Suppose you have a solution that contains 0.0420 M Ca2 and 0.0900 M Ag . If soli

Question

Suppose you have a solution that contains 0.0420 M Ca2 and 0.0900 M Ag . If solid Na3PO4 is added to this mixture, which of the following phosphate species would precipitate out of solution first?

Suppose you have a solution that contains 0.0420 M Ca^2+ and 0.0900 M Ag^+. If solid Na_3PC_4 is added to this mixture, which of the following phosphate species would precipitate out of solution first? Ca_3(PO_4)_2 Ag_3PO_4 Na_3PO_4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution?

Explanation / Answer

Ksp of Ag3PO4 =1.4*10-16

Ksp of Ca3PO4 = 1*10-25

Theksp of Ag3PO4 is high when compared to Ksp of Ca3PO4, so Ca3PO4 starts ppt first than Ag3PO4

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