Problem: The Ksp of AgCl is 1.6 x 10 -10. What is the solubility of AgCl in 0.0010 M FeCl 3?

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FREE Expert Solution

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.

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Problem Details

The Ksp of AgCl is 1.6 x 10 -10. What is the solubility of AgCl in 0.0010 M FeCl 3?