   # An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which [Cu 2+ ] = 2.5 × 10 −4 M? b. The copper electrode is placed in a solution of unknown [Cu 2+ ]. The measured potential at 25°C is 0.195 V. What is [Cu 2+ ]? (Assume Cu 2+ is reduced.) ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 17, Problem 79E
Textbook Problem
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## An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode.a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which [Cu2+] = 2.5 × 10−4 M?b. The copper electrode is placed in a solution of unknown [Cu2+]. The measured potential at 25°C is 0.195 V. What is [Cu2+]? (Assume Cu2+ is reduced.)

(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 the copper electrode is placed in a given concentration of solution.

### Explanation of Solution

Given

The concentration of Cu2+ is 2.5×104M

The reaction taking place on cathode,

Cu2++2eCuE°red=0.34V

The reaction taking place at anode,

H22H++2eE°ox=0.00V

Add both the reduction half and oxidation half-reaction.

Cu2++2eCuH22H++2e

The overall cell reaction is,

Cu2++H2Cu+2H+

The overall cell potential is calculated as,

E°cell=E°ox+E°red=0.00V+(0

(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 Cu2+ at the given measured potential.

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