Removing Pb2+ from Water: EPA Standards & NaCl Solution

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SUMMARY

The discussion focuses on the removal of Pb2+ from drinking water, emphasizing that the Environmental Protection Agency (EPA) sets a maximum concentration of 1.00 x 10-7 M for lead. To achieve this, a significant concentration of NaCl is required due to the solubility product constant (Ksp) of PbCl2, which is 1.6 x 10-5. However, using high concentrations of salt can create harmful saline environments detrimental to aquatic life. Additionally, the solubility of PbCl2 increases in hot water, posing further risks.

PREREQUISITES
  • Understanding of Ksp (Solubility Product Constant)
  • Knowledge of chemical precipitation reactions
  • Familiarity with the effects of salinity on aquatic ecosystems
  • Basic principles of water quality standards set by the EPA
NEXT STEPS
  • Calculate the required concentration of Cl- to precipitate PbCl2 using Ksp values.
  • Research the environmental impact of saline solutions on freshwater ecosystems.
  • Explore alternative methods for lead removal from water, such as ion exchange or reverse osmosis.
  • Study the solubility characteristics of PbCl2 in various temperatures and conditions.
USEFUL FOR

Environmental scientists, water quality engineers, and anyone involved in water treatment processes, particularly those addressing heavy metal contamination in drinking water.

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[SOLVED] Removing Pb from water

The Environmental Protection Agency recommends that Pb2+ have a concentration not exceeding 1.00 x 10-7 M in drinking water. What concentration of NaCl could be used to remove the lead from the water to bring it to a safe level? Ksp for PbCl2 is 1.6 x 10-5. What would the drawbacks of doing this be?

Could anyone get me going with this?
 
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sveioen said:
Could anyone get me going with this?

Ksp=[Pb2+][Cl-]^2 by definition.

You are given the KSP and Pb2+ values, simply find the concentration of Cl-. You will notice that you will need a LOT of salt to do this, and creating highly saline environments in water sources kills a lot of plants and wildlife.
 
gravenewworld said:
Ksp=[Pb2+][Cl-]^2 by definition.

You are given the KSP and Pb2+ values, simply find the concentration of Cl-. You will notice that you will need a LOT of salt to do this, and creating highly saline environments in water sources kills a lot of plants and wildlife.

Wow, so it is that easy. Thank you very much gravenewworld!:smile:
 
sveioen said:
Wow, so it is that easy. Thank you very much gravenewworld!:smile:
Ok, however don't do it with hot water, or you'll kill people (PbCl2 is quite soluble in hot water).
Furthermore, precipitating Pb with Cl- obviously take in solution the anion and this one can be not appropriate itself for a drinking water: NO3- for example.
 
Last edited:
This sounds more like Chemistry 101 homework than somebody with bad well water. But, you never know.
 
jim mcnamara said:
This sounds more like Chemistry 101 homework than somebody with bad well water. But, you never know.
Agree :approve:
 

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