Ammonium hypophosphite

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Ammonium hypophosphite
Names
IUPAC name
Ammonium hypophosphite
Other names
Ammonium phosphenite
Ammonium phosphinate
Properties
NH6PO2
NH4PH2O2
Molar mass 83.0269 g/mol
Appearance White hygroscopic solid
Odor Odorless
Density 1.634 g/cm3 (20 °C)[1]
Melting point 200–240 °C (392–464 °F; 473–513 K) (decomposition)[5]
Boiling point Decomposes
83 g/100 ml (20 °C)[2][3]
Solubility Slightly soluble in alcohols
Insoluble in acetone, pyridine, toluene
Solubility in ethanol 6.3 g/100 ml (25 °C)[4]
Vapor pressure ~0 mmHg
Hazards
Safety data sheet Sigma-Aldrich
Related compounds
Related compounds
Sodium hypophosphite
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Ammonium hypophoshpite is an inorganic chemical compound, used as a reducing agent. It has the formula NH4PH2O2.

Properties

Chemical

Ammonium hypophosphite decomposes when heated above 240 °C to yield ammonia and phosphine.[6]

Physical

Ammonium hypophoshpite is a hygroscopic colorless crystalline solid, soluble in water, and slightly less soluble in alcohols.

Availability

It is sometimes sold by chemical suppliers.

Preparation

Ammonium hypophosphite can be easily prepared by neutralizing a solution of hypophosphorous acid (ca. 50%) with a conc. aq. solution of ammonia.[7]

NH3 + HPH2O2 → NH4PH2O2

Another route involves addition of white phosphorus to a conc. aq. solution of ammonia:[8]

P4 + NH3 + H2O → NH4PH2O2 + PH3

Phosphine is generated as side product.

Another way ammonium hypophosphite can be produced is by adding an aq. solution of ammonium sulfate to barium hypophosphite. The insoluble barium sulfate precipitates out of the reaction, while the ammonium hypophosphite is recystallized from the solution.

Ba(PH2O2)2 + (NH4)2SO4 → 2 NH4PH2O2 + BaSO4

Projects

  • Reducing agent
  • Prepare other hypophosphites

Handling

Safety

Like with all hypophosphites, ammonium hypophosphite can decompose to release the toxic phosphine gas. It is also a strong reducing agent, and may explode when mixed with chlorates.

Storage

In airtight closed plastic bottles, away from oxidizers and moisture.

Disposal

Like all hypophosphites, it can be neutralized using a solution of hydrogen peroxide, which converts it into ammonium phosphate.

References

  1. Zachariasen, W. H.; Mooney, R. L.; Journal of Chemical Physics; vol. 2; (1934); p. 34
  2. Solubility Handbook - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961
  3. Aliev, Vahid; Dolinina, Raissa; Gadjiev, Sardar; Comptes rendus de l'Academie des sciences. Serie II, Mecanique, physique, chimie, sciences de l'univers, sciences de la terre; vol. 310; (1990); p. 1191 - 1194
  4. Dean J.A. Lange's handbook of chemistry. - 1999 pp. 3.16
  5. Wurtz, A.; Annales de Chimie et de Physique; vol. 16; (1846); p. 193
  6. Rammelsberg, c.; Journal of the Chemical Society; vol. 26; (1873); p. 4
  7. Yoshida, Yusuke; Inoue, Katsuya; Kyritsakas, Natalie; Kurmoo, Mohamedally; Inorganica Chimica Acta; vol. 362; nb. 5; (2009); p. 1428 - 1434
  8. Stock, A.; Chemische Berichte; vol. 36; (1903); p. 1120 - 1123

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