It is desired to separate silver in a solution that is 0.0481 M BiO+, 0.119 M Cu²+, 0.0916 M Ag+, and 0.500 M HCIO, by controlled-potential electrolysis. Ag+ (aq) + 1e → Ag(s) E = 0.799 V Cu²+ + 2e → Cu(s) E = 0.337 V BIO+ (aq) + 2 H+ (aq) + 3 e¯ →→→ Bi(s) + H₂O(1) E = 0.320 V Between what cell potentials can silver be quantitatively removed from the solution without also removing one of the othe ions using controlled-potential electrolysis? Use 1.00 x 10-6 M as the criterion for quantitative removal. Report all cell potentials versus Ag|AgCl (E = 0.197 V). List the higher (more positive) potential first. between Ecell = V and Ecell = =

It is desired to separate silver in a solution that is 0.0481 M BiO+, 0.119 M Cu²+, 0.0916 M Ag+, and 0.500 M HCIO, by controlled-potential electrolysis. Ag+ (aq) + 1e → Ag(s) E = 0.799 V Cu²+ + 2e → Cu(s) E = 0.337 V BIO+ (aq) + 2 H+ (aq) + 3 e¯ →→→ Bi(s) + H₂O(1) E = 0.320 V Between what cell potentials can silver be quantitatively removed from the solution without also removing one of the othe ions using controlled-potential electrolysis? Use 1.00 x 10-6 M as the criterion for quantitative removal. Report all cell potentials versus Ag|AgCl (E = 0.197 V). List the higher (more positive) potential first. between Ecell = V and Ecell = =

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 120AE

See similar textbooks

Similar questions

At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)
What is the standard cell potential you would obtain from a cell at 25C using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3(aq)?
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)
An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Cu2+(aq)+Ni(s)Cu(s)+Ni2+(aq) (b) 2Ag(s)+Cl2(g)2AgCl(s) (c) Cl2(g)+2I(aq)2Cl(aq)+I2(s)
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
The cell potential of the following cell at 25C is 0.480 V. ZnZn2+(1M)H+(testsolution)H2(1atm)Pt What is the pH of the test solution?
Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)