Problem: The solubility of lead(II) chloride is 0.016 mol/L. What is the Ksp of PbCl2?A) 4.9 × 10–2B) 1.7 × 10–5C) 8.5 × 10–6D) 4.2 × 10–6E) < 1.0 × 10–6

FREE Expert Solution

For this problem, we’re being asked to calculate the Ksp of PbCl2


Since the PbCl2 is an ionic compound, it forms ions when dissociating in water. The dissociation of PbCl2 in water is as follows:


The chloride ion, Cl, has a charge of –1. So lead must have a charge of +2:

PbCl2(s)  Pb2+(aq) + 2 Cl(aq)



We can construct an ICE table for the dissociation of PbCl2

Remember that solids are ignored in the ICE table and Ksp expression.


85% (46 ratings)
View Complete Written Solution
Problem Details

The solubility of lead(II) chloride is 0.016 mol/L. What is the Ksp of PbCl2?

A) 4.9 × 10–2

B) 1.7 × 10–5

C) 8.5 × 10–6

D) 4.2 × 10–6

E) < 1.0 × 10–6

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.