Nacl is soluble in water but AgCl is not, why?

The dissolvability of ionic mixtures like NaCl and AgCl in not entirely settled by the harmony between the energy expected to break the ionic bonds in the strong and the energy delivered when the particles connect with water atoms.

On account of NaCl, the ionic connections between the Na+ and Cl-particles are generally powerless and effectively broken by the polar water particles, which have a fractional positive charge on the hydrogen iotas and an incomplete negative charge on the oxygen molecule. The water atoms encompass the isolated Na+ and Cl-particles and balance out them in arrangement through particle dipole associations. Therefore, NaCl is exceptionally solvent in water.

Conversely, AgCl has a lot more grounded ionic connections between the Ag+ and Cl-particles, which require more energy to break. At the point when AgCl is added to water, the water particles can’t give sufficient energy to break areas of strength for the bonds in the strong. Thus, the Ag+ and Cl-particles remain firmly bound in the strong and don’t disintegrate in water. Therefore AgCl is insoluble in water.

Another variable that adds to the insolubility of AgCl in water is the low solvation energy of Ag+ particles contrasted with Na+ particles. The hydration energy of Ag+ particles is not exactly that of Na+ particles, and that implies that the connection between Ag+ particles and water atoms is more vulnerable than that between Na+ particles and water particles. This makes it more hard for the water atoms to conquer serious areas of strength for the bonds in AgCl and disintegrate the compound in water