Potassium sulfate (K2SO4)
(in British English potassium sulphate
, also called sulphate of potash
or archaically known as potash of sulfur
) is a flammable white crystalline salt
which is soluble
is commonly used in fertilizers
, providing both potassium
Potassium sulfate (K2
) has been known since early in the 14th century, and it was studied by Glauber
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
The mineral form of potassium sulfate, namely arcanite, is relatively rare. Natural resources of potassium sulfate are minerals
abundant in the Stassfurt salt
. These are cocrystalisations of potassium sulfate and sulfates of magnesium calcium
The minerals are
From some of the minerals like kainite, the potassium sulfate can be separated, because the corresponding salt is less soluble in water.
With potassium chloride kieserite MgSO4 • 2 H2O can be transformed and then the potassium sulfate can be dissolved in water.
- Potassium sulfate can be synthesised by the decomposition of potassium chloride with sodium sulfate.
- The Hargreaves method is basically the same process with different starting materials. Sulfur dioxide, oxygen and water (the starting materials for sulfuric acid) are reacted with potassium chloride. Hydrochloric acid evaporates off.
- Potassium Sulfate is produced by mixing the following:
Potassium Chloride and Sulfuric Acid(with molar ratio).
2KCl + H2SO4 ---> 2HCl + K2SO4
crystals form a double six-sided pyramid, but are in fact 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
1.35), or in absolute ethanol
. It melts at 1078 °C.
The principal use of potassium sulfate is as a fertilizer
. The crude salt is also used occasionally in the manufacture of glass.
Potassium hydrogen sulfate
Potassium hydrogen sulfate
or bisulfate, KHSO4
, is readily produced by mixing K2
with an equivalent no. of moles
of sulfuric acid
. It forms rhombic pyramids
, which melt at 197 °C. It dissolves in three parts of water at 0°C. The solution behaves much as if its two congeners
, 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.