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. After calculations the Kc average was equivalent to 0.1031 Introduction: Chemical equilibrium in a reaction occurs when the rate of the forward reaction is
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The equilibrium concentrations were determined through a series of experiments where a known base‚ Sodium Hydroxide (NaOH)‚ was titrated into different reaction mixtures until an endpoint was reached. The equilibrium concentrations were then placed into the following equation to determine the constant: Kc = [R2OH] [ R1COOH]
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Unit Plan On Acids & Bases May 25‚ 2006 Table of Contents I. General Objectives Page 3 II. Learning Outcomes Page 4 III. Assessment‚ Grading & Resources Page 5 IV. Tending to different Learning styles Page 7 V. Schedule Page 8 VI. Appendix 1 Page 20 Acids and bases Unit plan Grade 12 General Objectives: ▪ Introduce pH‚ acid and base definition ▪ Discuss acid
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HCl and NaOH Lab Report Introduction: It is important to standardize solutions in order to have the accurate amount of concentration known. A standard solution can be prepared in either of two ways: A primary standard is carefully weighed‚ dissolved‚ and diluted accurately to a known volume. Its concentration can be calculated from this data. A solution is made to an approximate concentration and then standardized by titrating an accurately weighed quantity of a primary standard. Solid NaOH has the
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precipitation reactions. The experiment calls for a neutralization reaction‚ the analytes are the acidic soft drink samples and the titrant is the base NaOH. The equation for the titration reaction is as follows: H3C6H5O7 + 3NaOH -----> 3H2O + Na3C6H5O7 But before proceeding to the titration of soft drink samples‚ the exact concentration of NaOH must be known through the process of standardization which involves performing a titration with a known amount of a stable acid‚ which in this case is the
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Detection of Ions in Solutions Using Acid/Base Chemistry: A Quality Control Test Objective: This lab focuses on the detection of ions using titration as an analysis tool. You will standardize NaOH and HCl solutions so that you know the exact concentration and then prepare samples of common household items in order to determine the amount of calcium in Tang®‚ Mg(OH)2 in Milk of Magnesia‚ etc. You will learn to prepare samples of a specified concentration‚ learn about acids and bases through
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[Zn 2+][OH –]2 pH 9.35 = pOH 4.65; [OH –] = 10–4.65 = 2.24 x10–5 M Zn2+ = Ksp/[OH -]2 = 7.7x10-17/[2.24 x10-5]2 = 1.5 x10-7 M (ii) At 25˚C‚ 50.0 mL of 0.100-M Zn(NO3)2 is mixed with 50.0 mL of 0.300-M NaOH. Calculate the molar concentration of Zn2+ (aq) in the resulting solution once equilibrium has been established. Assume that volumes are additive. [Zn2+]init = (0.100M )(0.050 L) = 0.0500 M [OH–]init = (0.300M)(0.050 L) = 0.150 M X =
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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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Chemistry 200 Exam 1 Review Problems 1. Calculate the number of atoms in 10.0 grams of Fe. 2. Give the mass number‚ #protons‚ #neutrons and #electrons for the isotope strontium-88. 3. Calculate the number of moles of carbon in 50.0 g of benzene C6H6 4. A substance is found to be 38.7 % C‚ 9.7 % H and 51.6 % O by mass. Its molar mass is 62.1 g/mole. What is its molecular formula? 5. Name the following: a) Ca(OH)2 b) KCN c) HClO4(aq) d) FeSO4 e) Na2O f) SF6 g)
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for a titration (including mounted pH meter). Turn the burette’s stopcock with care! Discuss the process of standardization‚ which will be used to determine the exact concentration of a “0.01 M” NaOH solution. Introduce potassium hydrogen phthalate (KHP)‚ a weak acid used to react with added NaOH. Draw and discuss a titration curve for this standardization (titration of weak acid with strong base). You won’t actually measure this titration curve‚ but it is very instructive! Draw the first
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