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Hypophosphoric acid can be prepared by the reaction of red phosphorus with sodium chlorite at room temperature. [2]2 P + 2 NaClO 2 + 2 H 2 O → Na 2 H 2 P 2 O 6 + 2 HCl. A mixture of hypophosphoric acid, phosphorous acid (H 3 PO 3) and phosphoric acid (H 3 PO 4) is produced when white phosphorus oxidises in air when partially immersed in water.
A general formula for such cyclic compounds is [HPO 3] x where x = number of phosphoric units in the molecule. When metaphosphoric acids lose their hydrogens as H +, cyclic anions called metaphosphates are formed. An example of a compound with such an anion is sodium hexametaphosphate (Na 6 P 6 O 18), used as a sequestrant and a food additive.
The name "orthophosphoric acid" can be used to distinguish this specific acid from other "phosphoric acids", such as pyrophosphoric acid. Nevertheless, the term "phosphoric acid" often means this specific compound; and that is the current IUPAC nomenclature .
Other important organic compounds that contain oxygen are: glycerol, formaldehyde, glutaraldehyde, citric acid, acetic anhydride, acetamide, etc. Epoxides are ethers in which the oxygen atom is part of a ring of three atoms. Oxygen reacts spontaneously with many organic compounds at or below room temperature in a process called autoxidation. [7]
In chemistry, phosphorus oxoacid (or phosphorus acid) is a generic name for any acid whose molecule consists of atoms of phosphorus, oxygen, and hydrogen. [1] There is a potentially infinite number of such compounds. Some of them are unstable and have not been isolated, but the derived anions and organic groups are present in stable salts and ...
The phosphate ion has a molar mass of 94.97 g/mol, and consists of a central phosphorus atom surrounded by four oxygen atoms in a tetrahedral arrangement. It is the conjugate base of the hydrogen phosphate ion H(PO 4) 2−, which in turn is the conjugate base of the dihydrogen phosphate ion H 2 (PO 4) −
Phosphorous acid (or phosphonic acid) is the compound described by the formula H 3 PO 3. This acid is diprotic (readily ionizes two protons), not triprotic as might be suggested by this formula. Phosphorous acid is an intermediate in the preparation of other phosphorus compounds.
The compound is a triprotic acid with acid dissociation constants pK a1 = 1.1, pK a2 = 5.5 and pK a3 = 12.8. In aqueous solutions it slowly undergoes hydrolysis to hydrogen peroxide and phosphoric acid. [7] H 3 PO 5 + H 2 O → H 3 PO 4 + H 2 O 2. With excess water, the hydrolysis can be considered pseudo-first order.