Question

Ag+ ions are added to the solution with
(Br-) = (Cl- ​) = (CO3​2-) = (AsO4)3-= 0.1 M
which compound will precipitate at the lowest [Ag+]?
a) AgBr [Ksp = 5 x 10 -13]
b) Ag2CO3[Ksp = 8.1 x 10 -12]
c) AgCl [Ksp = 1.8 x 10 -10]
d) Ag3AsO4[Ksp = 10 -22]
Also explain why ??

Answer 1

agci(ksp=1.8×10-10)

Answer 2

Answer:

d)  Ag3AsO4 [Ksp = 10 -22]

Explanation:

Precipitation occurs when the ionic product of the solute exceeds the solubility product Ksp.

Thus, ionic product is the product of the concentration of the ions Qsp = [M+[A-]

For precipitation - Ksp<Qsp

Thus, the lesser the solubility of the product, the lesser the concentration of the ions is required.

Since the concentration of anion is same, the concentration of Ag+ will be required the least in case that has the lowest solubility product which will be Ag3AsO4.