Variation in Conductivity Models

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Variation in Conductivity Models

 Conductivity (κκ) and molar conductivity (

Λm\Lambda_mΛm​) vary with concentration due to the interactions between ions in solution and the degree of ionization. Here’s how they typically change:

Conductivity (κ\kappaκ):

  1. Increase in Concentration:
    • Strong Electrolytes: Conductivity increases with concentration because more ions are present to conduct electricity.
    • Weak Electrolytes: Initially, conductivity increases with concentration as more ions are produced through ionization.
  2. Higher Concentrations:
    • For both strong and weak electrolytes, at higher concentrations, the increase in conductivity starts to level off or even decrease. This is due to ion pairing and increased ion interactions, which reduce the mobility of ions.

Molar Conductivity (Λm\Lambda_mΛm​):

Molar conductivity is defined as the conductivity divided by the molar concentration (Λm=κ/C\Lambda_m = \kappa / CΛm​=κ/C).

  1. Strong Electrolytes:
    • Dilute Solutions: Molar conductivity increases as concentration decreases. This is because ions experience less interionic attraction and can move more freely.
    • Concentrated Solutions: Molar conductivity decreases as concentration increases due to ion pairing and decreased ion mobility.
  2. Weak Electrolytes:
    • Dilute Solutions: Molar conductivity increases significantly with dilution due to increased ionization (more ions are produced as the solution is diluted).
    • Concentrated Solutions: Molar conductivity is relatively low because weak electrolytes are not fully ionized.

Graphical Representation:

  • Conductivity (κ\kappaκ) vs. Concentration (C): For strong electrolytes, the graph starts high and increases more slowly at higher concentrations. For weak electrolytes, it starts lower but increases initially before leveling off.
  • Molar Conductivity (Λm\Lambda_mΛm​) vs. Concentration (C): For strong electrolytes, the graph shows a steep decrease at low concentrations, flattening out at higher concentrations. For weak electrolytes, the graph shows a sharp increase at low concentrations (due to increased ionization) and then levels off.

Kohlrausch’s Law for Strong Electrolytes:

At infinite dilution, the molar conductivity of a strong electrolyte can be expressed as:Λm=Λm∘−KC

where Λm∘\Lambda_m^\circΛm∘​ is the molar conductivity at infinite dilution, and KKK is a constant.

Understanding these variations helps in analyzing electrolyte solutions and their behaviors in different concentrations.

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