Question

First, you observe the reaction of SbCl₃ and distilled H₂O to be a cloudy white solution. You then add HCl and the solution becomes clear.

1. Did the addition of HCl favor the products or reactants? Did the relative concentrations of SbCl3, H₂O, and SbOCl increase or decrease? Justify yout answer.

Next, you add distilled water to the same solution and it becomes cloudy and white again.

2. How does the addition of H₂O affect the equilbirum? How did the relative concentrations of SbCl₃, SbOCl, and HCl change after the addition of H₂O? justify your answer.

Answer 1

SbCl3 + H2O SbOCl + 2HCl

a) The addition of HCl to the above equilibrium favors the reactants.

As a result, the relative concentrations of SbCl3 and H2O will increase, whereas, the relative concentration of SbOCl decreases.

Explanation: According to Le-Chatelier's principle, the equilibrium shifts in a direction to nullify the stress applied to the system. i.e. The addition of HCl makes the equilibrium to shift towards the side, where there is less HCl concentration, i.e. reactant side.

b) The addition of H2O to the above equilibrium favors the products according to the Le-Chatelier's principle explained above.

As a result, the relative concentrations of SbOCl and HCl will increase, whereas, the relative concentration of SbCl3 decreases.