Maximizing Precipitation Efficiency: Balancing Common Ions in Ksp Equations

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Discussion Overview

The discussion revolves around the feasibility of precipitating 99.0% of 0.010 M Ce3+ ions by adding oxalate (C2O42-) while avoiding the precipitation of 0.010 M Ca2+ ions. Participants explore the implications of the solubility product constants (Ksp) for calcium oxalate and cerium oxalate in this context.

Discussion Character

  • Homework-related
  • Mathematical reasoning
  • Technical explanation

Main Points Raised

  • One participant presents the Ksp equations for both calcium oxalate and cerium oxalate, indicating a need to analyze these to determine the conditions for selective precipitation.
  • Another participant questions the concentration of Ce3+ after 99% has been removed, suggesting a concentration of 1 x 10-4 M, but does not provide further context on how this affects the precipitation process.
  • A subsequent post reiterates the question about the concentration of Ce3+ after removal, indicating a focus on the implications of this concentration for the overall problem.
  • There is a question about whether the calculated concentration of Ce3+ aids in solving the original problem, suggesting uncertainty about the relevance of this information.

Areas of Agreement / Disagreement

Participants do not appear to reach a consensus on how to proceed with the problem or the implications of the concentration of Ce3+ after precipitation. Multiple viewpoints and questions remain unresolved.

Contextual Notes

The discussion lacks specific details on how to convert molarity to moles and mass, which may affect the calculations. There is also an absence of clarity regarding the volume of the solution, which is critical for determining the actual amounts involved in the precipitation process.

ReidMerrill
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Homework Statement


Is it possible to precipitate 99.0% of 0.010 M Ce3+ by adding oxalate (C2O42-) without precipitating 0.010 M Ca2+
CaC2O4 Ksp = 1.3 x 10-8 Ce2(C2O4)3 Ksp = 5.9 x 10-30

Homework Equations


1.3x10-8 = [0.01M][C2O4-]
5.9x10-30=[0.01M]2[C2O4]3

The Attempt at a Solution


All I've been able to do is set up those Ksp equations but I'm not sure what to do from here
 
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What is the concentration of Ce3+ after 99% has been removed?
 
Borek said:
What is the concentration of Ce3+ after 99% has been removed?
1x10-4M presumably considering no volume is given to convert molarity to moles and mass
 
Does this number help in solving the problem further?
 

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