Solubility
Solubility refers to the ability of a substance (solute) to dissolve in a solvent to form a homogeneous solution. It depends on temperature, pressure, and the nature of the solute and solvent.
Factors Affecting Solubility
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Nature of Solute and Solvent
- “Like dissolves like”: Polar solutes dissolve in polar solvents; nonpolar solutes dissolve in nonpolar solvents.
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Temperature
- Most solids: Solubility increases with temperature
- Most gases: Solubility decreases with temperature
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Pressure (mainly affects gases)
- Higher pressure increases gas solubility in liquids (Henry’s Law: S = kP)
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Common Ion Effect
- Presence of ions already in solution reduces solubility of a salt due to Le Chatelier’s principle.
Saturation
- Unsaturated: Contains less solute than maximum; more can dissolve
- Saturated: Contains maximum solute at given conditions; dynamic equilibrium exists
- Supersaturated: Contains more solute than equilibrium; unstable, may crystallize spontaneously
Importance
- Predicting precipitation reactions in chemistry
- Designing pharmaceutical formulations and solutions
- Understanding environmental processes such as gas absorption in water
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