a) One liter of solution contains 0.10 mol of Ag+ and 0.10 mol of Ba2+. If a highlyconcentrated solution of K2CrO4 is added drop by drop, which will precipitatefirst, Ag2CrO4 or BaCrO4?(Ksp for Ag2CrO4 = 2.0 x 10-12; Ksp for BaCrO4 = 1.2 x 10-10)%3D%3Db) If the solution in part “a" contains 0.0010 mol of Ag+ and 0.0010 mol of Ba2+instead, which will precipitate first, Ag2CrO4 or BaCrO4?

Precipitation occurs if the ionic product is greater than solubility product. Ag2CrO4 The…

Answered: a) One liter of solution contains 0.10…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 15.BCP

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The KSP for BaCro4 is 1.2X10-10. Will BaCrO4 precipitate when 10mL of 1.0X10-5M Ba(NO3)2 is mixed with 10mL of 1.0X10-3M K2Cro4?
What would be the minimum molar concentrations of carbonate ion needed to precipitate each cation? What cation will precipitate first? Given: Sodium carbonate(Na2CO3) is added dropwise to a solution that contains 1.0x10-2M Ag+ and 5.0x10-2M Cd2+ Ksp for Ag2CO3 is 8.1x10-12 Ksp for CaCO3 is 1.8x10-14
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PART 2: A solution is prepared by mixing 150.0 mL of 0.0010 M magnesium nitrate and 250.0 mL of 0.100 M sodium fluoride (Ksp = 7.4x10-11). Is Ksp greater than , equal to, or lower than Qsp? Will a precipitate form, Y/N? What is the fluoride ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3). What is the magnesium ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3).
A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba+2 ions. At what F- concentration will BaF2 start to precipitate? Neglect volume changes. For BaF2, Ksp = 1.7 x 10-6 2.7 × 10-3 M 1.1 × 10-2 M 2.4 × 10-8 M 5.9 × 10-5 M 1.2 x 10-4 M
Will a precipitate form when 25 mL of 0.020M AgNO3 is mixed with 35 mL of 0.020M Na2SO4? (Ksp Ag2SO4 = 1.2 x 10-5 )
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In which solution will 0.00015 M BaCl2 form a precipitate? 7.0x10-7M H2SO4 (Ksp of BaSO4=1.1x10-10) 0.10 M Pb(NO3)2 (Ksp of PbCl2=1.7x10-5) 0.010 M NaF (Ksp of BaF2=1.7x10-6) 5.0x10-7M AgNO3 (Ksp of AgCl=1.8x10-10)
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