) Calculate the amount of unreacted aqueous ethanoic acid (CH3COOH(aq)) in the sample taken for titration with aqueous potassium hydroxide(KOH(aq)). Clearly show the steps in your calculation. (1 mark)
(v) Hence calculate the amount of aqueous ethanoic acid CH3COOH(aq)) in the sealed flask at equilibrium. Clearly show the steps in your calculation and comment on any assumptions that you make. (2 marks)
(vi) Using the amount of aqueous ethanoic acid (CH3COOH(aq)) present at equilibrium, calculate the amount of ethanol that reacted in the process of attaining equilibrium. Clearly show the steps in your calculation / reasoning. (3 marks)
(vii) Calculate the amount of ethanol (C2H5OH(aq)), ethylethanoate (CH3COOC2H5(aq)) and water (H2O(l)) present in the reaction mixture at equilibrium. Clearly show the steps in your calculation /reasoning. (4 marks)
(viii) Calculate the value of Kc(323K) clearly showing the steps in your calculation.
A lost of writing but no numbers. You can't calculate anything without numbers.
To calculate the different quantities mentioned in the question, we will need information about the reaction between ethanoic acid (CH3COOH) and potassium hydroxide (KOH). Let's go step by step through each part of the question:
(v) Calculate the amount of unreacted aqueous ethanoic acid (CH3COOH(aq)) in the sample taken for titration with aqueous potassium hydroxide (KOH(aq)).
To calculate the amount of unreacted ethanoic acid, we first need to know the initial moles of ethanoic acid present in the sample taken for titration. This information is not provided in the question, so we cannot proceed with this calculation.
(vi) Calculate the amount of aqueous ethanoic acid (CH3COOH(aq)) in the sealed flask at equilibrium.
To calculate the amount of ethanoic acid at equilibrium, we need to know the balanced chemical equation for the reaction between CH3COOH and KOH. From the balanced equation, we can determine the stoichiometry and use the amount of KOH used in the titration.
For example, if the equation is:
CH3COOH(aq) + KOH(aq) → CH3COOK(aq) + H2O(l)
Assuming we have performed the titration and know the volume and concentration of KOH used, we can calculate the moles of KOH used. By stoichiometry, we can then find the moles of CH3COOH used.
To find the amount of CH3COOH at equilibrium, we need to know if CH3COOH is a limiting reactant or not. If it is not a limiting reactant, then the amount of CH3COOH at equilibrium will be equal to the amount used. Otherwise, we need additional information to determine the extent of the reaction.
(vii) Calculate the amount of ethanol (C2H5OH(aq)), ethylethanoate (CH3COOC2H5(aq)), and water (H2O(l)) present in the reaction mixture at equilibrium.
To calculate the amounts of ethanol, ethylethanoate, and water at equilibrium, we again need the balanced chemical equation for the reaction between CH3COOH and KOH. From the stoichiometry of the equation, we can determine the molar ratios and use the information on the amount of CH3COOH at equilibrium.
For example, if the equation is:
CH3COOH(aq) + KOH(aq) → CH3COOK(aq) + H2O(l)
If we know the moles of CH3COOH at equilibrium, we can determine the moles of CH3COOK produced and the corresponding moles of H2O. Using the molar masses of ethanol and ethylethanoate, we can calculate their amounts based on the stoichiometry of the reaction.
(viii) Calculate the value of Kc (323K).
To calculate the value of Kc, we need the balanced chemical equation and the concentrations of the reactants and products at equilibrium. From the stoichiometry, we can write the equilibrium expression for the reaction and substitute the concentrations into the expression.
For example, if the equation is:
aCH3COOH(aq) + bKOH(aq) → cCH3COOK(aq) + dH2O(l)
The equilibrium expression would be:
Kc = ([CH3COOK]^c [H2O]^d) / ([CH3COOH]^a [KOH]^b)
By substituting the equilibrium concentrations of the reactants and products into the equation, we can calculate the value of Kc.
Please note that without the specific values and more information, it is not possible to provide numerical answers to the calculations.