Question

Consider the system at equilibrium.

CaCl2(s)↽−−⇀Ca2+(aq)+2Cl−(aq)CaCl2(s)↽−−⇀Ca2+(aq)+2Cl−(aq)

How will adding more CaCl2CaCl2 shift the equilibrium?

to the left

no effect

to the right

How will removing some Ca2+Ca2+ shift the equilibrium?

to the right

to the left

no effect​

Answer 1

Answer:

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Answer 2

Answer:

The equilibrium will shift to the right to produce more Ca2+ ions. Therefore, removing some Ca2+ ions will shift the equilibrium to the right.

Explanation:

Adding more CaCl2 to the system will increase the concentration of Ca2+ and Cl- ions in the solution. According to Le Chatelier's principle, if we increase the concentration of any species in a system at equilibrium, the equilibrium will shift in the direction that reduces the concentration of that species. In this case, adding more CaCl2 will increase the concentration of Ca2+ and Cl- ions, so the equilibrium will shift to the left to reduce the concentration of these ions. Therefore, adding more CaCl2 will shift the equilibrium to the left.

Removing some Ca2+ from the system will decrease the concentration of Ca2+ ions in the solution. According to Le Chatelier's principle, if we decrease the concentration of any species in a system at equilibrium, the equilibrium will shift in the direction that produces more of that species. In this case, removing some Ca2+ ions will decrease the concentration of Ca2+ ions, so the equilibrium will shift to the right to produce more Ca2+ ions. Therefore, removing some Ca2+ ions will shift the equilibrium to the right.

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