fbpx
Wikipedia

Potassium sulfate

November 28, 2023

Not to be confused with potassium sulfide.

Potassium sulfate (US) or potassium sulphate (UK), also called sulphate of potash (SOP), arcanite, or archaically potash of sulfur, is the inorganic compound with formula K2SO4, a white water-soluble solid. It is commonly used in fertilizers, providing both potassium and sulfur.

Potassium sulfate

Arcanite
Names
Other names
Potassium sulphate
Identifiers
  • 7778-80-5 Y
3D model (JSmol)
  • Interactive image
ChEBI
  • CHEBI:32036 Y
ChEMBL
  • ChEMBL2021424 Y
ChemSpider
  • 22915 Y
ECHA InfoCard 100.029.013
EC Number
  • 231-915-5
E number E515(i) (acidity regulators, ...)
KEGG
  • D01726 Y
  • 24507
RTECS number
  • TT5900000
UNII
  • 1K573LC5TV Y
  • DTXSID6029701
  • InChI=1S/2K.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2 Y
    Key: OTYBMLCTZGSZBG-UHFFFAOYSA-L Y
  • InChI=1/2K.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
    Key: OTYBMLCTZGSZBG-NUQVWONBAU
  • [K+].[K+].[O-]S([O-])(=O)=O
Properties
K2SO4
Molar mass 174.259 g/mol
Appearance White solid
Odor odorless
Density 2.66 g/cm3[1]
Melting point 1,069[2] °C (1,956 °F; 1,342 K)
Boiling point 1,689 °C (3,072 °F; 1,962 K)
111 g/L (20 °C)
120 g/L (25 °C)
240 g/L (100 °C)
1.32 (120 g/L)
Solubility slightly soluble in glycerol
insoluble in acetone, alcohol, CS2
−67.0·10−6 cm3/mol
1.495
Structure
orthorhombic
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Irritant
GHS labelling:
Warning
H318
P280, P305+P351+P338, P310
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
6600 mg/kg (oral, rat)[3]
Safety data sheet (SDS) External MSDS
Related compounds
Other anions
 Potassium selenate
Potassium tellurate
Other cations
 Lithium sulfate
Sodium sulfate
Rubidium sulfate
Caesium sulfate
Related compounds
 Potassium hydrogen sulfate
Potassium sulfite
Potassium bisulfite
Potassium persulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)

History edit

Potassium sulfate (K2SO4) has been known since early in the 14th century. It was studied by Glauber, Boyle, and Tachenius. In the 17th century, it was named arcanuni or sal duplicatum, as it was a combination of an acid salt with an alkaline salt. It was also known as vitriolic tartar and Glaser's salt or sal polychrestum Glaseri after the pharmaceutical chemist Christopher Glaser who prepared it and used medicinally.[4][5]

Known as arcanum duplicatum ("double secret") or panacea duplicata in pre-modern medicine, it was prepared from the residue (caput mortuum) left over from the production of aqua fortis (nitric acid, HNO3) from nitre (potassium nitrate, KNO3) and oil of vitriol (sulphuric acid, H2SO4) via Glauber's process:

2 KNO3 + H2SO4 → 2 HNO3 + K2SO4

The residue was dissolved in hot water, filtered, and evaporated to a cuticle. It was then left to crystallise. It was used as a diuretic and sudorific.[6]

According to Chambers's Cyclopedia, the recipe was purchased for five hundred thalers by Charles Frederick, Duke of Holstein-Gottorp. Schroder, the duke's physician, wrote wonders of its great uses in hypochondriacal cases, continued and intermitting fevers, stone, scurvy, and more.[6]

Natural resources edit

The mineral form of potassium sulfate, arcanite, is relatively rare. Natural resources of potassium sulfate are minerals abundant in the Stassfurt salt. These are cocrystallizations of potassium sulfate and sulfates of magnesium, calcium, and sodium.

Relevant minerals are:

The potassium sulfate can be separated from some of these minerals, like kainite, because the corresponding salt is less soluble in water.

Kieserite, MgSO4·H2O, can be combined with a solution of potassium chloride to produce potassium sulfate.

Production edit

Approximately 1.5 million tons were produced in 1985, typically by the reaction of potassium chloride with sulfuric acid, analogous to the Mannheim process for producing sodium sulfate.[7] The process involves intermediate formation of potassium bisulfate, an exothermic reaction that occurs at room temperature:

KCl + H2SO4 → HCl + KHSO4

The second step of the process is endothermic, requiring energy input:

KCl + KHSO4 → HCl + K2SO4

Structure and properties edit

Two crystalline forms are known. Orthorhombic β-K2SO4 is the common form, but it converts to α-K2SO4 above 583 °C.[7] These structures are complex, although the sulfate adopts the typical tetrahedral geometry.[8]

  •  

    Structure of β-K2SO4.

  •  

    Coordination sphere of one of two types of K+ site.

  •  

    SO4 environment in β-K2SO4.

It does not form a hydrate, unlike sodium sulfate. The salt crystallizes as double six-sided pyramids, classified as rhombic. They are transparent, very hard and have a bitter, salty taste. The salt is soluble in water, but insoluble in solutions of potassium hydroxide (sp. gr. 1.35), or in absolute ethanol.

Uses edit

The dominant use of potassium sulfate is as a fertilizer. K2SO4 does not contain chloride, which can be harmful to some crops. Potassium sulfate is preferred for these crops, which include tobacco and some fruits and vegetables. Crops that are less sensitive may still require potassium sulfate for optimal growth if the soil accumulates chloride from irrigation water.[9]

The crude salt is also used occasionally in the manufacture of glass. Potassium sulfate is also used as a flash reducer in artillery propellant charges. It reduces muzzle flash, flareback and blast overpressure.

It is sometimes used as an alternative blast media similar to soda in soda blasting as it is harder and similarly water-soluble.[10]

Potassium sulfate can also be used in pyrotechnics in combination with potassium nitrate to generate a purple flame.

A 5% solution of potassium sulfate was used in the beginning of the 20th century as a topical mosquito repellent.[citation needed]

Reactions edit

Acidification edit

Potassium hydrogen sulfate (also known as potassium bisulfate), KHSO4, is readily produced by reacting K2SO4 with sulfuric acid. It forms rhombic pyramids, which melt at 197 °C (387 °F). It dissolves in three parts of water at 0 °C (32 °F). The solution behaves much as if its two congeners, K2SO4 and H2SO4, were present side by side of each other uncombined; an excess of ethanol the precipitates normal sulfate (with little bisulfate) with excess acid remaining.

The behavior of the fused dry salt is similar when heated to several hundred degrees; it acts on silicates, titanates, etc., the same way as sulfuric acid that is heated beyond its natural boiling point does. Hence it is frequently used in analytical chemistry as a disintegrating agent. For information about other salts that contain sulfate, see sulfate.

References edit

  1. ^ Patnaik, Pradyot (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 978-0-07-049439-8.
  2. ^ Windholtz, M; Budavari, S, eds. (1983). The Merck Index. Rahway, New Jersey: Merck & Co.
  3. ^ Chambers, Michael. "Potassium sulfate RN: 7778-80-5". ChemIDplus. United States National Library of Medicine.
  4. ^ De Milt, Clara (1942). "Christopher Glaser". Journal of Chemical Education. 19 (2): 53. Bibcode:1942JChEd..19...53D. doi:10.1021/ed019p53.
  5. ^ van Klooster, H. S. (1959). "Three centuries of Rochelle salt". Journal of Chemical Education. 36 (7): 314. Bibcode:1959JChEd..36..314K. doi:10.1021/ed036p314.
  6. ^ a b   Chambers, Ephraim, ed. (1728). "Arcanum duplicatum". Cyclopædia, or an Universal Dictionary of Arts and Sciences. Vol. 1 (1st ed.). James and John Knapton, et al. p. *125.
  7. ^ a b Schultz, H.; Bauer, G.; Schachl, E.; Hagedorn, F.; Schmittinger, P. (2005). "Potassium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a22_039. ISBN 3527306730.
  8. ^ Gaultier, M.; Pannetier, G. (1968). "Structure cristalline de la forme 'basse température' du sulfate de potassium K2SO4-beta" [Crystal structure of the "low temperature" β-form of potassium sulfate]. Bulletin de la Société Chimique de France (in French). 1: 105–112.
  9. ^ United Nations Industrial Development Organization; International Fertilizer Development Center (1998). Fertilizer manual (3rd ed.). Dordrecht, Netherlands: Kluwer Academic. ISBN 978-0-7923-5032-3.
  10. ^ . American Surface Prep. Archived from the original on 9 December 2014. Retrieved 7 December 2014.

External links edit

  • mindat.org: Arcanite
  • webmineral: Arcanite

November 28, 2023
potassium, sulfate, confused, with, potassium, sulfide, potassium, sulphate, also, called, sulphate, potash, arcanite, archaically, potash, sulfur, inorganic, compound, with, formula, k2so4, white, water, soluble, solid, commonly, used, fertilizers, providing,. Not to be confused with potassium sulfide Potassium sulfate US or potassium sulphate UK also called sulphate of potash SOP arcanite or archaically potash of sulfur is the inorganic compound with formula K2SO4 a white water soluble solid It is commonly used in fertilizers providing both potassium and sulfur Potassium sulfate ArcaniteNamesOther names Potassium sulphateIdentifiersCAS Number 7778 80 5 Y3D model JSmol Interactive imageChEBI CHEBI 32036 YChEMBL ChEMBL2021424 YChemSpider 22915 YECHA InfoCard 100 029 013EC Number 231 915 5E number E515 i acidity regulators KEGG D01726 YPubChem CID 24507RTECS number TT5900000UNII 1K573LC5TV YCompTox Dashboard EPA DTXSID6029701InChI InChI 1S 2K H2O4S c 1 5 2 3 4 h H2 1 2 3 4 q2 1 p 2 YKey OTYBMLCTZGSZBG UHFFFAOYSA L YInChI 1 2K H2O4S c 1 5 2 3 4 h H2 1 2 3 4 q2 1 p 2Key OTYBMLCTZGSZBG NUQVWONBAUSMILES K K O S O O OPropertiesChemical formula K2SO4Molar mass 174 259 g molAppearance White solidOdor odorlessDensity 2 66 g cm3 1 Melting point 1 069 2 C 1 956 F 1 342 K Boiling point 1 689 C 3 072 F 1 962 K Solubility in water 111 g L 20 C 120 g L 25 C 240 g L 100 C Solubility product Ksp 1 32 120 g L Solubility slightly soluble in glycerol insoluble in acetone alcohol CS2Magnetic susceptibility x 67 0 10 6 cm3 molRefractive index nD 1 495StructureCrystal structure orthorhombicHazardsOccupational safety and health OHS OSH Main hazards IrritantGHS labelling PictogramsSignal word WarningHazard statements H318Precautionary statements P280 P305 P351 P338 P310Flash point Non flammableLethal dose or concentration LD LC LD50 median dose 6600 mg kg oral rat 3 Safety data sheet SDS External MSDSRelated compoundsOther anions Potassium selenatePotassium tellurateOther cations Lithium sulfateSodium sulfateRubidium sulfateCaesium sulfateRelated compounds Potassium hydrogen sulfatePotassium sulfitePotassium bisulfitePotassium persulfateExcept where otherwise noted data are given for materials in their standard state at 25 C 77 F 100 kPa N verify what is Y N Infobox references Contents 1 History 2 Natural resources 3 Production 4 Structure and properties 5 Uses 6 Reactions 6 1 Acidification 7 References 8 External linksHistory editPotassium sulfate K2SO4 has been known since early in the 14th century It was studied by Glauber Boyle and Tachenius In the 17th century it was named arcanuni or sal duplicatum as it was a combination of an acid salt with an alkaline salt It was also known as vitriolic tartar and Glaser s salt or sal polychrestum Glaseri after the pharmaceutical chemist Christopher Glaser who prepared it and used medicinally 4 5 Known as arcanum duplicatum double secret or panacea duplicata in pre modern medicine it was prepared from the residue caput mortuum left over from the production of aqua fortis nitric acid HNO3 from nitre potassium nitrate KNO3 and oil of vitriol sulphuric acid H2SO4 via Glauber s process 2 KNO3 H2SO4 2 HNO3 K2SO4The residue was dissolved in hot water filtered and evaporated to a cuticle It was then left to crystallise It was used as a diuretic and sudorific 6 According to Chambers s Cyclopedia the recipe was purchased for five hundred thalers by Charles Frederick Duke of Holstein Gottorp Schroder the duke s physician wrote wonders of its great uses in hypochondriacal cases continued and intermitting fevers stone scurvy and more 6 Natural resources editThe mineral form of potassium sulfate arcanite is relatively rare Natural resources of potassium sulfate are minerals abundant in the Stassfurt salt These are cocrystallizations of potassium sulfate and sulfates of magnesium calcium and sodium Relevant minerals are Kainite KMg SO4 Cl 3H2O Schonite now known as picromerite K2SO4 MgSO4 6H2O Leonite K2SO4 MgSO4 4H2O Langbeinite K2Mg2 SO4 3 Aphthitalite previously known as glaserite K3Na SO4 2 Polyhalite K2SO4 MgSO4 2CaSO4 2H2OThe potassium sulfate can be separated from some of these minerals like kainite because the corresponding salt is less soluble in water Kieserite MgSO4 H2O can be combined with a solution of potassium chloride to produce potassium sulfate Production editApproximately 1 5 million tons were produced in 1985 typically by the reaction of potassium chloride with sulfuric acid analogous to the Mannheim process for producing sodium sulfate 7 The process involves intermediate formation of potassium bisulfate an exothermic reaction that occurs at room temperature KCl H2SO4 HCl KHSO4The second step of the process is endothermic requiring energy input KCl KHSO4 HCl K2SO4Structure and properties editTwo crystalline forms are known Orthorhombic b K2SO4 is the common form but it converts to a K2SO4 above 583 C 7 These structures are complex although the sulfate adopts the typical tetrahedral geometry 8 nbsp Structure of b K2SO4 nbsp Coordination sphere of one of two types of K site nbsp SO4 environment in b K2SO4 It does not form a hydrate unlike sodium sulfate The salt crystallizes as double six sided pyramids classified as rhombic They are transparent very hard and have a bitter salty taste The salt is soluble in water but insoluble in solutions of potassium hydroxide sp gr 1 35 or in absolute ethanol Uses editThe dominant use of potassium sulfate is as a fertilizer K2SO4 does not contain chloride which can be harmful to some crops Potassium sulfate is preferred for these crops which include tobacco and some fruits and vegetables Crops that are less sensitive may still require potassium sulfate for optimal growth if the soil accumulates chloride from irrigation water 9 The crude salt is also used occasionally in the manufacture of glass Potassium sulfate is also used as a flash reducer in artillery propellant charges It reduces muzzle flash flareback and blast overpressure It is sometimes used as an alternative blast media similar to soda in soda blasting as it is harder and similarly water soluble 10 Potassium sulfate can also be used in pyrotechnics in combination with potassium nitrate to generate a purple flame A 5 solution of potassium sulfate was used in the beginning of the 20th century as a topical mosquito repellent citation needed Reactions editAcidification edit Potassium hydrogen sulfate also known as potassium bisulfate KHSO4 is readily produced by reacting K2SO4 with sulfuric acid It forms rhombic pyramids which melt at 197 C 387 F It dissolves in three parts of water at 0 C 32 F The solution behaves much as if its two congeners K2SO4 and H2SO4 were present side by side of each other uncombined an excess of ethanol the precipitates normal sulfate with little bisulfate with excess acid remaining The behavior of the fused dry salt is similar when heated to several hundred degrees it acts on silicates titanates etc the same way as sulfuric acid that is heated beyond its natural boiling point does Hence it is frequently used in analytical chemistry as a disintegrating agent For information about other salts that contain sulfate see sulfate References edit Patnaik Pradyot 2002 Handbook of Inorganic Chemicals McGraw Hill ISBN 978 0 07 049439 8 Windholtz M Budavari S eds 1983 The Merck Index Rahway New Jersey Merck amp Co Chambers Michael Potassium sulfate RN 7778 80 5 ChemIDplus United States National Library of Medicine De Milt Clara 1942 Christopher Glaser Journal of Chemical Education 19 2 53 Bibcode 1942JChEd 19 53D doi 10 1021 ed019p53 van Klooster H S 1959 Three centuries of Rochelle salt Journal of Chemical Education 36 7 314 Bibcode 1959JChEd 36 314K doi 10 1021 ed036p314 a b nbsp Chambers Ephraim ed 1728 Arcanum duplicatum Cyclopaedia or an Universal Dictionary of Arts and Sciences Vol 1 1st ed James and John Knapton et al p 125 a b Schultz H Bauer G Schachl E Hagedorn F Schmittinger P 2005 Potassium Compounds Ullmann s Encyclopedia of Industrial Chemistry Weinheim Wiley VCH doi 10 1002 14356007 a22 039 ISBN 3527306730 Gaultier M Pannetier G 1968 Structure cristalline de la forme basse temperature du sulfate de potassium K2SO4 beta Crystal structure of the low temperature b form of potassium sulfate Bulletin de la Societe Chimique de France in French 1 105 112 United Nations Industrial Development Organization International Fertilizer Development Center 1998 Fertilizer manual 3rd ed Dordrecht Netherlands Kluwer Academic ISBN 978 0 7923 5032 3 Super K Potassium Sulphate American Surface Prep Archived from the original on 9 December 2014 Retrieved 7 December 2014 External links editmindat org Arcanite webmineral Arcanite Retrieved from https en wikipedia org w index php title Potassium sulfate amp oldid 1185787629, wikipedia, wiki, book, books, library,

article

, read, download, free, free download, mp3, video, mp4, 3gp, jpg, jpeg, gif, png, picture, music, song, movie, book, game, games.