= Dissolution
<Dissolution> transfers material into a <chemical solution>. It can include separation from an <ionic crystal> and <solvation>, or dispersal of neutral <molecules>. For <sucrose> and <sodium chloride>, respectively,
$$
\mathrm{C}_{12}\mathrm{H}_{22}\mathrm{O}_{11}(s)\longrightarrow\mathrm{C}_{12}\mathrm{H}_{22}\mathrm{O}_{11}(aq),\qquad
\mathrm{NaCl}(s)\longrightarrow\mathrm{Na}^{+}(aq)+\mathrm{Cl}^{-}(aq).
$$
Here $(aq)$ specifies <water> as the <solvent>; it does not specify a fixed number of attached <water> <molecules>. The neutral <sucrose> remains molecular. <Dissociation of an ionic compound> separates pre-existing <ions> in the second example; <solvation> stabilizes their new surroundings.<Chemistry 2e by Paul Flowers and others/11.1 The Dissolution Process>[Chemistry 2e by Paul Flowers and others; Opening molecular and ionic dissolution examples]{ref}<Chemistry 2e by Paul Flowers and others/11.2 Electrolytes>[Chemistry 2e by Paul Flowers and others; “Ionic Electrolytes”]{ref}
<Ionization> instead creates <ions> from neutral species. <Hydrogen chloride> reacting with <water> illustrates <protonation> of <water> rather than mere rearrangement of a <hydration shell>:
$$
\mathrm{HCl}+\mathrm{H}_2\mathrm O\longrightarrow\mathrm{H}_3\mathrm O^{+}+\mathrm{Cl}^{-}.
$$
The <hydronium> and negative <ion> together preserve total <electric charge>. <Solvation> can influence this <chemical reaction>, but an <ion>'s <solvation> does not itself change its net <electric charge>.<Chemistry 2e by Paul Flowers and others/11.2 Electrolytes>[Chemistry 2e by Paul Flowers and others; “Covalent Electrolytes”, HCl proton-transfer example]{ref}
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