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.
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
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