Editing Sodium chloride (section)

===Aqueous solutions===
[[File:WatNaCl.png|thumb|right|upright=1.15|Phase diagram of water–NaCl mixture]]
The attraction between the Na<sup>+</sup> and Cl<sup>−</sup> ions in the solid is so strong that only highly [[polar solvent]]s like water dissolve NaCl well.

When dissolved in water, the sodium chloride framework disintegrates as the Na<sup>+</sup> and Cl<sup>−</sup> ions become surrounded by polar water molecules. These solutions consist of [[metal aquo complex]] with the formula [Na(H<sub>2</sub>O)<sub>8</sub>]<sup>+</sup>, with the Na–O distance of 250&nbsp;[[picometer|pm]]. The chloride ions are also strongly solvated, each being surrounded by an average of six molecules of water.<ref name="Lincoln">Lincoln, S. F.; Richens, D. T. and Sykes, A. G. (2003) "Metal Aqua Ions" Comprehensive Coordination Chemistry II Volume 1, pp. 515–555. {{doi|10.1016/B0-08-043748-6/01055-0}}.</ref> Solutions of sodium chloride have very different properties from pure water. The [[eutectic point]] is {{convert|−21.12|C|F}} for 23.31% [[mass fraction (chemistry)#Mass percentage|mass fraction]] of salt, and the boiling point of saturated salt solution is near {{convert|108.7|C|F}}.<ref name="u1">Elvers, B. ''et al.'' (ed.) (1991) ''Ullmann's Encyclopedia of Industrial Chemistry'', 5th ed. Vol. A24, Wiley, p. 319, {{ISBN|978-3-527-20124-2}}.</ref>