To determine what will happen if more [tex]\(BiCl_3\)[/tex] is added to the reaction:
[tex]\[ BiCl_3(aq) + H_2O(l) \rightleftharpoons BiOCl(s) + 2 HCl(aq) \][/tex]
we need to employ Le Chatelier's Principle. Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
Let's break this down step-by-step:
1. Identify the Disturbance:
- In this case, more [tex]\(BiCl_3\)[/tex] is being added to the system. This is a change in the concentration of one of the reactants.
2. Predict the Response of the System:
- According to Le Chatelier's Principle, the system will respond by trying to consume the added [tex]\(BiCl_3\)[/tex] to counteract the disturbance and re-establish equilibrium.
3. Shift in Equilibrium:
- To consume the additional [tex]\(BiCl_3\)[/tex], the equilibrium will shift to the right. This means the forward reaction (which produces [tex]\(BiOCl\)[/tex] and [tex]\(HCl\)[/tex]) will be favored.
4. Resulting Changes:
- As the forward reaction is favored, more [tex]\(BiOCl\)[/tex] (a solid) will precipitate out of the solution.
- Additionally, more [tex]\(HCl\)[/tex] will be produced in the aqueous phase.
Given these steps, we can determine that adding more [tex]\(BiCl_3\)[/tex] will result in the production of more [tex]\(BiOCl\)[/tex].
Therefore, the correct answer is:
A. More [tex]\(BiOCl\)[/tex] will be produced.
