1.) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, or -log[Cu2+], in an aqueous solution of NaOH which has a pH of 12.45 and is saturated in Cu(OH)2.3.) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if we were to dissolve 2.52 g of CuCl2 in 1.000 L of a solution 0.946 M in NaCN. The addition of CuCl2 does not alter the volume (the final volume is still 1.000 L).

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Answered: 1.) The solubility product of Cu(OH)2…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.6: Equilibria Involving Complex Ions

Problem 1.3ACP: Use the formation constant of [Au(CN)2] in Appendix K to determine the equilibrium concentration of...

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1.) The solubility product of Cu(OH)₂ is 4.8 x 10^-20. Calculate the value of pCu²⁺, or -log[Cu²⁺], in an aqueous solution of NaOH which has a pH of 12.45 and is saturated in Cu(OH)₂.

3.) The equilibrium constant for the formation of Cu(CN)₄^2- is 2.0 x 10³⁰. Calculate the value of pCu²⁺, or -log[Cu²⁺], if we were to dissolve 2.52 g of CuCl₂ in 1.000 L of a solution 0.946 M in NaCN. The addition of CuCl₂ does not alter the volume (the final volume is still 1.000 L).

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