Chemistry:Potassium carbonate
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| Names | |
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| IUPAC name
Potassium carbonate
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| Other names
Carbonate of potash, dipotassium carbonate, sub-carbonate of potash, pearl ash, potash, salt of tartar, salt of wormwood.
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| Identifiers | |
3D model (JSmol)
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PubChem CID
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| Properties | |
| K2CO3 | |
| Molar mass | 138.205 g/mol |
| 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] | |
Heat capacity (C)
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114.4 J·mol−1·K−1 |
Std molar
entropy (S |
155.5 J·mol−1·K−1 |
Std enthalpy of
formation (ΔfH⦵298) |
−1151.0 kJ·mol−1 |
Gibbs free energy (ΔfG˚)
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−1063.5 kJ·mol−1 |
Enthalpy of fusion (ΔfH⦵fus)
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27.6 kJ·mol−1 |
| Hazards | |
| Safety data sheet | ICSC 1588 |
| GHS pictograms | 
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| GHS Signal word | Warning |
| H302, H315, H319, H335 | |
| P261, P305+351+338 | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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1870 mg/kg (oral, rat)[2] |
| Related compounds | |
Other anions
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Potassium bicarbonate |
Other cations
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Lithium carbonate Sodium carbonate Rubidium carbonate Caesium carbonate |
Related compounds
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Ammonium carbonate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
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]
History
Potassium carbonate is the primary component of potash and the more refined pearl ash or salts of tartar. 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][6]
In late 18th-century North America, before the development of baking powder, pearl ash was used as a leavening agent for quick breads.[7][8]
Production
Potassium lye (which in this case can alternatively be called potash), a substance which contains potassium carbonate, potassium bicarbonate, and potassium hydroxide,[9][10] was historically produced by dissolving the lye found in the wooden ashes inside of water for at least 24 hours, disposing of the undissolved ashes, and then drying/evaporating the remaining liquid.[9][11]
With modern observation, this process would produce greater yields if done with the ashes of banana peels due to their increased amounts of potassium carbonate.[11]
As previously mentioned, Samuel Hopkins created an improved method of making pearl ash. One of those procedures was putting the lye/potash in a kiln to remove impurities.
Potassium carbonate is today, prepared commercially, by the reaction of potassium hydroxide with carbon dioxide:[3]
- 2 KOH + CO2 → K2CO3 + H2O
From the solution crystallizes the sequestrate K2CO3·3⁄2H2O ("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
- (historically) for soap, glass, and dishware production
- as a mild drying agent where other drying agents, such as calcium chloride and magnesium sulfate, may be incompatible. It is not suitable for acidic compounds, but can be useful for drying an organic phase if one has a small amount of acidic impurity. It may also be used to dry some ketones, alcohols, and amines prior to distillation.[12]
- in cuisine, where it has many traditional uses. It is used in some types of Chinese noodles and mooncakes, as well as Asian grass jelly and Japanese ramen. German gingerbread recipes often use potassium carbonate as a baking agent, although in combination with hartshorn.
- in the alkalization of cocoa powder to produce Dutch process chocolate by balancing the pH (i.e., reduce the acidity) of natural cocoa beans; it also enhances aroma. The process of adding potassium carbonate to cocoa powder is usually called "Dutching" (and the products referred to as Dutch-processed cocoa powder), as the process was first developed in 1828 by Dutchman Coenraad Johannes van Houten.
- as a buffering agent in the production of mead or wine.
- in antique documents, it is reported to have been used to soften hard water.[13]
- as a fire suppressant in extinguishing deep-fat fryers and various other B class-related fires.
- in condensed aerosol fire suppression, although as the byproduct of potassium nitrate.
- as an ingredient in welding fluxes, and in the flux coating on arc-welding rods.
- as an animal feed ingredient to satisfy the potassium requirements of farmed animals such as broiler breeder chickens.
- as an acidity regulator in Swedish snus snuff tobacco
References
- ↑ 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.
- ↑ Chambers, Michael. "ChemIDplus - 584-08-7 - BWHMMNNQKKPAPP-UHFFFAOYSA-L - Potassium carbonate [USP - Similar structures search, synonyms, formulas, resource links, and other chemical information."]. https://chem.nlm.nih.gov/chemidplus/rn/584-08-7.
- ↑ 3.0 3.1 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.
- ↑ List, Jenny (October 19, 2022). "Crusty Leaking Cells Kill Your Tech. Just What's Going On?". https://hackaday.com/2022/10/19/crusty-leaking-cells-kill-your-tech-just-whats-going-on/.
- ↑ "Milestones in U.S. patenting" (in en-US). https://www.uspto.gov/patents/milestones.
- ↑ "Samuel Hopkins (inventor)" (in en), Wikipedia, 2023-04-09, https://en.wikipedia.org/w/index.php?title=Samuel_Hopkins_(inventor)&oldid=1149042067, retrieved 2023-08-04
- ↑ See references to "pearl ash" in "American Cookery" by Amelia Simmons, printed by Hudson & Goodwin, Hartford, 1796.
- ↑ 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.
- ↑ 9.0 9.1 "Potassium carbonate - Sciencemadness Wiki". https://www.sciencemadness.org/smwiki/index.php?title=Potassium_carbonate&oldid=14431#Preperation.
- ↑ "Lye" (in en), Wikipedia, 2023-08-08, https://en.wikipedia.org/w/index.php?title=Lye&oldid=1169383280, retrieved 2023-09-08
- ↑ 11.0 11.1 Smith, Jess (24 April 2017). "How to Make Potassium Carbonate". https://sciencing.com/make-potassium-carbonate-7480553.html.
- ↑ Leonard, J.; Lygo, B.; Procter, G. "Advanced Practical Organic Chemistry" 1998, Stanley Thomas Publishers Ltd
- ↑ Child, Lydia M. "The American Frugal Housewife" 1832
Bibliography
- A Dictionary of Science, Oxford University Press, New York, 2004
- Yu. Platonov, Andrew; Evdokimov, Andrey; Kurzin, Alexander; D. Maiyorova, Helen (29 June 2002). "Solubility of Potassium Carbonate and Potassium Hydrocarbonate in Methanol". Journal of Chemical & Engineering Data 47 (5): 1175–1176. doi:10.1021/je020012v. https://www.researchgate.net/publication/231535294.
External links
| H2CO3 | He | ||||||||||||||||
| Li2CO3, LiHCO3 |
BeCO3 | B | C | (NH4)2CO3, NH4HCO3 |
O | F | Ne | ||||||||||
| Na2CO3, NaHCO3, Na3H(CO3)2 |
MgCO3, Mg(HCO3)2 |
Al2(CO3)3 | Si | P | S | Cl | Ar | ||||||||||
| K2CO3, KHCO3 |
CaCO3, Ca(HCO3)2 |
Sc | Ti | V | Cr | MnCO3 | FeCO3 | CoCO3 | NiCO3 | CuCO3 | ZnCO3 | Ga | Ge | As | Se | Br | Kr |
| Rb2CO3 | SrCO3 | Y | Zr | Nb | Mo | Tc | Ru | Rh | Pd | Ag2CO3 | CdCO3 | In | Sn | Sb | Te | I | Xe |
| Cs2CO3, CsHCO3 |
BaCO3 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg | Tl2CO3 | PbCO3 | (BiO)2CO3 | Po | At | Rn | |
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | |||||||||||||||||
| La2(CO3)3 | Ce2(CO3)3 | Pr | Nd | Pm | Sm | Eu | Gd | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac | Th | Pa | UO2CO3 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||
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