1) Which of the following compounds will have the highest molar solubility in pu

ID: 515180 • Letter: 1

Question

Which of the following compounds will have the highest molar solubility in pure water?

Fe(OH)3, Ksp =2.79×1039

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2) = 1.7 × 10-6.

Ag2S, Ksp=6.0×1051 ZnS, Ksp=2.0×1025 ZnSe, Ksp=3.6×1026 PbS, Ksp=9.04×1029

Fe(OH)3, Ksp =2.79×1039

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2) = 1.7 × 10-6.

2.3 × 10-5 M 1.2 × 10-2 M 8.5 × 10-7 M 3.0 × 10-4 M 0.0750 M

1) answer : Fe(OH)3, Ksp =2.79×10^39

Explanation :

Fe(OH)3 ------------> Fe+3 + 3 OH-

S 3S

Ksp = [Fe+3][OH-]^3

2.79×10^39 = S x (3S)^3

S = 1.0 x 10^-10 M

remaining all are less solubility in pure water. because number of ions. are less .

2) answer : 3.0 x 10^-4 M

BaF2 ---------------> Ba+2 + 2 F-

S 0.0750

Ksp = [Ba+2][F-]^2

1.7 x 10^-6 = S x 0.0750^2

S = 3.0 x 10^-4

molar solubility = 3.0 x 10^-4 M