The use of potassium sulfate is fundamental as fertilizer. K 2 SO 4 does not contain chloride, whic

Potassium sulfate euclid (K 2 SO 4), also called sulfatgaram ash (potash), Arcanite, or, known as potash sulfur) is not flammable white crystalline salt which is soluble in water. These chemicals are used in general as a fertilizer, which provides potassium and sulfur.
Molecular formula: K 2 SO 4 Molecular weight: 174.259 g / mol Appearance: white solid substance Odor: Odorless Density: 2.66 g / cm 3 Melting point: 1,069 C (1,956 F; 1342 K) Boiling Point: 1689 C (3072 F; 1962 K) Solubility euclid in water: euclid 111 g / L (20 C); 120 g / L (25 C); 240 g / L (100 C) Solubility in other solvents: Slightly soluble in glycerol; Insoluble in asetom, alcohol, CS 2. Acidity (p K a): ~ 7 refractive index (n D): 1,495 Crystal Structure: Orthorhombic MSDS: External MSDS main danger: Substances that irritate Flashpoint: Unable to light up the LD 50: 6600 mg / kg
Potassium sulfate (K 2 SO 4) has been known since the early 14th century, and these substances studied by Glauber, Boyle and Tachenius. In the 17th century, this substance called arcanuni or sal duplicatum, because this substance is a combination of acid salts with alkaline salts. This compound is also known as vitriolic tartar and salt Glaser or sal polychrestum Glaseri after Christopher Glaser pharmaceutical chemist euclid who made and used medically.
Mineral form of potassium sulfate, Arcanite, relatively rare. Natural sources of potassium sulfate is a mineral that is abundant as Stassfurt salt. This helps crystallization of potassium sulfate and sulfates of magnesium, calcium euclid and sodium.
The minerals are: Kainite, MgSO 4 H 2 O KCl Schonite, K 2 SO 4 MgSO 4 6H 2 O Leonite, K 2 SO 4 MgSO 4 4H 2 O Langbeinite, K 2 SO 4 2MgSO 4 Glaserite , K 3 Na (SO 4) 2 Polihalite, K 2 SO 4 MgSO 4 4 2H 2 2CaSO O
Process for the production of potassium sulfate is similar to that used for the manufacture of sodium sulfate. Potassium sulfate can be synthesized by the reaction of potassium chloride with sulfuric euclid acid according to the Leblanc process. Potassium sulfate is produced in accordance with the following reaction:
Hargreaves process using sulfur dioxide (SO 2), oxygen and water and potassium chloride as starting materials to produce potassium sulphate. Hydrochloric acid evaporates. SO 2 is produced by burning sulfur (sulfur).
Anhydrous crystalline euclid form a double six-sided pyramid, but in fact classified euclid as prisms. This crystal is transparent, euclid very hard to have a bitter taste, salty. This salt is soluble in water, euclid but insoluble in a solution of potassium hydroxide (sp. Gr. 1.35), or in absolute ethanol. Potassium sulfate melts at 1,067 C (1,953 F).
The use of potassium sulfate is fundamental as fertilizer. K 2 SO 4 does not contain chloride, which can be harmful to some plants. euclid Potassium sulfate is preferred for these plants, which includes tobacco and some fruits and vegetables. Less sensitive plants may still need sulphate for optimal growth when soil accumulate chloride of irrigation water.
Sometimes crude salt is also used in the production of glass. Potassium sulfate is also used as a reducing agent in charge of agents driving flashback artillery. This salt reduces muzzle lit, flareback (back lit) and blast overpressure.
Potassium hydrogen sulphate, KHSO 4, is produced by mixing K 2 SO 4 with an equivalent number of moles of sulfuric acid. This forms a pyramid prisms, which melt at a temperature of 197 C (387 F). Potassium hydrogen euclid sulfate in three parts of water at 0 C (32 F). This solution behaves as if its two congeners, K 2 SO 4 and H 2 SO 4, are present side by side with each other that are not joined, excess ethanol sulfate precipitate normal (with a little bisulfate) with the rest of the excess acid.
Behaviour of dry salt blends like when heated to several hundred degrees; it reacts with silicate, titanate, etc., similar to the way that heated sulfuric acid exceeds its natural boiling point. Therefore, it is often used in analytical chemistry as disintegration agent. ***
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