An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered. Concept introduction: The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes. The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation. The value of E cell is calculated using Nernst formula, E = E ° − ( R T n F ) ln ( Q ) At room temperature the above equation is specifies as, E = E ° − ( 0.0591 n ) log ( Q ) To determine: The potential of the cell at 25 ° C if a nickel metal electrode immersed in a solution with a given concentration and is separated by a porous disk from an aluminum metal electrode.

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Chapter 18, Problem 78E

(a)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

To determine: The potential of the cell at 25 °C if a nickel metal electrode immersed in a solution with a given concentration and is separated by a porous disk from an aluminum metal electrode.

(b)

Interpretation Introduction

Interpretation:

An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.

Concept introduction:

The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.

The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.

The value of Ecell is calculated using Nernst formula,

E=E°−(RTnF)ln(Q)

At room temperature the above equation is specifies as,

E=E°−(0.0591n)log(Q)

To determine: The value of concentration of Al3+ at the given measured potential.

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