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?

Solution

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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