The complex ion Cu(NH3)4 is formed in a solution made of 0.0500 M Cu(NO3)2 and 0.400 M NH3. What are the 24 concentrations of Cu NH3, and Cu(NH3)4 at equilibrium? 2+ 13 The formation constant*, K₁, of Cu(NH3)4 is 1.70 x 10 [Cu²+] = (NH₂) = .0500 Incorrect [Cu(NH,)*] = 40 Incorrect 1.70 x10¹3 Incorrect M M M

The complex ion Cu(NH3)4 is formed in a solution made of 0.0500 M Cu(NO3)2 and 0.400 M NH3. What are the 24 concentrations of Cu NH3, and Cu(NH3)4 at equilibrium? 2+ 13 The formation constant, K₁, of Cu(NH3)4 is 1.70 x 10 [Cu²+] = (NH₂) = .0500 Incorrect [Cu(NH,)] = 40 Incorrect 1.70 x10¹3 Incorrect M M M

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 64E: In the presence of NH3, Cu2+ forms the complex ion Cu(NH3)42+. If the equilibrium concentrations of...

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In the presence of NH3, Cu2+ forms the complex ion Cu(NH3)42+. If the equilibrium concentrations of Cu2+ and Cu(NH3)42+ are 1.8 1017 M and 1.0 103 M, respectively, in a 1.5-M NH3 solution, calculate the value for the overall formation constant of Cu(NH3)42+. Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)Koverall=?
What is a complex ion? The stepwise formation constants for the complex ion Cu(NH3)42+ are K1 1 103, K2 1 104, K3 = 1 103, and K4 1 103. Write the reactions that refer to each of these formation constants. Given that the values of the formation constants are large, what can you deduce about the equilibrium concentration of Cu(NH3)42+ versus the equilibrium concentration of Cu2+?
Calculate the solubility of copper(II) iodate, Cu(IO3)2 (Ksp = 7.4 108), in (a) water. (b) a 0.10 M copper(II) nitrate solution.
At 25C, 10.24 mg of Cr(OH)2 are dissolved in enough water to make 125 mL of solution. When equilibrium is established, the solution has a pH of 8.49. Estimate Ksp for Cr(OH)2.
Use the formation constant of [Au(CN)2] in Appendix K to determine the equilibrium concentration of Au+(aq) in a solution that is 0.0071 M CN and 1.1 104 M [Au(CN)2]. Is it reasonable to conclude that 100% of the gold in solution is present as the [Au(CN)2] complex ion? Explain.
The solubility of cadmium oxalate. CdC2O4, in 0.150 M ammonia is 6.1 103 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for cadmium oxalate is 1.5 108, what must be the cadmium-ion concentration in the solution? Now calculate the formation constant for the complex ion Cd(NH3)42+.
Solutions of sodium thiosulfate are used to dissolve unexposed AgBr (Ksp = 5.0 1013) in the developing process for black-and-white film. What mass of AgBr can dissolve in 1.00 L of 0.500 M Na2S2O3? Ag+ reacts with S2O32 to form a complex ion: Ag+(aq)+2S2O32(aq)Ag(S2O3)23(aq)K=2.91013
The solubility of zinc oxalate, ZnC2O4, in 0.0150 M ammonia is 3.6 104 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for zinc oxalate is 1.5 109, what must be the zinc-ion concentration in the solution? Now calculate the formation constant for the complex ion Zn(NH3)42+.
Predict whether nickel(II) hydroxide, Ni(OH)2, will precipitate from a solution that is 0.0020 M NiSO4, 0.010 M NaOH, and 0.10 M NH3. Note that nickel(II) ion forms the Ni(NH3)62+ complex ion.
In the presence of CN, Fe3+ forms the complex ion Fe(CN)63. The equilibrium concentrations of Fe3+ and Fe(CN)63 are 8.5 1040 M and 1.5 103 M, respectively, in a 0.11-M KCN solution. Calculate the value for the overall formation constant of Fe(CN)63. Fe3+(aq)+6CN(aq)Fe(CN)63(aq)Koverall=?
Tooth enamel is composed of the mineral hydroxyapatite. The Ksp of hydroxyapatite, Ca5(PO4)3OH, is 6.8 1037. Calculate the solubility of hydroxyapatite in pure water in moles per liter. How is the solubility of hydroxyapatite affected by adding acid? When hydroxyapatite is treated with fluoride, the mineral fluorapatite, Ca5(PO4)3F, forms. The Ksp of this substance is 1 1060. Calculate the solubility of fluorapatite in water. How do these calculations provide a rationale for the fluoridation of drinking water?

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