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

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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