Potassium nitrate is a chemical compound with the formula KNO3. It is an ionic salt of potassium ions K+ and nitrate ions NO3−, and is therefore an alkali metal nitrate.
Potassium nitrate has an orthorhombic crystal structure at room temperature, which transforms to a trigonal system at 129 °C (264 °F). It is moderately soluble in water, but its solubility increases with temperature.
Uses of Potassium Nitrate [KNO3]
Potassium nitrate is a very versatile substance and has a wide variety of uses, largely as a source of nitrate in fertilizers, tree stump removal, rocket propellants, meat processing, gunpowder, and fireworks.
The Natural Origin of Potassium Nitrate
Potassium nitrate is one of several nitrogen-containing compounds collectively referred to as saltpeter. It occurs in nature as the mineral Niter which, as derived from its name, is a source of Nitrogen.
A major natural source of KNO3 was the deposits crystallizing from cave walls and the accumulations of bat guano in caves. It can be extracted by immersing the guano in water for a day, filtering, and harvesting the crystals from the filtered water.
How to Make KNO3
Potassium nitrate can be made by combining ammonium nitrate and potassium hydroxide.
- NH4NO3 (aq) + KOH (aq) → NH3 (g) + KNO3 (aq) + H2O (l)
An alternative way of producing potassium nitrate without a by-product of ammonia is to combine ammonium nitrate, found in instant ice packs, and potassium chloride, easily obtained as a sodium-free salt substitute.
- NH4NO3 (aq) + KCl (aq) → NH4Cl (aq) + KNO3 (aq)
Potassium nitrate can also be produced by neutralizing nitric acid with potassium hydroxide. This reaction is highly exothermic.
- KOH (aq) + HNO3 → KNO3 (aq) + H2O (l)
On an industrial scale, it is prepared by the double displacement reaction between sodium nitrate and potassium chloride.
- NaNO3 (aq) + KCl (aq) → NaCl (aq) + KNO3 (aq)
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