Kaliumoxide

Kaliumoxid, also known as potassium oxide, is an inorganic compound with the chemical formula K2O. It is a white, highly hygroscopic solid that readily absorbs moisture from the air and reacts with water to form potassium hydroxide (KOH), releasing heat in the process: K2O + H2O → 2 KOH. As a basic oxide, it reacts with acids to give potassium salts and with carbon dioxide to form potassium carbonate: K2O + CO2 → K2CO3.

Production and occurrence: In industry, potassium oxide is typically obtained by the high-temperature decomposition of potassium carbonate or other potassium compounds. It can also be formed by burning potassium metal in air, though this is not a common preparation route for bulk supplies. In nature, K2O occurs primarily as a component of complex mineral phases and is ordinarily encountered in the form of its hydrates or in mixed alkali oxides in industrial materials.

Properties: Potassium oxide has a high melting point around 740 °C and is highly reactive with water and moisture. It is soluble in water, yielding a strongly alkaline solution, and its reactivity makes it a powerful base. It reacts with atmospheric moisture to form KOH and with carbon dioxide to form K2CO3.

Applications: K2O is used as a flux in glass and ceramic production, lowering melting temperatures and helping to form silicate structures. It also serves as a laboratory reagent and a precursor to potassium hydroxide and various potassium salts. In certain industrial materials, it may be present as part of alkali oxide blends.

Safety: Kaliumoxide is corrosive and reacts vigorously with water, causing heat and caustic conditions. It can cause severe chemical burns and releases caustic fumes. It should be handled in dry environments with appropriate personal protective equipment and stored in moisture-free, sealed containers.