphthalenemethanol had the R-configuration since it reacted the fastest with S-HBTM and much slower with R-HBTM. TLC was a qualitative method and ImageJ served as a quantitative method for determining which reaction was the faster esterification. Finally, 1H NMR assisted in identifying the unknown from a finite list of possible alcohols by labeling the hydrogens to the corresponding peaks.
Opium, the first opioid, is derived from the sap of opium poppies, whose growth and cultivation dates back to the ancient civilization of Mesopotamia around 3400 BC. Egyptians and Persians initially used opium. Eventually spreading to various parts of Europe, India, China, and the Middle East. During the 18th century, physicians in the U.S. used opium as a therapeutic agent for multiple purposes, including relieving pain in cancer, spasms from tetanus, and pain attendant to menstruation and childbirth. It was merely towards the end of the 18th century that some physicians came to recognize the addictive quality of opium.
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.
The conical vial was placed in a small beaker and allowed to cool to room temperature. The mixture was Cooled thoroughly in an ice bath for 15-20 minutes and crystals collected by vacuum filtration on a Hirsch funnel. The vial was rinsed with about 5 mL of ice water and transferred into to the Hirsch funnel and again washed with two additional 5mL portions of ice water. Crystals were dried for 5-10 minutes by allowing air to be drawn through them while they remained on the Hirsch funnel. The product was transferred to a watch glass plate and allow the crystals to dry in air. Crude acetaminophen product was weighed and set aside a small sample for a melting point determination and a color comparison after the next step. Calculation of the percentage yield of crude acetaminophen (MW = 151.2). was done and recorded in the lab notebook.
medicine, "Herbal," in the 2nd century B.C., and was used in China as an anesthetic 5,000 years ago. The ancient Assyrians, Persians, Greeks, Romans, and East Indians used the drug to control muscle spasms, reduce pain, and to treat indigestion. It was commonly used in folk medicines in Africa and Asia. As early as 1611, marijuana was cultivated for its fiber in Jamestown, Virginia. In 19th century America, marijuana was used by the medical profession for treating spastic conditions, headaches, labor pains, insomnia, and menstrual cramps. It is still used as a medicine in the Middle East and in Asia (9).
Today, everyone from health care consumers to providers are learning about natural options to help with being healthy. “Herbalists, or individuals who use herbal remedies to alleviate pain, are on the rise in the United States” (Tremmel 1). In 1995, a survey was taken with about 600 physicians across the count...
Background Information Aspirin is an analgesic (pain relieving) and an antipyretic drug (a drug that lowers body temperature). The main constituent of aspirin is 2 - ethanoythydroxybenzoic acid, also known as acetylsalicyclic acid (shown below right). It was originally made from just salicylic acid (which is found in the bark of a willow tree) when used by the Ancient Greeks to counter fever and pain, but its bitterness and tendency to irritate the stomach caused problems. These were resolved by the German chemist Felix Hoffman, who made the acetyl derivative of salicylic acid in the
·Aspirin (salicylic acid acetate) is an anti-inflammatory (decreases swelling and inflammation), anti-pyretic (fever reducing), and anti-platelet (decreases platelets in the body to thin blood). Many heart treatment patients take an aspirin a day to prevent blood clotting. However, if aspirin is taken in large quantities over long periods of time, it may cause gastric ulcers or other internal damage. The molecular formula of aspirin is C9H8O4. Some examples of Aspirin are Bayer, Ecotrin, and Aspergum.
A mixture of 2 mL aniline, 15 mL deionized water and 3 mL acetic anhydride were stirred. After thirty minutes the reaction was complete and the product was completely precipitated out of the solution. Vacuum filtration was used to isolate the crude acetanilide using a 125 mL filter flask and porcelain Büchner funnel. The product was then washed with 2 mL of ice water and left to dry for about twenty minutes. The observed melting point for the crude acetanilide was 114.3 °C - 115.7 °C. The second procedure dealt with finding a suitable solvent to recrystallize the crude acetanilide. A sand bath was set up and 0.5 mL of each solvent was added to 50 mg of acetanilide in four different test tubes. The four solvents used to test the solubility of the acetanilide were water, ethanol, dichloromethane and hexanes. If the solid dissolved in the solvent at room temperature then it was too soluble and that solvent could be eliminated. The acetanilide completely dissolved in ethanol and dichloromethane, therefore eliminating them from being the suitable solvent. If the solid did not dissolve in room temperature then it was placed in the sand bath and left to boil. If the solid dissolved, it was placed in the ice bath and if crystals were observed coming out of the solution then the suitable solvent was found. The suitable solvent was water as the crystals came out once placed in the ice bath. The