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

Question

1)

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

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

Fe(OH)3, Ksp =2.79×1039

2)

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

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

2)

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

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

Explanation / Answer

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

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