Potassium bicarbonate: Difference between revisions
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a light edit of the entire article with expansion - research indicating this is a salt-free substitute for sodium bicarbonate that is being studied for use with autoimmune diseases - data re potassium bicarbonate is at the end of the second source, but both sources might be used better for the reference |
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'''Potassium bicarbonate''' (also known as '''potassium hydrogen carbonate''' or '''potassium acid carbonate''') is the [[inorganic compound]] with the chemical formula KHCO<sub>3</sub>. It is a white solid.<ref name=Ullmann>{{cite encyclopedia|authors=H. Schultz, G. Bauer, E. Schachl, F. Hagedorn, P. Schmittinger|title=Potassium Compounds|encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry|year=2005|publisher=Wiley-VCH|location=Weinheim|doi=10.1002/14356007.a22_039}}</ref> |
'''Potassium bicarbonate''' (also known as '''potassium hydrogen carbonate''' or '''potassium acid carbonate''') is the [[inorganic compound]] with the chemical formula KHCO<sub>3</sub>. It is a white solid.<ref name=Ullmann>{{cite encyclopedia|authors=H. Schultz, G. Bauer, E. Schachl, F. Hagedorn, P. Schmittinger|title=Potassium Compounds|encyclopedia=Ullmann's Encyclopedia of Industrial Chemistry|year=2005|publisher=Wiley-VCH|location=Weinheim|doi=10.1002/14356007.a22_039}}</ref> |
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[[File:Potassium bicarbonate purple-K.jpg|thumb|right|A fire extinguisher containing potassium bicarbonate |
[[File:Potassium bicarbonate purple-K.jpg|thumb|right|A fire extinguisher containing potassium bicarbonate]] |
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==Production and reactivity== |
==Production and reactivity== |
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This reaction is employed to prepare high purity potassium carbonate. |
This reaction is employed to prepare high purity potassium carbonate. |
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==Uses== |
==Uses== |
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This compound is a source of [[carbon dioxide]] for [[leavening]] in baking, extinguishing fire in dry chemical [[fire extinguisher]]s. |
This compound is a source of [[carbon dioxide]] for [[leavening]] in baking, and for extinguishing fire in dry chemical [[fire extinguisher]]s. |
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===Acidity regulator=== |
===Acidity regulator=== |
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As an inexpensive, nontoxic base, it is widely used in diverse application to [[acidity regulator|regulate pH]] or as a [[reagent]]. |
As an inexpensive, nontoxic base, it is widely used in diverse application to [[acidity regulator|regulate pH]] or as a [[reagent]]. Examples include as [[buffering agent]] in medications, an additive in [[winemaking]]. |
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Potassium bicarbonate is often found added to [[club soda]] to improve taste,<ref>{{cite web | url = http://time.com/3029191/bottled-water-ingredients-nutrition-health/ | title = Why Your Bottled Water Contains Four Different Ingredients | publisher = Time Magazine}}</ref> to soften the effect of effervescence. |
Potassium bicarbonate is often found added to [[club soda]] to improve taste,<ref>{{cite web | url = http://time.com/3029191/bottled-water-ingredients-nutrition-health/ | title = Why Your Bottled Water Contains Four Different Ingredients | publisher = Time Magazine}}</ref> and to soften the effect of effervescence. |
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===Substitute for sodium bicarbonate=== |
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Research in which [[sodium bicarbonate]] is being studied for efficacy in treatment of autoimmune diseases such as rheumatoid arthritis,<ref>Boynew-Shuck, Ashley, ''[https://www.healthline.com/health-news/baking-soda-may-be-what-the-doctor-ordered-for-rheumatoid-arthritis?slot_pos=article_2&utm_source=Sailthru%20Email&utm_medium=Email&utm_campaign=rheumatoidarthritis&utm_content=2019-05-14&apid=26988450#1 Baking Soda May Be What the Doctor Ordered for Rheumatoid Arthritis]'', Healthline, April 29, 2019</ref> indicates that potassium bicarbonate is a useful alternative, being a salt-free substitute for sodium bicarbonate,<ref>Hand, Julie, ''[https://blog.bulletproof.com/baking-soda-combats-autoimmune-disease-study/ A Daily Dose of Baking Soda Can Treat Autoimmune Disease, Study Finds. Here’s How to Drink It]'', Bulletproof.com, accessed 2019.05.24 </ref> while providing the same beneficial results. Both compounds once were described as, ''saleratus'', which included either of the two. (see, History) |
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===Fire extinguishers=== |
===Fire extinguishers=== |
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==History== |
==History== |
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The word ''saleratus'', from [[Latin language|Latin]] ''sal æratus'' meaning "aerated salt", was widely used in the |
The word ''saleratus'', from [[Latin language|Latin]] ''sal æratus'' meaning "aerated salt", was widely used in the nineteenth century for both potassium bicarbonate and sodium bicarbonate. The term has now fallen out of common usage. |
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==References== |
==References== |
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Revision as of 01:07, 25 May 2019
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| Names | |
|---|---|
| IUPAC name
potassium hydrogen carbonate
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| Other names
potassium acid carbonate
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.005.509 |
| EC Number |
|
| E number | E501(ii) (acidity regulators, ...) |
PubChem CID
|
|
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| KHCO3 | |
| Molar mass | 100.115 g/mol |
| Appearance | white crystals |
| Odor | odorless |
| Density | 2.17 g/cm3 |
| Melting point | 292 °C (558 °F; 565 K) (decomposes) |
| 22.4 g/100 mL (20 °C)[1] | |
| Solubility | practically insoluble in alcohol |
| Acidity (pKa) | 10.329[2]
6.351 (carbonic acid)[2] |
| Thermochemistry | |
Std enthalpy of
formation (ΔfH⦵298) |
-963.2 kJ/mol |
| Pharmacology | |
| A12BA04 (WHO) | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-Flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
|
> 2000 mg/kg (rat, oral) |
| Safety data sheet (SDS) | MSDS |
| Related compounds | |
Other anions
|
Potassium carbonate |
Other cations
|
Sodium bicarbonate Ammonium bicarbonate |
Related compounds
|
Potassium bisulfate Potassium hydrogen phosphate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Potassium bicarbonate (also known as potassium hydrogen carbonate or potassium acid carbonate) is the inorganic compound with the chemical formula KHCO3. It is a white solid.[1]
Production and reactivity
It is manufactured by treating an aqueous solution of potassium carbonate with carbon dioxide:[1]
- K2CO3 + CO2 + H2O → 2 KHCO3
Decomposition of the bicarbonate occurs between 100 and 120 °C (212 and 248 °F):
- 2 KHCO3 → K2CO3 + CO2 + H2O
This reaction is employed to prepare high purity potassium carbonate.
Uses
This compound is a source of carbon dioxide for leavening in baking, and for extinguishing fire in dry chemical fire extinguishers.
Acidity regulator
As an inexpensive, nontoxic base, it is widely used in diverse application to regulate pH or as a reagent. Examples include as buffering agent in medications, an additive in winemaking.
Potassium bicarbonate is often found added to club soda to improve taste,[3] and to soften the effect of effervescence.
Substitute for sodium bicarbonate
Research in which sodium bicarbonate is being studied for efficacy in treatment of autoimmune diseases such as rheumatoid arthritis,[4] indicates that potassium bicarbonate is a useful alternative, being a salt-free substitute for sodium bicarbonate,[5] while providing the same beneficial results. Both compounds once were described as, saleratus, which included either of the two. (see, History)
Fire extinguishers
Potassium bicarbonate is used as a fire suppression agent ("BC dry chemical") in some dry chemical fire extinguishers, as the principal component of the Purple-K dry chemical, and in some applications of condensed aerosol fire suppression. It is the only dry chemical fire suppression agent recognized by the U.S. National Fire Protection Association for firefighting at airport crash rescue sites. It is about twice as effective in fire suppression as sodium bicarbonate.[6]
Agriculture
Potassium bicarbonate has widespread use in crops, especially for neutralizing acidic soil.[7]
Potassium bicarbonate is an effective fungicide against powdery mildew and apple scab, allowed for use in organic farming.[8][9][10][11]
History
The word saleratus, from Latin sal æratus meaning "aerated salt", was widely used in the nineteenth century for both potassium bicarbonate and sodium bicarbonate. The term has now fallen out of common usage.
References
- ^ a b c "Potassium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. 2005. doi:10.1002/14356007.a22_039.
{{cite encyclopedia}}: Unknown parameter|authors=ignored (help) - ^ a b Goldberg, Robert N.; Kishore, Nand; Lennen, Rebecca M. (2003). "Thermodynamic quantities for the ionization reactions of buffers in water". In David R. Lide (ed.). CRC handbook of chemistry and physics (84th ed.). Boca Raton, FL: CRC Press. pp. 7–13. ISBN 978-0-8493-0595-5. Retrieved 6 March 2011.
- ^ "Why Your Bottled Water Contains Four Different Ingredients". Time Magazine.
- ^ Boynew-Shuck, Ashley, Baking Soda May Be What the Doctor Ordered for Rheumatoid Arthritis, Healthline, April 29, 2019
- ^ Hand, Julie, A Daily Dose of Baking Soda Can Treat Autoimmune Disease, Study Finds. Here’s How to Drink It, Bulletproof.com, accessed 2019.05.24
- ^ "Purple-K-Powder". US Naval Research Laboratory. Retrieved 8 February 2012.
- ^ "Potassium Bicarbonate Handbook" (PDF). Armand Products Company.
- ^ "Use of Baking Soda as a Fungicide".
- ^ "Powdery Mildew - Sustainable Gardening Australia". Archived from the original on 2016-03-03.
{{cite web}}: Unknown parameter|deadurl=ignored (|url-status=suggested) (help) - ^ "Organic Fruit Production in Michigan".
- ^ "Efficacy of Armicarb (potassium bicarbonate) against scab and sooty blotch on apples" (PDF).
External links
- Potassium Bicarbonate Handbook
- OMRI Potassium Bicarbonate
- Safety Data sheet - potassium bicarbonate
- . New International Encyclopedia. 1905.
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