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Determine what will happen if more [tex]\( \text{BiCl}_3 \)[/tex] is added to the following reaction:

[tex]\[ \text{BiCl}_3 (aq) + \text{H}_2 \text{O} (l) \rightleftharpoons \text{BiOCl} (s) + 2 \text{HCl} (aq) \][/tex]

A. More [tex]\( \text{BiOCl} \)[/tex] will be produced.
B. Less [tex]\( \text{BiOCl} \)[/tex] will be produced.
C. More [tex]\( \text{BiCl}_3 \)[/tex] will be produced.
D. Less [tex]\( \text{HCl} \)[/tex] will be produced.



Answer :

GinnyAnswer
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.

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