We made Acetylsalicylic Acid by reacting Salicylic Acid and Acetic Anhydride. We conducted a series of tests which included white powder comparison, melting point, Iron (Ⅲ) ion, and spectrophotometer to determine the purity. All these tests indicated that we had some amount of contamination. By combining the results of our tests, and spectrophotometer readings, we concluded that our sample was not very pure. We calculated that we had about 14% Salicylic Acid in our purified sample. We claim that a safe dose of our aspirin to take is 7.06 milligrams or 84.72 milligrams in day. Introduction: Acetylsalicylic Acid or more commonly known as aspirin, is a nonsteroidal drug used as a moderate pain reliever, a fever reducer and for anti-inflammatory …show more content…
To make aspirin, we reacted Salicylic Acid (C7H6O3) and Acetic Anhydride (C4H6O3) to make Acetylsalicylic Acid (C9H8O4) and Acetic Acid (C2H4O2). To start we made a 1000 milliliter boiling water bath using a hotplate that was warm enough to keep the water boiling. We put 4.00 grams of Salicylic Acid and 10.0 milliliters of Acetic Anhydride in a 250 milliliter Erlenmeyer flask. Then we carefully added in 10 drops of concentrated Sulfuric Acid (H2SO4) as a catalyst for the reaction. Next we suspended the flask in the boiling water for the full 10 minutes to ensure a complete reaction. We then removed the flask from the boiling water bath and let it cool. When cool, we added 4 milliliters of water dropwise into the solution and swirled. After swirling for a few minutes, we added 80 milliliters of distilled water and stirred the solution with a glass rod until crystals began to form. Once we noticed crystallization, we placed the flask into an ice water bath for 10 minutes in order for crystallization to continue. Using filter paper and a funnel, we filtered the Acetylsalicylic Acid crystals from the solution of Salicylic Acid and Acetic Acid. We rinsed the crystals twice with 10 milliliters of water each time. We then split our sample in half and purified one …show more content…
In our experiment we reacted Salicylic Acid (C7H6O3) and Acetic Anhydride (C4H6O3) to make Acetylsalicylic Acid (C9H8O4) and Acetic Acid (C2H4O2). We used Sulfuric Acid (H2SO4) as a catalyst in the reaction. To calculate the limiting reagent we figured that 4.00 grams of Salicylic Acid is 0.02897081 moles. For Acetic Anhydride, we found that the conversion to grams is 1.08 grams per milliliter. We used that to find that in 10 milliliters of Acetic Anhydride we had 10.8 grams or 0.10584085 moles. The ratio of the coefficients are 1:1 so there should be the same amount of moles for Acetic Anhydride and Salicylic Acid. Since the moles are not the same, Salicylic Acid is the limiting reagent and Acetic Anhydride is the excess reagent. We expected to have 7.84 grams excess of Acetic Anhydride. We predicted that we would make 5.23 grams of Acetylsalicylic Acid and 1.66 milliliters of Acetic Acid. We actually made 1.61 grams of aspirin and we did not measure the amount of Acetic Anhydride
The experimental Fischer esterification of 8.92g of acetic acid with 5.0g of isopentyl alcohol using concentrated sulfuric acid as a catalyst yielded 4.83g (65.3% yield) of isopentyl acetate. The product being isopentyl acetate was confirmed when the boiling point during distillation had similar characteristics to that of the literature boiling points2. Physical characteristics like color and smell also concluded a match of our product with what was intended. 1H-NMR spectroscopy analysis supported this claim due to the fact that the integration values and chemical shifts were comparable to isopentyl acetate. Lastly, infrared spectroscopy (IR) showed similar key characteristics of our product’s wavelengths to that of pure isopentyl acetate5.
The weight of the final product was 0.979 grams. A nucleophile is an atom or molecule that wants to donate a pair of electrons. An electrophile is an atom or molecule that wants to accept a pair of electrons. In this reaction, the carboxylic acid (m-Toluic acid), is converted into an acyl chlorosulfite intermediate. The chlorosulfite intermediate reacts with a HCL. This yields an acid chloride (m-Toluyl chloride). Then diethylamine reacts with the acid chloride and this yields N,N-Diethyl-m-Toluamide.
From the both derived calculations, the aspirin obtained is relatively pure. This result could be due to possible experimental errors or inaccurate techniques performed which led to a percent yield that is not up to expectation. Furthermore, the reaction might not have been completely reacted or the salicylic acid in the solution of acetic anhydride and concentrated sulphuric acid did not dissolve completely when it was being heated. These factors might affect the overall results of the aspirin yield
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].
1. Read through the steps in this procedure. Prepare a data table to record the mass of the solute, the initial volume of water, the total volume of water after step 9, and the temperatures at which the solutions began to crystallize.
All the bond types in this molecule are covalent bonds because all the elements involved are non-metals. There are three carbon rings in the molecule and each carbon ring is connected with an oxygen. The inactive ingredients alcohol, camphor, castor oil, collodion, ether, ethylcellulose, hypophosphorous acid, menthol, and polysorbate 80. The active ingredient in Compound W is salicylic acid. Salicylic acid, also called ortho-hydroxybenzoic acid, is mainly used for pharmaceutical products such as aspirin and Compound W. The chemical formula for salicylic acid is C7H6O3. In 1838, an Italian chemist Raffaele Piria created salicylic acid from salicylaldehyde. This was the first time salicylic acid was ever prepared. Later on in 1860, two German chemists discovered an synthesis based on phenol and carbon dioxide. However, today salicylic acid is not made either of these ways. It is made from dry sodium phenoxide and carbon dioxide which is then followed by treatment with acid. Even though salicylic acid is prepared, it can be found in small quantities in plants of the genus
Introduction Acetaminophen, also known as Paracetamol, is an organic compound that is commonly used as a medication for pain and fever relief. It has been around for a while and is found under several different brand names around the world. With research, the chemistry behind acetaminophen can be discovered as well as its practical applications, its adverse effects to society and the environment, and other information surrounding this compound. The History
The collected crystals were rinsed in warm water to remove any additional mother liquor. Care was taken during rinsing to avoid dissolving the crystals. A few crystals were taken and observed closely. Hot water was used to let all the crystals to be collected in the container; we used as little water as we can to avoid any destruction of the crystals. The crystals contain a small amount of water was transferred to a small pot and heat was applied to the crystals dissolved, and some frothing were seen.
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.
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
After a while you will start to see your crystals forming. Times may vary based on where you put them and what salt you use. Once you see your crystals forming you can take them out and examine them. Depending on the salt they will have different forms. Some may be clumpy, small, needle like, pointed, rounded, large or discolored. Some of these will also depended on where you grow them and how long you let them
First, weigh 17.50 grams of coconut or vegetable oil in a 250-mL beaker. You may use the graduated cylinder for this because 1 gram is equal to 1 milliliter. Second, using the scientific balance, weigh 0.125 grams of stearic acid in a small watch glass. Then add the stearic acid into the oil in the beaker. Third, heat the oil until the stearic acid dissolves altogether. Fourth, cool the oil and stearic acid mixture to 40-45 °C. You can determine the temperature with the use of the thermometer. While waiting for the mixture to cool, you may wash your graduated cylinder. Fifth, add 32.0 mL of 32.5% sodium hydroxide (NaOH) or lye solution to the above mixture using a graduated cylinder. Maintain the temperature at 40°C and continue on stirring until the saponification process is complete. Lastly, pour the solution into a mold and allow it to harden overnight. During this process, problems may unexpectedly arise. If you accidentally spilled any chemicals such as the stearic acid, use a tissue to gather them and immediately dispose afterwards. If a clear layer of liquid appears at the bottom of the beaker even after a prolonged period of stirring, add a very small quantity of stearic acid and continue on stirring and heating the mixture. There are also additional options available, such as pouring about 0.5 mL of any body-safe, essential oil or perfume. You may also try to use other acids
1. The labels have fallen off of three bottles thought to contain hydrochloric acid, or sodium chloride solution, or sodium hydroxide solution. Describe a simple experiment which would allow you to determine which bottle contains which solution.
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
: 0.001 Therefore 0.001 moles of H2SO4 (~ 0.05 moldm-3) is needed to produce 24.00 cm3 of CO2 Volume of H2SO4 0.001 moles of H2SO4, I will use the same approx concentration of H2SO4 ~ 0.05 moldm-3 as I have already prepared it. Volume = moles / concentration = (0.001 / 0.05) × 1000 =20.0cm3 Mass of MgCO3 F.mass of MgCO3= 24.3+ 12.0 + (3 × 16.0) = 84.3 Mass= formula mass × Moles = 84.3 × 0.001 ~ 0.0843g In order to ensure that all of the aqueous sulphuric acid reacts I will use MgCO3 in excess and so I will use 1g of MgCO3.