SUMMARY
The discussion focuses on the feasibility of precipitating 99.0% of 0.010 M Ce3+ ions using oxalate (C2O4^2-) without simultaneously precipitating 0.010 M Ca2+ ions. The Ksp values for calcium oxalate (CaC2O4) and cerium oxalate (Ce2(C2O4)3) are provided as 1.3 x 10^-8 and 5.9 x 10^-30, respectively. The user has set up the Ksp equations but requires guidance on calculating the concentration of Ce3+ after precipitation. The concentration of Ce3+ after 99% removal is determined to be 1 x 10^-4 M, which is crucial for further calculations.
PREREQUISITES
- Understanding of solubility product constant (Ksp) calculations
- Knowledge of ion concentration and precipitation reactions
- Familiarity with chemical equilibrium concepts
- Basic skills in manipulating molarity equations
NEXT STEPS
- Explore advanced Ksp calculations for multiple ions
- Learn about selective precipitation techniques in analytical chemistry
- Study the impact of ion concentration on solubility equilibria
- Investigate the role of complexation in precipitation reactions
USEFUL FOR
Chemistry students, analytical chemists, and educators focusing on precipitation reactions and solubility equilibria in solution chemistry.