
(a)
Interpretation:
The Nernst equation for given cell has to be written.
Concept introduction:
Nernst Equation:
For Half-reaction,
The Nernst equation results in the half-cell potential E as,
Here,
T =Temperature (in K)
N = number of electrons in half-reaction
F = Faraday constant (
A = Activity of species, i
The voltage of a battery is calculated as
Cell voltage = potential of right hand electrode (
(a)

Explanation of Solution
To write: The Nernst equation for given cell.
(b)
Interpretation:
The cell voltage for the given cell and direction of flow of electrons have to be determined.
Concept introduction:
Nernst Equation:
For Half-reaction,
The Nernst equation results in the half-cell potential E as,
Here,
T =Temperature (in K)
N = number of electrons in half-reaction
F = Faraday constant (
A = Activity of species, i
The voltage of a battery is calculated as
Cell voltage = potential of right hand electrode (
(b)

Explanation of Solution
To determine: The cell voltage for the given cell and direction of flow of electrons.
The concentration of silver ion is calculated using solubility product
The cell voltage is determined as
The flow of electron from right hand electrode silver to left hand electrode platinum because the cell voltage is positive.
(c)
Interpretation:
The standard reduction potential by deriving Nernst equation has to be determined.
Concept introduction:
Nernst Equation:
For Half-reaction,
The Nernst equation results in the half-cell potential E as,
Here,
T =Temperature (in K)
N = number of electrons in half-reaction
F = Faraday constant (
A = Activity of species, i
The voltage of a battery is calculated as
Cell voltage = potential of right hand electrode (
(c)

Explanation of Solution
To determine: The standard reduction potential by deriving Nernst equation.
Applying the cell voltage in Nernst equation, the standard electrode potential is calculated as
The appendix value
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Chapter 14 Solutions
Quantitative Chemical Analysis
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