Form A 18. A solution contains 0.021 M Cl- and 0.017 MI. A solution containing copper (I) ions is added to selectively precipitate one of the ions. At what concentration of copper (I) ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuC]) = 1.0 × 106, Ksp(Cul) = 5.1 × 10-12 A. 3.0 x 10-10 M, Cul B. 3.0 x 10-10 M, CuCl C. 4.8 x 10-5 M, CuCl D. 4.8 x 10-5 M, Cul E. 2.4 × 10-10 M, Cul

Form A 18. A solution contains 0.021 M Cl- and 0.017 MI. A solution containing copper (I) ions is added to selectively precipitate one of the ions. At what concentration of copper (I) ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuC]) = 1.0 × 106, Ksp(Cul) = 5.1 × 10-12 A. 3.0 x 10-10 M, Cul B. 3.0 x 10-10 M, CuCl C. 4.8 x 10-5 M, CuCl D. 4.8 x 10-5 M, Cul E. 2.4 × 10-10 M, Cul

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section: Chapter Questions

Problem 96GQ: A solution contains 0.10 M iodide ion, I, and 0.10 M carbonate ion, CO32. (a) If solid Pb(NO3)2 is...

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According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
Some barium chloride is added to a solution that contains both K2SO4 (0.050 M) and Na3PO4 (0.020 M). (a) Which begins to precipitate first: the barium sulfate or the barium phosphate? (b) The concentration of the first anion species to precipitate, either the sulfate or phosphate, decreases as the precipitate forms. What is the concentration of the first species when the second begins to precipitate?
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Suppose you have a water solution that is 0.0010 M Ca2+ and 0.0010 M Mg2+. Describe the precipitation reactions as you slowly add a concentrated solution of sodium carbonate, Na2CO3, to this solution. What would be the concentration of carbonate ion, CO32, when at least 90.0% of Ca2+ and Mg2+ have been precipitated.
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
A solution contains Ca2+ and Pb2+ ions, both at a concentration of 0.010 M. You wish to separate the two ions from each other as completely as possible by precipitating one but not the other using aqueous Na2SO4 as the precipitating agent. (a) Which will precipitate first as sodium sulfate is added, CaSO4 or PbSO4? (b) What will be the concentration of the first ion that precipitates (Ca2+ or Pb2+) when the second, more soluble salt begins to precipitate?
A solution contains 0.10 M iodide ion, I, and 0.10 M carbonate ion, CO32. (a) If solid Pb(NO3)2 is slowly added to the solution, which salt will precipitate first, Pbl2 or PbCO3? (b) What will be the concentration of the first ion that precipitates (CO32 or I) when the second, more soluble salt begins to precipitate?
You will often work with salts of Fe3+, Pb2+, and Al3+ in the laboratory. (All are found in nature, and all are important economically.) If you have a solution containing these three ions, each at a concentration of 0.10 M, what is the order in which their hydroxides precipitate as aqueous NaOH is slowly added to the solution?
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. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
Magnesite (magnesium carbonate, MgCO3) is a common magnesium mineral. From the solubility product constant, find the solubility of magnesium carbonate in grams per liter of water.