Calculate the solubility of each of the following compounds in moles per liter.Ignore any acid-base properties

Question

PbI2, Ksp = 1.4 10^(-8)=?
Ag3PO4, Ksp = 1.8 10^(-18)=?
CaCO3, Ksp = 8.7 10^(-9)=?

Answer 1

In each case, let the solubility to be X.

Case 1:
PbI2, Ksp = 1.4 10^(-8)
Since [PbI2]=X, [Pb]=X and [I] = 2X
we have: Ksp = 1.4x10^(-8) = [Pb]*[I]^2 = 4X^3

Case 2:
Ag3PO4, Ksp = 1.8 10^(-18)
Ksp = 1.8x10^(-18) = 27X^4

CaCO3, Ksp = 8.7x10^(-9)
Ksp = 8.7x10^(-9) = X^2

Now you do the math to solve X (in each case).

Answer 2

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