Problem: The solubility product, Ksp, for PbCl2 is 1.7 × 10–5. What is the solubility of PbCl 2 in water, in moles per litre?a. 1.6 × 10–2 mol L–1b. 6.2 × 10–2 mol L–1c. 2.4 × 10–4 mol L–1d. 7.7 × 10–3 mol L–1

FREE Expert Solution

For this problem, we’re being asked to calculate the solubility (in mol/L) 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 –1Lead then has a charge of +2:

PbCl2(s)  Pb2+(aq) + 2 Cl(aq)



We will do the following steps to solve the problem:

Step 1: Construct an ICE table

Step 2: Calculate the molar solubility



Step 1: Construct an ICE table


We can construct an ICE table for the dissociation of Ni(OH)2

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


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Problem Details

The solubility product, Ksp, for PbCl2 is 1.7 × 10–5. What is the solubility of PbCl 2 in water, in moles per litre?

a. 1.6 × 10–2 mol L–1

b. 6.2 × 10–2 mol L–1

c. 2.4 × 10–4 mol L–1

d. 7.7 × 10–3 mol L–1

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.

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