Electrolytic Solutions Conductance Basics

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Electrolytic Solutions Conductance Basics

 Conductance of electrolytic solutions refers to the ability of an electrolytic solution to conduct electricity. It depends on the presence and mobility of ions in the solution. Here are some key concepts:

  1. Conductance (G): It is the ability of a solution to conduct electric current and is the reciprocal of resistance (R). The unit is Siemens (S).
  2. Specific Conductance (κ or kappa): It is the conductance of a solution of unit length and unit cross-sectional area. It depends on the nature of the electrolyte, concentration, temperature, and solvent. Its unit is S/m.
  3. Molar Conductance (Λm): It is the conductance of all the ions produced by one mole of an electrolyte in a given volume of solution. It is related to specific conductance by the formula:Λm=κC\Lambda_m = \frac{\kappa}{C}Λm​=Cκ​where CCC is the concentration of the solution in mol/m³. Its unit is S·m²/mol.
  4. Equivalent Conductance (Λe): Similar to molar conductance, but it refers to the conductance of one equivalent of electrolyte.
  5. Factors Affecting Conductance:
    • Concentration: Generally, as the concentration of an electrolyte increases, conductance increases due to more ions being present.
    • Temperature: Higher temperatures usually increase conductance because ions move faster at higher temperatures.
    • Nature of Electrolyte: Strong electrolytes (fully dissociate) have higher conductance compared to weak electrolytes (partially dissociate).
    • Nature of Solvent: Solvents with higher dielectric constants can dissolve more ionic compounds, thus affecting conductance.
  6. Kohlrausch’s Law of Independent Migration of Ions: It states that at infinite dilution, each ion contributes to the conductance of the solution independently of the other ions present.

Understanding the conductance of electrolytic solutions is crucial 

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