What is the molar solubility of PbF2 in 0.30 M Pb(NO3)2 solution? Ksp(PbF2) = 3.6×10–8

Question

What is the molar solubility of PbF2 in 0.30 M Pb(NO3)2 solution?  Ksp(PbF2) = 3.6×10–8

matt101 · Answer

The molar solubility refers to how many moles of solute can be dissolved in an aqueous solution before the solution is saturated. The molar solubility is expressed in terms of molarity, M.

You can figure out the molar solubility using the solubility product and Ksp. What would be the equation for Ksp in this case?

jfraser · Answer

this is also a problem with the common-ion effect. You need to use the KSP equation and an ICE box approach, as @matt101 suggests, but your initial concentrations of the ions no longer start at zero, like a "normal" ICE box