Sodium pyrosulfate

Sodium pyrosulfate is a topic that has captured the attention of many people in recent years. With its impact on society and culture, it has generated numerous debates and conflicting opinions. From its origins to the current moment, Sodium pyrosulfate has been the subject of study and research, and continues to be a point of interest for academics, experts and the general public. In this article we will explore different aspects related to Sodium pyrosulfate, analyzing its influence, its challenges and its opportunities.

Sodium pyrosulfate^[1]

Names
IUPAC name Disodium disulfate
Other names Sodium pyrosulphate; Disulfuric acid disodium salt, disodium disulfate; Sodium metabisulfate
Identifiers
CAS Number	13870-29-6 Y
3D model (JSmol)	Interactive image
ChEMBL	ChEMBL111016 Y
ChemSpider	7970254
ECHA InfoCard	100.034.190
EC Number	237-625-5
PubChem CID	9794487
CompTox Dashboard (EPA)	DTXSID60889631
InChI InChI=1S/2Na.H2O7S2/c;;1-8(2,3)7-9(4,5)6/h;;(H,1,2,3)(H,4,5,6)/q2*+1;/p-2 Key: JXAZAUKOWVKTLO-UHFFFAOYSA-L
SMILES ..S(=O)(=O)OS(=O)(=O)
Properties
Chemical formula	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)
Solubility in water	hydrolyses[2]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). N verify (what is YN ?) Infobox references

Chemical compound

Sodium pyrosulfate is an inorganic compound with the chemical formula of Na₂S₂O₇.^[1] It is a colorless salt.^[3] It hydrolyses in water to form sodium bisulfate with a chemical formula of NaHSO₄ which has a pH of around 1.

Preparation

Sodium pyrosulfate is obtained by heating sodium bisulfate to 280 °C (536 °F) ^[4][5]

2 NaHSO₄ → Na₂S₂O₇ + H₂O

Temperatures above 460 °C further decompose the compound, producing sodium sulfate and sulfur trioxide:

Na₂S₂O₇ → Na₂SO₄ + SO₃

Applications

Sodium pyrosulfate was used in analytical chemistry. Samples are fused with sodium pyrosulfate to ensure complete dissolution before a quantitative analysis.^[6][7]

See also

• Pyrosulfate
• Potassium bisulfate
• Potassium pyrosulfate

References

1. ^ ^{a b} Olsen, J. C., ed. (1934). Van Nostrand's Chemical Annual. London: Chapman and Hall.
2. ^ Heinz K. Hofmeister; John R. Van Wazer (1962). "Hydrolysis of Sodium Pyrosulfate". Inorganic Chemistry. 1 (4). ACS: 811–812. doi:10.1021/ic50004a019.
3. ^ Helmold Plessen (2000). "Sodium Sulfates". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a24_355. ISBN 978-3527306732.
4. ^ Noyes, William (1913). A Textbook of Chemistry. New York: Henry Holt and Company. p. 186. Retrieved 13 January 2016.
5. ^ von Plessen, Helmold (2000). "Sodium Sulfates". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a24_355. ISBN 9783527303854.
6. ^ 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.
7. ^ 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. Bibcode:1965SSASJ..29..159K. doi:10.2136/sssaj1965.03615995002900020015x.