how can AgCl(s) be dissolved completely? write an equation for the reaction

AgCl(s) + 2NH3(aq) ==>Ag(NH3)2Cl(aq) ==> Ag(NH3)2^+(aq) + Cl^-(aq)

To dissolve AgCl(s) completely, you need to use a suitable solvent that can break down the bonds between the silver (Ag) and chloride (Cl) ions in the solid compound. In this case, water (H2O) is commonly used as the solvent. Here's the equation for the dissolution of AgCl(s) in water:

AgCl(s) + H2O(l) → Ag+(aq) + Cl-(aq)

In this equation, (s) denotes a solid state, (l) represents a liquid state, and (aq) signifies an aqueous solution where the Ag+ and Cl- ions are solvated by water molecules.

By dissolving AgCl in water, the AgCl crystal lattice breaks apart, and the individual Ag+ and Cl- ions become separated and dispersed throughout the solution. This process is commonly known as dissociation or ionization.

It's important to note that not all ionic compounds are soluble in water or other solvents. The solubility of a compound depends on various factors such as the nature of the compound, temperature, and the solvent used.