The drinking water standard for lead is 0.05 mg/L total soluble lead. One method for removing lead from water is by pH adjustment in order to precipitate the metal hydroxide [i.e., Pb(OH)₂(s)]. Consider the reactions governing the solubility of lead hydroxide in pure water: Pb(OH)2(s) →→Pb²+ + 2OH* Pb²+ + OH →PbOH+ Pb²+ + 2OH Pb(OH)₂º Pb²+ + 3OH →Pb(OH)3 Kso-10-15.6 B₁=106.3 B₂=1010.9 B3-1013.9 a) Construct a logC-pH diagram for the Pb(OH)2(s) system. b) Indicate the region of Pb(OH)2 supersaturation by shading the appropriate portion of the diagram. c) What is the lowest possible lead concentration (in mg/L as Pb) that could be attained by precipitating Pb(OH)2(s)? At what pH would the precipitation need to be carried out to achieve this level? How does this Pb value compare to the regulatory limit?

The drinking water standard for lead is 0.05 mg/L total soluble lead. One method for removing lead from water is by pH adjustment in order to precipitate the metal hydroxide [i.e., Pb(OH)₂(s)]. Consider the reactions governing the solubility of lead hydroxide in pure water: Pb(OH)2(s) →→Pb²+ + 2OH* Pb²+ + OH →PbOH+ Pb²+ + 2OH Pb(OH)₂º Pb²+ + 3OH →Pb(OH)3 Kso-10-15.6 B₁=106.3 B₂=1010.9 B3-1013.9 a) Construct a logC-pH diagram for the Pb(OH)2(s) system. b) Indicate the region of Pb(OH)2 supersaturation by shading the appropriate portion of the diagram. c) What is the lowest possible lead concentration (in mg/L as Pb) that could be attained by precipitating Pb(OH)2(s)? At what pH would the precipitation need to be carried out to achieve this level? How does this Pb value compare to the regulatory limit?

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

The drinking water standard for lead is 0.05 mg/L total soluble lead. One method for
removing lead from water is by pH adjustment in order to precipitate the metal hydroxide
[i.e., Pb(OH)₂(s)]. Consider the reactions governing the solubility of lead hydroxide in pure
water:
Pb(OH)2(s) →→Pb²+ + 2OH-
Pb²+ + OH →PbOH+
Pb²+ + 2OH →Pb(OH)₂⁰
Pb²+ + 3OH Pb(OH)3
Kso-10-15.6
B₁=106.3
B₂=1010.9
B3-1013.9
a) Construct a logC-pH diagram for the Pb(OH)2(s) system.
b) Indicate the region of Pb(OH)2 supersaturation by shading the appropriate portion of the
diagram.
c) What is the lowest possible lead concentration (in mg/L as Pb) that could be attained by
precipitating Pb(OH)2(s)? At what pH would the precipitation need to be carried out to
achieve this level? How does this Pb value compare to the regulatory limit?

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