the solubility of lead (II) sulfate is 8.0x10^-2 g/L. what is the solubility product constant for lead (II) sulfate?
Solution :-
Lets first calculate the molarity of the PbSO4
moles = mass / molar mass
= 8.0*10^-2 g / 303.26 g per mol
= 2.638*10^-4 mol
molarity = moles / volume in liter
= 2.638*10^-4 mol / 1 L
= 2.638*10^-4 M
PbSO4 ------ > Pb^2+ + SO4^2-
ksp = [Pb^2+][SO4^2-]
ksp = [2.638*10^-4] [2.638*10^-4]
ksp =6.96*10^-8
Therefore the solubility product constant ksp = 6.96*10^-8
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