Consider a solution that is 1.5×10−2 M in Ba2+ and 1.9×10−2 M in Ca2+. What minimum...

Consider a solution that is 1.5×10−2 M in Ba2+ and 1.9×10−2 M in Ca2+.

What minimum concentration of Na2SO4 is required to cause the precipitation of the cation that precipitates first?

Minimum Na2SO4 required to cause PPt is 7.1×10^−9.

What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate?

Expert Solution

queen_honey_blossom answered 2 years ago

Consider a solution that is 2.1×10?2 M in Fe2+and 1.8×10?2 M in Mg2+. I know that...

Consider a solution that is 2.1×10?2 M in Fe2+and 1.8×10?2 M in Mg2+. I know that the Fe2+ was the first to precipitate and that the minimum concentration of K2CO3 is 1.5×10?9 M What I need to know is What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate?

a solution contains 0.050 0 M Ca2+ and 0.030 0 M Ag+. Can 99% of Ca2+...

a solution contains 0.050 0 M Ca2+ and 0.030 0 M Ag+. Can 99% of Ca2+ be precipitated by sulfate without precipitating Ag+? What will be the concentration of Ca2+ when Ag2SO4 begins to precipitate?

75.0 mL of 0.250 M hydrochloric acid is added to 225.0 mL of 0.0550 M Ba(OH)2 solution. What is the concentration of Ba2+ ion left in solution?

75.0 mL of 0.250 M hydrochloric acid is added to 225.0 mL of 0.0550 M Ba(OH)2 solution. What is the concentration of Ba2+ ion left in solution? 75.0 mL of 0.250 M hydrochloric acid is added to 225.0 mL of 0.0550 M Ba(OH)2 solution. What is the concentration of Cl- ion left in solution?

Calculate the pH of a solution that is 1.5 x 10^-8 M NaOH. This is a...

Calculate the pH of a solution that is 1.5 x 10^-8 M NaOH. This is a very dilute solution

When 100 mL each of 2.0 × 10-4 M Ca2+ and 2.0 × 10-2 M F-...

When 100 mL each of 2.0 × 10-4 M Ca2+ and 2.0 × 10-2 M F- are mixed, what is the remaining Ca2+ ion concentration ? The solubility product constant of CaF2 is 5.3 × 10-9. (Hint: Determine the limiting reactant, the concentration of excess reactant after precipitation, and how the concentration of excess reactant influences the solubility of CaF2).

A solution is 0.020 M in each Ca2+ and Cd2+. Adjusting the pH of the solution...

A solution is 0.020 M in each Ca2+ and Cd2+. Adjusting the pH of the solution to which of the following values would achieve the best separation by precipitation of the hydroxides? solubility product constants Best pH = ---Select--- 13.0 12.5 12.0 11.5 11.0 10.5 10.0 9.5 9.0 8.5 8.0 What would be the resulting concentrations of the ions if the solution were adjusted to this pH? [Ca2+] = M [Cd2+] = M

A solution containing the following was prepared: 0.19 M Pb2 , 1.5 × 10-6 M Pb4...

A solution containing the following was prepared: 0.19 M Pb2 , 1.5 × 10-6 M Pb4 , 1.5 × 10-6 M Mn2 , 0.19 M MnO4–, and 0.81 M HNO3. For this solution, the following balanced reduction half-reactions and overall net reaction can occur. 5[Pb^4+ + 2e^- > Pb^2+] E^o=1.690 2[MnO4^-+8H^+ + 5e^-> Mn^2+ + 4H2O] E^o=1.507V ---------------------------------------- 5Pb^4+ + 2Mn^2+ + 8 H2O> 5Pb^2+ + 2MnO4^- + 16H^+ A) Determine E^ocell, deltaG, and K for the Reaction. B) Calculate...

1.5×10−2 M Sr(NO3)2 Express your answer using two significant figures. Part B 1.5×10−2 M NaF Express...

1.5×10−2 M Sr(NO3)2 Express your answer using two significant figures. Part B 1.5×10−2 M NaF Express your answer using two significant figures.

Suppose you have a solution that contains 0.0430 M Ca2 and 0.0910 M Ag . If...

Suppose you have a solution that contains 0.0430 M Ca2 and 0.0910 M Ag . If solid Na3PO4 is added to this mixture, which of the following phosphate species would precipitate out of solution first? Ca3(PO4)2 When the second cation just starts to precipitate, what percentage of the first cation remains in solution?

Calculate the pH of a 0.177 M aqueous solution of pyridine (C5H5N, Kb = 1.5×10-9) and...

Calculate the pH of a 0.177 M aqueous solution of pyridine (C5H5N, Kb = 1.5×10-9) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C5H5N]equilibrium = M [C5H5NH+]equilibrium = M

Question