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Part I In Part I the reaction you observed was Mg(OH)2 (s) ó Mg (aq) +...

Part I In Part I the reaction you observed was Mg(OH)2 (s) ó Mg (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?

B. Which way should the equilibrium shift when Na2EDTA is added? How do your results support your answer?

C. Is this reaction endothermic or exothermic? How do you know?

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Answer #1

A)
HCl is acid
It will reaction with OH-
So concentration of OH- is decreasing
Equilibrium will shift to right

b)
Na2EDTA will react with Mg to form MeEDTA
So concentration of Mg2+ is decreasing
Equilibrium will shift to right

c)
Breaking of bond is endothermic process
So it will be endothermic reaction

You need to know find out this by experiment
Just increase the temperature:
if forward reaction favours, it is endothermic
if backward reaction favours, it is exothermic

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