(Q88) The following redox reaction Cr3+ (aq) + Fe (s) ---> Cr (s) + Fe3+ (aq) will be: The reduction potentials for the two half-reactions involved are: Cr3+ + 3 e- --> Cr (s) (E°RED) = -0.73 V Fe3+ + 3 e- --> Fe (s) (E°RED) = -0.036 V O Spontaneous O Nonspontaneous

(Q88) The following redox reaction Cr3+ (aq) + Fe (s) ---> Cr (s) + Fe3+ (aq) will be: The reduction potentials for the two half-reactions involved are: Cr3+ + 3 e- --> Cr (s) (E°RED) = -0.73 V Fe3+ + 3 e- --> Fe (s) (E°RED) = -0.036 V O Spontaneous O Nonspontaneous

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.20QAP

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What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
The cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode has a potential of —0.2094 V when the solution in the right-hand compartment is a buffer of pH 4.006. The following potentials are obtained when the buffer is replaced with unknowns: (a) —0.2806 V and (b) —0.2132 V. Calculate the pH and the hydrogen ion activity of each unknown. (c) Assuming anuncertainty of 0.001 Vin the junction potential, what is the range of hydrogen ion activities withinwhich the true value might be expected to lie?
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The standard reduction potential of the permanganate ion, MnO4-, to Mn2+ is 1.51 volt, when it takes place in an acidic aqueous solution. The normal reduction potentials of ions Zn2+, Ag+ and Au+ are, respectively, 0.7618, 0.7992 and 1.692 V (in aqueous solution).Introducing a Pt electrode in a MnO4-/ Mn2+ solution, with a salt bridge, and putting it together with the other electrodes (Zn, Au or Ag) and their aqueous solutions,a) Comment in which case will the permanganate oxide the metalsb) Justify your answerc) In those cases where the oxidation takes place, write the diagram of the celld) Calculate the standard potential of the cells, Eºcell. Result: a) Eºcell >0 d) 0.7108 V, 0.7482 V
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An aqueous solution of an unknown salt of ruthenium Is electrolyzed by a current of 2.70A passion for 20.0min. If 1.132g of Ru is produced at the cathode, what js the charge on the ruthenium ions in solution?
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