Difference between revisions of "Ammonium hypophosphite"
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==Preparation== | ==Preparation== | ||
| − | Ammonium hypophosphite can be easily prepared by neutralizing a solution of [[hypophosphorous acid]] ( | + | Ammonium hypophosphite can be easily prepared by neutralizing a solution of [[hypophosphorous acid]] (ca. 50%) with a conc. aq. solution of [[ammonia]].<ref>Yoshida, Yusuke; Inoue, Katsuya; Kyritsakas, Natalie; Kurmoo, Mohamedally; Inorganica Chimica Acta; vol. 362; nb. 5; (2009); p. 1428 - 1434</ref> |
: NH<sub>3</sub> + HPH<sub>2</sub>O<sub>2</sub> → NH<sub>4</sub>PH<sub>2</sub>O<sub>2</sub> | : NH<sub>3</sub> + HPH<sub>2</sub>O<sub>2</sub> → NH<sub>4</sub>PH<sub>2</sub>O<sub>2</sub> | ||
Revision as of 23:25, 13 November 2021
| 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.
Contents
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
- ↑ Zachariasen, W. H.; Mooney, R. L.; Journal of Chemical Physics; vol. 2; (1934); p. 34
- ↑ Solubility Handbook - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961
- ↑ 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
- ↑ Dean J.A. Lange's handbook of chemistry. - 1999 pp. 3.16
- ↑ Wurtz, A.; Annales de Chimie et de Physique; vol. 16; (1846); p. 193
- ↑ Rammelsberg, c.; Journal of the Chemical Society; vol. 26; (1873); p. 4
- ↑ Yoshida, Yusuke; Inoue, Katsuya; Kyritsakas, Natalie; Kurmoo, Mohamedally; Inorganica Chimica Acta; vol. 362; nb. 5; (2009); p. 1428 - 1434
- ↑ Stock, A.; Chemische Berichte; vol. 36; (1903); p. 1120 - 1123
