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Chlorous acid is an inorganic compound with the formula HClO 2.It is a weak acid.Chlorine has oxidation state +3 in this acid. The pure substance is unstable, disproportionating to hypochlorous acid (Cl oxidation state +1) and chloric acid (Cl oxidation state +5):
The free acid, chlorous acid HClO 2, is the least stable oxoacid of chlorine and has only been observed as an aqueous solution at low concentrations. Since it cannot be concentrated, it is not a commercial product.
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 −.
Acid strength is the tendency of an acid, symbolised by the chemical formula, to dissociate into a proton, +, and an anion, .The dissociation or ionization of a strong acid in solution is effectively complete, except in its most concentrated solutions.
Chlorine acid can refer to: ... Chlorous acid, HClO 2; Chloric acid, HClO 3; Perchloric acid, HClO 4; Gallery. Chlorine acids. Molecular structure of hydrochloric acid.
This is an accepted version of this page This is the latest accepted revision, reviewed on 29 September 2024. Not to be confused with sodium chloride. Sodium chlorite The sodium cation Space-filling model of the chlorite anion Names IUPAC name Sodium chlorite Other names Chlorous acid, sodium salt Textone Identifiers CAS Number 7758-19-2 Y 49658-21-1 (trihydrate) Y 3D model (JSmol) Interactive ...
Chlorous acid (HOClO) is even more unstable and cannot be isolated or concentrated without decomposition: it is known from the decomposition of aqueous chlorine dioxide. However, sodium chlorite is a stable salt and is useful for bleaching and stripping textiles, as an oxidising agent, and as a source of chlorine dioxide.
Chlorine dioxide reacts rapidly with H 2 O 2 to form chlorous acid. 2ClO 2 + H 2 O 2 → 2HClO 2 + O 2. Also the formation of oxygen gives good indication of the progress of the reaction. However, problems sometimes arise due to the formation of singlet oxygen in this reaction, which may oxidize organic materials (i.e. the Schenck ene reaction).