Hypophosphorous acid

From Wikipedia, the free encyclopedia
Jump to: navigation, search
Hypophosphorous acid[1]
Wireframe model of hypophosphorous acid
IUPAC name
Phosphinic acid
Other names


Oxo-λ5-phosphinous acid
6303-21-5 YesY
57583-56-9 (2H3)
ChEBI CHEBI:29031 YesY
ChemSpider 10449263 YesY
10459437 (17O2) N
2342086 (2H3) N
Jmol-3D images Image
KEGG D02334 YesY
PubChem 3085127 (2H3)
UN number UN 3264
Molar mass 66.00 g/mol
Appearance colorless, deliquescent crystals or oily liquid
Density 1.493 g/cm3[2]
Melting point 26.5 °C (79.7 °F; 299.6 K)
Boiling point 130 °C (266 °F; 403 K) decomposes
Solubility very soluble in alcohol, ether
Acidity (pKa) 1.2
Molecular shape pseudo-tetrahedral
EU Index Not listed
Flash point Non-flammable
Related compounds
Phosphorous acid
Phosphoric acid
Related compounds
Sodium hypophosphite
Barium hypophosphite
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 YesY verify (what isYesY/N?)
Infobox references

Hypophosphorous acid is a phosphorus oxoacid and a powerful reducing agent with molecular formula H3PO2. Inorganic chemists refer to the free acid by this name (also as "HPA"), or the acceptable name of phosphinic acid. It is a colorless low-melting compound, which is soluble in water, dioxane, and alcohols. The formula for hypophosphorous acid is generally written H3PO2, but a more descriptive presentation is HOP(O)H2 which highlights its monoprotic character. Salts derived from this acid are called phosphinates (hypophosphites).

HOP(O)H2 exists in equilibrium with the minor tautomer HP(OH)2. Sometimes the minor tautomer is called hypophosphorous acid and the major tautomer is called phosphinic acid.

Preparation and availability[edit]

The acid is prepared industrially via a two step process. Hypophosphite salts of the alkali and alkaline earth metals result from treatment of white phosphorus with hot aqueous solution of the appropriate hydroxide, e.g. Ca(OH)2.

P4 + 3OH + 3H2O → 3H2PO2 + PH3

The free acid may be prepared by the action of a strong acid on these hypophosphite salts.

H2PO2 + H+ → H3PO2

Alternatively, H3PO2 arises by the oxidation of phosphine with iodine in water.

PH3 + 2I2 + 2H2O → H3PO2 + 4I + 4H+

HPA is usually supplied as a 50% aqueous solution.


Hypophosphorous acid is used in the formulation of pharmaceuticals, discoloration of polymers, water treatment, retrieval of precious or non-ferrous metals. Its main use is for electroless plating; i.e. deposition of select metal films from solution on a sensitized surface. In organic chemistry, H3PO2 best known for their use in the reduction of arenediazonium salts, converting ArN2+ to Ar-H.[3][4] When diazotized in a concentrated solution of hypophosphorous acid, an amine substituent can be removed from arenes, selectively over alkyl amines.

DEA List I chemical status[edit]

Because hypophosphorous acid can reduce elemental iodine to form hydroiodic acid, which is a reagent effective for reducing ephedrine or pseudoephedrine to methamphetamine,[5] the United States Drug Enforcement Administration designated hypophosphorous acid (and its salts) as a List I precursor chemical effective November 16, 2001.[6] Accordingly, handlers of hypophosphorous acid or its salts in the United States are subject to stringent regulatory controls including registration, recordkeeping, reporting, and import/export requirements pursuant to the Controlled Substances Act and 21 CFR §§ 1309 and 1310.[6][7][8]

Inorganic and organic derivatives[edit]

Numerous derivatives are known in which the two hydrogen atoms directly bound to phosphorus are replaced by organic groups. These derivatives are known as phosphinic acids, and their salts as phosphinates. For example, formaldehyde and H3PO2 react to give (HOCH2)2PO2H. The reaction is akin to the addition of thiols and HCN to aldehydes. Similarly, it adds to Michael acceptors, for example with acrylamide it gives H(HO)P(O)CH2CH2C(O)NH2.

Few metal complexes have been prepared from H3PO2, one example is Ni(O2PH2)2.


  • Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5 
  • ChemicalLand21 Listing
  • D. E. C. Corbridge "Phosphorus: An Outline of its Chemistry, Biochemistry, and Technology" 5th Edition Elsevier: Amsterdam. ISBN 0-444-89307-5.
  • V. V. Popik, A. G. Wright, T. A. Khan, J. A. Murphy "Hypophosphorous Acid" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. doi:10.1002/047084289.
  • D. W. Rich, M. C. Smith, Electroless Deposition of Nickel, Cobalt & Iron. IBM Corporation, Poughkeepsie, NY (1971)


  1. ^ Ralph H. Petrucci, General Chemistry, Ninth Edition, 2007, p. 946
  2. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  3. ^ Robison, M. M.; Robison, B. L. (1956). "2,4,6-Tribromobenzoic acid". Org. Synth. 36:94; Coll. Vol. 4:947.
  4. ^ Kornblum, N. (1941). "3,3'-Dimethoxybiphenyl and 3,3'-dimethylbiphenyl". Org. Synth. 21:30; Coll. Vol. 3:295.
  5. ^ Gordon, P.E.; Fry, A.J.; Hicks, L.D. Further studies on the reduction of benzylic alcohols by hypophosphorous acid/iodine. 23 August 2005. ARKIVOC 2005 (vi) 393-400. ISSN 1424-6376.
  6. ^ a b 66 FR 52670—52675. 17 October 2001.
  7. ^ 21 CFR 1309
  8. ^ 21 USC, Chapter 13 (Controlled Substances Act)