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Ammonia Water Equation
The chemical change in the world, the reaction between ammonia and water, is an important example. Ammonia ($NH_3 $) into water, there is a wonderful change.
Ammonia dissolves in water, there is this reaction: $NH_3 + H_2O\ rightleftharpoons NH_3 · H_2O $. This is the process of combining ammonia with water to form ammonia monohydrate. This reaction is not one-way, but in dynamic equilibrium.
And ammonia monohydrate is not stable, it will undergo partial ionization: $NH_3 · H_2O\ rightleftharpoons ^ NH_4 ++ OH ^ - $. Although this ionization is not complete, it makes the ammonia solution alkaline.
Looking at the equation of ammonia hydrolysis, it can be seen that ammonia does not simply dissolve in water, but interacts with water to form new particles. The state of equilibrium in this state is affected by many factors. When the temperature increases, the equilibrium often moves in the endothermic direction. In this reaction, the reverse is endothermic, so when the temperature increases, ammonia escapes and ammonia monohydrate decomposes more. If the concentration of ammonia is increased, the equilibrium will move forward, resulting in more hydrous ammonia, which in turn will move the ionization equilibrium forward and enhance the alkalinity of the solution.
Furthermore, from an ionic perspective, ammonium ions ($NH_4 ^ + $) and hydroxide ions ($OH ^ - $) produced by ammonia hydrolysis play an important role in many chemical processes. In short, the chemical phenomena and principles revealed by the ammonia hydrolysis equation are of great significance in many fields such as chemical research and industrial production.
Ammonia dissolves in water, there is this reaction: $NH_3 + H_2O\ rightleftharpoons NH_3 · H_2O $. This is the process of combining ammonia with water to form ammonia monohydrate. This reaction is not one-way, but in dynamic equilibrium.
And ammonia monohydrate is not stable, it will undergo partial ionization: $NH_3 · H_2O\ rightleftharpoons ^ NH_4 ++ OH ^ - $. Although this ionization is not complete, it makes the ammonia solution alkaline.
Looking at the equation of ammonia hydrolysis, it can be seen that ammonia does not simply dissolve in water, but interacts with water to form new particles. The state of equilibrium in this state is affected by many factors. When the temperature increases, the equilibrium often moves in the endothermic direction. In this reaction, the reverse is endothermic, so when the temperature increases, ammonia escapes and ammonia monohydrate decomposes more. If the concentration of ammonia is increased, the equilibrium will move forward, resulting in more hydrous ammonia, which in turn will move the ionization equilibrium forward and enhance the alkalinity of the solution.
Furthermore, from an ionic perspective, ammonium ions ($NH_4 ^ + $) and hydroxide ions ($OH ^ - $) produced by ammonia hydrolysis play an important role in many chemical processes. In short, the chemical phenomena and principles revealed by the ammonia hydrolysis equation are of great significance in many fields such as chemical research and industrial production.
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