SUMMARY
The Ksp (solubility product constant) of lead(II) iodide (PbI2) at 25°C can be calculated using the formula Ksp = [Pb2+][I-]^2. Given that the concentration of a saturated solution of PbI2 is 540 mg/L, this value can be converted to molarity to determine the Ksp. The molar mass of PbI2 is approximately 461 g/mol, leading to a molarity of 0.00117 M for Pb2+ and 0.00234 M for I-. Thus, the Ksp can be calculated as Ksp = (0.00117)(0.00234)^2.
PREREQUISITES
- Understanding of solubility product constants (Ksp)
- Basic knowledge of molarity and concentration calculations
- Familiarity with lead(II) iodide (PbI2) and its dissociation in water
- Ability to perform unit conversions (mg/L to molarity)
NEXT STEPS
- Learn about the dissociation of ionic compounds in solution
- Study the calculation of Ksp for other salts, such as AgCl and CaF2
- Explore the impact of temperature on solubility and Ksp values
- Investigate the applications of Ksp in predicting precipitation reactions
USEFUL FOR
Chemistry students, educators, and professionals involved in analytical chemistry or environmental science who require a deeper understanding of solubility and Ksp calculations.