Sodium pyrosulfate
 | |
| Names | |
|---|---|
| IUPAC name
Disodium disulfate | |
| Other names
Sodium pyrosulphate; Disulfuric acid disodium salt. | |
| Identifiers | |
13870-29-6  | |
| 3D model (Jmol) | Interactive image |
| ChEMBL | ChEMBL111016  |
| ECHA InfoCard | 100.034.190 |
| |
| Properties | |
| Na2S2O7 | |
| Molar mass | 222.12 g/mol |
| Appearance | Translucent white crystals |
| Density | 2.658 g/cm3 |
| Melting point | 400.9 °C (753.6 °F; 674.0 K) |
| Boiling point | decomposes at 460 °C (860 °F; 733 K) |
| Soluble | |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| verify (what is ?) | |
| Infobox references | |
Sodium pyrosulfate, or Disodium disulfate, is an inorganic compound with the chemical formula is Na2S2O7.[1]
Preparation
Sodium pyrosulfate is obtained by the dehydration of sodium bisulfate:[2]
- 2 NaHSO4 → Na2S2O7 + H2O
Temperatures above 460 °C further decompose the compound, producing sodium sulfate and sulfur trioxide:
- Na2S2O7 → Na2SO4 + SO3
Applications
Sodium pyrosulfate is used in analytical chemistry; samples are fused with sodium pyrosulfate to ensure complete dissolution prior to a quantitative analysis.[3][4]
See also
References
- 1 2 Olsen, J. C., ed. (1934). Van Nostrand's Chemical Annual. London: Chapman and Hall.
- ↑ Noyes, William (1913). A Textbook of Chemistry. New York: Henry Holt and Company. p. 186. Retrieved 13 January 2016.
- ↑ Nemodruk, Aleksandr; Karalova, Zinaida (1969). Analytical chemistry of boron: Analytical chemistry of the elements. Charlottesville, VA: Ann Arbor-Humphrey Science Publishers. pp. 23 & 193. ISBN 9780250399192.
- ↑ Kiely, P. V.; Jackson, M. L. (1965). "Quartz, Feldspar, and Mica Determination for Soils by Sodium Pyrosulfate Fusion". Soil Science Society of America Journal. 29 (2): 159–163. doi:10.2136/sssaj1965.03615995002900020015x.
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