Bc Synthesis Lab Report

In experiment two, the drug Panacetin was separated by a series of chemical reactions into its three components: sucrose, aspirin, and an unknown active ingredient, either acetanilide or phenacetin. The purpose of this lab was to determine what percentages of each component is present in the pain-killer. The initial step was to dissolve Panacetin in dichloromethane. However, sucrose is insoluble in dichloromethane because organic molecules are soluble in organic solvents, and dichloromethane is an inorganic solvent, so only aspirin and the unknown dissolved. By using gravity filtration, sucrose was filtered from the solution and 0.30g of solid was collected.

The NMR spectra solution #33 (the unknown) matched closest to that of 4-tert-butylbenzylphenolether 14) The yield (.468 g) makes sense because it was lower than the theoretical yield calculated (1.57 g). Yield may have been lost because the crystals formed too quickly, causing some of them to be small in size and seep through the filter and into the filtrate. 15) The percent recovery of 55.7% makes sense.

Pre-Lab: Analgesic drugs are known for reducing pain, while antiseptic drugs reduce symptoms such as fevers and swelling. However, some of these drugs can reduce both illnesses. To obtain a pure compound in these drugs, the scientist needs to separate the desired compound by taking advantage of the different physical and chemical properties. Such as; different boiling points, melting points and their solubility properties. To do this a chemist can also asses the differences between acidic and basic substances when they are added to water soluble mixtures. Within this current experiment I will asses the

The experimental results indicate that the identity of the unknown tablet was determined by measuring and comparing the distance traveled by the known standards to the unknown standard. The Rf value of Caffeine was 0.2 and of the unknown was also 0.2 as shown by the calculations above, this proves that the unknown substance was Caffeine, given that the unknown substance traveled 1.5cm and was equal to the distance traveled by Caffeine, showing that they were the same. Acetaminophen had a Rf value of 0.7 with Aspirin having a Rf value of 0 and Ibuprofen also having a Rf value of 0. This shows that the unknown tablet was Caffeine.

The vial was removed from the heat and cooled to room temperature. The spin vane was rinsed with 2-3 drops of warm water over the conical vial. The vial was cooled to room temperature then placed in an ice bath for 15 minutes. The liquid was decanted from the mixture and the resulting crystals were dried on filter paper. The crystals were then placed on a watch glass for further drying. The crystals were weighed and a small sample was placed into a capillary tube for melting point determination.

The problem proposed in the experiment is an unknown ingredient found in generic Panacetin tablets that must be discovered. Panacetin tablets are known to contain aspirin, acetaminophen, and sucrose; therefore, the tablets tested, containing aspirin and sucrose, are thought to contain an unknown of something similar to that of acetaminophen such as acetanilide or phenacetin. Another problem trying to be sought out in the experiments is whether or not the composition of Panacetin as stated on the label is accurate.

TLC Analysis of Analgesic Drugs Author: Monique Amanda Mendez Lab Instructor: Wenmo Sun Organic Chemistry Lab 243A: Section 038 Date Work Performed: 02 September 2015 Discussion: Lab 1a - TLC Analysis of Analgesic Drugs Discuss the relative polarities of the components of the analgesic drugs based on their functional groups The relative polarity of the analgesic drugs depends on their functional groups. Polarity of the drugs depends on several differentiating factors which include how the compound can hydrogen bond to itself or another compound, the number of electronegative atoms that are present within the structure of the compound, the net dipole moment of the molecule and the polarizability of the bonds or atoms that are present within the compound, which can highly define how polarizable the compound is or will be. The more polar the functional group, the stronger the bond is to the stationary phase, making it slower for the molecules to move down the TLC plate, thus the stronger it will be absorbed on the surface of the solid phase.

Which brand of painkilling medicine dissolves the fastest and does flavor, coating, and color of the pill affect the dissolution time? If several different pain neutralizing pills are placed in stomach acid and timed in order to find out which pill dissolves first, then the most effective pill will be the first to dissolve. In order to test this, eight different types of pain neutralizing medicine were put into simulated stomach acid and timed. Normal strength, liquid gel capsules, and children's flavored pills were all tested. In order to accurately simulate stomach acid, vinegar, which has the same pH levels of stomach acid, was heated to thirty seven degrees Celsius and stirred constantly and evenly. The pills tested were Advil, Children's

Aspirin, also known as acetylsalicylic acid, was among the earliest drugs to be synthesized and is still commonly used worldwide today. Aspirin is useful as an anti pyretic, anti platelet, analgesic, as well as, anti-inflammatory drugs. Its main clinical importance now is in the treatment of cardiovascular disease. It can be orally administered and is rapidly absorbed as the liver metabolizes 75%, but can’t be given to human beings under the age of 16. The elimination of aspirins metabolite, salicylate, follows first-order kinetics at low doses, but at high doses, it follows saturation kinetics. (Rang et al., 2012).

In this experiment, I collected the willow bark then boil it using the heating flask. I used the rotary evaporator to separate water from the crude product. I further used centrifugation and crystallization of the compound. At last, I compared my aspirin sample with an analgesic aspirin using the NMR at Boston College.

Aspirin is a commonly used pain killer and an anti-inflammatory. Hagiwara, Kaneko, Murata, Ikegami, and Oshima (2014) reported that aspirin or acetylsalicylic acid (ASA) is used to treat trauma, infections, and rheumatic diseases. Hagiwara et al. (2014) stated that,” a dose of ASA of greater than 150 mg/kg is toxic, and ASA intake of more than 500 mg/kg causes severe toxicosis” (p. 72). Since an overdose of ASA could be fatal, it is important that companies list the exact amount of aspirin in one tablet. The purpose of this lab is to confirm that aspirin tablets contain the amount of medicine that is advertised on the bottle. If the aspirin bottle states that there is 325 mg in one tablet, then there should be 325 mg of aspirin found when titrated. In an acid base reaction, both solutions are neutralized when there are equal parts of acid and base. This relationship is vital to determine the concentration of a solution through standardization. (Northern Virginia Community College, 2016, para. 1). Solutions are standardized by using titration, which is a method of measuring the volume of a solution needed to fully react and neutralize another reagent (Northern Virginia Community College, 2016, para. 1). To know when the solutions are equivalent, an indicator called phenolphthalein is put into the solution with

This series of labs aimed to synthesize and characterize aspirin from salicylic acid and acetic anhydride. The synthesis and recrystallization procedures entail the production and purification of aspirin. Several characterization techniques utilized in order to test its purity. Methods to characterize purity include determining the melting point of pure and crude aspirin, the pH

The objectives of this lab are, as follows; to understand what occurs at the molecular level when a substance melts; to understand the primary purpose of melting point data; to demonstrate the technique for obtaining the melting point of an organic substance; and to explain the effect of impurities on the melting point of a substance. Through the experimentation of three substances, tetracosane, 1-tetradecanol and a mixture of the two, observations can be made in reference to melting point concerning polarity, molecular weight and purity of the substance. When comparing the two substances, it is evident that heavy molecule weight of tetracosane allowed

Alkaloids occur naturally and considered an organic compound that provides many benefits for both humans and animals. Nevertheless, alkaloids embrace caffeine as a member of the family, which exists in many natural drinks and manufactured drinks. Furthermore, the extraction of caffeine was done through the previous experiment in which boiling water and dichloromethane separated the organic layer and sodium carbonate worked on excluding the Tannins acid. Later on, caffeine was completely extracted by removing the solution via heating (Rains, 2016). Proceeding with experiment, the duration of boiling for tea was eight minutes whereas for coffee, boiling duration was fifteen minutes. Moreover, after boiling process, both liquids were transferred to a separatory funnel and was inverted for a total of four times and vented after every invertion to allow for the accumulation of undesired gas to

Thus, an important determinant for the diffusion of the substance through the SC is the logP value (table (18). According to this, caffeine has high aqueous solubility so will be presented to the SC in high concentration but its partitioning to the SC will be low. On the other hand, the hydrophobic molecule butyl paraben has good partitioning properties to the SC but its low aqueous solubility will limit the available concentration. The unionized and ionized forms of ibuprofen will behave similar to butyl paraben and caffeine respectively. Methyl paraben has an intermediate hydrophobic character which allows acceptable aqueous solubility and partitioning tendency to the SC, thus higher diffused amounts and flux values were