Ammonium hydroxide ionizes as follows: NH4OH(s) NH4 +(aq) + OH-(aq). If an excess of ammonium salt, such as NH4Cl (which ionizes to give NH4 +(aq) ions) is added to the equilibrium shown above, you could predict that the result will be to....

Respuesta :

Decrease the concentration of OH-

Answer: The dissociation of the base will be further suppressed.

Explanation: Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

[tex]NH_4OH(s)\rightleftharpoons NH_4^+(aq)+OH^-(aq)[/tex]

If an excess of ammonium salt, such as [tex]NH_4Cl[/tex] (which ionizes to give [tex]NH_4^+[/tex](aq) ions)

[tex]NH_4Cl\rightarrow NH_4^++Cl^-[/tex]

If the concentration of [tex]NH_4^+[/tex] that is the product is increased, so according to the Le-Chatelier's principle, the equilibrium will shift in the direction where decrease of concentration of [tex]NH_4^+[/tex] takes place. Therefore, the equilibrium will shift in the backward direction and the ions will start associating to form [tex]NH_4OH[/tex].