Ethyl Acetate Lab Report

In this experiment, an alkyne—diphenylacetylene—was prepared by a double dehydrobromination. Potassium hydroxide (KOH) and high heat were used to accomplish this. The precipitate of this reaction was collected by vacuum filtration. It was then washed with water and recrystallized using ethanol. The product was then isolated again before the weight was taken for further analysis of percent yield. The melting point was also taken to identify that it was the desired product.

1-butanol and ethanoic acid, and the product, 1-butyl-ethanoate exist in the same mixture due to the reflux setup, the reaction can never go to completion. Moreover, when isolating and purifying the ester, 1-butyl-ethanoate, some of the product will be lost. This will also occur when separating the ester in distillation, hence, it is not possible to obtain 100% of the product. So, if a theoretical yield were to be calculated, it would not be very accurate. The resulting value of the theoretical yield would most probably represent the maximum yield of the experiment as opposed to an actual yield of how much product will be obtained in the end. Therefore, it is not possible to get the theoretical yield in the experiment due to the lost of product (the ester) throughout the process in numerous occasions.

This experiment combined all the knowledge of the previous labs performed throughout the semester. An unknown mixture containing an organic acid or base and an organic neutral compound in nearly equal amounts needs to be separated to its separate components. An understanding of solubility, extraction, crystallization and vacuum filtration is necessary in order to

The mole is a convenient unit for analyzing chemical reactions. Avogadro’s number is equal to the mole. The mass of a mole of any compound or element is the mass in grams that corresponds to the molecular formula, also known as the atomic mass. In this experiment, you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride, determine the number of moles of iron used up in the reaction of iron and copper (II) chloride, determine the ratio of moles of iron to moles of copper, and determine the number of atoms and formula units involved in

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.

Note: Your prelab/lab report is to be done in your carbon copy lab notebook (sold in FIU bookstore)

To prepare and purify an ester: 1-pentyl ethanoate, using pent-1-ol and ethanoic acid. An annotated reaction showing this reaction is shown below:

Discussion As part of the experiment, the percent composition of each component of the mixture was calculated. 51% of the components were retrieved from filtration while 49% of the solvents were retrieved from dissolving the components in a solvent. The original mixture was one globular solid-like structure.

3 mL of a 1:1 isopropyl acetate and toluene mixture along with a spin vane was added to a 5 mL conical vial using a calibrated Pasteur pipette. A Hickman still and heating block was assembled. The connector and lower portion of the Hickman still was wrapped with aluminum foil and the top of the still was loosely covered with foil. The thermometer was placed into the heating block and was moved into the Hickman still once the temperature of the heating block was near the listed temperature from the lab manual. The solution was stirred slowly while the hot plate was turned on.

In this experiment, the pKa, dissociation constant, of 2-naphthol was determined by measuring the UV-visible absorption spectra of solution of the acid at different pH values.

The objective of this experiment is to acquire isopentyl acetate from isopentyl alcohol and acetic acid through esterification. This ester, isopentyl acetate, can also be called banana oil because it smells a similar to this fruit. Isopenyl acetate is prepared by esterification of acetic acid with ispoentyl alcohol. The equilibrium of this reaction does not favor the formation of an ester so it must be shifted to the right. Since it was shifted to the right to favor the product it must have an excess amount of acetic acid.

Esters are compounds that has a pleasant smell and which are obtained from reaction between a carboxylic acid and alcohol (Kotz et al., 2009, 737). This type of reaction is known as esterification reaction (Jespersen & Jespersen, 2010, 376). Ethyl ethanoate is a good example of the products of esterification. This compound is produced from a reaction between ethanoic acid and ethanol in the presence of strong acid catalyst. The equation of reaction that takes place during this reaction is as shown below.

Objective: The objective of this experiment is to use acid-base extraction techniques to separate a mixture of organic compounds based on acidity and/or basicity. After the three compounds are separated we will recover them into their salt forms and then purify them by recrystallization and identify them by their melting points.

Part 1: Esters aromas are very distinct and often pleasant, they are often used in food aroma and fragrances.1 Esters chemical properties are distinguished by their low molecular weight and low boiling points, caused by their dipole-dipole and dispersion interaction.2 Esters are the result of a condensation reaction, in which a carboxylic acid, an alcohol, and an acid catalyst react to create a water molecule and an ester.

In section IV, Experimental results are discussed and analysis is briefed. Finally, Conclusions are drawn.