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Potassium carbonate

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Potassium carbonate
Names
IUPAC name
Potassium carbonate
Other names
Carbonate of potash, dipotassium carbonate, sub-carbonate of potash, pearl ash, potash, salt of tartar, salt of wormwood.
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.008.665 Edit this at Wikidata
E number E501(i) (acidity regulators, ...)
RTECS number
  • TS7750000
UNII
  • InChI=1S/CH2O3.2K/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2 checkY
    Key: BWHMMNNQKKPAPP-UHFFFAOYSA-L checkY
  • InChI=1/CH2O3.2K/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2
    Key: BWHMMNNQKKPAPP-NUQVWONBAS
  • C(=O)([O-])[O-].[K+].[K+]
Properties
K2CO3
Molar mass 138.205 g·mol−1
Appearance White, hygroscopic solid
Density 2.43 g/cm3
Melting point 891 °C (1,636 °F; 1,164 K)
Boiling point Decomposes
110.3 g/(100 mL) (20 °C)
149.2 g/(100 mL) (100 °C)
Solubility
Acidity (pKa) 10.25
−59.0·10−6 cm3/mol
Thermochemistry[1]
114.4 J/(mol·K)
155.5 J/(mol·K)
−1151.0 kJ/mol
−1063.5 kJ/mol
Enthalpy of fusion fHfus)
27.6 kJ/mol
Hazards
GHS labelling:
GHS07: Exclamation mark
Warning
H302, H315, H319, H335
P261, P305+P351+P338
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
1870 mg/kg (oral, rat)[2]
Safety data sheet (SDS) ICSC 1588
Related compounds
Other anions
Potassium bicarbonate
Other cations
Related compounds
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 carbonate is the inorganic compound with the formula K2CO3. It is a white salt, which is soluble in water and forms a strongly alkaline solution. It is deliquescent, often appearing as a damp or wet solid. Potassium carbonate is mainly used in the production of soap and glass.[3] Commonly, it can be found as the result of leakage of alkaline batteries.[4] Potassium carbonate is a potassium salt of carbonic acid. This salt consists of potassium cations K+ and carbonate anions CO2−3, and is therefore an alkali metal carbonate.

History

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Potassium carbonate is the primary component of potash and the more refined pearl ash or salts of tartar. Historically, pearl ash was created by baking potash in a kiln to remove impurities. The fine, white powder remaining was the pearl ash. The first patent issued by the US Patent Office was awarded to Samuel Hopkins in 1790 for an improved method of making potash and pearl ash.[5]

In late 18th-century North America, before the development of baking powder, pearl ash was used as a leavening agent for quick breads.[6][7]

Production

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The modern commercial production of potassium carbonate is by reaction of potassium hydroxide with carbon dioxide:[3]

2 KOH + CO2 → K2CO3 + H2O

From the solution crystallizes the sesquihydrate K2CO3·1.5H2O ("potash hydrate"). Heating this solid above 200 °C (392 °F) gives the anhydrous salt. In an alternative method, potassium chloride is treated with carbon dioxide in the presence of an organic amine to give potassium bicarbonate, which is then calcined:

2 KHCO3 → K2CO3 + H2O + CO2

Applications

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References

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  1. ^ CRC handbook of chemistry and physics: a ready-reference book of chemical and physical data. William M. Haynes, David R. Lide, Thomas J. Bruno (2016-2017, 97th ed.). Boca Raton, Florida. 2016. ISBN 978-1-4987-5428-6. OCLC 930681942.{{cite book}}: CS1 maint: location missing publisher (link) CS1 maint: others (link)
  2. ^ Chambers, Michael. "ChemIDplus - 584-08-7 - BWHMMNNQKKPAPP-UHFFFAOYSA-L - Potassium carbonate [USP] - Similar structures search, synonyms, formulas, resource links, and other chemical information". chem.sis.nlm.nih.gov. Archived from the original on 2014-08-12.
  3. ^ a b H. Schultz; G. Bauer; E. Schachl; F. Hagedorn; P. Schmittinger (2005). "Potassium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a22_039. ISBN 3-527-30673-0.
  4. ^ List, Jenny (October 19, 2022). "Crusty Leaking Cells Kill Your Tech. Just What's Going On?". Hackaday. Archived from the original on May 30, 2023.
  5. ^ "Milestones in U.S. patenting". www.uspto.gov. Archived from the original on 2023-03-22. Retrieved 2023-08-04.
  6. ^ See references to "pearl ash" in "American Cookery" by Amelia Simmons, printed by Hudson & Goodwin, Hartford, 1796.
  7. ^ Civitello, Linda (2017). Baking powder wars: the cutthroat food fight that revolutionized cooking. Urbana, Illinois: University of Illinois Press. pp. 18–22. ISBN 978-0-252-04108-2.
  8. ^ Zakiah, K.; Maulana, M. R.; Widowati, L. R.; Mutakin, J. (2021). "Applications of guano and K2CO3 on soil potential-P, potential-K on Andisols". IOP Conference Series: Earth and Environmental Science. 648: 012185. doi:10.1088/1755-1315/648/1/012185.
  9. ^ "Office of Dietary Supplements - Potassium". Archived from the original on 2022-08-11. Retrieved 2024-12-18.
  10. ^ "Potassium Carbonate: What is it and where is it used?". Archived from the original on 2024-07-17. Retrieved 2024-12-18.
  11. ^ Leonard, J.; Lygo, B.; Procter, G. "Advanced Practical Organic Chemistry" 1998, Stanley Thomas Publishers Ltd
  12. ^ Lydia M. Child (1832). The American Frugal Housewife.

Bibliography

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