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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): 2 HClO 2 → HClO + HClO 3
The chlorate must be dissolved in boiling water and the acid should be somewhat diluted in water and heated before mixing. Another method which can be used to produce solutions up to 10% concentration is by the use of cation exchange resins and a soluble salt such as NaClO 3, where the Na+ cation will exchange with H+. [2]
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 −.
Standard protective group approaches, such as the use of t-BOC, are a viable solution to these problems. [12] Thioethers are also highly susceptible to oxidation. For example, Pinnick oxidation of thioanisaldehyde gives a high yield of carboxylic acid products, but with concomitant conversion of the thioether to the sulfoxide or sulfone. [7]
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 ...
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.
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.
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.