CHM2021: Chemical Principles 3 Laboratory CJT 01/10 Determination of an Equilibrium Constant Lecture Notes Page 1 of 6 Objectives:•Explain the action of a catalyst. •Describe the objective and process of titration •Define the term indicator•Describe what is meant for a system to be at equilibrium•Describe how you would prepare a buret for titration and explain the purpose of each step. •In accord with the Law of Mass Action, provide the equilibrium expression for this reaction •Describe the "I.C.E." problem-solving technique for determining equilibrium concentrations for system components. •Identify the organic functional groupspresent in the reactants and products •Explain the reason why twotitrations are performed in this first part of the experiment: one for the initial concentration mixture and another for the H2SO4-water solution. •Assuming work load is not a factor, explain why this experiment must be divided over twoweeks. •Predict the chemical composition of the reaction mixture next week, including what will have changed and what will have remained the same •Determine the number of moles of H+are present due to the H2SO4catalyst •Determine the number of moles of H+are present due to CH3COOH present at equilibrium •Determine the equilibrium concentration of CH3COOH •Determine the value of the equilibrium constant, Kc, for the synthesis of isopropyl acetate Important Definitions•Catalyst: a substance which increases the rate of a chemical reaction without being consumed by the reaction. Catalysts may exist in the same phase as the reacting materials (homogeneous catalysis) or a different phase (heterogeneous catalysis). •Titration(also known as Volumetric Analysis): a laboratory technique wherein the concentration of unknown material is determined by adding small volumes of a solution of known concentration. Pasteur pipet Erlenmeyer flask Flask containing reaction mixture Foil-wrapped stopper Buret Serological pipet Pipet pump Ring stand
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