The Equilibrium Constant of an Ester Hydrolysis Reaction Jesus Flores March 30th‚ 2015 Abstract: This experiment was conducted in order to discover the Kc‚ equilibrium constant‚ of a hydrolysis reaction of an unknown ester #2‚ unknown acid‚ and alcohol #2 products. The first week consisted of creating the reaction mixtures in bottles‚ next was preparing a NaOH solution while neutralizing with KHP. The final week consisted of titrating the bottles with the NaOH solution prepared previously
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The Equilibrium Constant of an Ester Hydrolysis Reaction Julia Stanley CHM 152 LL Dr. Asmita Kane Budruk Goal of the lab: The purpose of this laboratory is to determine the equilibrium constant‚ Kc‚ for the acid-catalyzed reaction between an unknown ester and water to produce an unknown alcohol and an unknown carboxylic acid. I was using Unknown Ester #3 with a density of 0.9342 and Molar Mass of 74.08 g/mol; alcohol with density 0.7914 and Molar Mass 32.04 g/mol. Chemical
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For Acidic hydrolysis‚ SAC was found to be well susceptible to acid hydrolysis with 0.05 M HCl at 40 ˚C for 30 min caused about 8% reduction in the peak area of SAC (Fig.4a). While this mild condition didn’t affect VAL. While‚ nearly 27% was the reduction in SAC’s peak area when subjected to alkaline hydrolysis. This considerable decline in the peak area of SAC when subjected to 0.01 M NaOH at 40°C for 30 min revealed degradation products peaks appeared at 3.339 and 9.482 minutes (Fig.4b) and they
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That is‚ the entering group does not for the most part have the same position on the ring as that purged by the halogen substituent. Case in point‚ the hydrolysis of 4-chloromethylbenzene at 340° gives an equimolar mix of 3-and 4-methylbenzenols: Significantly all the more striking is the elite development of 3-methoxybenzenamine in the amination of 2-chloromethoxybenzene. Notice that this outcome is an
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Determination of the Equilibrium Constant of an Unknown Ester Hydrolysis Reaction Abstract The experiments to follow determined that the equilibrium concentrations of the reaction: ester + water ↔ alcohol + acid‚ are equal to 0.0363 moles of ester‚ 0.2852 moles of water‚ and 0.0268 moles each of alcohol and acid. Using this information the equilibrium constant was determined to be 0.06938. 1. Introduction In this lab the equilibrium constant‚ Kc‚ for the acid catalyzed reaction
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Esterification and Hydrolysis: Methyl Benzoate by Fisher Esterification Nitration of Methyl Benzoate Jingling Li 2/16/2014 Purpose of the experiment: To understand the mechanisms for Fisher esterification reactions as an equilibrium process and hydrolysis is the reversal reaction of esterification. Nitrate methyl benzoate by an electrophilic aromatic substitution reaction. Summary of procedures: Add sulfuric acid to the mixture of benzoic and methanol‚ heat up the mixture to 65 oC
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Hydrolysis of tert-butyl Chloride in different solvents Practical conducted on 5 March‚ 2013 Reported by Pham Vu Hung on 10 March‚ 2013 Introduction: This practical is meant to measure the rate of reaction of the hydrolysis of tertiary-butyl chloride –a colorless‚ liquid organic compound at room temperature that is sparingly soluble in water - in water/acetone and water/isopropanol mixtures. Since there are many influencing factors for the rate of reaction‚ all are kept constant but the
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Purpose The purpose of this experiment is to determine the rate constants‚ k1‚ for the methyl acetate hydrolysis reaction at 25 °C and 35 °C‚ as well as the overall activation energy of the reaction. Methods Methyl acetate was placed in an HCl solution‚ in which it reacts with water to form acetic acid over time. At each time interval‚ an aliquot of the mixture was removed for titration against NaOH to determine the concentration of the acetic acid produced. From the amount of acetic acid produced
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Abstract: The main reason for this experiment is to prepare a simple soap made from vegetable oil. The physical properties will be tested in order to demonstrate the reactions that occur. The experiment can conclude that the vegetable oil had a primary fatty acid called linoleic acid‚ which was evident during the saponification reaction. The simple soap did appear to be a good emulsifier because the soap did dissolve in the mixture of mineral oil and water. In hard water the calcium and magnesium
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Carbohydrate Polymers 44 (2001) 319–324 www.elsevier.com/locate/carbpol Hydrolysis of diethyl diferulates by a tannase from Aspergillus oryzae ´ M.-T. Garcıa-Conesa a‚*‚ P. Østergaard b‚ S. Kauppinen b‚ G. Williamson a a Phytochemicals Team‚ Division of Diet‚ Health & Consumer Sciences‚ Institute of Food Research‚ Norwich Research Park‚ Colney‚ Norwich NR4 7UA‚ UK. b ´ Screening Biotechnology‚ Enzyme Research Novo Nordisk A/S‚ Novo Alle‚ bldg. 1BM1.05 DK-2880 Bagsvaerd‚ Denmark. Abstract
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