13.5 Solubility Equilibria
Solubility and Ksp
Ksp is the equilibrium constant for an ionic solid dissociating into aqueous ions.
AgCl(s) → Ag+(aq) + Cl-(aq)
Ksp = [Ag+][Cl-]
Mg(OH)2(s) → Mg2+(aq) + 2OH-(aq)
Ksp = [Mg2+][OH-]2
BiI3(s) → Bi3+(aq) + 3I-(aq)
Ksp = [Bi3+][I-]3
What is the molar solubility of AgCl (Ksp = 1.8 × 10-10)?
What is the molar solubility of Mg(OH)2 (Ksp = 1.6 × 10-12)?
The molar solubility of BiI3 is 1.32 × 10-5. Calculate Ksp.
Common Ion Effect
What is the molar solubility of AgCl in 0.1M HCl? (Ksp = 1.8 × 10-10)
| RELATION OF Ksp TO MOLAR SOLUBILITY | ||
|---|---|---|
| 2 Ions | 3 Ions | 4 Ions |
| Ksp = x2 | Ksp = 4x3 | Ksp = 27x4 |
| Ksp | |
|---|---|
| AgCl | 1.8 × 10-10 |
| AgBr | 5.0 × 10-13 |
| AgI | 8.3 × 10-17 |