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Potassium sulfate

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Potassium sulfate Basic information
Potassium sulfate Chemical Properties
  • Melting point:1067°C
  • Boiling point:1689°C
  • Density 2.66
  • Flash point:1689°C
  • storage temp. Store at RT.
  • solubility H2O: 0.5 M at 20 °C, clear, colorless
  • form Very Fine Crystals or Powder
  • color White
  • Specific Gravity2.662
  • OdorOdorless
  • PH5.5-7.5 (25℃, 0.5M in H2O)
  • PH Range~7
  • Water Solubility 110 g/L (20 ºC)
  • λmaxλ: 260 nm Amax: 0.01
    λ: 280 nm Amax: 0.01
  • Merck 14,7674
  • Stability:Stable.
  • InChIKeyOTYBMLCTZGSZBG-UHFFFAOYSA-L
  • CAS DataBase Reference7778-80-5(CAS DataBase Reference)
  • NIST Chemistry ReferencePotassium sulfate(7778-80-5)
  • EPA Substance Registry SystemPotassium sulfate (7778-80-5)
Safety Information
MSDS
Potassium sulfate Usage And Synthesis
  • DescriptionPotassium sulfate (K2SO4) is a kind of chemical compounds that is commonly used in agriculture. The dominant application of potassium sulfate is as a fertilizer, which is commonly applied to offer both potassium and sulfur, thus improving the quality and yield of crops growing in soils that lack an adequate supply of this essential elements. Besides, the crude potassium sulfate is sometimes employed in the production of glass. It also has applications in other industries, which is used as a flash reducer in artillery propellant charges and as an alternative blast media similar to soda in the process of soda blasting.
    potassium sulfate powder
    potassium sulfate powder
  • Chemical PropertiesPotassium sulfate,K2804, also known as salt of Lemery and arcanite, is a colorless crystalline solid that melts at 1072°C(1960 OF). It is soluble in water,but insoluble in alcohol. Potassium sulfate is used in manufacturing glass, aluminum, fertilizers, and in medicine.
  • Chemical PropertiesPotassium sulfate, sulfate of potash, K2SO4, white solid, soluble. Common constituent of potassium salt minerals.
  • Physical propertiesColorless or white crystals or white granules or powder; rhombohedral structure; bitter taste; density 2.66 g/cm3; melts at 1,069°C; vaporizes at 1,689°C; moderately soluble in water, 12 g/100mL at 25°C and 24g/100mL at 100°C; slightly soluble in glycerol; insoluble in alcohol, acetone, and carbon disulfide.
  • OccurrencePotassium and sodium sulfates and their double sulfates with calcium and magnesium occur naturally in various salt lakes. Potassium sulfate also occurs in certain volcanic lava. Its double salt with magnesium occurs in nature, as the mineral langbeinite.
    Potassium sulfate is used in fertilizers as a source of potassium and sulfur, both of which are essential elements for plant growth. Either in sim-ple form or as a double salt with magnesium sulfate, potassium sulfate is one of the most widely consumed potassium salts in agricultural applications. It is preferred over potassium chloride for certain types of crops; such as, tobac-co, citrus, and other chloride-sensitive crops. Some other applications include making gypsum cements; to make potassium alum; in the analysis of Kjeldahl nitrogen; and in medicine.
  • UsesTechnical grades are used in fertilizers for manufacture of potassium alum, potassium carbonate and glass; the reagent grade is used in the Kjeldahl determination of nitrogen.
  • Usespotassium sulfate is a reagent in cosmetics. Potassium sulfate is an inorganic salt with a primary function as a viscosity-increasing agent.
  • UsesPotassium Sulfate is a flavoring agent that occurs naturally, consisting of colorless or white crystals or crystalline powder having a bitter, saline taste. it is prepared by the neutralization of sulfuric acid with potassium hydroxide or potassium carbonate.
  • DefinitionA white crystallinepowder, K2SO4, soluble inwater and insoluble in ethanol;rhombic or hexagonal; r.d. 2.66; m.p.1069°C. It occurs naturally assch?nite (Strassfurt deposits) and inlake brines, from which it is separatedby fractional crystallization. Ithas also been produced by the Hargreavesprocess, which involves theoxidation of potassium chloride withsulphuric acid. In the laboratory itmay be obtained by the reaction ofeither potassium hydroxide or potassiumcarbonate with sulphuric acid.Potassium sulphate is used in cements,in glass manufacture, as afood additive, and as a fertilizer(source of K+) for chloride-sensitiveplants, such as tobacco and citrus.
  • Production MethodsPotassium sulfate is produced by various methods, selection of process depending on availability and cost of raw materials.
    The salt may be obtained from its naturally occurring mineral, langbeinite,K2SO4?2MgSO4. The ore first is crushed and washed with water to separate sodium chloride. After that, magnetite is separated from the washed langbei-nite by magnetic separation. After the separation of these two major impuri-ties, the purified double salt is treated with an aqueous solution of potassium chloride to obtain potassium sulfate:
    K2SO4?2MgSO4 + 4KCl →3K2SO4+ 2MgCl2
    The solution is filtered to remove insoluble residues and the products are separated from their aqueous mixture by crystallization.
    Potassium sulfate also is produced from the mineral kieserite, MgSO4?H2O by treatment with potassium chloride. The intermediate double salt obtained reacts further with potassium chloride to form potassium sulfate:MgSO4?H2O + 2KCl + 4H2O →K2SO4?MgSO4?6H2O + MgCl2
    K2SO4?MgSO4?6H2O + 2KCl →2K2SO4+ MgCl2
    Potassium sulfate is separated from the more soluble magnesium chloride by crystallization.
    Also, potassium sulfate can be made by two other processes in which no naturally occurring mineral is employed. In the Mannheim process, the salt is produced by action of sulfuric acid on potassium chloride:2KCl + H2SO4→K2SO4+ 2HCl
    In Hargreaves process, which is a slight variation of the Mannheim method, potassium sulfate is made by heating a mixture of potassium chlo-ride, sulfur dioxide, air and water:4KCl + 2SO2+ 2H2O + o2→2K2SO4+ 4HCl.
  • Safety ProfileModerately toxic to humans by ingestion. Moderately toxic experimentally by subcutaneous route. Swallowing large doses causes severe gastrointestinal tract effects. When heated to decomposition it emits toxic fumes of K2O and SOx. See also SULFATES.
  • Purification MethodsPotassium sulfate [7778-80-5] M 174.3, m 1069o, d 4 2.67 It crystallised from distilled water (4mL/g at 20o; 8mL/g at 100o) between 100o and 0o.
  • Referenceshttps://en.wikipedia.org/wiki/Potassium_sulfate
    http://www.cropnutrition.com/potassium-sulfate
    http://study.com/academy/lesson/what-is-potassium-sulfate-structure-uses-formula.html
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