A solution contains [Ba2+] = 5.0 × 10-5 M, [Ag+] = 3.0 × 10-5 M, and...

A solution contains [Ba2+] = 5.0 × 10-5 M, [Ag+] = 3.0 × 10-5 M, and [Zn2+] = 2.0 × 10-7 M. Sodium oxalate is slowly added so that [C2O42-] increases. Salt BaC2O4 ZnC2O4 Ag2C2O4 Ksp 1.5 × 10-8 1.35 × 10-9 1.1 × 10-11 What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

Expert Solution

queen_honey_blossom answered 2 hours ago

A) 1 L of solution contains 0.10 mol Ag+ and 0.10 mol of Ba2+. If a...

A) 1 L of solution contains 0.10 mol Ag+ and 0.10 mol of Ba2+. If a highly concentrated solution of K2CrO4 is added drop by drop, which will precipitate first, Ag2CrO4 or BaCrO4? Ksp for AgCrO4 = 2.0 x 10^-12; Ksp for BaCrO4= 1.2 x 10^-10 B) If the solution in part "A" contains 0.0010 Ag+ and 0.0010 mol of Ba2+ instead, which will precipiate first, Ag2CrO4 or BaCrO4? Answers: A) Ag2CrO4 and B) BaCrO4

Calculate the initcial I^- concentration in a solution containing 3.0 mL of 0.20 M KI, 5.0...

Calculate the initcial I^- concentration in a solution containing 3.0 mL of 0.20 M KI, 5.0 mL of 0.15 M (NH4)2S2O8, 5.0 mL of 0.25 M (NH4)SO4, 6.0 mL of 0.10 M KNO3, and 1.0 mL of 0.012 M Na2S2O3.

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?

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?

A solution contains 0.036 M0.036 M Ag+Ag+ and 0.013 M0.013 M Pb2+.Pb2+. If you add Cl−,Cl−,...

A solution contains 0.036 M0.036 M Ag+Ag+ and 0.013 M0.013 M Pb2+.Pb2+. If you add Cl−,Cl−, AgClAgCl and PbCl2PbCl2 will begin to precipitate. What is the concentration of Cl−Cl− required, in molarity, when AgClAgCl precipitation begins? concentration of Cl−=Cl−= M What is the concentration of Cl−Cl− required, in molarity when AgClAgCl precipitation is 99.99% complete? concentration of Cl−=Cl−= M What is the concentration of Cl−Cl− required, in molarity when PbCl2PbCl2 precipitation begins? concentration of Cl−=Cl−= M What is the concentration...

A solution contains 0.028 M Ag and 0.032 M Pb2 . If you add Cl–, AgCl...

A solution contains 0.028 M Ag and 0.032 M Pb2 . If you add Cl–, AgCl and PbCl2 will begin to precipitate. What is the concentration of Cl– required, in molarity, when: A. AgCl precipitation begins? B. AgCl precipitation is 99.99% complete? C. PbCl2 precipitation begins? D. PbCl2 precipitation is 99.99% complete? Finally, give the concentration range of Cl– for the complete precipitation of Ag and Pb2 . E. Concentration of Cl– at the start of precipitation: F. Concentration of...

A solution contains 0.041 M Ag and 0.047 M Pb2 . If you add Cl–, AgCl...

A solution contains 0.041 M Ag and 0.047 M Pb2 . If you add Cl–, AgCl and PbCl2 will begin to precipitate. What is the concentration of Cl– required, in molarity, when A. AgCl precipitation begins? B. AgCl precipitation is 99.99% complete? C. PbCl2 precipitation begins? D. PbCl2 precipitation is 99.99% complete? Finally, give the Cl– concentration range in which Ag can be completely separated from Pb2 by precipitation. E. Give the lowest Cl– concentration for the F. Give the...

1). A solution contains 0.0490 M Ca2+ and 0.0980 M Ag+. If solid Na3PO4 is added...

1). A solution contains 0.0490 M Ca2+ and 0.0980 M Ag+. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? (which one?) (a). Ca3(PO4)2 (b). Ag3PO4 (c). Na3PO4 2). When the second cation just starts to precipitate, what percentage of the first cation remains in solution? percentage = ?%

6.Suppose you have a solution that contains 0.0420 M Ca2 and 0.0960 M Ag . If...

6.Suppose you have a solution that contains 0.0420 M Ca2 and 0.0960 M Ag . If solid Na3PO4 is added to this mixture, which of the following phosphate species would precipitate out of solution first? first part is Ca3(PO4)2 When the second cation just starts to precipitate, what percentage of the first cation remains in solution? ______ %

A solution contains 0.306 M HA (Ka = 6.43 ⋅ 10 − 5 ) and 0.683...

A solution contains 0.306 M HA (Ka = 6.43 ⋅ 10 − 5 ) and 0.683 M NaA. What is the pH of this solution? What is the pH of this solution after 0.233 mol of HCl are added to 1.00 L of this solution? What is the pH of this solution after 0.466 mol of HCl are added to 1.00 L of this solution?

Question