A precipitate of AgCl is formed when equal volumes of 10-5AgNO3 and 10-4 MHCl are mixed together.
The ionic product must be greater than the solubility product for an electrolyte to precipitate.
[AgNO3] = [Ag+] = 10-4 /2M
[HCl] = [Cl-] = 10-4 /2M
Qsp = [Ag+] [Cl-] = 2.5x10-9
Ksp = 10-10
Qsp>Ksp
This conclusion leads to the AgCl precipitation.
Silver chloride is a well-known chemical compound in chemistry that appears as a white crystalline solid. It also goes by the name Silver Monochloride, and its chemical formula is AgCl. The substance is a mineral known as chlorargyrite that naturally exists in the environment. This substance has an extremely low solubility power in water, which makes it difficult to dissolve.
It is crucial to remember that due to its decreased affinity for water, it is also not soluble in other fluids like alcohol or any diluted acids. Silver chloride begins to decompose and transform into silver and chlorine when heated or when exposed to light. The compound changing from a greyish tone to black or a shade of purple makes this easy to spot.
An anion (Cl-) and a cation (Ag+) make up the chemical structure of this inorganic salt. Ammonia, sulphuric acids, hydrochloride, and potassium bromide solution all readily dissolve this substance. Silver chloride is particularly photosensitive and has a variety of applications in photography.