Phosphorous acid
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Phosphorous acid (or phosphonic acid) is the compound described by the formula Template:Chem2. It is diprotic (readily ionizes two protons), not triprotic as might be suggested by its formula. Phosphorous acid is an intermediate in the preparation of other phosphorus compounds. Organic derivatives of phosphorous acid, compounds with the formula Template:Chem2, are called phosphonic acids.
Nomenclature and tautomerism
Solid Template:Chem2 has tetrahedral geometry about the central phosphorus atom, with a Template:Chem2 bond of 132 pm, one Template:Chem2 double bond of 148 pm and two longer Template:Chem2 single bonds of 154 pm. In common with other phosphorus oxides with Template:Chem2 bonds (e.g.hypophosphorous acid and dialkyl phosphites),[1] it exists in equilibrium with an extremely minor tautomer Template:Chem2. (In contrast, arsenous acid's major tautomer is the trihydroxy form.) IUPAC recommends that the trihydroxy form Template:Chem2 be called phosphorous acid, and the dihydroxy form Template:Chem2 phosphonic acid.[2] Only the reduced phosphorus compounds are spelled with an "-ous" ending.
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Preparation
On an industrial scale, the acid is prepared by hydrolysis of phosphorus trichloride with water or steam:[4]
Template:Chem2 could be produced by the hydrolysis of phosphorus trioxide:
Reactions
Acid–base properties
Phosphorous acid has a pKa in the range 1.26–1.3.[5][6]
- Template:Chem2 pKa = 1.3
It is a diprotic acid, the hydrogenphosphite ion, Template:Chem2 is a weak acid:
- Template:Chem2 pKa = 6.7
The conjugate base Template:Chem2 is called hydrogen phosphite, and the second conjugate base, Template:Chem2, is the phosphite ion.[7] (Note that the IUPAC recommendations are hydrogen phosphonate and phosphonate respectively).
The hydrogen atom bonded directly to the phosphorus atom is not readily ionizable. Chemistry examinations often test students' appreciation of the fact that not all three hydrogen atoms are acidic under aqueous conditions, in contrast with Template:Chem2.
Redox properties
On heating at 200 °C, phosphorous acid disproportionates to phosphoric acid and phosphine:[8]
This reaction is used for laboratory-scale preparations of Template:Chem2.
Phosphorous acid slowly oxidizes in air to phosphoric acid.[4]
Both phosphorous acid and its deprotonated forms are good reducing agents, although not necessarily quick to react. They are oxidized to phosphoric acid or its salts. It reduces solutions of noble metal cations to the metals. When phosphorous acid is treated with a cold solution of mercuric chloride, a white precipitate of mercurous chloride forms:
Mercurous chloride is reduced further by phosphorous acid to mercury on heating or on standing:
As a ligand
Upon treatment with metals of d6 configuration, phosphorous acid is known to coordinate as the otherwise rare Template:Chem2 tautomer. Examples include Template:Chem2 and Template:Chem2.[9][10]
Heating a mixture of potassium tetrachloroplatinate and phosphorous acid gives the luminescent salt potassium diplatinum(II) tetrakispyrophosphite:[11]
Uses
The most important use of phosphorous acid (phosphonic acid) is the production of basic lead phosphite, which is a stabilizer in PVC and related chlorinated polymers.[4]
It is used in the production of basic lead phosphonate PVC stabilizer, aminomethylene phosphonic acid and hydroxyethane diphosphonic acid. It is also used as a strong reducing agent and in the production of synthetic fibres, organophosphorus pesticides, and the highly efficient water treatment agent ATMP.
Ferrous materials, including steel, may be somewhat protected by promoting oxidation ("rust") and then converting the oxidation to a metalophosphate by using phosphoric acid and further protected by surface coating. (See: Passivation (chemistry)).
Organic derivatives
The IUPAC (mostly organic) name is phosphonic acid. This nomenclature is commonly reserved for substituted derivatives, that is, organic group bonded to phosphorus, not simply an ester. For example, Template:Chem2 is "methylphosphonic acid", which may of course form "methylphosphonate" esters.
References
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- ↑ International Union of Pure and Applied Chemistry (2005). Nomenclature of Inorganic Chemistry (IUPAC Recommendations 2005). Cambridge (UK): RSC–IUPAC. Template:ISBN. Electronic version..
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- ↑ a b c Template:Ullmann.
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Further reading
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