Computer Data Analysis

1. The initial color is pink with HSO4- in water and yellow-orange in other cells.

2. Adding SO42- shifts equilibrium to left to pink.

3. Adding NaHSO4, increases HSO4-, shifts equilibrium to right, orange.

4. Heating shifts equilibrium to right to orange.

5. Colling brings back HSO4- to pink.

6. Cooling has no effect when only HSO4- is present.

7. Heating would form more ionized species to yellow color.

8. Net ionic equation,

HSO4-(aq) + H2O(aq)  

9. The equilibrium shifts to the left side, i.e. towards HSO4-. According to Le-Chatelier's principle, the increase in the concentration of SO42- shifts the equilibrium towards the direction, where there is less concentration of SO42-, i.e. to the left side of the equilibrium.

10. The observations always do support the prediction except in some cases, where there is some manual error or so.

11. The equilibrium shifts to the right side, i.e. towards SO42-. Explanation: According to Le-Chatelier's principle, the increase in the concentration of HSO4- shifts the equilibrium towards the direction, where there is less concentration of HSO4-, i.e. to the right side of the equilibrium.

12. Here also, the observations always do support the prediction except in some cases, where there is some manual error or so.

13. The reaction is endothermic. Explanation: The Ka1 for the H2SO4 is much greater than zero, but the Ka for HSO4- (Ka2 for H2SO4) is less than zero.

14. HSO4-(aq) + H2O(l) + heat  SO42-(aq)+ H3O+(aq) (The reaction favors products due to heat)

15. The intial color of wells is white.

16. When HCl is added, the color changes to colorless.

17. Blue color is formed when reacted with EDTA.

18. The initial color of wells would be white for precipitate presence.

19. Colorless and precipitate dissolved.

20. Cooling the mixture gives Mg(OH)2 precipitate back.

21. Color changes to white.

22. Color changes to transparent.

23. Net Ionic equation,

Mg2+ + EDTA^4- <==> [MgEDTA]2-

24. Adding HCl shifts reaction towards left hand side as more reactants is formed. this is according to Lechatellier's principle.

25. The color change of the solution proves this prediction

26. Adding Na4EDTA shifts reaction towards right hand side, as excess EDTA4– reacts with remaining Mg2+ to generate more products, according to LeChatellier's principle.

27. Change in color from initial and after addition proves this hypothesis.

28. When heated the color changed due to formation of [MgEDTA] 2– complex so forward reaction is endothermic in reaction.

29. Net ionic equation,

Mg2+ + EDTA4- + heat ----> [MgEDTA] 2–

30. Initial color is pink.

31. When water is added, color becomes light pink.

32. When HCl is added, according to LeChatellier's principle, incresed Cl- in solution shifts the equilibrium to [CoCl4] 2- formation and color becomes blue,

33. When AgNO3 is added, it reacts with Cl- and thus reduced Cl- concentration in solution shifts equilibrium to the right and solution becomes pink color.

34. When H2O is added to C-2, solution becomes dilute and color becomes pink.

35. When ethyl alcohol is added, no change is observed.

36. When water is added, reaction turns pink again.

37. When heated it turns blue as forward reaction is endothermic.

38. Cooling the reaction mixture gives back pink due to formation of [Co(H2O)6] 2+ again.

39. Net ionic reaction,

[Co(H2O)6] 2+ (pink) + 4Cl- <==> [CoCl2] 2- (blue) + 6H2O

40. Adding water shifts equilibrium to the left and color becomes pink.

41. Change in color to pink supports the theory.

42. Concentrated HCl addition, shifts equilibrium to the right (blue color).

43. The change in color supports this theory.

44. AgNO3 When added, forms AgCl, reduces Cl- in solution and equilibrium shifts to pink on the left side.

45. Formation of pink color, supports this theory.