A) A saturated solution of lead(II) fluoride, , was prepared by dissolving solid in water. The concentration of ion in the solution was found to be . Calculate for .
for is .
D) What is the pH of a buffer prepared by adding 0.809 of the weak acid to 0.305 of in 2.00 of solution? The dissociation constant of is . What is the after 0.150 of is added to the buffer from Part A? Assume no volume change on the addition of the acid. What is the after 0.195 of is added to the buffer from Part A? Assume no volume change on the addition of the base.
[Pb2+] = 2.08 * 10^-3 M
One mole of Pb F2 gives two moles of fluoride ions
so [F-] = 2 * 2.08 * 10^-3 M
Ksp = ionic product of a saturated solution
= [Pb^2+] [ Cl -]^2
= (2.08 * 10^-3 M) * (2.08 * 10^-3 M)^2
= 9.00 * 10^-9
Solubility of silver sulfate can be calculated using the Ksp formula:
Ksp = [Ag2+] [SO4^2-]
Hope this helps