What is the equilibrium Pb2+
concentration when 2.61 L of a
0.103 M lead acetate solution are
mixed with 2.82 L of a 0.370 M
ammonium bromidesolution?
[Pb2+] = M
The solubility of AgCl in water
is 1.34×10-5 M, but
increases in the presence of thiosulfate
ion. Calculate the solubility of
AgCl when the solid is added to a solution that is
0.520 M in thiosulfate
ion. For AgCl, Ksp =
1.80×10-10 and for
Ag(S2O3)23-,
Kf = 2.00×1013.
Solubility = M
What is the equilibrium Pb2+ concentration when 2.61 L of a 0.103 M lead acetate solution are mixed with 2.82 L of a 0.3...
The solubility of AgBr in water is 5.74×10-7 M, but increases in the presence of thiosulfate ion. Calculate the solubility of AgBr when the solid is added to a solution that is 0.795 M in thiosulfate ion. For AgBr, Ksp = 3.30×10-13 and for Ag(S2O3)23-, Kf = 2.00×1013. Solubility = M
The solubility of AgCN in water is 1.10×10-8 M, but increases in the presence of thiosulfate ion. Calculate the solubility of AgCN when the solid is added to a solution that is 0.785 M in thiosulfate ion. For AgCN, Ksp = 1.20×10-16 and for Ag(S2O3)23-, Kf = 2.00×1013. Solubility = M
The solubility of AgI in water is 1.22×10-8 M, but increases in the presence of thiosulfate ion. Calculate the solubility of AgI when the solid is added to a solution that is 0.694 M in thiosulfate ion. For AgI, Ksp = 1.50×10-16 and for Ag(S2O3)23-, Kf = 2.00×1013. Solubility = M
A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility of calcium iodate in mol/L? (b) What are the concentrations of Ca2+ and IO3 – ion, respectively, in the saturated solution? (c) Calculate the Ksp value for Ca(IO3)2. Part b ) Silver ion, Ag+ , readily forms complex ion, Ag(S2O3)2 3– , with thiosulfate, S2O3 2– , according to the following equation: Ag+ (aq) + 2S2O3 2– (aq) ⇌ Ag(S2O3)2 3– (aq); Kf =...
The solubility of AgCl in water is 1.34x10-M, but increases in the presence of thiosulfate ion. Calculate the solubility of AgCl when the solid is added to a solution that is 0.704 M in thiosulfate ion. For AgCI, Ksp = 1.80x10-10 and for Ag(S203)23, Kr=2.00x1013 Solubility =
1) Use equilibrium ion concentration to calculate Ksp. The Pb2+ concentration in a saturated solution of lead bromide is measured and found to be 1.19×10-2 M. Use this information to calculate a Ksp value for lead bromide. Ksp =___________ 2) Use solubility to calculate Ksp. The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide. Ksp =______________
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?
Question 4 07 1.5 pts What is the concentration of Pb2+ in a saturated solution of PbCl2 in 0.10 M KCl solution. (Ksp = 1.4 x 108)? Why is [Pb2') in this question (smaller/larger) than in Question 3? Hint: What is the initial [CI] before PbCl2 is dissolved? because the presence of chloride ion prevents the dissolution 1.4 x 10M of PbCl2 1.5 x 10M same as in Question 3 1.4 x 10-M, because the presence of chloride ion slows...
What is the equilibrium Agt concentration when 1.25 L of a 0.197 M silver acetate solution are mixed with 1.16 L of a 0.203 M ammonium sulfide solution? [Agt] = M
What is the equilibrium Ba2+ concentration when 2.38 L ofa 0.153 M barium acetate solution are mixed with 2.57 L of a 0.268 M ammonium sulfate solution? [Ba2]-