What is the Concentration of Cu^2+(aq) in the solution?Image upload answer is not allowed. 09 Question:A 1.00-L solution contains 2.25×104 M Cu(NO3)2 and 1.00×103 M ethylenediamine (en). The Kf for Cu(en) 22+ is 1.00 × 1020.Cu2+(aq) + 2en(aq) —Cu(en)+(aq)[Cu(en)+]K₁=[Cu²+] [en]²See page 795

Given: [M2+]=2.25x10−4M;[en]=1.00x10−3M;V=1.00LKf=1.00x1020;[Cu2+]=???MStep 1: Solve for the moles…

Answered: 09 Question: A 1.00-L solution contains…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 99QRT

See similar textbooks

Similar questions

QUESTION 6 The free energy change for the formation of the complex ion AlF63− is -140 kJ at 25°C. What is the equilibrium constant for the reaction? Use R = 8.314 J/(K·mol). Report your answer to 3 significant figures in the format of 6.022E23 for 6.022 × 1023.
Calculate the Ksp of AgBr when the concentration of Ag+ is 8.77 x 10-7 M?
Calculate the Ksp for the slightly soluble salt Ce(IO3)4, if at equlibrium, the salt has measured concentration shown: [Ce4+] = 1.8 x 10-4 M [IO3-] = 2.6 x 10-13 M
The formation constants at 25°C of the complex ions, Co(NH3)62+ and Co(EDTA)2–, are 7.70x104 and 2.00x1016, respectively. Answer the questions below.
What is the solubility (in g/L) for PbBr2(s) in a 1.00 L solution that has 251 g Pb(NO3)2 already dissolved in it? The Ksp for PbBr2 is 5.67 × 10-6. If you need more room, use a second sheet.
What is the solubility of Ag(PO₄)₃ in a solution that contains 0.400 M PO₄³⁻ ions? (Ksp of Ag(PO₄)₃ is 8.89 × 10⁻¹⁷) What is the solubility of Ag(PO₄)₃ in a solution that contains 0.500 M Ag⁺ ions? (Ksp of Ag(PO₄)₃ is 8.89 × 10⁻¹⁷)
Find the kps for a saturated solution of Zn(OH)2 in water if it has a pH of 8.35.
A metal complex, [Y(NH3)6]n+, gives a purple color. Suppose that Y is an unknown metal. A 0.0000258 M standard solution was scanned using UV-vis spectrometer, and the data collected is in Image 1. Four more standard solutions were also scanned at a lambda max which is related to the puple color. The data for this is in Image 2. Question: 1. Determine the lambda max used to read the solutions. How was this obtained? 2. Determine the molar absorptivity coefficient of the metal complex at lambda max using the 5 standard solutions. (Suppose that path length = 1 cm)
The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A]=0.100 M, [C]=0.0230 M, and [AC5]=0.100 M. Determine the formation constant, Kf, of AC5. Kf = 155367729.8 The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.152 M. What is the Ksp of AB? Ksp = ?
Potassium perchlorate, KClO4, has a Ksp at 25°C of 1.07 × 10-2 . Compute its solubility in grams per liter of solution.
What concentration of aqueous NH3 is necessary to just start precipitation of Mn(OH)2 from a 0.020 M solution of MnSO4? Kb for ammonia is 1.8 x 10-5, Ksp for Mn(OH)2 is 4.6 x 10-14 1.4 × 10-5 M 3.7 × 10-7 M 1.3 × 10-7 M 1.6 × 10-6 M 8.4 x 10-2 M
If you are able to dissolve 0.015 moles of Cu(CN)2 in a 20.0 L solution, what is the Ksp of Cu(CN)2?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

09 Question: A 1.00-L solution contains 2.25×104 M Cu(NO3)2 and 1.00×103 M ethylenediamine (en). The Kf for Cu(en) 22+ is 1.00 × 1020. Cu2+(aq) + 2en(aq) — Cu(en)+(aq) [Cu(en)+] K₁= [Cu²+] [en]² See page 795