The equilibrium constant for the esterification of ethanol and aceticacid in an aqueous solution CH3COOH(aq) + C2H5OH(aq) -----> CH3COOC2H5(aq) + H2O(l) amounts to 0.566 at 298 K. The reaction mixture initially contains 0.040 mol dm^â3 of acetic acid and 0.025 mol dm^â3 of ethanol. Find themolar concentration of ethyl acetate at the equilibrium. Assume that the pH is low enough that CH3COOH is not dissociated at all and thatthe activity of water equals 1 just like for pure liquid water (after all,the solution is quite dilute). Hint:This problem requires you to keep an extra large number ofsignificant digits in all intermediate calculations: otherwise, your finalanswer will be very inaccurate. Do not forget to check your answer in the end.
The equilibrium constant for the esterification of ethanol and aceticacid in an aqueous solution CH3COOH(aq) + C2H5OH(aq) -----> CH3COOC2H5(aq) + H2O(l) amounts to 0.566 at 298 K. The reaction mixture initially contains 0.040 mol dm^â3 of acetic acid and 0.025 mol dm^â3 of ethanol. Find themolar concentration of ethyl acetate at the equilibrium. Assume that the pH is low enough that CH3COOH is not dissociated at all and thatthe activity of water equals 1 just like for pure liquid water (after all,the solution is quite dilute). Hint:This problem requires you to keep an extra large number ofsignificant digits in all intermediate calculations: otherwise, your finalanswer will be very inaccurate. Do not forget to check your answer in the end.
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