Naphthalene Lab Report

Melting Point Data Table Compound Aspirin Caffeine Salicylamide Actual MP (ºC) 93 - 98 260 - 262 96 - 102 Expected MP (ºC) 135 236 140 Percent Error (%) ~30% ~12% ~30%

3. Common observations of a chemical reaction are described in the introduction section. For each observation, name a common or everyday occurrence that must involve a chemical reaction?

The primary goal of this laboratory is to correctly identify an unknown substance. To achieve this task, one may use various tests that reveal both chemical and physical properties of a substance. By comparing the results of a known substance and the unknown substance, one may eliminate alternative possibilities and more accurately predict the undisclosed compound. Furthermore, by performing these tests, data can be collected and verified regarding chemical and physical properties of the unknown. Understanding the chemical properties of a known substance aids one’s understanding of the unknown based on comparative analysis of the results of the tests.

No correction had to be made to the melting points because the standard melted in the range labeled on the bottle. The melted point observed is the correct melting point.

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 isolate benzoic acid, benzocaine and 9-fluorenone, each component needed to be separated from one another. All three compounds began together in one culture tube, dissolved in methylene chloride and formed into a homogenous mixture. In this culture tube, two milliliters of aqueous three molar hydrochloric acid was added, which immediately formed two layers, the top acidic aqueous layer was clear in color and contained benzocaine, and the bottom organic formed was yellow and contained benzoic acid and 9-fluorenone. Benzocaine’s amino group is protonated by the aqueous layer hydronium. This protonation forms the conjugate acid of benzocaine, benzocaine hydrochloride. Thus, the conjugate acid, benzocaine hydrochloride is a salt in which is soluble in water and furthermore can be isolated from the organic mixture. When testing out the pH levels in benzocaine, the pH test strip was dark blue in color, indicating a pH level of around 5 to 7. When isolating benzoic acid, two milliliters of aqueous three molar sodium hydroxide was added, which deprotonates the carboxylic group in benzoic acid, forming its conjugate base, sodium benzoate. As with benzocaine hydrochloride, sodium benzoate is a water soluble ionic salt in the aqueous layer that can then be separated from the bottom organic layer containing the 9-fluorenone. The pH test strip was a vibrant red for benzoic acid, indicating a pH of 2. Now the 9-fluorenone is left, deionized water is added to remove any excess

The problem that was trying to be solved in this study deals with analyzing unknown solutions. In this particular case, a chemical company has several unknown solutions and to correctly dispose of them they need to know their properties. To figure out the properties several qualitative tests were performed throughout the study (Cooper 2012).

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

The percent error for all experimental values are documented below. Experimental measurement Experimental Values Theoretical Values Percent Error Freezing Temperature of Naphthalene 80.4℃ Freezing Temperature of Biphenyl 69.2℃ Heat of Fusion of Naphthalene

Initially, we prepared a series of pincer copper-NHC complexes with small wingtips on the N atoms (R= Me, Et, iPr, tBu) carried out at room temperature using modified procedures recently developed by our group (Scheme 1) ref. These complexes have been characterized by elemental analysis, 1H and 13C NMR spectroscopies, and X-ray crystal structure that confirmed their structures. In the preliminary studies, we chose the coupling of iodobenzene with phenylacetylene as a model reaction to examine the efficacy of pincer Cu-NHC complexes (5-8) and to determine the optimum conditions. We used 20 mole % of the catalysts in the presence of K2CO3 (0.75 mmol) in N,N-dimethylformamide at 140 C .

Finally, the melting point of the aspirin was 110°C when it started melting and fully melted at

Isolation of a Natural Product by Steam Distillation: Cinnamaldehyde from Cinnamon Cinnamaldehyde Nojan Nasseri Niaki Thursdays 6:30pm – 9:20pm Organic Chemistry Laboratory (CHE.231.L.1) Instructor: Dr. Kafle Lab Report – Experiment II ABSTRACT: The main purpose of this lab is to extract the organic compound cinnamaldehyde from cinnamon. The process used in order to execute the extraction of the cinnamaldehyde is called steam distillation.

Description Nitric acid is commonly used in the chemistry laboratory. However, it has various uses in other industries as well such as in fertilizer production, and in the explosives industry. In this lesson, we will discuss nitric acid and its different uses. !!! Structure and Formula of Nitric Acid Nitric acid is a substance that we encounter more often than we think.

2-naphthol has a molecular weight of 144.17 g/mol, with a density of 1.22 g/cm3. The melting point of 2-naphthol is in the range of 121 to 123 °C. The stock solution of 2-naphthol has a concentration of 1.9844E-3 M.

Spots were circled and calculated. Based on the melting point analysis, the unknown sample was hydrocinnamic acid. The unknown sample melting point was around 46 to 51.2℃. Compound A- benzophenone- had a melting point of room temperature, while compound B- hydrocinnamic acid- had a melting point around 48 to 50.8℃.