Question

i need help with answering these questions from lab

G.C.2.7 Studying the Elect of Changes.in Conditions on an Equilibrium S 1 System No. 4: [Co(H20l + 4C C CP +6H.O. Solutions Observations Dissolved Cocl, 61,0 Pink SOLUTION Solution plus HCI Blue Solution Heated solution Blue Solution Cooled solution Pink Solution O r dine to the equilibrium equation, which ion(s) do you have after the solid was diluted Expl how you know the identity of the ion(s) present 10. Explain what happened when HCl was added to the solution 11 Explain what happened when the solution was heated. Was the shift in equilibrium cothermice endothermic? 12. Explain what happened when the solution was cooled. Was the shift in equilibrium exothermic or endothermic? System No. 5: Fe + SCNS [Fe(SCN) (Forward reaction is exothermic) Solutions Observations Fe(NO), + KSCN mixture Red Diluted solution Pale red Heated solution Cooled solution NO Change (red) Solution + Fe(NO, more red / same Solution + KSCN more red / same Solution + AgNO, milky white / AQSCN fomed Solution + NaOH Brown lorange (Fe(OH) formed 13. When the test tube was placed in the hot water bath, was the shift in equilibrium endothermic or exothermic? Explain. 14. Explain what happened when you added more Fe(NO), and KSCN. 15. Explain what happened after you added AgNO. Hint: Determine the potential products being formed from adding AgNO, to the solution 16. Explain what happened after you added NaOH. Hint: Determine the potential products being formed from adding NaOH to the solution. Light brown / orange

Answer 1

9. When the solid was dissolved in water it formed a complex ion [Co(H2O)6]2+ and the identity of the ion was found out by its colour change to pink whereas [CoCl]42- ion is blue in colour.

10. When HCl is added to the solution, there will be an increase in the concentration of chloride ions that is Cl- in the solution and thus according to the Le Chatelier's principle the equilibrium will be shifted towards right and the solution turns blue.

11.When we add heat as the reactant in the equilibrium state,the solution gets heated and equilibrium shifts towards the direction of [CoCl]42- that is towards the product side thus making the solution blue in colour.

12. When the hest is being removed from the equilibrium state, which is in a cooled condition,then the equilibrium shifts towards the direction of [Co(H2O)6]2+ that is towards the reactant side thus making the solution pink in colour.