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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?

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter15: Complex Ion And Precipitation Equilibria
Section: Chapter Questions
Problem 76QAP
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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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