Given a 1.00 L solution containting 1.00 x 10^-2 M each of Ca2+ and Ag+. A 1.00 M Na2CO3 solution is used to precipitate each ion in solution. What molar concentration of Co3^2- is needed to precipitate Ag+? Ksp of CaCO3 = 2.80 x 10^-9 Ksp of Ag2CO3 = 8.50 x 10^-12
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Given a 1.00 L solution containting 1.00 x 10^-2 M each of Ca2+ and Ag+. A 1.00 M Na2CO3 solution is used to precipitate each ion in solution. What molar concentration of Co3^2- is needed to precipitate Ag+?
Ksp of CaCO3 = 2.80 x 10^-9
Ksp of Ag2CO3 = 8.50 x 10^-12
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