13. The concentration of iodide ions in a saturated solution of lead (II) iodide

ID: 967980 • Letter: 1

Question

13. The concentration of iodide ions in a saturated solution of lead (II) iodide is ________ M.

The solubility product constant of PbI2 is 1.4 x 10-8.

[A] 1.4 x 10-8 [B] 1.5 x 10-3 [C] 3.5 x 10-9 [D] 3.8 x 10-4 [E] 3.0 x 10-3

14. The solubility of lead (II) chloride (PbCl2) is 1.6 x 10-2 M. What is the Ksp of PbCl2?

[A] 4.1 x 10-6 [B] 1.6 x 10-5 [C] 3.1 x 10-7 [D] 5.0 x 10-4 [E] 1.6 x 10-2

15. The solubility of manganese (II) hydroxide (Mn(OH)2) is 2.2 x 10-5 M. What is the Ksp of

Mn(OH)2?

[A] 2.2 x 10-5 [B] 2.1 x 10-14 [C] 1.1 x 10-14 [D] 4.8 x 10-10 [E] 4.3 x 10-14

16. Which of these expressions correctly expresses the solubility-product constant for

Ag3PO4 in water?

[A] [Ag][PO4] [B] [Ag+][PO43] [C] [Ag+]3[PO43]

[D] [Ag+][PO43]3 [E] [Ag+]3[PO43]3

17. A solution of NaF is added dropwise to a solution that is 0.0166 M in Ba2+. When the

concentration of F- exceeds ________ M, BaF2 will precipitate. Neglect volume changes.

For BaF2, Ksp = 1.7 10-6.

[A] 1.0 x 10-2 [B] 1.0 x 10-4 [C] 5.1 x 10-5 [D] 2.5 x 10-3 [E] 2.8 x 10-8

18. A solution contains 2.3 x 10-4 M Ag+ and NaI solution is being added drop wise. What

is the minimum concentration of I- to begin precipitation of AgI? Ksp (AgI)= 8.3 x 10-17

[A] 8.32 x10-17 M [B] 2.51 x 10-17 M [C] 3.01 x 10-15

[D] 3.51 x 10-14 M [E] 3.61 x 10-13 M

PbI2(aq) <-------------> Pb^2+(aq) + 2I-(aq)

Ksp = [Pb^2+] [I-]^2

1.4 x 10^-8 = [x][2x]^2

1.4 x 10^-8 = 4x^3

x^3 = 4.67 x 10^-9

x = 1.67 x 10^-3

Thus, Concentration of I- = [I-] = 2x = 2 x 1.67 x 10^-3 = 3.34 x 10^-3 M

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