91影视

First, we will write the balanced equilibrium equation for silver chloride dissolving in water: \[ \text{AgCl (s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{Cl}^- (aq) \]

Next, we'll look at the interaction between silver chloride and ammonia (NH鈧�). Ammonia reacts with the silver ion (Ag鈦�) to form a soluble complex ion, [Ag(NH鈧�)鈧俔鈦�. The balanced equation for this reaction is: \[ \text{Ag}^+ (aq) + 2 \, \text{NH}_3 (aq) \rightleftharpoons [\text{Ag}(\text{NH}_3)_2]^+ (aq) \] Due to the formation of this soluble complex ion, the presence of ammonia (NH鈧�) helps to remove the Ag鈦� ions from the solution. According to Le Chatelier's principle, this will shift the equilibrium of the dissolution of AgCl to the right, causing more AgCl to dissolve, thus increasing the solubility of AgCl in NH鈧�.

Now, let's explore the effect of ammonium nitrate (NH鈧凬O鈧�) on the solubility of AgCl. When NH鈧凬O鈧� dissolves in water, it dissociates into NH鈧勨伜 and NO鈧冣伝 ions: \[ \text{NH}_4 \text{NO}_3 (aq) \rightarrow \text{NH}_4^+ (aq) + \text{NO}_3^- (aq) \] The presence of excess NH鈧勨伜 ions in the solution suppresses the dissociation of NH鈧� from the equilibrium: \[ \text{NH}_4^+ (aq) \rightleftharpoons \text{NH}_3 (aq) + \text{H}^+ (aq) \] Therefore, there is not enough free NH鈧� to react with the Ag鈦� ions and form the soluble complex ion [Ag(NH鈧�)鈧俔鈦�. As a result, very little AgCl dissolves in NH鈧凬O鈧�. Moreover, the presence of high concentrations of the common ion (Cl鈦�) in the solution from NH鈧凜l formed by NH鈧勨伜 and Cl鈦� would further suppress the dissolution of AgCl according to Le Chatelier's principle. This will make AgCl less soluble in 2 M NH鈧凬O鈧�. To summarize, silver chloride is more soluble in 2 M NH鈧� due to the formation of a soluble complex ion, [Ag(NH鈧�)鈧俔鈦�, which removes Ag鈦� ions from the equilibrium and shifts the dissolution equilibrium to the right, while it is less soluble in 2 M NH鈧凬O鈧� due to the lack of free NH鈧� and the presence of a common ion, Cl鈦�.