Chemical Determination Of Panacetin

The purpose of this experiment is to separate the components of Panacetin and to see if the actual percentages of the three components matched the expected percentages. The second purpose of this experiment is to identify the unknown component that is present in Panacetin. In real world applications, this can be used to separate and identify components of many different things. One example is of “biofuels and chemicals produced by biological processes such as fermentation and algae often require a liquid-liquid extraction as the first step in recovery and purification” (Typical Industrial Applications, 2017). Another example that could be more relevant is “essential oil extraction that is used in pharmaceuticals, flavors, fragrances

The main goal of this lab was to determine which of the acetaminophen and acetylsalicylic acid exists in Anacin and which exists in Tylenol. In order to achieve this goal, Thin Layer Chromatography, an approach that uses the difference in the strength of intermolecular forces and polarity in molecules to separate mixtures, was used

Aspirin, Caffeine and Salicylamide were extracted from an over-the-counter pain reliever (BC Powder). These components were separated by manipulating their solubilities by adjusting the acidity and basicity of the solution. By doing this, the three components were forced into conjugate acid (or base) forms, causing selective solubility in either an aqueous or organic solvent. These layers were then separated by use of a separation funnel. Once separated, the components extracted were characterized by measuring the melting point and performing a TLC analysis. Also, the recovered aspirin from the first part of the experiment was recrystallized and compared to that of the

The purpose of experiment three was to identify the unknown component in the drug Panacetin. The use of physical properties can help identify unknown compounds and estimate the degree of their purities. In this experiment, solubility in boiling water and melting point were used to determine if the unknown was acetanilide or phenacetin. Since both compounds are soluble in boiling water and insoluble in cold water, recrystallization was used to remove any impurities from the solid.

Panacetin is an analgesic (pain reducing) and antipyretic (fever reducing) drug that is sold in drug stores. However, there is a suspicion that this bottle may be counterfeit, not containing the chemicals that it should. Panacetin should be made up of about 50 percent of the unknown component that we previously separated out of Panacetin for testing. We suspect that this unknown compound is either acetanilide or phenacetin, both of which can be toxic to humans. It is very important that this component is

This experiment involved three steps: synthesis of aspirin, isolation and purification, and the estimation of purity of the final product. The synthesis involved the reaction of salicylic acid and acetic anhydride in the presence of a catalyst, phosphoric acid, H3PO4. When the aspirin was prepared, it was isolated and filtered. The percentage yield of the synthesis was calculated to be 78.42%. The experimental melting point range of aspirin was determined to be 122 -132°C. Due to its wide range, and lower value than that of the theoretical melting point of 136°C, it was

Ever wonder about the chemical makeup of tablets that people take for pain relief? Before a tablet can be successfully made, the limiting and excess reactants must be considered. The limiting reactant will affect the amount of the product that can be made. Another reason why the starting reactants must be determined carefully is to make reduce the amount of the reactant in excess so that reactants are not wasted. This experiment uses an Alka-Seltzer tablet. Alka-Seltzer dissolves in water and is an antacid and a pain reliever1. The Alka-Seltzer tablet has many uses such as relief of headaches, ingestion, heart burns, or even upset stomachs2. The active ingredients in an Alka-Seltzer tablet is aspirin, also known as acetyl-salicylic acid (C8H12O4), citric acid (C6H8O7), and sodium bicarbonate (NaHCO3)2. The aspirin in the Alka-Seltzer tablet helps with pain relief. Because of the acid-base chemistry (Brønsted-Lowry), citric acid and sodium bicarbonate produce O2, which makes the tablet fizz when it is dropped in liquid. The Brønsted-Lowry theory shows how the Brønsted-Lowry acid donates a hydrogen ion while the Brønsted-Lowry base accepts the hydrogen ions3. The remaining NaHCO3 that is in excess post reaction with the citric acid is what is used to neutralize stomach acid which helps relief heart burn2. The problem in

The purpose of this lab is to investigate the composition of a compound suspected to be Panacetin, a type of pain-killer. Panacetin is typically made up of sucrose, aspirin, and acetaminophen, but the third component in this experiment is unknown. The unknown component is suspected to be a chemical relative of acetaminophen, either acetanilide or phenacetin. Using techniques such as extraction, evaporation, and filtration, the three components will be isolated based on their solubilities and acid-base properties. Then, the percent composition of Panacetin can be deduced based on the masses of the three dried components. The

Samples of benzophenone, malonic acid, and biphenyl were each tested with water, methyl alcohol, and hexane. Benzophenone was insoluble in water as it is nonpolar while water is highly polar. Benzophenone was soluble in methyl alcohol, dissolving in 15 seconds, because methyl alcohol is intermediately polar as benzophenone is nonpolar. Methyl alcohol is polar but not as much as water. Thus, the nonpolar benzophenone was soluble in methyl alcohol. Benzophenone was partially soluble in hexane because hexane is nonpolar as is benzophenone. Thus, benzophenone was dissolved in hexane. Malonic acid was soluble in water because both malonic acid and water are polar. It took 25 seconds for malonic acid to dissolve in water. Malonic acid was soluble in methyl alcohol because malonic acid is polar and methyl alcohol is intermediately polar, allowing malonic acid to dissolve in the methanol in 15 seconds. Malonic acid was insoluble in hexane because hexane is nonpolar while malonic acid is polar. Biphenyl was insoluble in water as water is highly polar whilst biphenyl is nonpolar. Biphenyl was partially soluble in methanol which is intermediately polar whilst biphenyl is nonpolar, allowing it to dissolve a little. Biphenyl was soluble in hexane because both biphenyl and hexane are nonpolar molecules. Biphenyl dissolved in hexane in 10 seconds.

In order to test the predictions of the hypotonic, hypertonic, and isotonic hypothesis for the solution  made during the study,  four samples of sucrose were taken and placed into two different beakers each containing a different concentration. Beaker 1 is  250- mL and contained 150-mL of 10% sucrose with dialysis tubing A, while beaker 2 (a large bowl) contained 1% sucrose, with dialysis tubing  B, C, and D. Tubing A contained 10-mL with 1% sucrose. Tubing B

In this experiment, 0.31 g (2.87 mmol) of 2-methylphenol was suspended in a 10 mL Erlenmeyer flask along with 1 mL of water and a stir bar. The flask was clamped onto a hotplate/stirrer and turned on so that the stir bar would turn freely. Based on the amount of 2-methylphenol, 0.957 mL (0.00287 mmol) NaOH was calculated and collected in a syringe. The NaOH was then added to the 2-methylphenol solution and allowed to mix completely. In another 10 mL Erlenmeyer flask, 0.34 g (2.92 mmol) of sodium chloroacetate was calculated based on the amount of 2-methylphenol and placed into the flask along with 1 mL of water. The sodium chloroacetate solution was mixed until dissolved. The sodium chloroacetate solution was poured into the 2-methylphenol and NaOH solution after it was fully dissolved using a microscale funnel.

The experiment was divided into a series of separation phases, a purification phase, and an analysis. Initially, 3.00g of Panacetin was weighed and dichloromethane (DCM) was added to the drug. Sucrose was filtered from this mixture by gravity filtration because it is not soluble in DCM while aspirin and is unknown are. Sodium bicarbonate was then added in order to extract aspirin from the filtrate. The base converted aspirin into its salt, allowing it to move into the aqueous layer of the mixture. The aqueous layers were obtained and hydrochloric acid was added,

The procedure shown demonstrated how to determine the composition of unknown compounds, based off of information that’s known from given analgesics, by using thin-layer chromatography (TLC)2. With some silica gel, a coated plate, and developmental solvent, it was possible to distinguish unique measurements and characteristics of each unknown compound3. This was all possible due to chemistry and the bonds that exist within the different compounds and materials. Polarity and non polarity played a big part in how the results were achieved, as well as the chemical structure and shape of the compounds1. The chemical structures of each compound are what allows for them to be either polar or non polar. Within the experiment, depending on the polarity

Firstly, aspirin was weigh to 0.25g which was then dissolved in 100cm3 of distilled water by heating to >80°C using a hotplate. 2.0g of agar was added while stirring and was heated till dispersed, giving almost clear solution. The temperature was control so as not to overheat the agar. The agar was left to cool in an ice bath. Using a hollow cylinder, the agar was cut to approximately 4.0g (the exact weight of the agar was recorded). It was then transferred to a 250cm3 beaker filled with 50cm3 of distilled water and a conductivity probe was placed into the beaker to measure the conductance (Conductivity, Gt, S/cm) against time (measured every 1-2 minutes for the interval of 30 minutes). To ensure consistency, the solution was swirl for approximately 10 seconds before the minute was up. Next, the conductance of aqueous solution with only aspirin present was calculated by getting the amount of aspirin through the formula (Y=X/102g aspirin) and it was dissolved into 50cm3 of water. The conductance was measured in order to obtain the Control (Ga). From there, the fractions of Aspirin released at any given time (Qt) were measured thus providing the following of the release of the Aspirin by plotting the graph of Log Qt versus Log t.

The sample and drug substances were treated with a 3% solution of hydrogen peroxide and kept at room temperature (RT) under reflux conditions for approximately 30