s = mass of PbF2 dissolved / volume of solution
= 0.515 g / 1.00 L
= 0.515 g/L
Molar mass of PbF2,
MM = 1*MM(Pb) + 2*MM(F)
= 1*207.2 + 2*19.0
= 245.2 g/mol
Molar mass of PbF2= 245.2 g/mol
s = 0.515 g/L
To covert it to mol/L, divide it by molar mass
s = 0.515 g/L / 245.2 g/mol
s = 2.1*10^-3 mol/L
At equilibrium:
PbF2 <----> Pb2+ + 2 F-
s 2s
Ksp = [Pb2+][F-]^2
Ksp = (s)*(2s)^2
Ksp = 4(s)^3
Ksp = 4(2.1*10^-3)^3
Ksp = 3.706*10^-8
Answer: 3.71*10^-8
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