suppose you are given the following experimentally observed facts regarding the reactions of silver ion.

(a) Ag+ reacts w/ Cl- to give white AgCl (s)
(b) Ag+ reacts with ammonia to give a quite stable complex ion, Ag(NH3)2+
(c) a black suspension of solid silver oxide, Ag2O(s), shaken with NaCl solution, changes to white AgCl(s).
(d) AgCl(s) will dissolve when ammonia solution is added, but AgI(s) does not dissolve under these conditions.

What is the question?

Write equations for any net reacts in the cases above; then, based on these observations, arrange each of the substances AgCl, AgI, Ag2O, and Ag(NH3)2 + in such an order that their solutions with water would give a successively decreasing concentration of Ag+.

How much of this do you not understand? That is, how much can you do. Show what you don't understand. I'm not likely to spend a lot of time writing equation you already know how to do.

You're a jerk unknownuser.

Get some manners.

To explain the given experimental facts regarding the reactions of silver ion, let's break down each fact and understand it one by one:

(a) Ag+ reacts with Cl- to give white AgCl(s)
To determine why this reaction occurs, we need to consider the solubility rules for ionic compounds. AgCl is a white solid because it has low solubility in water. When Ag+ reacts with Cl-, they form a precipitate known as AgCl(s), which is insoluble in water. The formation of a white precipitate indicates the formation of AgCl in the reaction.

(b) Ag+ reacts with ammonia to give a quite stable complex ion, Ag(NH3)2+
In this reaction, Ag+ forms a complex ion with ammonia (NH3). Complex ions are formed when a central metal ion is surrounded by ligands (in this case, ammonia molecules). The complex ion formed is Ag(NH3)2+, which is quite stable. This reaction occurs because ammonia has a lone pair of electrons, which can donate to the empty orbital of Ag+ to form the complex ion.

(c) A black suspension of solid silver oxide, Ag2O(s), shaken with NaCl solution, changes to white AgCl(s)
When solid silver oxide (Ag2O) is shaken with NaCl solution, it reacts to form AgCl(s) and water. This reaction occurs due to the higher reactivity of chloride ions (Cl-) compared to oxide ions (O2-). Chloride ions displace oxide ions from Ag2O, resulting in the formation of white AgCl(s) and water.

(d) AgCl(s) will dissolve when ammonia solution is added, but AgI(s) does not dissolve under these conditions
AgCl is soluble in ammonia solution because it forms a soluble complex ion with ammonia, known as [Ag(NH3)2]+. The ammonia molecules in the solution coordinate with Ag+ ions, causing the AgCl(s) to dissolve. On the other hand, AgI does not dissolve in ammonia solution because the formation of a stable complex ion with I- is less favorable compared to Cl-. Therefore, AgI(s) remains insoluble under these conditions.

In summary, the given experimental facts demonstrate different reactions involving silver ions (Ag+). The reactions demonstrate the formation of AgCl(s) and Ag(NH3)2+ complex ion, as well as the insolubility of AgI(s) in ammonia solution. These reactions can be understood by considering the solubility rules and the ability of different ligands to coordinate with silver ions.