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Data and observations obtained during the experiment in recrystallization
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Synopsis The general objective of this experiment was for the students to familiarise with the preparation of a simple organic compound and to purify the compound by recrystallization. This experiment allows the students to conduct synthesis of aspirin, reinforcing the skills of recrystallization and the technique of melting point determination. 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. Both experimental successes and errors were analysed. The mass of aspirin …show more content…
The aspirin crystals were packed into 3 small capillary tubes to ensure that they are compressed so as to prevent any air gaps. Subsequently, the aspirin crystals that are in the 3 capillary tubes are placed into the melting apparatus and the temperature range was recorded. Since the range is quite far from the theoretical value of 140°C, aspirin's purity attained was low due to impurities present. One potential reason is because of the swift cooling. When the aspirin is left to cool, the crystal lattices will form too rapidly which will surround other molecules thus making the aspirin impure. Another reason could be because the recrystallized aspirin has not dry completely and there might me left over solvent that will affect the temperature range of the aspirin. 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
In the first section, the Synthesis of Aspirin, salicylic acid was weight to be 3.029 grams using mass by difference since it was weighed on a 150 milliliter beaker. 9.23 milliliters of the acetic anhydride and 14 drops of 85 percent phosphoric acid were added to this beaker. A Bunsen burner provided by the laboratory was then used to boil the just mixed combination by producing a flame underneath the positioned beaker on top, and then allowed to cool for several minutes after the Bunsen burner flame was terminated. Two quantities of distilled water were then added to this mixture to make it cool even further, which were 41 drops and 30 milliliters. After cooling for some time, this beaker was placed into an ice bath in order to start the crystallization process. A glass rod was used to scratch around the bottom and the sides to catch all of the crystallized Aspirin that was being formed during this whole process. Then, by using a Buchner funnel and filter paper, which was placed on top of the flask connected to a water aspirator with rubber tubing, the excess liquid was removed from the just scraped Aspirin crystals when the Aspirin was placed on the filter paper. Using a medicine dropper, the Aspirin crystals on the filter paper were washed with distilled water just so that any non-pure substances were removed from the crude product. When these crystals were then ultimately dry, they were placed on a watch glass and put into an oven for 30 minutes. Then they were weighed by mass by difference to yield 2.4667 grams of crude s...
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
Aspirin is also known as Acetylsalicylic acid. It is composed of nine Carbon atoms, eight Hydrogen atoms, and four Oxygen atoms. There are many chemical properties to it. The melting point of aspirin is about one hundred and thirty-five degrees Celsius and the boiling point is one hundred and forty degrees Celsius. It has a density of 1.35 grams per milliliter and the molar mass is 180,160 g/mol (1). This means that the molecule is relatively dense. There is more weight than there is volume. Aspirin is described as odorless and colorless to where the color is white. It looks like a crystal-line powder at room temperature. It is a relatively stable molecule that should be stored at room temperature (2).
The purpose of conducting this experiment was to synthesise and characterise for the preparation of benzocaine via a fishcer esterification reaction by the means of amino benzoic acid alongside ethanol. The product was also precipitated from a solution in order to gain a pH of 8.The secondary aim was to esterify the reaction in an equilibrium reaction catalysed via the addition of acid shown below:
Aspartame or known by its chemical formula of C14H18N2O5, is a very common chemical food additive usually added in artificial sweeteners for coffee and other products like Splenda and Equal. It is also mixed with other food products like candy, gum, vitamins and supplements. Its molar mass is 294 grams per mol or it has 294 as its molecular mass. Its chemical structure forms a dipeptide-methyl ester (Walters, 2001). Aspartame is known as a synthetic chemical combination which is built approximately on phenylalanine, aspartic acid and methanol (Wells, 2011). It is a solid and can dissolve with water (Walters (2)). It is chemically manufactured by using tritylation and chlorination ("Chemical Process Steps," n.d.). But when its manufacturing process is discussed, its patent reveals that it uses by-products of genetically-modified cells and later treated with chemicals and methanol to produce aspartame (Butler, 2013).
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.
Aspirin (acetylsalicylic acid) is a type of acid categorized as a salicylate, this acid works as a pain reliever in the body because once digested it lowers the amount of substances already in the body that cause pains, fevers and flare ups. Also, this chemical is administered to people for prevention of heart attacks, strokes, and angina which is also known as severe chest pains. Aspirin is created by chemically synthesizing salicylic acid through the acetylation with acetic anhydride, synthesizing aspirin comprises of three steps, synthesis of it, isolation and purification of it, and testing the purity of the aspirin made. Synthesizing aspirin is done by reacting salicylic acid and acetic anhydride with a catalyst, in which phosphoric acid (H3PO4) is used. After the aspirin has been prepared (synthesized), it must be isolated and purified. Aspirin is insoluble in cold water, therefore it can be isolated by filtering the cold solution product of the reaction. In order to remove the unreacted salicylic acid, acetic anhydride, acetic acid product and phosphoric acid the solution must be purified, the acetic anhydride is decomposed simply through the use of adding water after the reaction has finished (C4H602 + H20 2C2H402). Acetic acid and phosphoric acid can be removed from the solution by soaking the aspirin in cold water since they are soluble in water. The final ending step of purifying the aspirin is through a process referred to as recrystallization. This is when the aspirin is placed in warm ethanol, the solution is cooled, and the aspirin crystallizes leaving the salicylic acid and other impurities inside the solution. Lastly testing the purity of the finished product is achieved mainly from a melting point test a common...
During the first part of the lab the crude sample of acetylsalicylic acid, Aspirin, was synthesized. The synthesis of Aspirin shows a general trend of chemical reactions known as esterification reactions. The compound containing a hydroxyl group reacts with a compound containing a carboxylic acid group, producing an ester molecule and water. Since this reaction is slow, the lab used acetic anhydride instead of acetic acid to drive the reaction to completion. As a result, the chemical formula is
It could have been lower than 100% because some product was lost during the recrystallization process, or due to an incorrect separation of the impurities when cooling the mixtures. The melting point data confirmed that the synthesized crystals were likely identical to the methoxybenzyl phenol ether because the mixed melting point was the same as the purified crystals. If the products were different or the synthesized product had to many impurities in it then the mixed melting point would have been lower than that of just the crystals, by themselves. The TLC made sense, after looking at the TLC plates under UV light and the calculation of the Rf values, it was confirmed that the 4- Methoxy-phenol was present in the unknown.
Organic compounds are naturally permeated with impurities that can possibly pose problems in organic synthesis reactions. Therefore, an important part of organic chemistry lab is in the purification of substances. Unit three was a technique experiment in distillation, and its purpose was in the introduction of two types of distillation methods, although there are various other types. The main purpose of the lab was learning how to distinguish the appropriate time to use either of the distillation methods and learning how to interpret the analysis tools employed to determine the purity of a distillate. The first week of the unit separated acetone and ethanol via the fractional distillation method, while the second week separated the acetone
This research task and practical is performed with the aim of investigating the formation of esters through the reaction between different alcohols with carboxylic acids and discussing their usage as
The purpose of this experiment was to study the reactions of amino acids and aspartame. Several solutions were prepared and used in TLC analysis. A permanganate test and a ceric nitrate test were also performed. The summary of the results is shown below.
...light of paracetmol’s physiological effects. The compound exhibits characteristics that mirror other analgesics and anti-pyretics but also displays unique properties that can be advantageous in certain treatment plans. Its anti-inflammatory activity is not as strong as other similar medications known as NSAIDS; fully refereed to as non-steroidal anti-inflammatory drugs. The main mechanism proposed for paracetamol involves the highly selective inhibition of an enzyme called cyclooxygenase; abbreviated COX. There are two isoenyzmes of cyclooxygenase are of similar molecular weight and structure but each take on different functions. They are labeled COX-1 and COX-2. COX-1 is present in most tissues and but functions more specifically on maintaining the lining of the stomach. It also plays other vital roles within the body such as platelet and kidney function.
·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.