Le Chatelier’s principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish an equilibrium. If a chemical reaction is at equilibrium and experiences a change in pressure, temperature, or concentration of products or reactants, the equilibrium shifts in the opposite direction to offset the change. This page covers changes to the position of equilibrium due to such changes and discusses briefly why catalysts have no effect on the equilibrium position.
Question 1
a) Write down the overall equation showing the formation of [Fe(acac)3] from [Fe(H2O)6] 3+ and acetylacetone [Fe(H2O)6] 3+(aq) + 3acacH(aq) [Fe(acac)3](aq) + 6H2O(l) +3H+ (aq).
b) What reagent (chemical agent) do you weigh out that ends up being the source of the [Fe(H2O)6] 3+?
Question 2
a) Circle the correct word in bold text to complete the following statements: A pH of less than 7 means a solution is acidic/basic. A pH of greater than 7 means a solution is acidic/basic.
b) The equation showing acetylacetone, acacH, forming the acac¯ ion is below:
acacH => acac¯ + H+
What is it about this equation that results in a solution of acacH being slightly acidic?
c) Given that sodium acetate is a base (remember that sodium acetate can be considered as sodium ions and acetate ions), complete the following equation showing the reaction of acetate ions with H+ :
CH3COO– + H+ => _________
Question 3
a) What is the connection between the two equations below?
acacH => acac¯ + H+
[Fe(H2O)6] 3+ + acac¯ => [Fe(H2O)4(acac)]2+ + 2H2O
b) Using your answer to Question 3(a), explain why the pH of a mixture of [Fe(H2O)6] 3+ and acacH is lower than a solution of either of the components by themselves.
c) Explain why the pH increases on addition of sodium acetate.
d) Therefore, explain why more [Fe(acac)3] is produced after the addition of sodium acetate. (Hint: use the Equation [Fe(H2O)6] 3+(aq) + 3acacH(aq) [Fe(acac)3](aq) + 6H2O(l) +3H+ (aq) and Le Châtelier’s Principle.) (refer to the document for the principle).
Question 4: [Pg 11 on the document, also need to scroll back to Part 1 to answer this]
a) Steps 1 and 2 in the PROCEDURE describe test tubes A and B in Diagram 1. Test tube A should contain the neutral [Fe(acac)3] complex synthesised in Part One and polar water, test tube B should contain [Fe(acac)3] and non-polar dichloromethane. Using the idea of “like dissolves like”, which test tube – A or B – do you predict will contain the dissolved [Fe(acac)3]? (Hint: see the notes on solubility in the Introduction section for help.)
b) If the intensity of the colour of the solutions can be taken as a rough guide as to the concentration, which solvent layer in test tube B, the top or the bottom, contains the most [Fe(acac)3]?
c) Is the layer you chose in question 4 (b) the polar (water) layer or the non-polar (dichloromethane) layer?
Question 5
a) Complete the equations that describe the stepwise formation of the tris-acac iron complex, [Fe(acac)3]:
1) [Fe(H2O)6] 3+ + acac¯ => [Fe(H2O)4(acac)]2+ + 2H2O
2) _________________ => ______________________
3) _________________ => [Fe(acac)3] + 2H2O
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