Test

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.

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.

4- chlorobenzoic acid which was the aqueous layer has a theoretical melting point of 240-243°C, the organic layer, 4-chlorobenzyl alcohol has a theoretical melting point of 68-71°C. During our experiment we were unable to collect any data for the organic

6. The solubility of the solids were tested using a micro tray, by placing them in water and oil to observe their polarity,

Maleic acid has a melting point of C and Fumaric acid has a melting point of C. The substance that has a higher melting

Procedure: Filled each test tube with substances provided and subjected them to various conditions. These conditions included, heat, cold water, hot water, acid and basic additions and tested on litmus paper. The reactions were observed and documented at each step.

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

Starting with 8.03 grams of maleic anhydride crystals, the students successfully converted them into two isomers of butenedioic acid. From the experiment, the students learned that maleic acid converts to fumaric acid in the presence of a proton. Little occurred during the reaction between the maleic anhydride and water. The solution remained clear during the heating. Moreover, all the crystals produced during the experiment are white and brittle. Furthermore, the students obtained 6.09 grams of maleic acid, the crystals produced in the first part of the lab and 0.90 grams of fumaric acid, the crystals produced in the second part of the lab. During the melting point test, the crystals of maleic acid begin melting at 121oC and fully melted

Identifying this organic acid was an extensive task that involved several different experiments. Firstly, the melting point had to be determined. Since melting point can be determined to an almost exact degree, finding a close melting point of the specific unknown can accurately point to the identification of the acid. In this case the best melting point

In part II of the lab six small glass tubes were obtained in a test tube rack. Ten drops of distilled water were then added to test tube 1, five drops to tubes 2-4, and no drops in tubes 5 and 6. Five drops of 0.1M HCl were added to test tube 5 and five drops of 0.1M NaOH to test tube 6. Five drops of enzyme were then added to all tubes except tube 1. Tube 3 was then placed in the ice bucket and tube 4 was placed in the hot bucket at 80-900C for five minutes, the remaining tubes were left in the test tube rack. After the five minutes five drops of 1% starch was added to every tube and left to sit for ten minutes. After ten minutes five drops of DNSA were then added to all the tubes. All the tubes were then taken and placed in the

The appearance is stated to be monoclinic crystals. When the substances melted completed, it went from solids to liquids.In Part 1, the melting point range of Urea was 132.5-133.5°C. It had a precise melting point in comparison to the given melting points. The melting point range of Trans-Cinnamic Acid had a melting range of 132.5-133.6°C. The Trans-Cinnamic Acid also had a precise melting point in comparison to the given information. The mixture of the two had an ending melting point of 129°C. The starting point of the mixture was not taken because the start of the melting point was missed. The starting temperature in Part 1 was 120°C, the ramp was 2, and the ending temperature was 190°C. In Part A of Part 2, the Unknown #2 had a melting range of 121-128.4°C. In Part A of Part 2, the starting temperature was 60°C, the ramp was 10, and the ending temperature was 170°C. In Part B of Part 2, the Unknown #2 had a melting range of 122-126.8°C. Succinimide had a melting range of

If a substance is pure, the melting points would be similar; however, for the 50-50 mixture, the melting point was depressed due to the amount of impurity between the two substances. In part two of the experiment, in order to determine the identity of the unknown substance, the compound was heated rapidly at a rate ramp of 10C in order to find the approximate melting point. The substances were similar in ranges as the unknown held a value of 3.8 while acetanilide had a value of 3.7. By using the melting point 115.2C-119.0C, it was determined that the unknown substance was most likely acetanilide. After testing the unknown mixture with acetanilide, it was confirmed that the unknown chemical was in fact

Samples A, B, and U were prepared by depositing 1-3mg of the solid- compound A, B, and the unknown- in a test-tube; dissolved with acetone. A TLC plate was made by drawing a horizontal line at the top and bottom of the plate with four ticks- A, B, U and A+U or B+U. The solutions were distributed to the ticks with a spotting capillary tube; however, based on the results from the melting point analysis, the determined unknown- compound A or B- and the unknown would be place on the fourth tick.

The beaker was slowly heated on a hot plate with low stirring until most of the stilbene was dissolved. 0.4 g of pyridinium tribromide was measured and added to the beaker after 5 minutes of heating. Small amounts of ethanol were used to clean the sides of the beaker. The beaker was heated for an additional 10 minutes on low temperature. An ice bath was prepared. The beaker was removed from the hot plate and left to cool to room temperature. Once at room temperature, the beaker was placed in the ice bath for 15 minutes. The solid product was collected through vacuum filtration and the product was weighed and a melting point was taken. Waste was disposed of in the correct waste bins and lab bench was cleaned

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