12-6. Calculate the potential of the following cells:(a) a galvanic cell consisting of a lead electrodeimmersed in 0.0848 M Pb2 and a zineelectrode in contact with 0.1364 M Zn+.(b) a galvanic cell consisting of a standardhydrogen electrode and a platinum elec-trode immersed in a solution that is 1.46 X10- M in TiO+,0.02723 M in Ti-, andbuffered to a pH of 3.00.

Cell potential : It is the measure of potential difference of constituting half cells in any…

12-6. Calculate the potential of the following cells: (a) a galvanic cell consisting of a lead electrode immersed in 0.0848 M Ph and a zine electrode in contact with 0.1364 M Zn²*. (b) a galvanic cell consisting of a standard hydrogen electrode and a platinum elec- trode immersed in a solution that is 1.46 X 10- M in TiO,0.02723 M in Ti-, and buffered to a pH of 3.00.

12-6. Calculate the potential of the following cells: (a) a galvanic cell consisting of a lead electrode immersed in 0.0848 M Ph and a zine electrode in contact with 0.1364 M Zn²*. (b) a galvanic cell consisting of a standard hydrogen electrode and a platinum elec- trode immersed in a solution that is 1.46 X 10- M in TiO,0.02723 M in Ti-, and buffered to a pH of 3.00.

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 50QRT

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Similar questions

The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.
At what pH does Ecell = 0.00 V for the reduction of dichromate by iodide ion in acid solution, assuming standard-state concentrations of all species except H+ ion?
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-.
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1, calculate the equilibrium constant at 25C for the reaction A13+(aq)+6F(aq)A1F63(aq)K=?
From the standard potentials Tl++eTl(s)E0=0.336V TlCl(s)+eTl(s)+ClE0=0.557V calculate the solubility product constant for TlCl.
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)
What is the cell potential of the following cell at 25C? Ni(s)Ni2+(1.0M)Sn2(1.5104M)Sn(s)
From the standard potentials Ag2SeO4(s)+2e2Ag(s)+SeO42-E0=0.355V Ag++2eAg(s)E0=0.799V calculate the solubility product constant for Ag2SeO4.