Ammonium heptamolybdate
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| Names | |
|---|---|
| IUPAC name
Ammonium docosaoxoheptamolybdate(6–) | |
| Other names
Ammonium molybdate Ammonium paramolybdate (see text) | |
| Identifiers | |
12027-67-7  12054-85-2 (tetrahydrate) | |
| ChemSpider | 23786 |
| EC number | 234-320-9 |
| |
| Jmol-3D images | Image |
| PubChem | 71306766 |
| |
| UNII | 21Y68J178E |
| Properties | |
| (NH4)6Mo7O24 | |
| Molar mass | 1163.9 g/mol 1235.86 g/mol (tetrahydrate) |
| Appearance | white to yellow-green crystalline solid |
| Density | 2.498 g/cm3 |
| Melting point | ~90 ˚C (loses water molecule) 190 °C (decomp.) |
| 43 g/100 ml (tetrahydrate) | |
| Hazards | |
| MSDS | External MSDS |
| Main hazards | Irritant |
| EU Index | Not listed |
| NFPA 704 | |
| Flash point | Non-flammable |
| Related compounds | |
| Other anions |
Ammonium orthomolybdate Ammonium dimolybdate |
| Other cations |
Potassium paramolybdate |
| Related compounds |
Molybdenum(VI) oxide Molybdic acid |
| Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
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| Infobox references | |
Ammonium heptamolybdate is an odourless crystalline compound ranging in colour from white to yellow-green. It is usually encountered as the tetrahydrate, whose chemical formula is (NH4)6Mo7O24·4H2O. It is often referred to as ammonium paramolybdate or simply as ammonium molybdate, although ammonium molybdate can also refer to ammonium orthomolybdate, (NH4)2MoO4, and several other compounds.
Synthesis
Ammonium heptamolybdate is easily prepared by dissolving molybdenum trioxide in an excess of aqueous ammonia and evaporating the solution at room temperature. While the solution evaporates, the excess of ammonia escapes. This method results in the formation of six-sided transparent prisms of the tetrahydrate of ammonium heptamolybdate.[1]
Solutions of ammonium paramolybdate react with acids to form molybdic acid and an ammonium salt. The pH value of a concentrated solution will lie between 5 and 6.
Uses
- as an analytical reagent to measure the amount of phosphates, silicates, arsenates and lead in aqueous solution (e.g. pigments, river water, sea water etc.)[2]
- in the production of molybdenum metal and ceramics
- in the preparation of dehydrogenation and desulphurisation catalysts
- in the fixing of metals
- in electroplating
- in fertilizers for crops.
- as a negative stain in biological electron microscopy, typically in the 3–5% (vol/vol) concentration range and in the presence of trehalose;[3] or at saturated concentration to perform cryo-negative staining.[4][5]
Safety
Ammonium paramolybdate is harmful if swallowed or inhaled. It causes irritation to the eyes, skin, and respiratory tract. It affects kidneys and blood.
References
- ↑ L. Svanberg & H. Struve, J. pr. Ch. 44 [1848], p. 282; cited in Gmelin's Handbuch für Anorganische Chemie, 53, p. 255.
- ↑ Parsons, T.; Maita, V. & Lalli, C. (1984). A manual of chemical and biological methods for seawater analysis. Oxford: Pergamon.
- ↑ Harris, J. R. and Horne, R. W. 1991. "Negative staining", in Harris J. R. (Ed.), Electron Microscopy in Biology, Oxford University Press, Oxford.
- ↑ Adrian, M.; Dubochet, J.; Fuller, S. D. and Harris, J. R. 1998. "Cryo-negative Staining". Micron 29, p. 145–160; doi:10.1016/S0968-4328(97)00068-1.
- ↑ De Carlo, S.; El-Bez, C.; Alvarez-Rúa, C.; Borge, J. and Dubochet, J. 2002. "Cryo-negative staining reduces electron-beam sensitivity of vitrified biological particles". J. Struct. Biol. 138, p. 216–226; doi:10.1016/S1047-8477(02)00035-7; PMID 12217660.
See Also
Phosphate test aka Deniges' method links to here.