SUMMARY
The concentration of Li+ ions in a saturated Li3PO4 solution is calculated using the solubility product constant (Ksp) of 2.37 × 10-4. The correct concentration of Li+ ions is 0.0544 M, not 0.163 M as initially calculated. The discrepancy indicates a misunderstanding of the stoichiometry involved in the dissolution of Li3PO4, where each formula unit produces three Li+ ions. Thus, the concentration must be adjusted accordingly based on the Ksp value.
PREREQUISITES
- Understanding of solubility product constants (Ksp)
- Basic knowledge of stoichiometry in chemical reactions
- Familiarity with lithium phosphate (Li3PO4) dissolution process
- Ability to perform concentration calculations in saturated solutions
NEXT STEPS
- Study the concept of solubility product constants (Ksp) in detail
- Learn about stoichiometric calculations in chemical equilibria
- Explore the dissolution process of ionic compounds in water
- Practice calculating ion concentrations from Ksp values using various compounds
USEFUL FOR
Chemistry students, educators, and professionals involved in analytical chemistry or materials science who require a deeper understanding of solubility and ion concentration calculations.