A solution has [Ag^+] = [Pb^2+] = [Hg2^2+] = 0.0040 M, what’s the concentration of Cl- to precipitate maximum amount of Hg2^2+ and Ag^+ without precipitate Pb^2+? Ksp (AgCl) = 1.8 × 10^-10, Ksp (PbCl2) = 1.2 × 10^-5, Ksp (Hg2Cl2) = 1.4 × 10^-18

A solution has [Ag^+] = [Pb^2+] = [Hg2^2+] = 0.0040 M, what’s the concentration of Cl- to precipitate maximum amount of Hg2^2+ and Ag^+ without precipitate Pb^2+? Ksp (AgCl) = 1.8 × 10^-10, Ksp (PbCl2) = 1.2 × 10^-5, Ksp (Hg2Cl2) = 1.4 × 10^-18

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section15.5: Factors Affecting Solubility

Problem 15.10CE: Consider 0.0010-M solutions of these sparingly soluble solutes in equilibrium with their ions....

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