Silver Sulfate Ksp

Silver sulfate (Ag2SO4) is an ionic compound that is sparingly soluble in water. When silver sulfate dissolves in water, it dissociates into its constituent ions: Ag+ and SO42-.

The solubility of silver sulfate in water can be expressed using the equilibrium constant Ksp, which is defined as the product of the concentrations of the dissolved ions raised to their stoichiometric coefficients.

The expression for the Ksp of silver sulfate is:

Ksp = [Ag+]^2[SO42-]

where [Ag+] and [SO42-] are the molar concentrations of the silver and sulfate ions in solution, respectively.

At a given temperature, the Ksp value of silver sulfate represents the maximum concentration of the ions that can coexist in equilibrium with the solid phase without precipitation occurring. If the ion concentrations exceed the Ksp value, then silver sulfate will start to precipitate out of solution until equilibrium is reestablished.

Experimental measurements of the Ksp value of silver sulfate at different temperatures have been reported in the literature. At room temperature (25°C), the reported Ksp values range from 1.4 x 10^-5 to 1.3 x 10^-5 mol^2/L^2, depending on the source of the data.

It is important to note that the Ksp value of silver sulfate can be affected by various factors such as temperature, pH, ionic strength, and the presence of other ions or complexing agents in solution. Therefore, accurate determination of the Ksp value requires careful experimental design and rigorous data analysis.