6. Suppose you wish to separate Cd²+ from Zn²+ by electrodeposition of metallic cadmium onto an inert cathode from an aqueous solution containing 0.015 M Cd(NH3)4²+, 0.010 M Zn(NH3)4²+, and 1.00 M uncomplexed NH3. You want to deposit 99.99% of the Cd while not depositing any Zn. What is the allowable range of potentials that you can use? Cd(NH3)4²+ + 2 e Cd(s) + 4 NH3 Zn(NH3)4²+ + 2e = Zn(s) + 4 NH3 E = -0.61 V vs. SHE E = -1.04 V vs. SHE

6. Suppose you wish to separate Cd²+ from Zn²+ by electrodeposition of metallic cadmium onto an inert cathode from an aqueous solution containing 0.015 M Cd(NH3)4²+, 0.010 M Zn(NH3)4²+, and 1.00 M uncomplexed NH3. You want to deposit 99.99% of the Cd while not depositing any Zn. What is the allowable range of potentials that you can use? Cd(NH3)4²+ + 2 e Cd(s) + 4 NH3 Zn(NH3)4²+ + 2e = Zn(s) + 4 NH3 E = -0.61 V vs. SHE E = -1.04 V vs. SHE

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A Cu electrode is immersed in a solution that is 1.00 Min [Cu(NH3)4]2+ and 1.00 M in NH3. When the cathodeis a standard hydrogen electrode, the emf of the cell isfound to be +0.08 V. What is the formation constant for[Cu(NH3)4]2+?
We construct a cell in which identical copper electrodes are placed in two solutions Solution A contains 0.75 M Cu 2+ . Solution B contains Cu 2+ at some concentration known to be lower than that in solution A. The potential of the cell is observed to be 0.040 V. What is [Cu 2+ ] in solution B ?
Use the standard reduction potentials given below to predict if a reaction will occur when Fe metal is put into a 1 M aqueous Cd²+ solution. Cd²+ red (aq) + 2e¯ → Cd(s) Ee Fe²+ (aq) + 2e → Fe(s) E red If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) -0.403 V -0.440 V + +
calculate the mass of chromium that can be deposited by electrolysis of an aqueous solution of chromium(III) sulfate, Cr 2(SO 4) 3, for 180 min using a constant current of 11.0 A. Assume 100% current efficiency. (F = 96485 C/mol)
5. With the help of the table of standard reduction potentials, Calculate the E of the reaction between Chromium (II) ions and Tin (IV) ions forming Chromium (III) ions and tin (II) ions.
8. Mass determination by electroplating. What mass of copper metal is deposited if a 5.12 A current is passed through a Cu(NO3)2solution for 10 hr.
29b
(III) ion? 6. The sulfite ions, SO;², is strong reducing agent. a. Balance the following half reaction: SO,² > SO,² (under acidic conditions) D. Write out the balanced reaction for the reduction of Fe*3 to Fe*2 with SO,² reducing agent. 7. Iron(II) compounds in foods are more easily absorbed by the body than iron(III) compounds. Based on the experiment, why is adequate amounts of Vitamin C necessary for good health? Experiment 9 0xidation and Rodusti
Standard Reduction Potentials at 25 °C Half-reaction. Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e →→Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Aut 2Au + Au³+ Will Au* disproportionate in aqueous solution? To justify your answer, what is the standard cell voltage for the disproportionation reaction?
9.)
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.
Which of the following is expected to have the largest magnitude of standard reduction potential (i.e. most easily reduced)? Consider 1 M concentration of starting Cu species. O a. Cu+2 +2e- ==> Cu(0) O b. Cu(NH3)2+2 +2e- ==> Cu(0) +2 O c. Cu(en)₂+² +2e- ==> Cu(0) O d. Cu(OH₂)2(0x)+2 +2e- ==> Cu(0)