Calculate the aqueous solubility, in moles per liter, of each of the following.

Question

Calculate the aqueous solubility, in moles per liter, of each of the following.

PbBr2 Ksp=4.0x10^-5

CeF2 Ksp=8x10^-16

Explanation / Answer

PbBr ===> Pb2+ + 2Br- Ksp = [Pb2+][Cl-]^2 = 4 x 10^-5 The molar solubility of PbBr2 = [Pb2+] Let [Pb2+] = x. Then [Br-] = 2x, and (x)(2x)^2 = 4 x 10^-5 4x^3 = 4 x 10^-5 x^3 = 10^-5 x = 0.0215 = molar solubility of PbBr2 CeF2 ===> Ce2+ + 2F- Ksp = [Ce2+][F-]^2 = 8x10^-16 The molar solubility of CeF2 = [Ce2+] Let [Ce2+] = x. Then [F-] = 2x, and (x)(2x)^2 = 8x10^-16 4x^3 = 8x10^-16 x^3 = 2x 10^-7 x = 0.00000584803= molar solubility of CeF2

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