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Determine the equilibrium constant - Kc; of ethanoic acid reacting with ethanol producing an equilibrium to form ethyl ethanoate and water.
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The Determination of an Equilibrium Constant Determine the equilibrium constant - Kc; of ethanoic acid reacting with ethanol producing an equilibrium to form ethyl ethanoate and water. CH3COOH(aq) + C2H5OH(aq) <=> CH3COOC2H5(aq) + H2O(l) Following the method as detailed, I conducted experiment 4 and these results were obtained: Titration Trial Volume of Sodium Hydroxide Neutralised (cm3) 1 7.65 2 7.75 3 7.80 4 7.70 5 7.75 µ 7.75 To calculate Kc, the concentrations of each reactant must be calculated from the point of equilibrium at which the titration was taken. Therefore, using 7.75cm3 as the average titre, Moles = 0.2M x (7.75cm3 / 1000 cm3) = 1.55 x 10-3. However, this represents the total amount of acid in the system which included ethanoic acid but also the acid catalyst: hydrochloric acid. Therefore this must be taken away from the number of moles of acid to calculate number of moles of ethanoic acid. Since 25 cm3 of 1.0M HCl was included in the initial 250 cm3 mixture, Moles = 1 x (25 / 250)...
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