Problems to do Chapter 16 #20 and #22 #28a Ag2SO4 is a sparingly soluble salt with Ksp = 1.6 x 10-5. In which of the following solutions would the molar solubility of Ag2SO4 be the lowest? 0.10 M AgNO3 0.20 M AgNO3 0.10 M NaNO3 0.10 M Na2SO4 0.20 M Na2SO4 #36 Calculate the milligrams of silver in 250 mL of a saturated solution of Ag2CO3. [Note: Ksp(Ag2CO3) = 8.1 x 10-12 ; Molar Mass = 274 g/mol] A solution is prepared by mixing 150.0 mL of 0.01 M of Mg(NO3)2 and 250.0 mL of 0.1 M NaF. Calculate the equilibrium concentration of Mg2+. Ksp MgF2 is 6.4 x 10-9. Consider the following data: Ksp MgCO3 3.5 x 10-8 CaCO3 2.8 x 10-9 A solution of sodium carbonate is added to a solution containing 0.10 M Mg2+ and 0.10 M Ca2+. CaCO3 precipitates first since it is less soluble. What is the concentration of Ca2+ remaining in solution when MgCO3 first precipitates? The Ksp for Mn(OH)2 is 2.0 x 10?13. At what pH will Mn(OH)2 begin to precipitate from a solution in which the initial concentration of Mn2+ is 0.10M? Which of the following sparingly soluble salts would be more soluble in an acidic solution than in pure water? More soluble in a solution of NH3 than an acidic solution? PbI2 PbF2 CaCO3 Ag3PO4 AgCl Zn2S AgBr(s) EMBED Equation.2 Ag+(aq) + Br-(aq) Ksp = 5.0 x 10-13 Ag+(aq) + 2NH3(aq) ( Ag(NH3)2+(aq) Kf = 1.6 x 107 Calculate the solubility of AgBr(s) in 2.0 M NH3(aq) solution.
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