A solution contains 0.01 M Ag and 0.1 M Pb²⁺. NaCl is gradually added to precipitate the Ag⁺ as AgCl, and the Pb²⁺ as PbCl₂. Given the following K_sp values: AgCl (K_sp = 1.6 x 10^-10)PbCl₂ (K_sp = 2.4 x 10^-4). What is the concentration of Ag⁺ when the Pb²⁺ begins to precipitate?

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Relatively straight forward multi-step problem including writing the balanced precipitation reactions, determining the chloride concentration required for precipitation of PbCl₂, and subsequently determining the concentration of Ag⁺at this Cl^- concentration.

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