What is the effect of dilution on the equivalent conductance of strong electrolyte

Options

A. Decrease on dilution
B. Remains unchanged
C. Increase on dilution
D. None of the above

Explanation

To understand the effect of dilution on the equivalent conductance of a strong electrolyte, we can break down the explanation into clear steps:

### Step 1: Understanding Equivalent Conductance
Equivalent conductance (\( \Lambda_n \)) is defined as the conductance of an electrolyte solution divided by the number of equivalents of the electrolyte in that solution. It can be expressed mathematically as:
\[ \Lambda_n = \frac{\kappa \times 1000}{n} \]
where \( \kappa \) is the specific conductance (conductivity) of the solution, and \( n \) is the normality (equivalents per liter).

### Step 2: Effect of Dilution on Volume
When we dilute a solution, we increase the volume of the solution. This is done by adding more solvent (usually water) to the solution. As a result, the concentration of the electrolyte decreases.

### Step 3: Understanding Normality
Normality (\( N \)) is defined as the number of equivalents of solute per liter of solution. When we dilute the solution, the volume increases, which leads to a decrease in normality:
\[ N = \frac{\text{Number of moles}}{\text{Volume in liters}} \]
Thus, if the volume increases due to dilution, the normality decreases.

### Step 4: Relationship Between Equivalent Conductance and Normality
From the equation for equivalent conductance, we see that \( \Lambda_n \) is inversely proportional to normality (\( N \)). Therefore, if the normality decreases due to dilution, the equivalent conductance must increase:
\[ \text{If } N \downarrow \Rightarrow \Lambda_n \uparrow \]

### Step 5: Conclusion
Thus, the effect of dilution on the equivalent conductance of a strong electrolyte is that it increases. Therefore, the correct answer to the question is:
**Increases on dilution.**

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