(a) Interpretation: The cathode potential required to lower the Hg ( II ) concentration of an aqueous solution of Hg 2 + to 1.00 × 10 − 6 M is to be stated. Concept introduction: To calculate the total voltage of an electrochemical cell the Nernst equation is used. It can also be used to calculate the reduction potential of half cell in an electrochemical cell.

BuyFind

Principles of Instrumental Analysis

7th Edition
Douglas A. Skoog + 2 others
Publisher: Cengage Learning
ISBN: 9781305577213
BuyFind

Principles of Instrumental Analysis

7th Edition
Douglas A. Skoog + 2 others
Publisher: Cengage Learning
ISBN: 9781305577213

Solutions

Chapter 24, Problem 24.5QAP
Interpretation Introduction

(a)

Interpretation:

The cathode potential required to lower the Hg(II) concentration of an aqueous solution of Hg2+ to 1.00×106M is to be stated.

Concept introduction:

To calculate the total voltage of an electrochemical cell the Nernst equation is used. It can also be used to calculate the reduction potential of half cell in an electrochemical cell.

Interpretation Introduction

(b)

Interpretation:

The cathode potential required to lower the Hg(II) concentration of an solution with an equilibrium SCN to 1.00×106M is to be stated.

Concept introduction:

To calculate the total voltage of an electrochemical cell the Nernst equation is used. It can also be used to calculate the reduction potential of half cell in an electrochemical cell.

Interpretation Introduction

(c)

Interpretation:

The cathode potential required to lower the Hg(II) concentration of a solution with an equilibrium Br concentration of 0.100M to 1.00×106M is to be stated.

Concept introduction:

To calculate the total voltage of an electrochemical cell the Nernst equation is used. It can also be used to calculate the reduction potential of half cell in an electrochemical cell.

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