Question 14A mixture contains 0.0100 M of both Ba2+ ions and Pb2+ ions. If NaF is slowly added to the solution,The minimum concentration of F required to precipitate the first ion is [Select][Select]The percentage of the first ion remaining in solution when the second ion begins to precipitate out is [Select]would start precipitating first? DQuestion 14A mixture contains 0.0100 M of both Ba2+ ions and Pb2+ ions. If NaF is slowly added to the solution,The minimum concentration of F required to precipitate the first ion is[Select][Select]The percentage of the first ion remaining in solution when the second ion begins to precipitate out i✓ [Select]99.95%0.0082%0.17%1.67E-5%would start precipitating first?

The two reactions that can take place upon adding NaF are- Ba2++ 2NaF→BaF2 +2Na+Pb2++ 2NaF→PbF2 +2Na+ Thus, which ion will start precipitating first depends on the solubility product of the salts formed. Now, Ksp of BaF2 =1.7×10-6 Ksp of PbF2 = 3.6×10-8 The lower the value of Ksp, less the salt is soluble. Now, as Ksp of PbF2 is smaller than the Ksp of BaF2 , thus PbF2 is less soluble in water. Hence, Pb2+ ions will precipitate out first.Now, [Pb2+] =0.0100 M The expression for Ksp is- Ksp=[Pb2+].[F-]2 3.6×10-8=(0.0100 M)×[F-]2[F-]2 =3.6×10-80.0100=3.6×10-6∴[F-] =(3.6×10-6)=1.89×10-3 Hence, the minimum concentration of F- required for precipitation is 1.89×10-3 M. [note: The value of Ksp may slightly vary from one source to other source of data, so choose the closest option]Now, when second ion, Ba2+, starts precipitating, the concentration of [F- ] is- [Ba2+][F-]2=1.7×10-6 (0.0100 M)[F-]2=1.7×10-6[F-]2=1.7×10-4[F-] =1.7×10-4=1.30×10-2M Next, at this fluoride concentration, the concentration of Pb2+ present in solution is- Ksp=[Pb2+].[F-]2 3.6×10-8=[Pb2+]×(1.30×10-2 )2[Pb2+] =3.6×10-8(1.30×10-2 )2=2.13×10-4∴[Pb2+] =2.13×10-4M Therefore, when second ion start precipitating, the lead ion (Pb2+) present in the solution =2.13×10-4M. Thus, initial concentration of Pb2+ = 0.0100 M Thus, the percentage of the first ion remaining in solution when second starts precipitating is- Percentage =2.13×10-4M0.0100×100 = 2.13 % Now, this answer is not matching with the given options. The format of the question and calculation part is all correct. Please try with the Ksp values available to you.

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Question 14 A mixture contains 0.0100 M of both Ba2+ ions and Pb2+ ions. If NaF is slowly added to the solution, [Select] The minimum concentration of F required to precipitate the first ion is [Select] The percentage of the first ion remaining in solution when the second ion begins to precipitate out is [Select] would start precipitating first?

Question 14 A mixture contains 0.0100 M of both Ba2+ ions and Pb2+ ions. If NaF is slowly added to the solution, [Select] The minimum concentration of F required to precipitate the first ion is [Select] The percentage of the first ion remaining in solution when the second ion begins to precipitate out is [Select] would start precipitating first?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question 14 A mixture contains 0.0100 M of both Ba2+ ions and Pb2+ ions. If NaF is slowly added to the solution, The minimum concentration of F required to precipitate the first ion is [Select] [Select] The percentage of the first ion remaining in solution when the second ion begins to precipitate out is [Select] would start precipitating first?
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