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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.[5][6]
See also
Pyrosulfate
Potassium bisulfate
Potassium pyrosulfate
References
Olsen, J. C., ed. (1934). Van Nostrand's Chemical Annual. London: Chapman and Hall.
Heinz K. Hofmeister; John R. Van Wazer (1962). "Hydrolysis of Sodium Pyrosulfate". Inorganic Chemistry. ACS. 1 (4): 811–812. doi:10.1021/ic50004a019.
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.[5][6]
See also
Pyrosulfate
Potassium bisulfate
Potassium pyrosulfate
References
Olsen, J. C., ed. (1934). Van Nostrand's Chemical Annual. London: Chapman and Hall.
Heinz K. Hofmeister; John R. Van Wazer (1962). "Hydrolysis of Sodium Pyrosulfate". Inorganic Chemistry. ACS. 1 (4): 811–812. doi:10.1021/ic50004a019.
