The solubility of AgCl is 0.000013 mol/L. Calculate the Ksp for AgCl
..........AgCl ==> Ag^+ + Cl^-
equil.............1.3E-5...1.3E-5
Substitute into Ksp expression and solve for Ksp.
To calculate the Ksp (solubility product constant) for AgCl (silver chloride), we need to know the molar solubility of AgCl. The molar solubility is given as 0.000013 mol/L.
The formula for Ksp is as follows:
Ksp = [Ag+][Cl-]
In this formula, [Ag+] represents the concentration of silver ions (Ag+) and [Cl-] represents the concentration of chloride ions (Cl-).
Since AgCl dissolves to form Ag+ and Cl- in a 1:1 ratio, the concentration of Ag+ and Cl- will be the same.
Therefore, we can substitute the molar solubility, 0.000013 mol/L, for both [Ag+] and [Cl-] in the Ksp formula:
Ksp = (0.000013 mol/L) x (0.000013 mol/L)
Simplifying this expression, we get:
Ksp = 1.69 x 10^-10
Therefore, the Ksp for AgCl is 1.69 x 10^-10.
To calculate the Ksp (solubility product constant) for AgCl, you can start by writing the balanced chemical equation for the dissolution of AgCl in water:
AgCl(s) ↔ Ag+(aq) + Cl-(aq)
The Ksp expression for AgCl is given by:
Ksp = [Ag+][Cl-]
You are given the value of solubility for AgCl, which is 0.000013 mol/L. Since AgCl dissociates into Ag+ and Cl-, the concentration of Ag+ and Cl- will be the same as the solubility.
Therefore, [Ag+] = [Cl-] = 0.000013 mol/L.
Now, substitute these values into the Ksp expression:
Ksp = (0.000013)(0.000013) = 1.69 x 10^-10 mol^2/L^2
Therefore, the Ksp for AgCl is 1.69 x 10^-10 mol^2/L^2.
Remember that when performing calculations involving the Ksp, make sure to use the proper units and significant figures, and check if any additional information is provided.