SUMMARY
The correct solubility product constant (Ksp) expression for calcium fluoride (CaF2) is Ksp = [Ca][F]^2, where [Ca] represents the concentration of calcium ions and [F] represents the concentration of fluoride ions. The confusion arises from misinterpreting the stoichiometry of the dissolution reaction, which is CaF2 ⇔ Ca²⁺ + 2F⁻. The expression Ksp = [x][2x]^2 is derived from the molar solubility (x) of CaF2, leading to Ksp = [Ca][2F]^2 being an incorrect interpretation.
PREREQUISITES
- Understanding of solubility product constants (Ksp)
- Basic knowledge of stoichiometry in chemical reactions
- Familiarity with ionic dissociation in solutions
- Knowledge of molar solubility concepts
NEXT STEPS
- Study the derivation of Ksp expressions for various ionic compounds
- Learn about the relationship between molar solubility and Ksp
- Explore stoichiometric calculations in chemical equilibria
- Investigate the effects of temperature on solubility and Ksp values
USEFUL FOR
Chemistry students, educators, and professionals involved in chemical analysis or studying solubility equilibria will benefit from this discussion.