The addition of 0.320 L of 1.37 M KCl to a solution containing Ag+ and Pb2+...
8) Calculate the following for 2.0 L solution containing [Ag+] = 0.100 M and [Pb2+] = 0.100 M. Assume no volume changes. (AgCl Ksp = 1.8 x 10-10, PbCl2 Ksp = 1.8 x 10-5). a) At what [Cl-] will each salt precipitate? b) What percent of the Ag+ has precipitated before the Pb2+ begins to precipitate? c) How much sodium chloride must be added (in grams) to precipitate a maximum AgCl before before any PbCl2 begins to precipitate?
A solution contains Ag^+ and Hg^2+ ions. The addition of 0.100 L of 1. 10 M Nal solution is just enough to precipitate all the ions as Agl and Hgl^2. The total mass of the precipitate is 25.6 g. Find the mass of Agl in the precipitate.
Lead ions can be precipitated from solution with KCl according to the following reaction: Pb2+(aq)+2KCl(aq) →PbCl2(s)+2K+(aq) When 28.5 g KCl is added to a solution containing 25.5 g Pb2+, a PbCl2 precipitate forms. The precipitate is filtered and dried and found to have a mass of 29.3 g. Determine the limiting reactant. Determine the theoretical yield of PbCl2. Determine the percent yield for the reaction.
200 mL of an aqueous solution contains 0.030 M concentrations of both Pb2+ and Ag+. If 100 mL of 6.0 x 10-2 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for PbCl2 and AgCl are 1.7 x 10-5 and 1.8 x 10-10]
1. 200 mL of an aqueous solution contains 0.030 M concentrations of both Pb2+ and Ag+. If 100 mL of 6.0 x 10-2 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for PbCl2 and AgCl are 1.7 x 10-5 and 1.8 x 10-
A solution contains all and Co. The addition of 0.3636 L of 1.752 M NaOH results in the complete precipitation of the ions as Al(OH), and Co(OH),. The total mass of the precipitate is 23.07 g. Find the masses of Art and Co2+ in the solution. mass of Al mass of Co2+ TOOLS x10
A solution contains Cr3+ and Mg2+. The addition of 1.00 L of 1.51 M NaF solution is required to cause the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 50.1 g . Find the mass of Cr3+ in the original solution.
A solution contains Al3 + and Co2 + .The addition of 0.3899 L of 1.695 M NaOH results in the complete precipitation of the ions as Al(OH)3 and Co(OH)2 .The total mass of the precipitate is 23.60 g . Find the masses of Al3 + and Co2 + in the solution. mass of Al 3 + : g mass of Co 2 + : g
A solution contains Al3+ and Co2+. The addition of 0.3969 L of 1.658 M NaOH results in the complete precipitation of the ions as Al(OH), and Co(OH)2. The total mass of the precipitate is 23.64 g. Find the masses of Alt and Co2+ in the solution. mass of A1P+: mass of Co2+: g
A solution contains Al3+ and Co2+. The addition of 0.3555 L of 1.823 M NaOH results in the complete precipitation of the ions as Al(OH), and Co(OH),. The total mass of the precipitate is 22.78 g. Find the masses of Alº+ and Co2+ in the solution. mass of A13+: 09 mass of Co2+: g