Problem: What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 x 10-5.

FREE Expert Solution

To solve for molar solubility of PbCl2 in 0.15 M HCl


Recall that Ksp is an equilibrium constant related to slightly soluble ionic compounds


The dissociation of slightly solublePbCl2 in solution is as follows:

PbCl2(s)  Pb2+(aq) + 2Cl(aq)


We can construct an ICE table for this dissociation. Remember that solids are ignored in the ICE table and Ksp expression.



View Complete Written Solution
Problem Details

What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 x 10-5.

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.