Hydrogen and Equilibrium Shift
Le Chatelier’s Principle
Part I:
Record your observations.
NaOH was dissolved in MgCl2, the color turned dark pink (from white)
Questions
In Part I the reaction you observed was Mg(OH)2 (s) Mg2+ (aq) + 2 OH- (aq). Compare the colors you observed in the experiment and answer these questions:
A. Which way should the equilibrium shift when HCl is added? How do your results support your answer?
It should shift to the left because adding any component causes the equilibrium to shift to the opposite side.
B. Which way should the equilibrium shift when Na2EDTA is added? How do your results support your answer?
It should shift to the right because the removal of a component causes the equilibrium to shift to the side from which the component was removed.
C. Is this reaction endothermic or exothermic? How do you know?
This reaction is endothermic because the solution HC1 and Na2EDTA added decreased the reaction as the equilibriums both shifted to the left.
Part II:
Record your observations.
Then HCl was added and the color changed back to white.
Questions
In Part II the reaction you observed was HSO4- (aq) + H2O (l) H3O+(aq)+SO42-. Compare the colors you observed in the experiment and answer these questions:
A. Which way should the equilibrium shift when Na2SO4 is added? How do your results support your answer?
It should shift to the left because adding any component causes the equilibrium to shift to the opposite side.
B. Which way should the equilibrium shift when NaHSO4 is added? How do your results support your answer?
It should shift to the right because the removal of a component causes the equilibrium to shift to the side from which the component was removed.
D. Is this reaction endothermic or exothermic? How do you know?
When acid is added to water the reaction is strongly exothermic. Because the hydrogen ion is so tiny, a large amount of charge is concentrated in a very small
Part I:
Record your observations.
NaOH was dissolved in MgCl2, the color turned dark pink (from white)
Questions
In Part I the reaction you observed was Mg(OH)2 (s) Mg2+ (aq) + 2 OH- (aq). Compare the colors you observed in the experiment and answer these questions:
A. Which way should the equilibrium shift when HCl is added? How do your results support your answer?
It should shift to the left because adding any component causes the equilibrium to shift to the opposite side.
B. Which way should the equilibrium shift when Na2EDTA is added? How do your results support your answer?
It should shift to the right because the removal of a component causes the equilibrium to shift to the side from which the component was removed.
C. Is this reaction endothermic or exothermic? How do you know?
This reaction is endothermic because the solution HC1 and Na2EDTA added decreased the reaction as the equilibriums both shifted to the left.
Part II:
Record your observations.
Then HCl was added and the color changed back to white.
Questions
In Part II the reaction you observed was HSO4- (aq) + H2O (l) H3O+(aq)+SO42-. Compare the colors you observed in the experiment and answer these questions:
A. Which way should the equilibrium shift when Na2SO4 is added? How do your results support your answer?
It should shift to the left because adding any component causes the equilibrium to shift to the opposite side.
B. Which way should the equilibrium shift when NaHSO4 is added? How do your results support your answer?
It should shift to the right because the removal of a component causes the equilibrium to shift to the side from which the component was removed.
D. Is this reaction endothermic or exothermic? How do you know?
When acid is added to water the reaction is strongly exothermic. Because the hydrogen ion is so tiny, a large amount of charge is concentrated in a very small