Melting Point Lab Report

Instead of approximately 28 mL of water being added, 140 mL of water was added. To correctly identify the compound, it was concentrated with nitrogen while the container was placed in a boiling water bath. After being concentrated enough, the experiment was able to continue. To confirm that the unknown was acetanilide, a comparison of the melting points between the acetanilide, phenacetin and the unknown was performed which led to confirming that the unknown was

The goal of this experiment was to find out active chemical components in Anacin and Tylenol, using Thin Layer Chromatography technique. This technique uses the difference in the intermolecular forcer and polarity to separate mixtures. Comparing Rf values were then used to determine the active chemical components in the two analgesics. The overall result was that Acetaminophen exists in Tylenol and Acetylsalicylic Acid exists in Anacin.

Every individual is different in a specific way. Like people, substances have unique qualities, such as properties, which aid chemists to differentiate and identify the particular components the substances consists of. These particular qualities are identified as either physical or chemical properties. Physical properties are properties which do not require a chemical change of its composition in order for the substance to be classified. A few examples of physical properties include color, density, odor, boiling point, melting

After each of the solids were completely dry, each was placed into a MelTemp device. The temperature at which each solid began to melt and completed melting was recorded.

Separation and Purification of the Components of an Analgesic Tablet. Cora Bruno, Lab Section E. Aspirin, Caffeine and Acetaminophen were separated from four analgesic tablets of Excedrin using extraction techniques. 5% wt/vol NaHCO3, 4M HCL, ethyl acetate and deionized water were used to separate the three active components. MgSO4 was used to dry each extraction. Aspirin was isolated using a hot water bath and weighed to determine the percent theoretical recovery and the actual percent recovery of aspirin. After separation, Aspirin (ASA), Caffeine (CAF), and Acetaminophen (ACE) were purified and identified using Thin Layer Chromatography (TLC). Standards and purified ASA, CAF, and ACE were spotted on the silica gel (stationary phase) of the

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 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

Acetic Anhydride and p-Aminophenol were heated in a vial attached to an air condenser to synthesize crude acetaminophen, resulting in 0.097 grams (47.48% yield). The crude acetaminophen was then recrystallized in a solvent of water and methanol over heat resulting in 0.082 grams (39.61% yield) of pure acetaminophen. Melting points of both crude and pure acetaminophen were taken, and found to be 165.9 - 170.9°C and 168.2 - 171.5°C, respectively. The literature melting point of acetaminophen is 169.5 – 171.0°C, indicating that our final product was pure.

In determining the melting point range of the aspirin, a capillary tube (sealed at one end) was one-third-filled with the dried aspirin. The capillary tube and a thermometer were immersed in an oil bath. The temperature at which the solid started to melt and the temperature when the entire sample was completely liquefied were recorded as the melting point temperature range.

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

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

Discussion: As seen in the melting point determination, the average melting point range of the product was 172.2-185.3ºC. The melting points of the possible products are listed as 101ºC for o-methoxybenzoic acid, 110ºC for m- methoxybenzoic acid, and 185ºC for p- methoxybenzoic acid. As the melting point of the sample

Melting range would be closely related to a mixed sample whose constituents are most identical. In other words, melting point will have a wide range and would be below 200°C and above 95°C.