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You're correct that specific conductance and molar conductance exhibit opposite trends upon dilution of a strong electrolyte solution. Here's the breakdown:

Specific Conductance (κ):

• Measures the ability of a solution to conduct electricity per unit volume (cm²/S).
• Decreases with dilution: When a strong electrolyte is diluted, the total number of ions per unit volume decreases. Although the total number of ions might increase due to slight dissociation changes, the dilution effect is dominant, leading to a decrease in κ.

Molar Conductance (Λm):

• Represents the ability of 1 mole of electrolyte to conduct electricity (S cm²/mol).
• Increases with dilution: Even though the number of ions per unit volume decreases upon dilution, the mobility of individual ions increases. This is because they experience less interionic attraction due to increased space and decreased concentration. This enhanced mobility outweighs the decrease in ion density, leading to an increase in Λm.

Here's an analogy: Imagine a crowded highway (concentrated solution). Each car (ion) can move slowly due to traffic (interionic interactions). When the highway is widened (dilution), the traffic eases, and individual cars (ions) can move faster, even if the overall number of cars (ions) per kilometer decreases. This translates to increased molar conductance with dilution.

Dr Murtadha Shukur thank you for your contribution to the discussion

When solution is diluted, the total number of ions increases due to increase in the degree of dissociation. Hence, molar conductance increases with dilution. But the number of ions per unit volume decreases. Hence, specific conductance decreases with dilution.Conductivity of weak electrolytic solution decreases with dilution whereas equivalent conductivity, molar conductivity increases with dilution. Reason: On dilution, the ionic mobility and number of ions present in solution increases but the number of ions per mL decreases. Specific Conductivity decreases with a decrease in concentration. Since the number of ions per unit volume that carry current in a solution decrease on dilution. Hence, concentration and conductivity are directly proportional to each other. Specific Conductivity decreases with a decrease in concentration. Since the number of ions per unit volume that carry current in a solution decrease on dilution. Hence, concentration and conductivity are directly proportional to each other. Both the terms molar conductivity and conductivity are different. Molar conductivity is the conductivity of one molar electrolytic solution placed between two electrodes which are one centimetre apart and have enough area of cross section to hold the entire volume.