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A solution contains 1.0 x 10-5 M Na3PO4. What is the minimum concentration of silver nitrate that would cause precipitation of solid silver phosphate (Ksp = 1.8 x 10-18)?

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Related questions

What is the silver ion concentration in a solution prepared by mixing 405 mL of 0.381 M silver nitrate with 391 mL of 0.449 M sodium phosphate? The Ksp of silver phosphate is 2.8 × 10-18

A basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation. The I– concentration, which is 8.40×10-5 M, is 10,000 times less than that of the PO43– ion at 0.840 M . A solution containing the silver(I) ion is slowly added. Answer the questions below. Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17.

Calculate the minimum Ag+ concentration required to cause precipitation of AgI.
Calculate the minimum Ag+ concentration required to cause precipitation of Ag3PO4.

basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation. The I– concentration, which is 8.60×10-5 M, is 10,000 times less than that of the PO43– ion at 0.860 M . A solution containing the silver(I) ion is slowly added. Answer the questions below. Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17.

Part 1:

Calculate the minimum Ag+ concentration required to cause precipitation of AgI. (mol/L)

Part 2:

Calculate the minimum Ag+ concentration required to cause precipitation of Ag3PO4. (mol/L)

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