ps 27. A solution contains 0.0497 M SO4 (aq) and 0.0894 M CO32 (aq). If Ag+ (aq) ions are slowly added, whichla compound (Ag2SO4 or Ag2CO3) will ppt first and at what [Ag]? (In other words, which of the following isalentirely correct?) (Suggestion: Write the dissolving equations and Ksp expressions for Ag2SO4 and Ag2CO3before starting this problem.)a. Ag2SO4 precipitates first at [Ag+] = 1.8 x 102 Mb. Ag2CO3 precipitates first at [Ag+] = 9.6 x 106 Mc. Ag2CO3 precipitates first at [Ag+] = 9.2 x 10-11 Md. Ag2SO4 precipitates first at [Ag+] = 3.2 x 104 Me. Ag2CO3 precipitates first at [Ag+] = 1.3 x 10-5 M0. bCarsidong01 1.8-0301-01 x 1.8-9 d100to squads llenavo odi staluple 08.0

To determine which compound precipitates first and at what concentration of Ag⁺, we need to compare…

Answered: ps 27. A solution contains 0.0497 M SO4…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter11: Solving Equilibrium Problems For Complex Systems

Section: Chapter Questions

Problem 11.16QAP

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A scientist was interested in how soluble rust is in acidic soils, so she set up an idealized problem to get an initial feel for the situation. A fairly acidic soil has a pH of 4.50. Also, rust is essentially Fe(OH)3. Therefore, she considered the following problem: Suppose a 1.00-g sample of iron(III) hydroxide is exposed to 1.00 L of a buffer with a pH of 4.50. She then calculated the nanograms of Fe3+ that dissolve in a liter of this buffer. Show how you would do this problem. Explain your work.
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A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?
A saturated solution of copper(II) iodate in pure water has a copper-ion concentration of 2.7 103 M. a What is the molar solubility of copper iodate in a 0.35 M potassium iodate solution? b What is the molar solubility of copper iodate in a 0.35 M copper nitrate solution? c Should there be a difference in the answers to parts a and b? Why?
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A solution is 0.15 M in both Pb2+ and Ag+. If Cl- is added to this solution, what is [Ag+] when PbCl2 begins to precipitate?
Although silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia. AgCl(s)+2NH3(aq)Ag(NH3)2+(aq)+Cl(aq) a What is the equilibrium constant for this dissolving process? b Ammonia is added to a solution containing excess AgCl(s). The final volume is 1.00 L and the resulting equilibrium concentration of NH3 is 0.80 M. Calculate the number of moles of AgCl dissolved, the molar concentration of Ag(NH3)2+, and the number of moles of NH3 added to the original solution.

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