SUMMARY
The solubility of silver chloride (AgCl) can be calculated using its solubility product constant (Ksp), which is 1.8x10-10 mol2dm-6 at room temperature (RTP). To find the solubility in pure water, the equation Ksp = [Ag+] x [Cl-] is applied, leading to S = √(1.8x10-10). The conversion from moles to grams per cubic decimeter (g dm-3) requires knowledge of the molar mass of AgCl. Additionally, silver chloride is less soluble in a silver nitrate solution due to the common ion effect, and it is more soluble in aqueous ammonia due to the formation of soluble complexes.
PREREQUISITES
- Understanding of solubility product constant (Ksp)
- Knowledge of molar mass calculations
- Familiarity with the common ion effect
- Basic principles of complex ion formation in aqueous solutions
NEXT STEPS
- Research the calculation of solubility from Ksp values
- Learn about the common ion effect and its implications on solubility
- Study the formation of complex ions in solutions, specifically with ammonia
- Explore the molar mass of silver chloride (AgCl) for conversion purposes
USEFUL FOR
Chemistry students, educators, and professionals involved in analytical chemistry or solubility studies, particularly those focusing on ionic compounds and their behavior in various solutions.