hhhhh - Introduction: The objective is to determine the...

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Introduction: The objective is to determine the rate constant k for the reaction of ethyl acetate with hydroxide ion. The reaction: CH 3 COOC 2 H 5(aq) + OH-(aq) ===== CH 3 COO (aq) + C 2 H 5 OH (aq) is first order with respect to [EA] and first order with respect to [OH]. Thus it is a second order overall reaction. For run A: When [EA]o = [OH]o then [EA]=[OH] and the rate is : 1/[EA] = 1/[EA]o + kt For run B: When [EA]o [OH]o then the rate law is: ln{[EA][OH]o/[EA]o[OH]} = {[EA]o - [OH]o} kt [OH] can be measured at any time by removing an aliquot from the reaction mixture, adding it to excess HCl to stop the reaction by consuming the unreacted OH, and back titrating with standard NaOH solution. The rate constant k can be determined by studying the variation of the [OH] as a function of time. Procedure: Look in the experimental book pages:55-57 Data: Molarities of solutions: [EA]=[NaOH]=[HCl]=0.020 M The volume of NaOH added in the two runs in different time as follows: Time (min) Volume(ml) of NaOH added in run A Volume (ml) of NaOH added in run B 5 2.5 1.6 10 3.75 2.07 15 4.7 2.75 20 5.45 3.25 30 6.55 3.75 40 7.05 4.1 50 7.5 4.2 60 7.75 4.55
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hhhhh - Introduction: The objective is to determine the...

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