Write an expression for the equilibrium constant, $K_c$, for this reaction, and state the units clearly.
Calculate the amount, in moles, of $\text{NaOH}$ used in the titration.
What amount, in moles, of this $\text{NaOH}$ reacted with the hydrogen chloride?
Write a balanced equation showing the reaction between ethanoic acid and $\text{NaOH}$.
Hence calculate the amount, in moles, of $\text{NaOH}$ that reacted with the ethanoic acid.
Use your results from (b) to calculate the amount, in moles, of ethanoic acid present at equilibrium. Hence complete the table below.
Use your results to calculate a value for $K_c$ for this reaction.
Esters are hydrolysed by sodium hydroxide. During the titration, sodium hydroxide reacts with ethanoic acid and the hydrogen chloride, but not with the ester. Suggest a reason for this.
What would be the effect, if any, on the amount of ester present if all of the water were removed from the flask and the flask kept for a further week at $25\,^{\circ}\text{C}$? Explain your answer.