each part of each problem carefully. ● Write your answers legibly in the corresponding spaces of the attached sheets. ● For problems requiring calculations‚ you must show these calculations clearly and indicate all values‚ including physical constants used to obtain your quantitative result. Significant figure and unit usage must be correct. ● If you do not understand what the problem is asking‚ raise your hand and a proctor will come to your desk. ● Some relevant equations and the periodic
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adrenoreceptors 1”. Atenolol has the molecular formula of C14H22N2O3. Its molecular mass is 266.3 grams and its IUPAC name is (RS)-4-(2-hydroxy-3-isopropylaminopropoxy) phenylacetamide. Its melting point 152-155 degrees Celsius‚ has a dissociation constant (pKa) of 9.6 at 24 degrees Celsius. It is soluble in water‚ ethanol and methanol but it is insoluble in ether 2.Atenolol can be synthesized in two parts. The first synthesis is with the reaction of phenol and formaldehyde to form the 4-(hydroxymethyl)phenol
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In the reverse reaction‚ NH4+‚ the conjugate acid‚ loses a proton‚ forming our base NH3. Acid-Base Strength and Conjugate: The relative strength of acids is often described in terms of an acid-dissociation equilibrium constant‚ Ka. Generic Equation: HA(aq) + H20(l) ↔ H3O+(aq) + A-(aq) Therefore‚ Ka = [H3O+][A-]/HA When a strong acid dissolved in water‚ the acids reacts extensively with water to form H3O+ and A- ions. The product of the concentrations for both these ions
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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 intended variable: the solvents. If the reactant is more stabilized by interaction with solvent molecules than is the transition state‚ the activation barrier for the reaction will be increased‚ and the rate will decrease. Conversely‚ if
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Menbere Wendimu Che101 Laboratory Report Acid Base Laboratory Objective: Introduction: Experimental: 2.04 g of KHP‚ 100ml volumetric flask‚ distilled H2O‚ approximately 0.1 M of NaOH‚ Vinegar‚ Phenolphthalein‚ 250ml Erlenmeyer flask‚ weighing balance‚ Graduating Cylinder‚ burette and pH meter were used in our experiment. In our first part of our experiment to prepare a primary standard‚ 0.1 M solution of KHP‚ we carefully weighed out 2.04g of KHP in a weigh paper using the weighing balance
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Weak Acid Titration Abstract: Our method for determining the unknown weak acid was to determine the equilibrium constant K from the molecular weight of the weak acid from our titration data. In this lab the acid Potassium hydrogen phthalate and two unknown acids were titrated. We determined the molar mass of the Potassium hydrogen phthalate‚ for the unknown acids we calculated the molar mass and the Ka values. We used NaOH as the known base for titrating in all three of the titrations. Our
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Partitioning of organic acid food preservatives between oil and water Olaya Iturbe Navalpotro Student of Food National Institute -DTU Technical University of Denmark Index 1. Introduction …………………………………………………………..pg. 2-4 2. Theoretical background……………………………………………….pg. 5-18 2.1. Preservatives (Sorbic acid and Benzoic acid) 2.2. Solubility and partitioning of food preservatives in food system 2.3. Measurements of the preservatives partitioning in oil-water system 2.4. Influences of
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contains four sections‚ SECTION A to SECTION D. Instructions: Answer all questions in SECTION A - SECTION D. Make sure that the section heading is included and your answers are correctly numbered. The assignment must have a completed cover sheet. It must be placed in the drop-box on or before the deadline. st SECTION A ELECTRONIC STRUCTURE & IONIZATION ENERGY 1. 2. Write the electronic structure in s‚p‚d notation of the following: O‚ Na‚ Na+‚ Al‚ Cl- and Co
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2.5 10-5 M 4.9 10-5 M 7.0 10-3 M 3.7 10-2 M 5. What is the pH of the buffer that results when 12.5 g of NaH2PO4 and 22.0 g Na2HPO4 are mixed and diluted with water to 0.500 L? (The acid dissociation constants for phosphoric acid are Ka1 = 7.5 10-3‚ Ka2 = 6.2 10-8‚ and Ka3 = 3.6 10-13) (Points : 10) 2.30 7.04 7.38 12.27 12.62 6. Which of the following combinations would be the best to buffer an aqueous
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reactants. Very little data is available on how does the carbon chain length of carboxylic acid and alcohol affects the rate constant and equilibrium constant of esterification. Thus‚ the research topic of this investigation is: How does the carbon chain length of the alcohols and carboxylic acids affect the rate constants of the forward and backward reactions and equilibrium constant of the esterification reaction? The affect of the carbon chain length of carboxylic acid and alcohol was measured separately
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