(a) Interpretation: The electrode potentials calculated from concentrations and activity data should be compared for the HCl(0 .0200 M), NaCl(0 .0300 M)|H 2 (1 .00 atm), Pt half cell. Concept introduction: Nernst equation gives the cell potential under non-standard conditions. E = E 0 − 2.303 R T n F log K E − cell potential E 0 − standard cell potential R − universal gas constant T − temperature in Kelvin n − number of electrons transferred F − Faraday constant K − equilibrium constant Activity a x of species X is given by, a x = γ x [ X ] γ x - activity coefficient [ X ] - concentration of X Activity coefficient of ions can be calculated by Debye-Huckel equation, − log γ x = 0.509 Z x 2 μ 1 + 3.28 α x μ Z x − charge on the species X μ - ionic strength of the solution α x - the effective diameter of the hydrated ion in nanometers. Ionic strength is defined by the equation, μ = 1 2 ( c 1 Z 1 2 + c 2 Z 2 2 + c 3 Z 3 2 + ..... ) C 1 , C 2 , C 3 − molar concentrations of various ions in the solution Z 1 , Z 2 , Z 3 − charges on the ions.

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 22, Problem 22.3QAP
Interpretation Introduction

(a)

Interpretation:

The electrode potentials calculated from concentrations and activity data should be compared for the

HCl(0.0200 M), NaCl(0.0300 M)|H2(1.00 atm), Pt half cell.

Concept introduction:

Nernst equation gives the cell potential under non-standard conditions.

E=E02.303RTnFlogK

E − cell potential

E0 − standard cell potential

R − universal gas constant

T − temperature in Kelvin

n − number of electrons transferred

F − Faraday constant

K − equilibrium constant

Activity ax of species X is given by,

ax=γx[X]

γx - activity coefficient

[X] - concentration of X

Activity coefficient of ions can be calculated by Debye-Huckel equation,

logγx=0.509Zx2μ1+3.28αxμ

Zx − charge on the species X

μ - ionic strength of the solution

αx - the effective diameter of the hydrated ion in nanometers.

Ionic strength is defined by the equation,

μ=12(c1Z12+c2Z22+c3Z32+.....)

C1, C2, C3 − molar concentrations of various ions in the solution

Z1, Z2, Z3 − charges on the ions.

Interpretation Introduction

(b)

Interpretation:

The electrode potentials calculated from concentrations and activity data should be compared for the Fe(ClO4)2(0.0111 M), Fe(ClO4)3(0.0111 M)|Pt half cell.

Concept introduction:

Nernst equation gives the cell potential under non-standard conditions.

E=E02.303RTnFlogK

E − cell potential

E0 − standard cell potential

R − universal gas constant

T − temperature in Kelvin

n − number of electrons transferred

F − Faraday constant

K − equilibrium constant

Activity ax of species X is given by,

ax=γx[X]

γx - activity coefficient

[X] - concentration of X

Activity coefficient of ions can be calculated by Debye-Huckel equation,

logγx=0.509Zx2μ1+3.28αxμ

Zx − charge on the species X

μ - ionic strength of the solution

αx - the effective diameter of the hydrated ion in nanometers.

Ionic strength is defined by the equation,

μ=12(c1Z12+c2Z22+c3Z32+.....)

C1, C2, C3 − molar concentrations of various ions in the solution

Z1, Z2, Z3 − charges on the ions.

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