For this problem, we’re being asked to calculate the solubility (in g/L) of AgCl(s) in 0.010 M FeCl3(aq). Since the compounds are ionic compounds, they form ions when dissociating in water. The dissociation of AgCl and AlCl3 in water are as follows:
The chloride ion, Cl–, has a charge of –1. Ag has a charge is +1:
AgCl(s) ⇌ Ag+(aq) + Cl–(aq)
The chloride ion, Cl–, has a charge of –1. Fe has a charge is +3:
AlCl3(s) ⇌ Al3+(aq) + 3 Cl–(aq)
Calculate the molarity of Cl-:
= 0.030 M Cl-
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.
The Ksp of AgCl is 1.6 x 10-10. What is the solubility of AgCl in 0.010 M AlCl3? Give your answer using scientific notation (1.23E-4) and to 2 significant figures (i.e., one decimal place).
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 Goodwin's class at HCC.