To complete the objective of this density lab, the following equipment were used two 600-mL beakers, 250-mL Erlenmeyer flask, hot plate, ring stand, 250-mL beaker, stirring rod, balance, Büchner funnel, filter paper, stopper, water aspirator, watch glass, fume hood, 10 mL and 50 mL graduated cylinder. To synthesize aspirin a boiling-water bath was prepared by adding 300-mL tap water to the 600-mL beaker and placed on a hot plate with a ring stand around the beaker. Then 2.1g of salicylic acid, 4-mL acetic anhydride, and 5 drops of concentrated H2SO4 solution were added to the Erlenmeyer flask and the flask was swirled gently until some of the solids dissolved and some undissolved. Utilizing the clamp, the Erlenmeyer flask was placed inside …show more content…
The rubber tube was connected to the water aspirator to form a vacuum suction which would help filter the pure aspirin out. By the 25-mL of chilled distilled water added to the flask would break up crystal lumps utilizing the stirring rod. The filter paper was moistened by adding 2-mL of chilled distilled water after applying the filter paper to the Büchner funnel and turn on the aspirator. The reaction mixture was then gradually added to the Büchner funnel and the water aspirator was disconnected. Then 15-mL of chilled distilled water was added to the Büchner funnel and the aspirator was turned on for 15 minutes and was disconnected when the crystals looked …show more content…
To test the synthesized aspirin, three test tubes were taken, and 1-mL of 95% ethanol and 1 drop of 1% iron (III) chloride solution were added to all the three test tubes. Salicylic acid was added to test tube A, a few crystals of the synthesized aspirin was added to test tube B, and test tube C was used as a control test tube. Each test tube was stirred using a glass stirring rod and the results were recorded. The solutions were then poured into the “Discarded Test Solution” containers. To treat the discarded reaction mixtures, another test tube was taken, and synthesized aspirin was added to it. Then it was clamped and placed under a gentle heat utilizing the Bunsen burner until the crystals were liquified. The odor of the vapor was noted from the test tube. Then 3 drops of phenolphthalein solution were added to the synthesized aspirin and the color was noted. If the solution was colorless 1M sodium hydroxide solution was added dropwise until the solution turned pink. If the solution was pink, then the 1M hydrochloric acid solution was added dropwise until the solution turned colorless. Finally, the solutions were poured out and washed and dry the
Then the reaction tube was capped but not tightly. The tube then was placed in a sand bath reflux to heat it until a brown color was formed. Then the tube was taken out of the sand bath and allowed to cool to room temperature. Then the tube was shaken until a formation of a white solid at the bottom of the tube. After formation of the white solid, diphenyl ether (2 mL) was added to the solution and heated until the white solid was completely dissolved in the solution. After heating, the tube was cooled to room temperature. Then toluene (2 mL) was added to the solution. The tube was then placed in an ice bath. Then the solution was filtered via vacuum filtration, and there was a formation of a white solid. Then the product was dried and weighed. The Final product was hexaphenylbenzene (0.094 g, 0.176 mmol,
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.
* It was almost impossible to tell when the Alka-Seltzer tablet had dissolved, each time the experiment was done. This was a huge problem for the experiment as this could have totally caused problems to the experiment. A special type of detector apparatus, which bleeped when the correct amount of Alka-Seltzer tablet dissolved, could improve this, each time the experiment was done.
A condenser and heat reflux was used to prevent reagents from escaping. Then the solid product was vacuum filtered. The product was recrystallized to purify it and the unknown
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].
Planning Firstly here is a list of equipment I used. Boiling tubes Weighing scales Knife Paper towels 100% solution 0% solution (distilled water) measuring beakers potato chips Cork borer. We planned to start our experiment by doing some preliminary work. We planned to set up our experiment in the following way.
The purpose of this lab was to see firsthand the diffusion of a substance across a selectively permeable membrane. Diffusion is the movement of molecules from an area of high concentration to an area of lower concentration until both concentrations are equal, or as you could more professionally call it, equilibrium. This concept is one that we have been studying in depth currently in Biology class.
Aspirin is derived from a chemical extracted from willow bark: Salicylate Acid. Salicylate Acid has a long history of uses. During Medieval times herbalists used it for its palliative properties. In the mid 1900’s, chemists isolated the active ingredient of willow bark, salicylic acid, and Aspirin was developed. It quickly became the drug of choice as a pain reliever, antipyretic and anti-inflammatory. The first company to develop Aspirin for commercial use was the Bayer Company. Today Aspirin is used daily by millions of Americans to help reduce the risk a heart attack. Until the late 1900’s, with the development of Aspirin alternatives such as acetaminophen and ibuprofen, Aspirin was the most widely used drug around, and a common drug of choice for the overdose patient.
Title: The following lab write-up was based on the “Scientific Measurements” data sheet. The experiments were performed on September 1, 2016. The instructor for the lab was Dr. Larsen.
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
where m is the mass, and V is the volume of the fluid. Density of a fluid can be obtained through various means. One of the methods to determine a fluid’s density is by using the density measuring device, or called
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
Summary and procedures: the use of the different types of apparatus to get the correct results is always knowing it functionality and the correct significant digits. We always must make sure the balance should be 0.000 g when it is completely empty. In the case of the electric balance, the tray must to be clean and free of water or dirt, this machine is very accurate and precise. In the use of the flask and beaker, those should be cleaned before and after the use, that is how we avoid and create accidents for unknow chemicals or substances that were used before in the containers. Starting with the procedure, first is determine the mass for each balance in use, then record all the necessary data of that.
The experiments that have been done with density is to see how it works. It may seem like magic with liquids stacking on top of each other. They also have to see what is more dense for other experiments, or to invent something for the future for new and smarter people. Experiments are probably very important because like anything, you need to figure out how, and why what happens actually does happen. Some experiments can even be done at home with everyday items like an empty water bottle, food coloring, and water to make an amazing
·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.