Solubility: A Detailed Explanation
Solubility is the maximum amount of a substance (solute) that can dissolve in a given amount of
solvent
at a specific temperature and pressure to form a homogeneous solution.
1. Definition and Units
- Expressed in terms like g/L, mol/L, or ppm.
2. Types of Solubility
- Saturated solution: Contains the maximum amount of dissolved solute.
- Unsaturated solution: Can dissolve more solute.
- Supersaturated solution: Contains more solute than can normally be dissolved.
3. Factors Affecting Solubility
- Nature of solute and solvent: 'Like dissolves like' (polar solutes dissolve in polar solvents).
- Temperature: Generally, solubility of solids increases with temperature, but gases decrease.
- Pressure: Affects gas solubility (Henry's Law).
- Common ion effect: Presence of a common ion decreases solubility.
4. Solubility Product Constant (Ksp)
- Used for sparingly soluble salts to predict precipitation.
5. Applications of Solubility
- Drug formulation, water purification, chemical reactions, etc.
Solubility is the maximum amount of a substance (solute) that can dissolve in a given amount of
solvent
at a specific temperature and pressure to form a homogeneous solution.
1. Definition and Units
- Expressed in terms like g/L, mol/L, or ppm.
2. Types of Solubility
- Saturated solution: Contains the maximum amount of dissolved solute.
- Unsaturated solution: Can dissolve more solute.
- Supersaturated solution: Contains more solute than can normally be dissolved.
3. Factors Affecting Solubility
- Nature of solute and solvent: 'Like dissolves like' (polar solutes dissolve in polar solvents).
- Temperature: Generally, solubility of solids increases with temperature, but gases decrease.
- Pressure: Affects gas solubility (Henry's Law).
- Common ion effect: Presence of a common ion decreases solubility.
4. Solubility Product Constant (Ksp)
- Used for sparingly soluble salts to predict precipitation.
5. Applications of Solubility
- Drug formulation, water purification, chemical reactions, etc.
