Course Content
Module 1: Introduction to Electrochemistry
Overview of electrochemistry, its applications, and relevance in daily life and industrial processes.
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Definition and Importance of Electrochemistry
Module 2: Redox Reactions
Understanding oxidation, reduction, oxidation numbers, and balancing redox equations.
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Oxidation and Reduction Concepts
Oxidation Numbers
Balancing Redox Equations
📘 Module 3: Electrolysis
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Introduction to Electrolysis
Faraday’s Laws of Electrolysis
Industrial Applications of Electrolysis
Electrolysis Calculations
📘 Module 4: Redox Titrations
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Introduction and Indicators
KMnO₄ and Fe²⁺ Titration – Theory and Procedure
Oxalic Acid vs KMnO₄ Titration – Theory and Procedure
Iodometric Titrations – Iodine vs Thiosulfate (S₂O₃²⁻)
Electrode Potentials
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Standard Electrode Potentials (E° Values)
Electrochemical Cells and E° Cell Calculations
The Nernst Equation – Effect of Concentration on E°cell
📘 Module 6: Corrosion
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🧪 Lesson 1: Causes, Mechanism, and Prevention of Corrosion
📘 Module 7: Conductivity of Electrolyte Solutions
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🧪 Lesson 1: Electrical Conductivity and Factors Affecting It
📘 Module 8: Electrolytic Cells
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🧪 Lesson 1: Electrolysis Mechanism and Product Prediction
🧪 Lesson 2: Electrolysis of Water and Brine
📘 Module 9: Applications of Electrolysis in Industry
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🧪 Lesson 1: Electrolysis in Metal Extraction, Refining, and Electroplating
📘 Module 10: Redox Titrations and Calculations
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🧪 Lesson 1: Introduction, Procedure, and Redox Calculations
Advanced Chemistry: Electrochemistry

Introduction
Electrical conductivity of electrolyte solutions depends on the presence of free-moving ions. These ions carry current when a voltage is applied across electrodes submerged in the solution. This topic is key in electrochemistry and widely tested in NECTA.

🔹 1. Definition

Electrical conductivity is the ability of a solution to conduct electric current due to the movement of ions.

Measured using a conductivity meter and expressed in:

  • S/m (Siemens per meter)

  • S/cm, mS/cm, or μS/cm

🔹 2. Types of Electrolytes

Type of Electrolyte Description Example
Strong electrolytes Fully dissociate into ions NaCl, HCl, H₂SO₄
Weak electrolytes Partially dissociate CH₃COOH, NH₄OH
Non-electrolytes Do not dissociate, no ions Sugar, ethanol

🔹 3. Conductivity vs Molar Conductivity

  • Conductivity (κ):
    Depends on concentration and type of ions

  • Molar Conductivity (Λₘ):
    Conductivity per mole of electrolyte

    r
    Λₘ = κ / c

    Where:

    • Λₘ = molar conductivity (S·cm²·mol⁻¹)

    • κ = conductivity (S/cm)

    • c = concentration (mol/cm³)

🔹 4. Factors Affecting Conductivity

Factor Effect on Conductivity
Concentration More ions → higher conductivity (up to a limit)
Temperature Higher temperature → more mobility → ↑ conductivity
Ion Charge & Size Smaller, highly charged ions conduct better (e.g. H⁺, OH⁻)
Type of Electrolyte Strong > weak > none
Solvent Nature Water is best due to high polarity

🧪 Example – Strong vs Weak Electrolytes

Question:
Compare conductivity of 0.1 M HCl and 0.1 M CH₃COOH.

Answer:

  • HCl is a strong acid, fully dissociates → high conductivity

  • CH₃COOH is a weak acid, partially dissociates → low conductivity

✅ HCl solution has higher conductivity

🔹 Applications in Chemistry and Industry

  • Quality control in water treatment

  • Determining ion concentration in titrations

  • Soil salinity tests in agriculture

  • Monitoring corrosion in industrial systems

🧠 NECTA Tips

  • Always differentiate between conductivity and molar conductivity

  • Use clear units in calculations

  • Include practical examples (e.g., conductometer setup)

  • Explain the role of mobility and concentration

✅ Summary

  • Electrolytic conductivity comes from ion movement

  • Depends on ion type, concentration, and temperature

  • Strong electrolytes conduct better than weak ones

  • Molar conductivity = conductivity ÷ concentration

  • Used in water analysis, titrations, and NECTA practicals

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