Why is Barium Chloride Preferred Over Lead Chloride for Sulfate Precipitation?

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SUMMARY

Barium chloride (BaCl2) is preferred over lead chloride (PbCl2) for sulfate precipitation in gravimetric analysis due to its higher solubility. This characteristic allows for more efficient precipitation of barium sulfate (BaSO4) compared to lead sulfate (PbSO4), which has lower solubility. The discussion confirms that the addition of BaCl2 to a heated solution containing sulfate ions results in a more effective and reliable determination of sulfate concentration.

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  • Understanding of gravimetric analysis techniques
  • Knowledge of solubility principles in chemistry
  • Familiarity with barium sulfate (BaSO4) and lead sulfate (PbSO4) properties
  • Basic laboratory skills for conducting precipitation reactions
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  • Research the solubility product constant (Ksp) of BaSO4 and PbSO4
  • Study the principles of gravimetric analysis in detail
  • Explore the effects of temperature on solubility in precipitation reactions
  • Investigate alternative precipitation agents for sulfate determination
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Chemistry students, laboratory technicians, and researchers involved in analytical chemistry and gravimetric analysis of sulfate ions.

Stroodle
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Hi there.

I'm just wanting to know the most important reason why barium chloride is chosen over lead chloride as the precipitation agent when trying to determine, by gravimetric analysis, how much sulfate is in a sample.

I think it's probably due to BaCl2 having a higher solubility, but I just want to confirm.
In the experiment the BaCl2 (or PbCl2) is added to a heated solution containing the sulfate ions.

Thanks!
 
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What about the solubilities of PbSO4 and BaSO4?
 

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