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In physical chemistry, supersaturation occurs with a solution when the concentration of a solute exceeds the concentration specified by the value of solubility at equilibrium. Most commonly the term is applied to a solution of a solid in a liquid , but it can also be applied to liquids and gases dissolved in a liquid.
Köhler curves showing how the critical diameter and supersaturation are dependent upon the amount of solute. It's assumed here that the solute is a perfect sphere of sodium chloride with a dry diameter Dp. Köhler theory describes the vapor pressure of aqueous aerosol particles in thermodynamic equilibrium with a humid atmosphere.
Supersaturation, where the concentration of a solute exceeds its maximum solubility at equilibrium; Undersaturation, where the concentration of a solute is less than its maximum solubility at equilibrium
The supersaturation is achieved by a gradual reduction in temperature of the solution in the autoclave. The disadvantage of this technique is the difficulty in controlling the growth process and introducing seed crystals. For these reasons, this technique is very seldom used.
where V l is the molar volume of the droplet, σ lv the liquid-vapor surface energy, and s is the degree of supersaturation [5] of the vapor. This equations restricts the minimum diameter of the droplet, and of any crystals which can be grown from it, under typically conditions to well above the nanometer level.
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A condition known as supersaturation may develop. Supersaturation by gas may be defined as a sum of all partial pressures of gases dissolved in the liquid which exceeds the ambient pressure in the liquid. [19] The gas will not necessarily form bubbles in the solvent at this stage, but supersaturation is necessary for bubble growth. [3]
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