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12 Dec 2019

Consider the reaction at equilibrium:

MgO(s) + H2O(ℓ) ←→ Mg(OH)2(aq)

If you remove Mg(OH)2 from the system, how will the system respond?

1.)nothing will happen

2.) the reaction will shift to the left

3.) not enough information

4.) the reaction will shift to the right

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Elin Hessel
Elin HesselLv2
13 Dec 2019

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Related questions

Consider the reaction at equilibrium:

MgO(s) + H2O(l) <---> Mg(OH)2(aq)

If you increase the system's pressure, how will the system respond?

a.) the reaction will shift to the left

b.) not enough information

c.) the reaction will shift to the right

d.) nothing will happen

Consider dissolving Mg(OH)2 in a solution at low pH:
Mg(OH)2 (s) ⇌ Mg2+(aq) + 2 OH− (aq)
What would you expect to happen?

A.  Equilibrium will shift to the right as the H3O+ ions of the

acid react with the OH− produced.

B.  Equilibrium will shift to the left as the H3O+ ions of the

acid react with the OH− produced.

C.  The solubility of Mg(OH)2 in solution will decrease.D.  Equilibrium is independent of the pH of solution.

I'd also like an explanation to the answer please, thanks!

Q1) The reaction shown below is endothermic.

NH4NO3 (s) NH4 + (aq) + NO3 − (aq)

a) Add energy (heat) to the above reaction as either a product or a reactant.

b) If the system shown above is cooled down, would the equilibrium shift to the right or to the left? Why?

c) Suppose you increase the concentration of NH4 + (aq). Would the equilibrium shift to the right or to the left? Why?

Q2) Consider the equilibrium reaction shown below.

HF(aq) + H2O(l) H3O + (aq) + F− (aq)

a) What will happen to the concentration of hydronium (H3O + ) in the system if a solution containing hydroxide (OH− ) is added? (Hint: see Equation (1).)

b) In which direction will the equilibrium shift if hydroxide is added? Why?

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