In this laboratory experiment, 3.030 g of Isopentyl Acetate was synthesized and formed by the esterification of acetic acid with Isopentyl Alcohol. 1.0 mL of Sulfuric acid was used as a catalyst in the reaction. The excess Isopentyl Acetate was used to shift the reaction to the right for esterification to occur. During the extraction, the excess of acetic acid and Isopentyl alcohol was extracted with sodium bicarbonate, and further purification of the Isopentyl acetate was done after through drying with anhydrous sodium sulfate and through simple distillation. The percent yield of the Isopentyl Acetate was 46.6 percent with a theoretical yield of 6.502g. In this laboratory experiment the acetic acid was in excess and the Isopentyl Alcohol was the limiting reagent, which ultimately the reaction depended upon on the …show more content…
The yield could never be hundred percent with a reverse reaction. This reverse reaction also occurred because of one of the products, which was water. Esterification is the process of splitting hydrogen from the carboxylic acid (acetic acid) and hydrogen along with oxygen from the alcohol (Isopentyl Alcohol) to form water as a byproduct. During the reflux, all of the molecules in the original solution remained in the round flask including the water as the byproduct. As more water was formed, the amount of the products began to surpass the amount of reactants, which the reaction begun to run in the reverse direction. If the water has been dispensed into another container, this reaction would have continuously run toward to the products side. Following the isolation of the ester, a drop of Isopentyl Acetate was placed into an infrared spectrometer. When bonds within molecules absorb photons at different frequencies the IR spectrometer produces a graph to represent the bonds within the ester
The contents of the reaction flask were slowly poured into the 250 ml Erlenmeyer flask which already contained 13.75 g ice and 25 ml of 10% H2SO2. The round bottom-flask was rinsed with 2.0 mL of 10% H2SO4 and 2.0 mL of diethyl ether, and the rinses were added to the mixture in an Erlenmeyer flask. Then, the mixture was swirled until all the salt was hydrolyzed, and the product distributed well into the ether layer. A
Intro: Chemical reactions are the foundation for all organisms to exist. Paragraph 1: Endergonic Anabolic Reactions Building Consumes energy to build complicated molecules from simpler ones Uphill Photosynthesis Uses water and carbon dioxide to create sugar and oxygen Protein synthesis from amino acids Dehydration reaction Monomers are covalently bonded to each other through the loss of water Bonds are created which means energy is used Endergonic Exergonic Breaking Release energy by breaking down complex molecules to simpler molecules
4.B Why do you think that the adding of sodium acetoacetate resulted in a 50% decrease in renal ammonia production? Sodium acetoacetate addition would result in a decrease in renal ammonia production because of the adjustment to the pH levels that it has. This happens due to direct oxidation. Some of the dogs in this experiment became tolerant to the sodium acetoacetate so their doses were changed. The conclusion was that since quantities that were essentially equal in tolerance were given that direct oxidation was the final outcome of why 50% was decreased.
In this diagram we can see that acetaminophen consists of a benzene ring core, with hydroxyl and amide functional groups in proxy. Benzene (C6H6) is a hydrocarbon composed of 6 carbon atoms (92.26% of the molecule) and 6 hydrogen atoms (7.74% of the molecule) with alternating double and single bonds (resonance bonds) and is aromatic because of this. Benzene is a natural part of petroleum, usually <1.0% by weight, but is found in many things used today. Benzenes most common use is to produce ethylbenzene, with over half of the benzene used in the production of ethylbenzene. Benzene is a clear, colourless and highly volatile liquid which is soluble in water at an average room temperature (23.5o).
The ester functional group can be synthesized a number of different ways. These esters have very pleasant aromas and contribute greatly to the flavour and smells of many fruits. Due to this, the food industry often uses single esters to obtain synthetic flavouring agents and odours. The synthesis in this experiment
There are three main types of ester hydrolysis reactions: base-facilitated hydrolysis (saponification), acid-catalyzed hydrolysis (with the reverse reaction the Fischer Esterification), and enzymatic hydrolysis, triggered by lipases. Base-facilitated hydrolysis generally uses aqueous NaOH as a reagent, providing the base that attacks the carbonyl and begins the hydrolysis. Saponification hydrolyzes esters into carboxylic acids or fatty acids and alcohols. This has been used for thousands of years to produce soap from fatty acids as the salts produced from saponification can dissolve fats, surrounding them with micelles and allowing them to be easily removed with water1. It can also be used to produce glycerol from triglycerides.
Lab Report 5: Acetylsalicylic Acid (Aspirin) Synthesis Name: Divya Mehta Student #: 139006548 Date Conducted: November 19th 2014 Date Submitted: November 26th 2014 Partner’s Name: Kirsten Matthews Lab Section: Wednesday 2:30 L9 IAs Name: Brittany Doerr Procedure: For the procedure, see lab manual (CH110 Lab Manual, Fall 2014) pages 96-98. Wilfrid Laurier University Chemistry Department. Fall 2014. Acetylsalicylic Acid (Aspirin) Synthesis.
Solvent n-hexane, ethyl acetate and acetone will use to elute the column in isolation of chemical constituents of figeroots chloroform partition. The solvent system of different ratios of hexane, hexane/ethyl acetate, hexane/acetone, and acetone will use. Silica gel 60 (mesh 230-400 ASTM) will use to pack CC. In order to achieve good separation, mass ratio of silica gel to compound 20:1and 50:1 will use. 3.10.2Column Packing Before starting to pack a column, a small piece of cotton is gently will insert into the centre hole of column with the aid of a long stick.
The experiment began by setting up the LabQuest and preparing a 2M solution of HCl and a 2M solution of NaOH. This was called “Part A”. Two general rules were noted throughout the experiment: add acid to water and pour stock solution into beaker before graduated cylinder. This prevented flash-boiling of the solution, chemical burns, and spills. To make the 2M HCl solution, 200mL deionized water was added to a 600mL beaker labelled “2M HCl” by using a graduated cylinder.
The reason for this is due to the alcohol functional group present in the salicylic acid starting material, as it has a higher Rf value when TLC is run on the compound in which it is contained at the start of the reaction. TLC of the Aspirin product contained an ester functional group, which was expected to have a lower Rf due to residual hydrogen bonding which occurred between the hydroxyl group of the carboxylic acid and adjacent carbonyl of the ester. Experimental results followed this expected outcome, indicating the successful synthesis of the experimental aspirin product, which maintained a lower Rf value than the reaction starting material (Rf Data Figure 1). Experimental IR results indicated the presence if characteristic wavelength peak values that are found in a successfully synthesized Acetylsalicylic Acid (2-acetoxybenzoic acid) or Aspirin product. The IR spectra revealed the presence of the ester functional group via a peak at 1760cm-1 indicating C=O carbonyl bonding of an ester.
3.1 ABSTRACT The intermolecular interactions in the N-methylformamide with acetophenone, cyclic ketones (cyclopentanone and cyclohexanone) binary liquid systems are studied in combined experimental and computational methodology. The speed of sound (u), density (ρ) and viscosity ( ) values are measured for binary mixtures of N-methylformamide with ketones over the entire range of mole fraction at temperatures T= (303.15 to 318.15) K, at atmospheric pressure. From the experimental results, the values of excess molar volume ( ), excess isentropic compressibility (κsE), deviation in viscosity (η) and excess Gibbs free energy of activation of viscous flow ( ) are evaluated. The experimental results indicate the intermolecular association between the binary liquid
In this experiment set-up, acetic anhydride is added to salicylic acid in the presence of a catalyst, concentrated sulphuric acid. Acetylsalicylic acid and acetic acid are then produced, after the mixture is heated. Esterification is the chemical process of ester formation. Esters are produced when alcohols and carboxylic acids are heated in the presence of an acid catalyst, and in this case, acetylsalicylic acid is produced when salicylic
The two reactants present in the esterification process are the functional groups; carboxylic acid and alcohol. This reaction can be catalysed by the presence of H+ ions, often sulphuric acid is used. This type of esterification, where carboxylic acid and alcohol with an acid catalyst are used is known as the Fischer esterification. This is the type of esterification process which will be undertaken within this experiment, where 4mL of concentrated sulphuric acid will be used to speed up the reaction. It is also important to note that the esterification reaction can also include reactions of; an acyl halide
2.EXPERIMENTAL 2.1. Materials Hydroxyethyl cellulose (HEC) as membrane material was purchased from Sigma Aldrich. Levulinic acid (LA), ethanol, phosphoric acid, sodium hydroxide was obtained from Merck Chemicals. The catalyst tungstosilicic acid hydrate and solvent isopropanol were supplied by Sigma Aldrich. 2.2.
Experimental Methods: 1. SYNTHESIS OF 4-BENZOYL BUTYRIC ACID METHYL ESTER Materials required * 5 oxopentanoic acid : 2 gm (Aldrich) * Methanol : 50 ml * Acetic Acid (Rankem) Procedure: * 2 grams of 5 oxopentanoic acid was weighed and placed in a round bottom flask and then to it 50 ml of methanol was added. It was placed on a hot plate and the temperature was increased to 50 degrees under ambient air conditions.