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Given: Ksp(Ag2Cro4) = 1.2x10-12 Ksp(BaCro4) 2.1x10-10 For a solution which is initially 0.002 M in Ba2...
Given: Ksp(Ag2CrO4) = 1.2×10-12 Ksp(BaCrO4) = 2.1×10-10 For a solution which is initially 0.060 M in Ba2+ and 0.060 M in Ag+, it is desired to precipitate one of these ions as its chromate (CrO42−) salt to the maximum possible degree without precipitating any of the other cation. From this solution, which ion can be selectively first-precipitated by controlled addition of CrO42− and, ideally, what is the maximum possible percentage of that ion which can be exclusively so precipitated? (Assume...
Given that, for AgCl, at 25°C, K = 1.6x10-10: What is the solubility (g/mL) of AgCl in water at 25°C? 1.26 x 10-5 M You have entered that answer before This question expects a numeric answer. Tries 0/5 Previous Tries Submit Answer 35.0 mL of 0.070 M NaCl is mixed with 35.0 mL of 0.140 M AgNO3. What is [CI] in the supernatant solution at equilibrium, at 25°C? Tries 0/5 Submit Answer What is the solubility (mass/volume) of AgCl in...
Timer Notes Evaluate Feedback Print Inf Course Contents >> ... >> Given: Ksp(Ag Croa) = 41.2x10-12 Ksp(Bacroa) = 2.1x10-10 For a solution which is initially 0.005 M in Ba2+ and 0.005 M in Ag+, it is desired to precipitate one of these ions as its chromate (Cro42-) salt to the maximum possible degree without precipitating any of the other cation. From this solution, which ion can be selectively first-precipitated by controlled addition of CrO42- and, ideally, what is the maximum...
Given that, for AgCl, at 25°C, Ksp 1.6x10 10 From a 1.0x102-M NaCl solution, precipitation of AgCl just begins at what concentration of added Ag*? I Tries 0/5 Submit Answer