🤓 Based on our data, we think this question is relevant for Professor Yang's class at UH.
For this problem, we’re being asked to calculate the solubility of AgCl in 0.0010 M FeCl3. Since the compounds are ionic compounds, they form ions when dissociating in water. The dissociation of AgCl and FeCl3 in water are as follows:
Chlorine is in Group 7A so its charge is –1. Silver must have a charge of +1:
AgCl(s) → Ag+(aq) + Cl–(aq)
Chlorine is in Group 7A so its charge is –1. Iron must have a charge of +3:
FeCl3(s) ⇌ Fe3+(aq) + 3 Cl–(aq)
Notice that there is a common ion present, Cl–. The common ion effect states that the solubility of a salt is lower in the presence of a common ion.
We can construct an ICE table for the dissociation of AgCl. Remember that solids are ignored in the ICE table.
The Ksp of AgCl is 1.6 x 10 -10. What is the solubility of AgCl in 0.0010 M FeCl 3?