5/31/2023 0 Comments Potassium densityHence it is frequently used in analytical chemistry as a disintegrating agent. 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. The solution behaves much as if its two congeners, K 2SO 4 and H 2SO 4, were present side by side of each other uncombined an excess of ethanol the precipitates normal sulfate (with little bisulfate) with excess acid remaining. It dissolves in three parts of water at 0 ☌ (32 ☏). It forms rhombic pyramids, which melt at 197 ☌ (387 ☏). Potassium hydrogen sulfate (also known as potassium bisulfate), KHSO 4, is readily produced by reacting K 2SO 4 with sulfuric acid. Potassium sulfate can also be used in pyrotechnics in combination with potassium nitrate to generate a purple flame.Ī 5% solution of potassium sulfate was used in the beginning of the 20th century as a topical mosquito repellent. It is sometimes used as an alternative blast media similar to soda in soda blasting as it is harder and similarly water-soluble. It reduces muzzle flash, flareback and blast overpressure. Potassium sulfate is also used as a flash reducer in artillery propellant charges. The crude salt is also used occasionally in the manufacture of glass. Crops that are less sensitive may still require potassium sulfate for optimal growth if the soil accumulates chloride from irrigation water. Potassium sulfate is preferred for these crops, which include tobacco and some fruits and vegetables. K 2SO 4 does not contain chloride, which can be harmful to some crops. The dominant use of potassium sulfate is as a fertilizer. The salt is soluble in water, but insoluble in solutions of potassium hydroxide ( sp. They are transparent, very hard and have a bitter, salty taste. The salt crystallizes as double six-sided pyramids, classified as rhombic. It does not form a hydrate, unlike sodium sulfate. These structures are complex, although the sulfate adopts the typical tetrahedral geometry. Orthorhombic β-K 2SO 4 is the common form, but it converts to α-K 2SO 4 above 583 ☌. KCl + KHSO 4 → HCl + K 2SO 4 Structure and properties The second step of the process is endothermic, requiring energy input: The process involves intermediate formation of potassium bisulfate, an exothermic reaction that occurs at room temperature:
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