Calculating Equivalent Weight of Salts and Redox Reactions
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Questions and Answers

What is the characteristic of an oxidant in a redox system?

  • It is a weak reductant
  • It is a strong conjugate reductant
  • It is a powerful reductant
  • It is a weak conjugate reductant (correct)

    • What happens when an inert electrode is placed in a redox system with oxidizing properties?

  • It becomes positively charged (correct)
  • It becomes neutral
  • It becomes negatively charged
  • It remains neutral

    • What is the purpose of the Nernst equation in redox systems?

  • To measure the reducing properties of the system
  • To relate the oxidation potential to the concentration of both oxidant and reductant (correct)
  • To calculate the standard oxidation potential
  • To determine the concentration of the oxidant

    • Which of the following is an example of a redox system?

    <p>All of the above</p> Signup and view all the answers

    What is the significance of the standard oxidation potential?

    <p>It is a measure of the oxidizing or reducing properties of the system</p> Signup and view all the answers

    What is the role of the platinum electrode in determining the standard oxidation potential?

    <p>It assumes a definite potential indicative of the position of the equilibrium</p> Signup and view all the answers

    What is the relationship between the oxidant and its conjugate reductant?

    <p>The more powerful the oxidant, the weaker its conjugate reductant</p> Signup and view all the answers

    What is the effect of concentration on the oxidation potential of a redox system?

    <p>The oxidation potential is dependent on the ratio of oxidant to reductant concentrations</p> Signup and view all the answers

    What is the significance of the equilibrium in a redox system?

    <p>It determines the position of the oxidation potential</p> Signup and view all the answers

    What is the purpose of the half cell in determining the standard oxidation potential?

    <p>To consist of an inert electrode dipped in a solution of equal concentration of both the oxidized and reduced form of a system</p> Signup and view all the answers

    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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    Description

    This quiz covers the concepts of equivalent weight, including the formulas for calculating it, and its application to redox reactions, such as oxidation of ferrous ions by potassium permanganate.

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