Lecture Notes on Determination of Equilibrium Constant

Lecture Notes on Determination of Equilibrium Constant -...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
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 groups present in the reactants and products Explain the reason why two titrations are performed in this first part of the experiment: one for the initial concentration mixture and another for the H 2 SO 4 -water solution. Assuming work load is not a factor, explain why this experiment must be divided over two weeks. 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 H 2 SO 4 catalyst Determine the number of moles of H + are present due to CH 3 COOH present at equilibrium Determine the equilibrium concentration of CH 3 COOH Determine the value of the equilibrium constant, K c , 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
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
CHM2021: Chemical Principles 3 Laboratory CJT 01/10 Determination of an Equilibrium Constant Lecture Notes Page 2 of 6 Titrant: the solution of known concentration which is added to the unknown solution via a buret Analyte: the chemical or material under analysis in an experiment or investigation Indicator: a naturally derived material which changes color when the ionic concentration in a solution changes. End Point: appearance of indicator color change during volumetric analysis Equivalence Point : a stage in volumetric analysis where the number of moles of titrant equal the number of moles of analyte. Chemical Equilibrium:
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 6

Lecture Notes on Determination of Equilibrium Constant -...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online