Questions and Answers
What is the characteristic of an oxidant in a redox system?
It is a weak conjugate reductant
What happens when an inert electrode is placed in a redox system with oxidizing properties?
It becomes positively charged
What is the purpose of the Nernst equation in redox systems?
To relate the oxidation potential to the concentration of both oxidant and reductant
Which of the following is an example of a redox system?
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What is the significance of the standard oxidation potential?
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What is the role of the platinum electrode in determining the standard oxidation potential?
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What is the relationship between the oxidant and its conjugate reductant?
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What is the effect of concentration on the oxidation potential of a redox system?
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What is the significance of the equilibrium in a redox system?
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What is the purpose of the half cell in determining the standard oxidation potential?
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Study Notes
Equivalent Weight
- Equivalent weight of a salt = molecular weight / number of cations x its valency or molecular weight / number of anions x its valency
- Example: Na2SO4, equivalent weight = molecular weight / 2 x 1 or molecular weight / 1 x 2
Equivalent Weight of Oxidant and Reductant
- Equivalent weight of oxidant or reductant = molecular weight / number of electrons gained or lost in the reaction
- Example: MnO4-, equivalent weight = molecular weight / 5; Fe2+, equivalent weight = molecular weight / 1
Redox Reactions
- Redox reactions involve transfer of electrons
- Electric current is essentially a transfer of electrons
- During redox reactions, a certain amount of electricity is transferred from the reductant to the oxidant
Electrochemical Properties
- Electrode potential: a certain potential difference is set up between the metal rod and the solution
- Electrolytic solution pressure: tendency of the metal to dissolve
- Ionic pressure: passage of metal cations from the solution to be deposited on the metal
- Prevailing tendency depends on the chemical nature of the system and the concentration of the solute present
Standard Oxidation Potential
- Standard oxidation potential: e.m.f. produced when a half cell consisting of an inert electrode dipped in a solution of equal concentration of both the oxidized and reduced form of a system
- Nernst equation for oxidation potential: E 25°C = Eo + 0.0591/n Log [Ox] / [Red]
- The magnitude of the potential is a measure of the oxidizing or reducing properties of the system
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