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 PbCl₂ residue 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

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Quizplus · Accepted Answer

The solubility of PbCl2 is 0.0162 M. The dissolution equation is PbCl2 ⇌ Pb^2+ + 2Cl^-. Therefore, [Pb^2+] = 0.0162 M and [Cl^-] = 2 × 0.0162 M = 0.0324 M. Ksp = [Pb^2+][Cl^-]^2 = (0.0162)(0.0324)^2 = 1.7 × 10^-5.

Use the Following Information to Calculate the Solubility Product Constant