The precipitation of sodium ferrocyanide
Now there is sodium ferrocyanide, which is gradually dissociated in water. Sodium ferrocyanide, the molecular formula is $Na_4 [Fe (CN) _6] $. In the water-soluble environment, it dissociates according to the following reaction formula: $Na_4 [Fe (CN) _6]\ longrightarrow 4Na ^ ++ [Fe (CN) _6] ^ {4 - }$ 。

sodium ion $Na ^ + $dissociates, moves freely in the solution, and has a positive charge. The $[Fe (CN) _6] ^ {4 -} $ions also exist in the solution, with a negative charge. The two balance each other, making the solution electrically neutral.

The dissociation of sodium ferrocyanide is affected by many factors. When the water temperature rises, the dissociation rate increases. Due to high temperature and high molecular kinetic energy, it is easier to break free from each other's forces and accelerate dissociation. And the concentration of the solution is also related. In dilute solutions, the ion spacing is large, the interaction is weak, and the dissociation is easier; in concentrated solutions, the ions are controlled by each other, and the dissociation is slightly difficult.

The ions after the dissociation of sodium ferrocyanide are useful in many fields. Sodium ions in living bodies are related to the regulation of osmotic pressure and the transmission of nerve impulses. And $[Fe (CN) _6] ^ {4 -} $ions, in some chemical reactions, can be used as ligands to participate in complexation reactions, which is of great significance for the synthesis and property regulation of substances.