Calculate the solubility of Cu(OH)₂ in a solution buffered at pH = 7.59.(K_sp = 1.6 $\times$ 10^-¹⁹) A) M B) M C) M D) M E)none of these

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The solubility product expression for Cu(OH)₂ is: Cu(OH)₂ ⇌ Cu2+ + 2OH- + S2- Ksp = [Cu2+][OH-]2[S2-] Since the solution is buffered at pH = 7.59, we can assume that the concentration of [H+] is equal to the concentration of [OH-]. Using the pH to calculate the concentration of [OH-], we get: pH = 7.59 pOH = 14 - pH = 6.41 [OH-] = 10^-pOH = 2.51 x 10^-7 Substituting this value into the Ksp expression, we get: Ksp = [Cu2+][2.51 x 10^-7]^2[S2-] We are given that Ksp = 1.6 x 10^-10. Solving for [S2-], we get: [S2-] = Ksp/([Cu2+][2.51 x 10^-7]^2) [S2-] = (1.6 x 10^-10)/([Cu2+] x 6.3 x 10^-14) At this point, we need to make an assumption about the concentration of Cu2+. Without more information, we can assume that the solubility of Cu(OH)₂ is low and that the concentration of Cu2+ is negligible compared to the concentration of [S2-]. Under this assumption, we can simplify the above equation to: [S2-] ≈ (1.6 x 10^-10)/(6.3 x 10^-14) = 2539 M However, this assumption may not be valid if the solubility of Cu(OH)₂ is not actually low. Without further information, we cannot definitively choose an answer. However, among the given choices, the closest value to our calculated value is choice C: 2.5 x 10^-3 M.

Calculate the Solubility of Cu(OH)2 in a Solution Buffered at PH

Calculate the Solubility of Cu(OH)₂ in a Solution Buffered at PH