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Copper is regulated in drinking water to protect public health. The relevant reaction is below. The solubility product (equilibrium constant) for the reaction is pK = 19.3.   Cu(OH)2 (s) = Cu+2 + 2 OH-         The regulatory “action limit” (concentration at which a drinking water utility must take action to reduce levels) is 1.3 mg/L dissolved copper.   If the water is at a pH of 7.2, is the level of dissolved copper above, at, or below the action limit? To reduce the concentration of dissolved copper, would you raise or lower the pH? Why?

Copper is regulated in drinking water to protect public health. The relevant reaction is below. The solubility product (equilibrium constant) for the reaction is pK = 19.3.   Cu(OH)2 (s) = Cu+2 + 2 OH-         The regulatory “action limit” (concentration at which a drinking water utility must take action to reduce levels) is 1.3 mg/L dissolved copper.   If the water is at a pH of 7.2, is the level of dissolved copper above, at, or below the action limit? To reduce the concentration of dissolved copper, would you raise or lower the pH? Why?

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter16: Solubility And Precipitation Equilibria
Section: Chapter Questions
Problem 70AP
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Copper is regulated in drinking water to protect public health. The relevant reaction is below. The solubility product (equilibrium constant) for the reaction is pK = 19.3.

 

Cu(OH)2 (s) = Cu+2 + 2 OH-

 

      The regulatory “action limit” (concentration at which a drinking water utility must take action to reduce levels) is 1.3 mg/L dissolved copper.

 

  1. If the water is at a pH of 7.2, is the level of dissolved copper above, at, or below the action limit?
  2. To reduce the concentration of dissolved copper, would you raise or lower the pH? Why?

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