1. Solubility Main Concept:
The solubility of a substance can be understood in terms of equilibrium.

2. Solubility Solubility Free Energy and Solubility Salts and Solubility
Common Ions pH

3. - The dissolution of a substance in a solvent is a reversible reaction  has an associated equilibrium constant
- For dissolution of salt, reaction quotient, Q, = solubility product, and equilibrium constant for reaction = Ksp (solubility-product constant)
- solubility of a substance can be calculated from Ksp for dissolution reaction  can be used to reason qualitatively about relative solubility of different substances

5. - free energy change (ΔG°) for dissolution of a substance reflects breaking of forces holding solid together and the interaction of dissolved species with solvent
- Also, entropic effects must be considered  solubility requires consideration of all of these contributions to the free energy

6. - All sodium, potassium, ammonium, and nitrate salts are soluble in water
- salts  less soluble in solutions that have ions in common with salt  affects solubility of salts in seawater and other natural bodies of water  think Le Chatelier’s principle

7. - solubility of salt will be pH sensitive when one of the ions is an acid or base  Applications include high pH’s leading to iron hydroxide precipitate in acid-mine drainage and effects of acid rain on solubility of carbonates  think Le Chatelier’s principle
- basic anions more soluble in acids
- acidic cations more soluble in bases