A saturated Agcl was found to have a concentration of 1.30×10^-5 mol.dm3. The solubility product of Agcl therefore is?
The solubility product constant (Ksp) for AgCl is defined as the equilibrium expression for the dissociation of AgCl in water, which is:
AgCl(s) ⇌ Ag+(aq) + Cl-(aq)
The equilibrium expression for this dissociation is:
Ksp = [Ag+][Cl-]
Given that the concentration of AgCl in water is 1.30×10^-5 mol.dm3 and assuming that this concentration is equal to the concentration of both Ag+ and Cl-, we can substitute these values into the equilibrium expression to solve for Ksp:
Ksp = (1.30×10^-5)(1.30×10^-5) = 1.69 x 10^-10
Therefore, the solubility product constant (Ksp) for AgCl is 1.69 x 10^-10.