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

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.

83% (345 ratings)
View Complete Written Solution
Problem Details

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

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Ksp concept. You can view video lessons to learn Ksp. Or if you need more Ksp practice, you can also practice Ksp practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Yang's class at UH.