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m Typo fixing per WP:HYPHEN, sub-subsection 3, points 3,4,5, replaced: highly- → highly , partially- → partially (3), moderately- → moderately using AWB (7940) |
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Solubility is commonly expressed as a concentration, either by mass (g of solute per kg of solvent, [[mass concentration|g per dL (100mL) of solvent]], [[molarity]], [[molality]], [[mole fraction]], or other similar descriptions of [[concentration]]. The maximum equilibrium amount of solute that can dissolve per amount of solvent is the solubility of that solute in that solvent under the specified conditions. The advantage of expressing solubility in this manner is its simplicity, while the disadvantage is that it can strongly depend on the presence of other species in the solvent (for example, the common ion effect).
[[Solubility constant]]s are used to describe Racquel cool ha ha saturated solutions of ionic compounds <!--not only ionic cmpds--> of relatively low solubility (see [[solubility equilibrium]]). The solubility constant is a special case of an [[equilibrium constant]]. It describes the balance between dissolved ions from the salt and undissolved salt. The solubility constant is also "applicable" (i.e., useful) to [[precipitation (chemistry)|precipitation]], the reverse of the dissolving reaction. As with other equilibrium constants, [[temperature]] can affect the numerical value of solubility constant. The solubility constant is not as simple as solubility, however the value of this constant is generally independent of the presence of other species in the solvent.
The [[Flory-Huggins solution theory]] is a theoretical model describing the solubility of polymers. The [[Hansen Solubility Parameters]] and the [[Hildebrand solubility parameter]]s are empirical methods for the prediction of solubility. It is also possible to predict solubility from other physical constants such as the [[enthalpy of fusion]].
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