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ChemistryPrinciples of Instrumental Analysis(a) Interpretation: The electrode potentials calculated from concentrations and activity data should be compared for the Sn(ClO 4 ) 2 ( 3.00 × 10 − 5 M), Sn(ClO 4 ) 4 (6 .00 × 10 − 5 M) | 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.Start your trial now! First week only $4.99!*arrow_forward*

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7th Edition

Douglas A. Skoog + 2 others

Publisher: Cengage Learning

ISBN: 9781305577213

Chapter 22, Problem 22.4QAP

Interpretation Introduction

**(a)**

**Interpretation:**

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

**Concept introduction:**

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

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,

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

Z_{x} − charge on the species X

Ionic strength is defined by the equation,

C_{1}, C_{2}, C_{3} − molar concentrations of various ions in the solution

Z_{1}, Z_{2}, Z_{3} − charges on the ions.

Interpretation Introduction

**(b)**

**Interpretation:**

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

**Concept introduction:**

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

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,

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

Z_{x} − charge on the species X

Ionic strength is defined by the equation,

C_{1}, C_{2}, C_{3} − molar concentrations of various ions in the solution

Z_{1}, Z_{2}, Z_{3} − charges on the ions.