Maximizing Precipitation Efficiency: Balancing Common Ions in Ksp Equations

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To precipitate 99.0% of 0.010 M Ce3+ using oxalate (C2O42-) without precipitating 0.010 M Ca2+, the Ksp values for both calcium oxalate (CaC2O4) and cerium oxalate (Ce2(C2O4)3) are crucial. The Ksp for CaC2O4 is 1.3 x 10-8, and for Ce2(C2O4)3, it is 5.9 x 10-30. After removing 99% of Ce3+, the concentration of Ce3+ would be approximately 1 x 10-4 M. This concentration is essential for determining the necessary oxalate concentration to achieve the desired precipitation without affecting calcium. Understanding these Ksp relationships is key to balancing the precipitation efficiency in this scenario.
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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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