SUMMARY
The solubility of silver chloride (AgCl) at 25℃ is calculated using its solubility product constant (Ksp), which is 1.8x10^-10. The dissociation of AgCl into Ag+ and Cl- ions is represented by the equation AgCl ⇔ Ag+ + Cl-. By applying the Ksp expression, Ksp = [Ag][Cl], and substituting [Ag] = [Cl], the molar solubility of AgCl is determined to be 1.3x10^-5 M.
PREREQUISITES
- Understanding of solubility product constant (Ksp)
- Knowledge of chemical equilibrium principles
- Familiarity with molarity calculations
- Basic concepts of ionic dissociation
NEXT STEPS
- Study the concept of solubility product constants (Ksp) for other salts
- Learn about the common ion effect on solubility
- Explore the relationship between temperature and solubility
- Investigate the calculation of molar solubility for various ionic compounds
USEFUL FOR
Chemistry students, educators, and professionals involved in analytical chemistry or materials science who require a solid understanding of solubility calculations and ionic equilibria.