A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a solution of ZnSO4. The Zn wire is attached to the positive terminal and the Ag/AgCl electrode is attached to the negative terminal of the potentiometer. Calculate the [Zn²+] in the solution if the cell potential, E cell, is -1.060 V. The standard reduction potential of the Zn²+/Zn half- reaction is -0.762 V. [Zn²+] = M

Q: A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a…

A: We will calculate the concentration of Zn2+ ion by using Nernst Equation.

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Q: A ZnZn wire and Ag/AgCl reference electrode saturated with KCl (?=0.197 V) are placed into a…

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A: Using Nerst equation  Ecell  = Eocell - (0.0591/n ) log [ Zn2+ ]/[ Cu2+ ]

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Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

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Q: The standard reduction potentials for Mg2+/Mg (E'= -2.37 V) and Fe2*/Fe (E'= -0.44 V). When a piece…

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Q: The cell notation for the Galvanic cell is              A(s)/A2+//B2(s)/B- The Standard Reduction…

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A: GALVANIC CELL: It is a type of an electrochemical cell which is utilized to provide electricity by…

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Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.2 M NISO4 solution…

A:

Q: Calculate the potential measured for the following cell at 298 K. Cr(s) | Cr3*(aq) (0.0055 M) ||…

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Q: A Zn wire and Ag/AgCl reference electrode saturated with KCl (E = 0.197 V) are placed into a…

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Q: Which of the following reactions occurs at the anode of an electrochemical cell composed of…

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