use Lewis structure to show A basic solution contains the lodide and phosphate i

Question

use Lewis structure to show
A basic solution contains the lodide and phosphate ions that are to be separated via selective precipitation.The I concentration, which is 9,.90x10 5 M, is 10,000 times less than that of the PO,3-ion at 0.990 M. A solution containing the silver) ion is slowly added.Answer the questions below. Kp of Agl is 8.30×10-17 and of Agfo. 8.90× 1017. 4th attempt Part 1 (1 point) l See Periodic Table See Hint Calculate the minimum Ag concentration required to cause precipitation of Ag x10 mol/L

Explanation / Answer

AgI = Ag+ + I-

Ksp= [Ag+][I-]

8.3*10^-17 = [Ag+][I-]

get [Ag+] from [I-]

[I-] = 9.9*10^-5

8.3*10^-17 = [Ag+](9.9*10^-5)

[Ag+] = (8.3*10^-17)/(9.9*10^-5) = 8.3838*10^-13 M

PART 2

find Ag+ min for Ag3PO4 formation

Ag3PO4 <-> 3Ag++ PO4-3

Ksp = [Ag+]^3 *¨[PO4-3]

8.9*10^-17 =  [Ag+]^3 * (0.99)

[Ag+] = ((8.9*10^-17 / (0.99))^(1/3)

[Ag+] = 0.0000044

[Ag+] = 4.4*10^-6 M

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