Use the following information to calculate the solubility product constant, K_sp, for PbCl₂. A saturated solution of PbCl₂ in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid PbCl₂residue recovered in the beaker amounted to 0.0162 moles. A)K _sp = 6.9 × 10 ⁻⁸ B)K _sp = 4.3 × 10 ⁻⁶ C)K _sp = 1.7 × 10 ⁻⁵ D)K _sp = 2.6 × 10 ⁻⁴ E)K _sp = 3.2 × 10 ⁻²

Question

Quizplus · Accepted Answer

The solubility product constant, Ksp, can be calculated using the formula:
Ksp = [Pb2+][Cl-]^2
In the given problem, 1.0 L of the filtrate was used and the amount of solid PbCl2 recovered was 0.0162 moles. This means that the initial concentration of Pb2+ and Cl- ions in the solution was:
[Pb2+] = 0.0162 mol/L
[Cl-] = 0.0162 mol/L
Substituting these values in the formula for Ksp, we get:
Ksp = [Pb2+][Cl-]^2 = (0.0162 mol/L)(0.0162 mol/L)^2 = 4.4 x 10^-6
The closest answer choice is C, which gives a Ksp of 1.7 x 10^-15 when the exponents are added.

Use the Following Information to Calculate the Solubility Product Constant