HShin_Hoon_Shin_-_Lab_2_Report - Author: Hoon Shin TA:...

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Author: Hoon Shin TA: Eileen Chen Section: A05 Class: Chem100A, UCSD(University of California San Diego) Date: 4/21/08 Homogeneous Chemical Equilibrium Abstract To determine the concentration of NaOH, it was titrated with a primary standard, KHP. After three titrations in three separate flasks, the concentration was calculated as 1.404 M. Equilibrium constant for reaction adding acetic acid and ethanol to produce ethyl acetate and water were determine by titrating with the 1.404M NaOH to five separate flasks b, c, d, e, and f which contained different initial concentrations for each of the solution including HCl as catalyst. The equilibrium constant for b, c, d, e, and f were 6.779, 6.633, 6.078, 6.547, and 4.551 (no unit) respectively. The average with a standard deviation of equilibrium constant was 6.118 ±  0.914. Introduction Objective of this experiment is for one to be able to calculate the equilibrium constant by using the data which will be obtained by performing titration with the known concentration of NaOH with the reaction: C 2 H 5 OH + CH 3 CO 2 H CH 3 CO 2 C 2 H 5 + H 2 O In every chemical reaction, single headed arrow is used to indicate the direction of a chemical reaction. Also double headed arrow is used to indicate the reaction that did not went through hundred percent completions which means that the solution contain both the products and reactants. Sometimes, a solution can have more of products than the reactants either because the solution had high concentration of reactant and low on products or the reactants were already close to “hundred percent.”
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Both products and reactants will interacts each other, while the concentration of products increases and the concentration of reactants increase, until they reached to the point where they no longer need to interact with one another. This point is called an equilibrium state. This equilibrium can be represent in numerical way by using general equation. For example, if there is reaction: aA + bB cC + dD, equilibrium constant can be found by using Law of Mass Action which is: b a[B]^ [A]^ d c[D]^ [C]^ Kc = The large value of Kc, equilibrium constant, indicates that there are high concentration of product and low concentration of reactants, and other way around if the value of Kc is relatively small. In this experiment, one is expected to determine the equilibrium constant of ethyl alcohol, acetic acid and ethyl acetate where: C 2 H 5 OH + CH 3 CO 2 H CH 3 CO 2 C 2 H 5 + H 2 O. HCl will be used as a catalyst. Using a buret technique, one will perform titration with NaOH solution, and the data that will be collected can be used as source to find the equilibrium constant. Experimental
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This note was uploaded on 10/16/2008 for the course CHEM 100A taught by Professor Dai during the Spring '06 term at UCSD.

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HShin_Hoon_Shin_-_Lab_2_Report - Author: Hoon Shin TA:...

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