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Physical properties of hydrochloric acid, such as boiling and melting points, density, and pH, depend on the concentration or molarity of HCl in the aqueous solution. They range from those of water at very low concentrations approaching 0% HCl to values for fuming hydrochloric acid at over 40% HCl.
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In part because of its high polarity, HCl is very soluble in water (and in other polar solvents). Upon contact, H 2 O and HCl combine to form hydronium cations [H 3 O] + and chloride anions Cl − through a reversible chemical reaction: HCl + H 2 O → [H 3 O] + + Cl −. The resulting solution is called hydrochloric acid and is a strong acid.
Trends in melting points can be even better explained when the structure and ionic size ratio is taken into account. [62] Above their melting point, salts melt and become molten salts (although some salts such as aluminium chloride and iron(III) chloride show molecule-like structures in the liquid phase). [ 63 ]
Hypochlorous acid is an inorganic compound with the chemical formula Cl O H, also written as HClO, HOCl, or ClHO. [2] [3] Its structure is H−O−Cl.It is an acid that forms when chlorine dissolves in water, and itself partially dissociates, forming a hypochlorite anion, ClO −.
In chemistry, a hydrochloride is an acid salt resulting, or regarded as resulting, from the reaction of hydrochloric acid with an organic base (e.g. an amine). An alternative name is chlorhydrate, which comes from French. An archaic alternative name is muriate, derived from hydrochloric acid's ancient name: muriatic acid.
It can also be produced by the addition of hydrochloric acid to a hot, concentrated solution of mercury(I) compounds such as the nitrate: [2] Hg 2 (NO 3) 2 + 4 HCl → 2 HgCl 2 + 2 H 2 O + 2 NO 2. Heating a mixture of solid mercury(II) sulfate and sodium chloride also affords volatile HgCl 2, which can be separated by sublimation. [2]
An electrolyte in a solution may be described as "concentrated" if it has a high concentration of ions, or "dilute" if it has a low concentration. If a high proportion of the solute dissociates to form free ions, the electrolyte is strong; if most of the solute does not dissociate, the electrolyte is weak.