Comparative Investigation of Organic Compounds

I. LIQUID - Identification of an Unknown Liquid: Using the physical properties of Solubility, Density, and Boiling Point.

1. Which reactants used in this experiment are flammable? Discuss the safety precautions that are necessary when working with flammable materials in the lab?

Perform the following with three 0.05g samples of unknown and the following solvents: methanol, water and toluene

As indicated in Table 1, each of the given substances for this lab were soluble in ethyl acetate. However, the solubility results varied based on the structure of each tested compound. 4-bromoacetanilide and fluorene are both insoluble within solvents of HCl and NaOH. Fluorene will stay soluble within the organic layer since its is a purely made of carbon and hydrogen. 4-bromoacetanilide will act similarly given its nonpolarity from balanced branches and lack of acid/basic characteristics. 4-nitroaniline and 2,5-dichloroaniline travel solubly into the HCl/H2O solvent when added to the separatory funnel, yet form a precipitate after a highly concentrated NaOH is added. Both 4-nitroaniline and 2,5-dichloroaniline are slightly basic organic compounds, and when an acid (HCl) is added a proton will transferred to make them ionic. In their ionic state, both compounds become water-soluble. When NaOH is added to 4-nitroaniline and 2,5-dichloroaniline, it removes the proton causing the compounds to become insoluble in water once again. The same concept can be applied in an opposite fashion to the acid organic compounds of 3-chlorobenzoic acid and resorcinol; both become water-soluble when they lose a proton after mixed with NaOH. They go back to their water insolubility if you add an acid to donate a proton back to 3-chlorobenzoic acid and resorcinol. Therefore, after completing this lab,

Abstract: One mixture of two unknown liquid compounds and one mixture of two unknown solid compounds were separated, isolated, purified, and characterized by boiling point. Two liquid unknowns were separated, isolated, and purified via simple distillation. Then, the process of an acid-base extraction and washing were used to separate two unknown compounds into two crude compounds: an organic acid and a neutral organic compound. Each crude compound was purified by recrystallization, resulting in a carboxylic acid (RCO2H) and a pure organic compound (RZ). The resulting mass of the pure carboxylic acid was 1.688g with a percent recovery of 31.80%, the boiling range was 244-245 °C, and its density was 2.0879g/mL. The resulting mass of the pure organic solid was 2.4902g with a percent recovery of 46.91%, the boiling range was 52.0-53.4°C, and its density was 1.5956 g/mL.

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

Substance A and B were weighed; Substance A weighed 0.502 g and substance B weighed 0.503 g. Both substances were put into two different test tube with approximately 8 ml of DI water into the test tub. Substance A and B were stirred and B dissolved while A did not. This shows that B is soluble in water compared to A. Thus, shows that B is soluble in water than A. The reason why B is soluble in water is because it has a higher dipole moment than A. With a higher dipole moment, it shows that it is soluble in water since it is polar and the bonds were easily broken.

The atom of an element has electrons that are found around the nucleus in regions known as orbitals. When energy is absorbed by the electrons of an atom they begin to jump to higher energy levels. When this happens the electrons are in an excited state. However when the electrons begin to release the energy and drop in energy levels they emit electromagnetic radiation. If the radiation that is emitted falls between 400 to 700 nanometers then the electrons emit photons which we can see as visible light.

What Is The Unknown White Compound By Alexander Medina Lab Partners Maxwell Yurs, Eugene Floersch, Mesih Harri Abstract A white compound is found, but its identity is unknown.

and 2D, separately. Separately describe and explain in your conclusions whether the experimental observations and results obtained from that part enabled you to confirm the solubility behavior of various compounds based upon what you had

Results: No substantial qualitative data was collected, except that the original reaction mixture turned a purple color. Upon the addition of anise oil and heat, the reaction mixture turned a brown color. And with the addition of NaHSO3 the mixture turned a white color. The mass of the final product sample was measured to be 0.08g (see Calculation 1). The melting point range for this sample was 172.8-185.4ºC in Trial 1 and 171.6-185.2ºC in Trial 2 (see Table 1). The IR spectrum of anise oil can be found attached. Peaks appear to exist at 3022.86, 3002.41, 2957.58, 2933.88, 2912.63, 2834.94, and 2723.19 (cm-1). Another set of peaks appear to exist at 1608.06, 1510.55, 1464.73, 1441.16, 1306.3, 1283.06, 1247.18, 1174.78, 1036.26, 964.58, 839.29, and 787.03 (cm-1). No other significant quantitative results were collected.

Table 1 shows the different alcohols and acids used for the production of esters. The name of the esters is shown in the last column of this table as well as how the team member identified the odors of the ester produced. Table 2 shows the results for all 5 groups in the class. Most of the esters produced in this laboratory experiment were easily identified as specific fragances such as banana, wintergreen, and menthol. It is shown in the table, that banana was the most identified one followed by tube M and tube A. The rest of the esters, E and B, had more variability in the identification of esters while C was identified as mouthwash, which can be associated to the menthol flavor and odor. Ester in tube B was the hardest to be identified according to Table 2, since it had 4 different associated smells to it. Students identified one of the odors as expo marker which can be due to experimental error in which the ester did not fully react and the solution smelled more like alcohol (ethanol or isopropanol), which are ingredients that most dry-erase markers such as the brand Expo

(1) Next test performed was the solubility test, which narrowed down the identity of the main functional group of the solution using the chart on page 455 of reference 1. Each solubility test was performed by taking 2mL of the solvent and adding 1 drop of the unknown in a small test tube. Once both solvent and solute were in the test tube it could be gently tapped with a finger to ensure mixing. If the mixture had a line of heterogeneous quality than the solute was insoluble in the solvent; if mixture appeared homogenous than it was soluble. Performing this technique throughout the chart with each solvent the functional group was eventually deduced down.

Koczanski, Krystyna; Xidos, James D. CHEM 1300 Laboratory Manual; UMSU Copy Centre: Winnipeg, MB, Canada, 2013, pp

Ethanoyl anhydride and concentrated sulfuric acid are highly corrosive. Ethanol is flammable, salicylic acid is irritant to eyes and skin. Chemicals were handled in the fume cupboard. Plastic gloves were worn throughout the experiment.