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.
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.
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