sorry Ksp of PbCl2 is 1.6 x 10-5
Answered below.
No problem! The Ksp is the equilibrium constant for the solubility product expression. In the case of PbCl2, it represents the equilibrium between the dissolved lead(II) chloride ions (Pb2+ and 2Cl-) and the solid PbCl2.
To find the value of the solubility product constant (Ksp) for PbCl2, you need to know the concentration of the dissolved lead(II) chloride ions in a saturated solution of PbCl2.
The given value of 1.6 x 10^-5 is the numerical value of Ksp for PbCl2. The smaller the value of Ksp, the less soluble the compound is in water. In this case, PbCl2 is relatively insoluble in water.
To calculate the equilibrium concentrations of the ions in a saturated solution, you can use an ICE (Initial, Change, Equilibrium) table. Assuming x represents the concentration of Pb2+ and 2x represents the concentration of Cl- ions in the saturated solution, you can set up the following equation:
PbCl2 (s) ⇌ Pb2+ (aq) + 2Cl- (aq)
Ksp = [Pb2+] x [Cl-]^2
Substituting the values into the equation, we have:
1.6 x 10^-5 = (x) x (2x)^2
Simplifying the equation, we get:
1.6 x 10^-5 = 4x^3
Solving for x, we find:
x = (1.6 x 10^-5 / 4)^(1/3)
Evaluating the expression, we get:
x ≈ 0.0347
Thus, the concentration of Pb2+ in a saturated solution of PbCl2 is approximately 0.0347 M.
Please note that this calculation assumes 100% dissociation of PbCl2. In reality, it may not be completely dissociated.