The molar conductivity of strong electrolyte

Options

A. Increases on dilution slightly
B. Does not change on dilution
C. Decreases on dilution
D. Depends on density of electrolyte itself

Answer

To solve the question regarding the molar conductivity of a strong electrolyte upon dilution, we can break it down into the following steps:

### Step 1: Understand Molar Conductivity
Molar conductivity (Λ) is defined as the conductivity (κ) of an electrolyte solution divided by its molar concentration (C). It indicates how well an electrolyte conducts electricity in a solution.

### Step 2: Effect of Dilution on Strong Electrolytes
When a strong electrolyte is dissolved in water, it dissociates completely into its constituent ions. For example, if we take a strong electrolyte like sodium chloride (NaCl), it dissociates into Na⁺ and Cl⁻ ions.

### Step 3: Analyze the Impact of Dilution
When we dilute a strong electrolyte:
- The concentration of ions decreases.
- The distance between the ions increases due to the increase in the volume of the solution.
- The forces of attraction between the ions decrease, allowing them to move more freely.

### Step 4: Conductivity and Molar Conductivity
As the ions move more freely in a diluted solution, the conductivity of the solution increases. Since molar conductivity is defined as the conductivity per unit concentration, we can analyze how it behaves:
- With dilution, although the concentration decreases, the increase in conductivity due to the increased mobility of ions results in an overall increase in molar conductivity.

### Step 5: Conclusion
Thus, for a strong electrolyte, the molar conductivity increases upon dilution, albeit slightly. Therefore, the correct answer to the question is that the molar conductivity of a strong electrolyte increases on dilution slightly.

### Final Answer
The molar conductivity of a strong electrolyte increases on dilution slightly.

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