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==Production==
==Production==
Potassium pyrosulfate is obtained by the thermal decomposition of other salts, most directly from [[potassium bisulfate]]:<ref>{{cite book|last1=Washington Wiley|first1=Harvey|title=Principles and Practice of Agricultural Analysis: Fertilizers|date=1895|publisher=Chemical Publishing Co.|location=Easton, PA.|page=[https://archive.org/details/principlesandpr03wilegoog/page/n232 218]|url=https://archive.org/details/principlesandpr03wilegoog|quote=Potassium disulfate.|accessdate=31 December 2015}}</ref>
Potassium pyrosulfate is obtained by the thermal decomposition of other salts, most directly from [[potassium bisulfate]]:<ref>{{cite book|last1=Washington Wiley|first1=Harvey|title=Principles and Practice of Agricultural Analysis: Fertilizers|date=1895|publisher=Chemical Publishing Co.|location=Easton, PA.|page=[https://archive.org/details/principlesandpr03wilegoog/page/n232 218]|url=https://archive.org/details/principlesandpr03wilegoog|quote=Potassium disulfate.|access-date=31 December 2015}}</ref>
: 2 KHSO<sub>4</sub> → K<sub>2</sub>S<sub>2</sub>O<sub>7</sub> + H<sub>2</sub>O
: 2 KHSO<sub>4</sub> → K<sub>2</sub>S<sub>2</sub>O<sub>7</sub> + H<sub>2</sub>O
Temperatures above 600°C further decompose potassium pyrosulfate to [[potassium sulfate]] and [[sulfur trioxide]] however:<ref>{{cite book|last1=Iredelle Dillard Hinds|first1=John|title=Inorganic Chemistry: With the Elements of Physical and Theoretical Chemistry|date=1908|publisher=John Wiley & Sons.|location=New York|page=[https://archive.org/details/inorganicchemist00hinduoft/page/547 547]|url=https://archive.org/details/inorganicchemist00hinduoft|quote=Potassium disulfate.|accessdate=31 December 2015}}</ref>
Temperatures above 600°C further decompose potassium pyrosulfate to [[potassium sulfate]] and [[sulfur trioxide]] however:<ref>{{cite book|last1=Iredelle Dillard Hinds|first1=John|title=Inorganic Chemistry: With the Elements of Physical and Theoretical Chemistry|date=1908|publisher=John Wiley & Sons.|location=New York|page=[https://archive.org/details/inorganicchemist00hinduoft/page/547 547]|url=https://archive.org/details/inorganicchemist00hinduoft|quote=Potassium disulfate.|access-date=31 December 2015}}</ref>
: K<sub>2</sub>S<sub>2</sub>O<sub>7</sub> → K<sub>2</sub>SO<sub>4</sub> + SO<sub>3</sub>
: K<sub>2</sub>S<sub>2</sub>O<sub>7</sub> → K<sub>2</sub>SO<sub>4</sub> + SO<sub>3</sub>


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Potassium pyrosulfate is used in [[analytical chemistry]]; samples are fused with potassium pyrosulfate, (or a mixture of potassium pyrosulfate and [[potassium fluoride]]) to ensure complete dissolution prior to a [[Quantitative analysis (chemistry)|quantitative analysis]].<ref>{{cite journal |title=Determination of quartz (free silica) in refractory clays |last=Trostbl |first=L. J. |last2=Wynne |first2=D. J. |journal=Journal of the American Ceramic Society |volume=23 |issue=1 |pages=18–22 |year=1940 |doi=10.1111/j.1151-2916.1940.tb14187.x }}</ref><ref>{{cite journal |title=Determination of gross alpha, plutonium, neptunium, and/or uranium by gross alpha counting on barium sulphate |first=C. W. |last=Sill |journal=Analytical Chemistry |year=1980 |volume=52 |issue=9 |pages=1452–1459 |doi=10.1021/ac50059a018 }}</ref>
Potassium pyrosulfate is used in [[analytical chemistry]]; samples are fused with potassium pyrosulfate, (or a mixture of potassium pyrosulfate and [[potassium fluoride]]) to ensure complete dissolution prior to a [[Quantitative analysis (chemistry)|quantitative analysis]].<ref>{{cite journal |title=Determination of quartz (free silica) in refractory clays |last=Trostbl |first=L. J. |last2=Wynne |first2=D. J. |journal=Journal of the American Ceramic Society |volume=23 |issue=1 |pages=18–22 |year=1940 |doi=10.1111/j.1151-2916.1940.tb14187.x }}</ref><ref>{{cite journal |title=Determination of gross alpha, plutonium, neptunium, and/or uranium by gross alpha counting on barium sulphate |first=C. W. |last=Sill |journal=Analytical Chemistry |year=1980 |volume=52 |issue=9 |pages=1452–1459 |doi=10.1021/ac50059a018 }}</ref>


The compound is also present in a [[catalyst]] in conjunction with [[vanadium(V) oxide]] in the industrial production of sulfur trioxide.<ref>{{cite web|last1=Burkhardt|first1=Donald|year=1965|title=Sulfur trioxide production, US3362786A|url=https://patents.google.com/patent/US3362786A/en|website=Google Patents|accessdate=31 December 2015}}</ref>
The compound is also present in a [[catalyst]] in conjunction with [[vanadium(V) oxide]] in the industrial production of sulfur trioxide.<ref>{{cite web|last1=Burkhardt|first1=Donald|year=1965|title=Sulfur trioxide production, US3362786A|url=https://patents.google.com/patent/US3362786A/en|website=Google Patents|access-date=31 December 2015}}</ref>


==See also==
==See also==

Revision as of 07:03, 1 February 2021

Potassium pyrosulfate
Names
IUPAC name
dipotassium (sulfonatooxy)sulfonate
Other names
Potassium pyrosulphate; potassium disulfate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.288 Edit this at Wikidata
EC Number
  • 232-216-8
UNII
  • InChI=1S/2K.H2O7S2/c;;1-8(2,3)7-9(4,5)6/h;;(H,1,2,3)(H,4,5,6)/q2*+1;/p-2 ☒N
    Key: KAQHZJVQFBJKCK-UHFFFAOYSA-L ☒N
  • InChI=1/2K.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: KAQHZJVQFBJKCK-NUQVWONBAQ
  • [O-]S(=O)(=O)OS(=O)(=O)[O-].[K+].[K+]
Properties
K2O7S2
Molar mass 254.31 g·mol−1
Density 2.28 g/cm3
Melting point 325 °C (617 °F; 598 K)
soluble
Hazards
GHS labelling:
GHS05: CorrosiveGHS06: Toxic
Danger
H314, H331
P260, P261, P264, P271, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P311, P321, P363, P403+P233, P405, P501
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Potassium pyrosulfate, or potassium disulfate, is an inorganic compound with the chemical formula K2S2O7.

Production

Potassium pyrosulfate is obtained by the thermal decomposition of other salts, most directly from potassium bisulfate:[1]

2 KHSO4 → K2S2O7 + H2O

Temperatures above 600°C further decompose potassium pyrosulfate to potassium sulfate and sulfur trioxide however:[2]

K2S2O7 → K2SO4 + SO3

Other salts, such as potassium trisulfate,[3] can also decompose into potassium pyrosulfate.

Chemical structure

Potassium pyrosulfate contains the pyrosulfate anion which has a dichromate like structure. The geometry can be visualized as a tetrahedron with two corners sharing the SO4 anion's configuration and a centrally bridged oxygen atom.[4] A semi-structural formula for the pyrosulfate anion is O3SOSO32−. The oxidation state of sulfur in this compound is +6.

Uses

Potassium pyrosulfate is used in analytical chemistry; samples are fused with potassium pyrosulfate, (or a mixture of potassium pyrosulfate and potassium fluoride) to ensure complete dissolution prior to a quantitative analysis.[5][6]

The compound is also present in a catalyst in conjunction with vanadium(V) oxide in the industrial production of sulfur trioxide.[7]

See also

References

  1. ^ Washington Wiley, Harvey (1895). Principles and Practice of Agricultural Analysis: Fertilizers. Easton, PA.: Chemical Publishing Co. p. 218. Retrieved 31 December 2015. Potassium disulfate.
  2. ^ Iredelle Dillard Hinds, John (1908). Inorganic Chemistry: With the Elements of Physical and Theoretical Chemistry. New York: John Wiley & Sons. p. 547. Retrieved 31 December 2015. Potassium disulfate.
  3. ^ Brauer, Georg (1963). Handbook of Preparative Inorganic Chemistry Vol. 2, 2nd Ed. New York: Academic Press. p. 1716. ISBN 9780323161299.
  4. ^ Ståhl, K.; Balic-Zunic, T.; da Silva, F.; Eriksen, K. M.; Berg, R. W.; Fehrmann, R. (2005). "The crystal structure determination and refinements of K2S2O7, KNaS2O7 and Na2S2O7 from X-ray powder and single crystal diffraction data". Journal of Solid State Chemistry. 178 (5): 1697–1704. Bibcode:2005JSSCh.178.1697S. doi:10.1016/j.jssc.2005.03.022.
  5. ^ Trostbl, L. J.; Wynne, D. J. (1940). "Determination of quartz (free silica) in refractory clays". Journal of the American Ceramic Society. 23 (1): 18–22. doi:10.1111/j.1151-2916.1940.tb14187.x.
  6. ^ Sill, C. W. (1980). "Determination of gross alpha, plutonium, neptunium, and/or uranium by gross alpha counting on barium sulphate". Analytical Chemistry. 52 (9): 1452–1459. doi:10.1021/ac50059a018.
  7. ^ Burkhardt, Donald (1965). "Sulfur trioxide production, US3362786A". Google Patents. Retrieved 31 December 2015.
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