Gold coast institute of tafe

Potassium Chromate(VI) and Chromate(VI) ion EquilibriaThis video demonstrates the shifting in the position of a dynamic equilibrium reaction. Potassium chromate(VI) solution contains yellow chromate(VI) ions. In acidicsolution, orange dichromate(VI) ions are formed.Chemical equilibrium is called dynamic equilibrium because the forward and the reverse reactions are both taking placeat the same rate.The position of equilibrium refers to equilibrium concentrations of the reactants and products.If the position of equilibrium lies to the left, the concentration of the reactants is greater than the concentration of the products.The position of equilibrium can be shifted by varying the temperature, pressure (if gases are involved), concentration of reactants or products. When a change is made to the system, the position of equilibrium shifts according to Le Chatelier’s principle.‘If a system is at equilibrium, and a change is made in any of the conditions, then the system responds to counteract thechange as much as possible’.The Potassium Chromate(VI) and Chromate(VI) ion Equilibriareaction is:2CrO42–(aq) + 2H+(aq)Cr2O72–(aq) + H2O(l)chromate(VI) iondichromate(VI) ionyelloworangeThe video shows a test tube containing a roughly equal mix of chromate(VI) and dichromate(VI) ions. Acid is added and this serves to favour the forward reactionshiftingthe equilibrium to the right. This takes place because the forward reaction serves to reduce the increased H+concentration thus opposing the change. The forward reaction converts chromate ions to dichromate ions and the solution turns from a yellow/orange solution to an orange solution.Sodium hydroxide is then added and this reacts with excess H+ions in a neutralization reaction. This serves to decrease the concentration of H+ions and the position of equilibrium moves to the left as the reverse reaction is favouredwhich opposes the change producing more H+ions. The reverse reaction converts dichromate ions to chromate ions and the solution turns from an orange solution to a yellow solution.
Questionsto ask when demonstrating this practical or videoBefore demonstrating this practical or video the students need to have been taught about chemical equilibria and Le Chatelier’s principle. Before initiating the demonstration the equation should be written up so that students can refer to it when observing the colour changes and when answering the questions directed at them.The Potassium Chromate(VI) and Chromate(VI) ion Equilibriareaction is:2CrO42–(aq) + 2H+(aq)Cr2O72–(aq) + H2O(l)chromate(VI) iondichromate(VI) ionyelloworange1.What colour is the solution in the test tube?2.What does this tell us about the concentrations of the reactants and products?3.What does this tell us about the position of equilibrium?4.When acid is added what happens to the colour of the solution?5.Which of the reactions, the forward or the reverse reaction has been favoured?6.What is the acid adding which forms part of the reaction?7.What happens to the H+concentration when the acid is added to the tube?8.What happens to the H+concentration when the forward reaction is favouredand takes place?9.Is this shift in equilibrium in line with Le Chatelier’s principle?10.When alkali is added what happens to the colour of the solution?11.Which of the reactions, the forward or the reverse reaction has been favoured?12.When the alkali is added what does it react with?13.What happens to the H+concentration when the alkaliis added to the tube?14.What happens to the H+concentration when the reverse reaction is favouredand takes place?15.Is this shift in equilibrium in line with Le Chatelier’s principle?