Brief description of the chemical properties of yellow blood salt
Yellow blood salt, that is, potassium ferrocyanide ($K_4 [Fe (CN) _6] $), has unique chemical properties and is of great significance in many chemical reactions and application fields.

In terms of stability, potassium ferrocyanide is quite stable at room temperature and pressure, and can maintain its own chemical structure and properties for a long time. However, when heated to a certain extent, it will decompose. For example, when heated to about 70 dollars ^ {\ circ} C $, it will gradually lose its crystal water, which in turn affects its chemical activity and physical form.

In redox reactions, potassium ferrocyanide exhibits certain characteristics. Its ferrous ions are in an intermediate oxidation state, which is both reductive and oxidizing. When exposed to strong oxidants, such as acidic potassium permanganate solutions, ferrous ions will be oxidized to iron ions, and they will undergo corresponding chemical changes to form new compounds. During this process, the color of the solution and other external manifestations will also change.

The reaction with metal ions is also worthy of attention. Potassium ferrocyanide can react with a variety of metal ions to form complexes with specific structures and properties. For example, when reacted with copper ions, copper ferrocyanide can be formed, which is often used in analytical chemistry to detect and quantify the content of copper ions.

In addition, potassium ferrocyanide will undergo weak ionization in aqueous solution, resulting in potassium ions and ferrocyanide ions. The degree of ionization is affected by temperature, pH and other factors. Under acidic conditions, the ionic stability of ferrocyanide decreases slightly, which may react with hydrogen ions, resulting in a change in the ion balance in the solution, which in turn affects its chemical properties and related applications.