Questions: Which direction will the equilibrium shift when the concentration of Cl- is decreased? Which direction will the equilibrium shift when the concentration of H2O is increased?

Which direction will the equilibrium shift when the concentration of Cl- is decreased? Which direction will the equilibrium shift when the concentration of H2O is increased?
Transcript text: Which direction will the equilibrium shift when the concentration of $\mathrm{Cl}^{-}$is decreased? Which direction will the equilibrium shift when the concentration of $\mathrm{H}_{2} \mathrm{O}$ is increased?
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Solution

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Solution Steps

Step 1: Analyze the Effect of Decreasing \(\mathrm{Cl}^{-}\) Concentration

According to Le Chatelier's principle, if the concentration of a reactant or product in a chemical equilibrium is changed, the system will adjust to counteract that change and restore equilibrium. In this case, decreasing the concentration of \(\mathrm{Cl}^{-}\) will cause the equilibrium to shift in the direction that produces more \(\mathrm{Cl}^{-}\), which is the direction of the reactants.

Step 2: Determine the Direction of Equilibrium Shift for \(\mathrm{Cl}^{-}\)

Since the equilibrium will shift to produce more \(\mathrm{Cl}^{-}\), it will shift to the left.

Step 3: Analyze the Effect of Increasing \(\mathrm{H}_{2}\mathrm{O}\) Concentration

Le Chatelier's principle also applies to changes in the concentration of other species in the reaction. If the concentration of \(\mathrm{H}_{2}\mathrm{O}\) is increased, the equilibrium will shift in the direction that consumes \(\mathrm{H}_{2}\mathrm{O}\). Assuming \(\mathrm{H}_{2}\mathrm{O}\) is a reactant, the equilibrium will shift to the right to consume the added \(\mathrm{H}_{2}\mathrm{O}\).

Final Answer

  • The equilibrium will shift to the left when the concentration of \(\mathrm{Cl}^{-}\) is decreased: \(\boxed{\text{shift left}}\).
  • The equilibrium will shift to the right when the concentration of \(\mathrm{H}_{2}\mathrm{O}\) is increased: \(\boxed{\text{shift right}}\).
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