Potassium sulfate
Structural formula | |||||||||||||||||||
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__ K + __ S 6+ __ O 2− | |||||||||||||||||||
Crystal system |
orthorhombic |
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Space group |
Pmcn (No. 62, position 5) |
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Lattice parameters |
a = 5.7704 Å , b = 10.0712 Å, c = 7.4776 Å |
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General | |||||||||||||||||||
Surname | Potassium sulfate | ||||||||||||||||||
other names | |||||||||||||||||||
Molecular formula | K 2 SO 4 | ||||||||||||||||||
Brief description |
colorless crystals or powder |
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External identifiers / databases | |||||||||||||||||||
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properties | |||||||||||||||||||
Molar mass | 174.26 g mol −1 | ||||||||||||||||||
Physical state |
firmly |
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density |
2.66 g cm −3 |
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Melting point |
1069 ° C |
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boiling point |
1689 ° C |
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solubility |
111 g l −1 at 20 ° C and 250 g l −1 at 100 ° C |
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safety instructions | |||||||||||||||||||
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Toxicological data | |||||||||||||||||||
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Potassium sulfate is the potassium salt of sulfuric acid . It is mainly used as a fertilizer .
history
The pharmacist and chemist Johann Rudolph Glauber was the first to produce the salt from potassium chloride and sulfuric acid, which has been known since the 14th century .
Occurrence
Pure potassium sulphate (K 2 SO 4 ) occurs naturally as the mineral arcanite .
In addition to ternary potassium sulfate, quaternary compounds with potassium and sulfate and another cation - so-called double salts - are known as minerals, such as belomarinaite (KNa [SO 4 ]), leonite (K 2 Mg [SO 4 ] 2 · 4H 2 O) , Picromerite (K 2 Mg [SO 4 ] 2 · 6H 2 O), langbeinite (K 2 Mg 2 [SO 4 ] 3 ) and the potash whim (generally KM III (SO 4 ) 2 · 12H 2 O).
Presentation and extraction
Initially, potassium sulfate was obtained from the mineral kainite (MgSO 4 · KCl · 3 H 2 O). However, this production method was soon abandoned in favor of more cost-effective processes based on potassium chloride.
One way in the production of potassium sulfate is the reaction of potassium chloride with sulfuric acid at a temperature of 700 ° C .
Alternatively, potassium sulfate is by double reaction with other metal sulfates such as. B. Magnesium sulfate can be represented:
The so-called Hargreaves process uses the reaction of potassium chloride with a mixture of sulfur dioxide , air and water to produce potassium sulfate :
Potassium sulfate is also a by-product in the production of nitric acid .
Potassium sulphate is easier to produce by reacting potassium hydroxide and sulfuric acid.
properties
The anhydrous crystals have orthorhombic symmetry ( space group Pmcn (space group no. 62, position 5) , lattice parameters a = 5.7704 Å, b = 10.0712 Å, c = 7.4776 Å). They are colorless and transparent, very hard and extremely stable in the air. Potassium sulfate has a bitter to salty taste. While it dissolves well in water, it is insoluble in ethanol .
use
Potassium sulfate is used for the production of potassium alum , potassium silicate , potassium persulfate , potassium , desensitizing agents , synthetic rubber and mixed fertilizers. In addition, it finds application in the Weinstein - and tartaric acid purification and diverse use in the dye -, explosives - and pharmaceutical industries.
Potassium sulfate is used in food technology as a firming agent , acid regulator or carrier . Potassium sulfate is used as a salt substitute in diet foods. It is approved in the EU as a food additive with the number E515 without a maximum quantity restriction ( quantum satis ) for all foods approved for additives.
It is also a component of potash fertilizers that are used to fertilize chloride- sensitive crops, for example in viticulture .
Potassium sulphate is also used as an active ingredient in extinguishing powders (mostly together with other alkali salts such as sodium hydrogen carbonate ) of fire classes B and C.
It is also used as a homeopathic medicine . As Schüßler salt , it is used there for all peeling skin diseases, such as neurodermatitis and psoriasis.
literature
- AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 , p. 1179.
Individual evidence
- ↑ a b K. Ojima, Y. Nishihata, A. Sawada: Structure of potassium sulfate at Temperatures from 296 K down to 15 K . In: Acta Crystallographica Section B . tape 51 , 1995, p. 287-293 , doi : 10.1107 / S0108768194013327 .
- ↑ Entry on POTASSIUM SULFATE in the CosIng database of the EU Commission, accessed on February 26, 2020.
- ↑ a b c d e f g h i Entry on potassium sulfate in the GESTIS substance database of the IFA , accessed on December 21, 2019 (JavaScript required)
- ↑ Entry on potassium sulfate. In: Römpp Online . Georg Thieme Verlag, accessed on March 24, 2019.