A solution contains 0.0490 M Ca²+ and 0.0930 M Ag*. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? O Ca3(PO4)2 Ag3PO4 Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution? percentage: %

9. A solution is prepared by adding 0.100 moles of AgNO3(s) to 1.00 L of 0.500 M NH3 aqueous solution. If NaCl(s) is then added to the solution, what is the maximum concentration of NaCl that can be present without AgCl(s) precipitating?

tion 14 of 32 A solution contains 0.0480 M Ca2+ and 0.0990 M Ag+. If solid Na PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? Ca3(PO4)2 Ag3PO4 NazPO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution? percentage:

The calcium in a 200 mL sample of water sample was determined by precipitating the cation as CaC2O4. The precipitate was filtered, washed and ignited in a crucible with an empty mass of 26.6002 g. The mass of the crucible plus Cao (56.077 g/mol) was 26.7134 g. Calculate the Molarity of Ca. a. 0.005 M O b. 0.040 M O c. 0.100 M O d. 0.080 M O e. 0.010 M

A 160.0 mL solution of 3.130 M strontium nitrate is mixed with 220.0 mL of a 3.361 M sodium fluoride solution. Calculate the mass of the resulting strontium fluoride precipitate. 43.1 mass: Incorrect Assuming complete precipitation, calculate the final concentration of each ion. Ksp values can be found in the table of solubility product constants. 1.87 [Na*] = M Incorrect [NO,] = 2.67 M 0.39 [Sr²*] M Incorrect [F] = M

A solution contains 0.036 M Ag+ and 0.031 M Pb²+. If you add Cl¯, AgCl and PbCl₂ will begin to precipitate. What is the concentration of Cl required, in molarity, when AgCl precipitation begins? concentration of Cl- = What is the concentration of Cl required, in molarity when AgCl precipitation is 99.99% complete? concentration of Cl- = What is the concentration of Cl required, in molarity when PbCl₂ precipitation begins? concentration of Cl- = What is the concentration of Cl required, in molarity when PbCl₂ precipitation is 99.99% complete? concentration of Cl- = Finally, give the Cl- concentration range in which Ag+ can be completely separated from Pb²+ by precipitation. Give the lowest CI concentration for the separation of Ag+ from Pb²+. concentration of Cl- = Give the highest Cl¯ concentration for the separation of Ag+ from Pb²+. concentration of Cl- = M M M M M M

8. When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of PbI2, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the recovered P6SO4 is found to have a mass of 0.0471g, what was the concentration of iodide ions in the original solution The answer is

A solution contains 7.4 x 10-5 M Naz PO4. What is the minimum concentration of AgNO, that would cause precipitation of solid Ag; PO4 ( Ksp = 1.8 x 10 18)? Concentration = M

A solution contains 0.0450 M Ca2+ and 0.0940 M Ag+. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? Ca3(PO4)2 Ag3PO4 Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution? percentage: 13.93 Incorrect %

The equation for the dissolving of lead (II) chloride (including heat) is: PbCl2(s) + heat Pb2*la q) + 2 CI (a q) solid 2 dissolved Which statement is true? When PbCl2s) is heated in water, the solid dissolves. When PbCl2(s) is heated in water, the solid remains.