The K_sp for Cu(OH)₂ is 4.8 × 10^-20.Determine the molar solubility of Cu(OH)₂ in a buffer solution with a pH of 10.1. A)6.0 × 10^-10 B)7.6 C)3.0 × 10^-12 D)2.2 × 10^-10 E)3.8 × 10^-16

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Quizplus · Accepted Answer

The molar solubility of Cu(OH)2 in a buffer solution with a pH of 10.1 can be calculated using the Ksp and the given pH. The Ksp of Cu(OH)2 is 4.8 × 10^-20. At pH 10.1, the concentration of OH- ions ([OH-]) can be found from the pH by first finding the pOH (14 - 10.1 = 3.9) and then calculating [OH-] = 10^-pOH = 10^-3.9. The solubility of Cu(OH)2 in such a solution is governed by the reaction Cu(OH)2(s) ⇌ Cu^2+(aq) + 2OH^-(aq), with the solubility product Ksp = [Cu^2+][OH^-]^2. Given the excess OH- from the buffer, the [OH^-] is essentially constant and determined by the buffer's pH, simplifying the calculation to finding the [Cu^2+] that satisfies the Ksp under these conditions. The correct calculation leads to a molar solubility of 3.0 × 10^-12 M, making option C the correct answer.

The Ksp for Cu(OH)2 Is 4

The K_sp for Cu(OH)₂ Is 4