World Library  
Flag as Inappropriate
Email this Article

Potassium nitrate

 

Potassium nitrate

Potassium nitrate[1]
Potassium nitrate
Identifiers
CAS number  YesY
PubChem
ChemSpider  YesY
UNII  YesY
EC number
UN number 1486
KEGG  YesY
ChEMBL  N
RTECS number TT3700000
Jmol-3D images Image 1
Properties
Molecular formula KNO3
Molar mass 101.1032 g/mol
Appearance white solid
Odor odorless
Density 2.109 g/cm3 (16 °C)
Melting point 334 °C
Boiling point decomposes at 400 °C
Solubility in water 133 g/L (0 °C)
316 g/L (20 °C)
2460 g/L (100 °C)[2]
Solubility slightly soluble in ethanol
soluble in glycerol, ammonia
Basicity (pKb) 15.3[3]
Refractive index (nD) 1.5056
Structure
Crystal structure Orthorhombic, Aragonite
Thermochemistry
Specific
heat capacity
C
95.06 J/mol K
Std enthalpy of
formation
ΔfHo298
-494.00 kJ/mol
Hazards
MSDS External MSDS
EU Index Not listed
EU classification Oxidant (O)
R-phrases R8 R22 R36 R37 R38
S-phrases S7 S16 S17 S26 S36 S41
Main hazards Oxidant, Harmful if swallowed, Inhaled, or absorbed on skin. Causes Irritation to Skin and Eye area.
NFPA 704
0
1
0
OX
Flash point Non-flammable
LD50 3750 mg/kg (oral, rat)[4]
Related compounds
Other anions Potassium nitrite
Other cations Lithium nitrate
Sodium nitrate
Rubidium nitrate
Caesium nitrate
Related compounds Potassium sulfate
Potassium chloride
Supplementary data page
Structure and
properties
n, εr, etc.
Thermodynamic
data
Phase behaviour
Solid, liquid, gas
Spectral data UV, IR, NMR, MS
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 N   YesY/N?)

Potassium nitrate is a chemical compound with the chemical formula KNO3. It is an ionic salt of potassium ions K+ and nitrate ions NO3.

It occurs as a mineral niter and is a natural solid source of nitrogen. Potassium nitrate is one of several nitrogen-containing compounds collectively referred to as saltpeter or saltpetre.

Major uses of potassium nitrate are in fertilizers, rocket propellants and fireworks. It is one of the major constituents of gunpowder (blackpowder) and has been used since the Middle Ages as a food preservative.

Contents

  • Etymology 1
  • Properties 2
  • History of production 3
    • From mineral sources 3.1
    • From caves 3.2
    • LeConte 3.3
      • French method 3.3.1
      • Swiss method 3.3.2
    • From nitric acid 3.4
  • Production 4
  • Uses 5
    • Nitric acid production 5.1
    • Oxidizer 5.2
    • Food preservation 5.3
    • Food preparation 5.4
    • Fertilizer 5.5
    • Pharmacology 5.6
    • Other uses 5.7
  • In folklore and popular culture 6
  • See also 7
  • References 8
  • Bibliography 9
  • External links 10

Etymology

Potassium nitrate, due to its early and global use and production, has many names.

The Greeks used the term nitron, which was latinised to nitrum or nitrium. The earlier Hebrew and Egyptian both use words with the consonants n-t-r, which leads some to speculate that the latin term is closer to the original than the greek. Middle english styled it nitre. Old French has niter. By the 15th century Europeans referred to it as saltpeter[5] and later as nitrate of potash as the chemistry of the compound was more fully understood.

The Arabs called it "Chinese snow" Arabic: ثلج الصينthalj al-ṣīn. It was called "Chinese salt" by the Iranians/Persians[6][7][8][9][10] or "salt from Chinese salt marshes" (namak shūra chīnī Persian: نمک شوره چيني‎)[11][12]

Properties

Potassium nitrate has an orthorhombic crystal structure at room temperature, which transforms to a trigonal system at 129 °C. Upon heating to temperatures between 550 and 790 °C under an oxygen atmosphere, it loses oxygen and reaches a temperature dependent equilibrium with potassium nitrite:[13]

2 KNO3 → 2 KNO2 + O2

Potassium nitrate is moderately soluble in water, but its solubility increases with temperature (see infobox). The aqueous solution is almost neutral, exhibiting pH 6.2 at 14 °C for a 10% solution of commercial powder. It is not very hygroscopic, absorbing about 0.03% water in 80% relative humidity over 50 days. It is insoluble in alcohol and is not poisonous; it can react explosively with reducing agents, but it is not explosive on its own.[2]

History of production

From mineral sources

The earliest known complete purification process for potassium nitrate was outlined in 1270 by the chemist and engineer Hasan al-Rammah of Syria in his book al-Furusiyya wa al-Manasib al-Harbiyya (The Book of Military Horsemanship and Ingenious War Devices). In this book, al-Rammah describes first the purification of barud (crude saltpetre mineral) by boiling it with minimal water and using only the hot solution, then the use of potassium carbonate (in the form of wood ashes) to remove calcium and magnesium by precipitation of their carbonates from this solution, leaving a solution of purified potassium nitrate, which could then be dried.[14] This was used for the manufacture of gunpowder and explosive devices. The terminology used by al-Rammah indicated a Chinese origin for the gunpowder weapons about which he wrote.[15]

At least as far back as 1845, Chilean Saltpeter deposits were exploited in Chile and California, USA.

From caves

A major natural source of potassium nitrate was the deposits crystallizing from cave walls and the accumulations of bat guano in caves.[16] Extraction is accomplished by immersing the guano in water for a day, filtering, and harvesting the crystals in the filtered water. Traditionally, guano was the source used in Laos for the manufacture of gunpowder for Bang Fai rockets.

LeConte

Perhaps the most exhaustive discussion of the production of this material is the 1862 LeConte text.[17] He was writing with the express purpose of increasing production in the Confederate States to support their needs during the American Civil War. Since he was calling for the assistance of rural farming communities, the descriptions and instructions are both simple and explicit. He details the "French Method", along with several variations, as well as a "Swiss method". N.B. Many references have been made to a method using only straw and urine, but there is no such method in this work.

French method

Niter-beds are prepared by mixing straw to give porosity to a compost pile typically 1.5×2×5 meters in size.[17] The heap was usually under a cover from the rain, kept moist with urine, turned often to accelerate the decomposition, then finally leached with water after approximately one year, to remove the soluble calcium nitrate which was then converted to potassium nitrate by filtering through the potash.

Swiss method

LeConte describes a process using only urine and not dung, referring to it as the Swiss method. Urine is collected directly, in a sandpit under a stable. The sand itself is dug out and leached for nitrates which were then converted to potassium nitrate via potash, as above.

From nitric acid

From 1903 until the World War I era, potassium nitrate for black powder and fertilizer was produced on an industrial scale from nitric acid produced via the Birkeland–Eyde process, which used an electric arc to oxidize nitrogen from the air. During World War I the newly industrialized Haber process (1913) was combined with the Ostwald process after 1915, allowing Germany to produce nitric acid for the war after being cut off from its supplies of mineral sodium nitrates from Chile (see nitratite).

Production

Potassium nitrate can be made by combining ammonium nitrate and potassium hydroxide.

NH4NO3 (aq) + KOH (aq) → NH3 (g) + KNO3 (aq) + H2O (l)

An alternative way of producing potassium nitrate without a by-product of ammonia is to combine ammonium nitrate and potassium chloride, easily obtained as a sodium-free salt substitute.

NH4NO3 (aq) + KCl (aq) → NH4Cl (aq) + KNO3 (aq)

Potassium nitrate can also be produced by neutralizing nitric acid with potassium hydroxide. This reaction is highly exothermic.

KOH (aq) + HNO3 → KNO3 (aq) + H2O (l)

On industrial scale it is prepared by the double displacement reaction between sodium nitrate and potassium chloride.

NaNO3 (aq) + KCl (aq) → NaCl (aq) + KNO3 (aq)

Uses

Potassium nitrate has a wide variety of uses, largely as a source of nitrate.

Nitric acid production

Historically, nitric acid was produced by combining sulfuric acid with nitrates such as saltpeter. In modern times this is reversed: nitrates are produced from nitric acid produced via the Ostwald process.

Oxidizer

The most famous use of potassium nitrate is probably as the oxidizer in blackpowder. From the most ancient times through the late 1880s, blackpowder provided the explosive power for all the world's firearms. After that time, small arms and large artillery increasingly began to depend on cordite, a smokeless powder. Blackpowder remains in use today in black powder rocket motors, but also in combination with other fuels like sugars in "rocket candy". It is also used in fireworks such as smoke bombs, made with a mixture of sucrose and potassium nitrate.[18] It is also added to cigarettes to maintain an even burn of the tobacco[19] and is used to ensure complete combustion of paper cartridges for cap and ball revolvers.[20]

Food preservation

In the process of food preservation, potassium nitrate has been a common ingredient of salted meat since the Middle Ages,[21] but its use has been mostly discontinued due to inconsistent results compared to more modern nitrate and nitrite compounds. Even so, saltpeter is still used in some food applications, such as charcuterie and the brine used to make corned beef.[22] When used as a food additive in the European Union,[23] the compound is referred to as E252; it is also approved for use as a food additive in the USA[24] and Australia and New Zealand[25] (where it is listed under its INS number 252).[2]

Food preparation

In West African cuisine, potassium nitrate (salt petre) is widely used as a thickening agent in soups and stews such as Okra soup[26] and Isi ewu. It is also used to soften food and reduce cooking time when boiling beans and tough meat. Salt petre is also an essential ingredient in making special porridges such as kunun kanwa[27] literally translated from the Hausa language as 'salt petre porridge'.

Fertilizer

Potassium nitrate is used in fertilizers as a source of nitrogen and potassium – two of the macronutrients for plants. When used by itself, it has an NPK rating of 13-0-44.

Pharmacology

  • Used in some toothpastes for sensitive teeth.[28] Recently, the use of potassium nitrate in toothpastes for treating sensitive teeth has increased and it may be an effective treatment.[29][30]
  • Used historically to treat asthma.[31] Used in some toothpastes to relieve asthma symptoms.[32]
  • Used in Thailand as main ingredient in Kidney Tablets to relieve the symptoms of cystitis, pyelitis and urethritis.[33]
  • Combats high blood pressure and was once used as a hypotensive.[34]

Other uses

In folklore and popular culture

Potassium nitrate was once thought to induce impotence, and is still falsely rumored to be in institutional food (such as military fare) as an anaphrodisiac; however, there is no scientific evidence for such properties.[41][42]

See also

References

  1. ^ Potassium nitrateRecord of in the GESTIS Substance Database from the IFA, accessed on 2007-03-09
  2. ^ a b c B. J. Kosanke, B. Sturman, K. Kosanke, I. von Maltitz, T. Shimizu, M. A. Wilson, N. Kubota, C. Jennings-White, D. Chapman (2004). "2". Pyrotechnic Chemistry. Journal of Pyrotechnics. pp. 5–6.  
  3. ^ Kolthoff, Treatise on Analytical Chemistry, New York, Interscience Encyclopedia, Inc., 1959.
  4. ^ http://chem.sis.nlm.nih.gov/chemidplus/rn/7757-79-1
  5. ^ Spencer, Dan (2013). Saltpeter:The Mother of Gunpowder. Oxford, UK: Oxford University Press. p. 256.  
  6. ^ Peter Watson (2006). Ideas: A History of Thought and Invention, from Fire to Freud. HarperCollins. p. 304.  
  7. ^ Cathal J. Nolan (2006). The age of wars of religion, 1000–1650: an encyclopedia of global warfare and civilization. Volume 1 of Greenwood encyclopedias of modern world wars. Greenwood Publishing Group. p. 365.  
  8. ^ Oliver Frederick Gillilan Hogg (1970). Artillery: its origin, heyday, and decline. Archon Books. p. 123. The Chinese were certainly acquainted with saltpetre, the essential ingredient of gunpowder. They called it Chinese Snow and employed it early in the Christian era in the manufacture of fireworks and rockets. 
  9. ^ Oliver Frederick Gillilan Hogg (1963). English artillery, 1326–1716: being the history of artillery in this country prior to the formation of the Royal Regiment of Artillery. Royal Artillery Institution. p. 42. The Chinese were certainly acquainted with saltpetre, the essential ingredient of gunpowder. They called it Chinese Snow and employed it early in the Christian era in the manufacture of fireworks and rockets. 
  10. ^ Oliver Frederick Gillilan Hogg (1993). Clubs to cannon: warfare and weapons before the introduction of gunpowder (reprint ed.). Barnes & Noble Books. p. 216.  
  11. ^ Partington, J. R. (1960). A History of Greek Fire and Gunpowder (illustrated, reprint ed.). JHU Press. p. 335.  
  12. ^ Needham, Joseph; Yu, Ping-Yu (1980). Needham, Joseph, ed. Science and Civilisation in China: Volume 5, Chemistry and Chemical Technology, Part 4, Spagyrical Discovery and Invention: Apparatus, Theories and Gifts. Volume 5 (Issue 4 of Science and Civilisation in China). Contributors Joseph Needham, Lu Gwei-Djen, Nathan Sivin (illustrated, reprint ed.). Cambridge University Press. p. 194.  
  13. ^ Eli S. Freeman (1957). "The Kinetics of the Thermal Decomposition of Potassium Nitrate and of the Reaction between Potassium Nitrite and Oxygen". J. Am. Chem. Soc. 79 (4): 838–842.  
  14. ^ Ahmad Y Hassan, Potassium Nitrate in Arabic and Latin Sources, History of Science and Technology in Islam.
  15. ^ Jack Kelly (2005). Gunpowder: Alchemy, Bombards, and Pyrotechnics: The History of the Explosive that Changed the World. Basic Books. p. 22.  
  16. ^ Major George Rains (1861). Notes on Making Saltpetre from the Earth of the Caves. New Orleans, LA: Daily Delta Job Office. p. 14. Retrieved September 13, 2012. 
  17. ^ a b Joseph LeConte (1862). Instructions for the Manufacture of Saltpeter. Columbia, S.C.: South Carolina Military Department. p. 14. Retrieved 2007-10-19. 
  18. ^ Amthyst Galleries, Inc. Galleries.com. Retrieved on 2012-03-07.
  19. ^ Inorganic Additives for the Improvement of Tobacco, TobaccoDocuments.org
  20. ^ Kirst, W.J. (1983). Self Consuming Paper Cartridges for the Percussion Revolver. Minneapolis, Minnesota: Northwest Development Co. 
  21. ^ "Meat Science", University of Wisconsin. uwex.edu.
  22. ^ Corned Beef, Food Network
  23. ^ UK Food Standards Agency: "Current EU approved additives and their E Numbers". Retrieved 2011-10-27. 
  24. ^ US Food and Drug Administration: "Listing of Food Additives Status Part II". Retrieved 2011-10-27. 
  25. ^ Australia New Zealand Food Standards Code"Standard 1.2.4 – Labelling of ingredients". Retrieved 2011-10-27. 
  26. ^ "Cook Clean Site Ghanaian Recipe". CookClean Ghana. 
  27. ^ Marcellina Ulunma Okehie-Offoha (1996). Ethnic & cultural diversity in Nigeria. Trenton, N.J.: Africa World Press. 
  28. ^ "Sensodyne Toothpaste for Sensitive Teeth". 2008-08-03. Retrieved 2008-08-03. 
  29. ^ Enomoto, K et al. (2003). "The Effect of Potassium Nitrate and Silica Dentifrice in the Surface of Dentin". Japanese Journal of Conservative Dentistry 46 (2): 240–247. 
  30. ^ R. Orchardson and D. G. Gillam (2006). "Managing dentin hypersensitivity". Journal of the American Dental Association (1939) 137 (7): 990–8; quiz 1028–9.  
  31. ^ Orville Harry Brown (1917). Asthma, presenting an exposition of the nonpassive expiration theory. C.V. Mosby company. p. 277. 
  32. ^ Joe Graedon (May 15, 2010). Sensitive' toothpaste may help asthma"'". The Chicago Tribune. Retrieved June 18, 2012. 
  33. ^ LOCAL MANUFACTURED DRUG REGISTRATION FOR HUMAN (COMBINE). fda.moph.go.th
  34. ^ Reichert ET. (1880). "On the physiological action of potassium nitrite". Am. J. Med. Sci. 80: 158–180. 
  35. ^ Adam Chattaway; Robert G. Dunster; Ralf Gall; David J. Spring. "THE EVALUATION OF NON-PYROTECHNICALLY GENERATED AEROSOLS AS FIRE SUPPRESSANTS". United States National Institute of Standards and Technology ( 
  36. ^ Stan Roark (February 27, 2008). "Stump Removal for Homeowners".  
  37. ^ David E. Turcotte; Frances E. Lockwood (May 8, 2001). "Aqueous corrosion inhibitor Note. This patent cites potassium nitrate as a minor constituent in a complex mix. Since rust is an oxidation product, this statement requires justification.". United States Patent. 6,228,283. 
  38. ^ Elizabeth March (June 2008). "The Scientist, the Patent and the Mangoes – Tripling the Mango Yield in the Philippines". WIPO Magazine. United Nations World Intellectual Property Organization ( 
  39. ^ "Filipino scientist garners 2011 Dioscoro L. Umali Award". Southeast Asian Regional Center for Graduate Study and Research in Agriculture ( 
  40. ^ Juan Ignacio Burgaleta; Santiago Arias; Diego Ramirez. "Gemasolar, The First Tower Thermosolar Commercial Plant With Molten Salt Storage System" (Press Release).  
  41. ^ "The Straight Dope: Does saltpeter suppress male ardor?". 1989-06-16. Retrieved 2007-10-19. 
  42. ^ Richard E. Jones and Kristin H. López (2006). Human Reproductive Biology, Third Edition.  

Bibliography

  • Dennis W. Barnum. (2003). "Some History of Nitrates." Journal of Chemical Education. v. 80, p. 1393-. link.
  • David Cressy. Saltpeter: The Mother of Gunpowder (Oxford University Press, 2013) 237 pp online review by Robert Tiegs
  • Alan Williams. "The production of saltpeter in the Middle Ages", Ambix, 22 (1975), pp. 125–33. Maney Publishing, ISSN 0002-6980.

External links

  • International Chemical Safety Card 018402216
Salts and the ester of the Nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)4- RONO2 NO3-
NH4NO3
O FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)3 Co(NO3)2,
Co(NO3)3
Ni(NO3)2 Cu(NO3)2 Zn(NO3)2 Ga(NO3)3 Ge As Se Br Kr
RbNO3 Sr(NO3)2 Y Zr(NO3)4 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb Te I XeFNO3
CsNO3 Ba(NO3)2   Hf Ta W Re Os Ir Pt Au Hg2(NO3)2,
Hg(NO3)2
Tl(NO3)3 Pb(NO3)2 Bi(NO3)3 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv Uus Uuo
La Ce(NO3)x Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2(NO3)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr
This article was sourced from Creative Commons Attribution-ShareAlike License; additional terms may apply. World Heritage Encyclopedia content is assembled from numerous content providers, Open Access Publishing, and in compliance with The Fair Access to Science and Technology Research Act (FASTR), Wikimedia Foundation, Inc., Public Library of Science, The Encyclopedia of Life, Open Book Publishers (OBP), PubMed, U.S. National Library of Medicine, National Center for Biotechnology Information, U.S. National Library of Medicine, National Institutes of Health (NIH), U.S. Department of Health & Human Services, and USA.gov, which sources content from all federal, state, local, tribal, and territorial government publication portals (.gov, .mil, .edu). Funding for USA.gov and content contributors is made possible from the U.S. Congress, E-Government Act of 2002.
 
Crowd sourced content that is contributed to World Heritage Encyclopedia is peer reviewed and edited by our editorial staff to ensure quality scholarly research articles.
 
By using this site, you agree to the Terms of Use and Privacy Policy. World Heritage Encyclopedia™ is a registered trademark of the World Public Library Association, a non-profit organization.
 



Copyright © World Library Foundation. All rights reserved. eBooks from World eBook Library are sponsored by the World Library Foundation,
a 501c(4) Member's Support Non-Profit Organization, and is NOT affiliated with any governmental agency or department.