Answerthis solution will not form a precipitateexplanationsolubility equilbrium: pbfβ(s) β pbΒ²βΊ(aq) + 2 fβ»(aq)the solubility product expression is
(we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as
then, we can interpret q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:
since q = 2.7 Γ 10β»βΈ < ksp = 4 Γ 10β»βΈ, a precipitate will not form.