The conductivity of 0.20M solution of KCL at 298K is 0.0248 S cm-1. Calculate its molar conductivity ?

To find the molar conductivity of a 0.20 M solution of KCl at 298 K, we can use the relationship between conductivity, molar conductivity, and concentration. Molar conductivity (Λ) is defined as the conductivity (κ) of the solution divided by its concentration (C) in moles per liter (mol/L). The formula we will use is:

Molar Conductivity Formula

The formula for molar conductivity is:

Λ = κ / C

Where:

• Λ = Molar conductivity (S cm²/mol)
• κ = Conductivity of the solution (S cm⁻¹)
• C = Concentration of the solution (mol/L)

Given Values

From the problem, we have:

• Conductivity (κ) = 0.0248 S cm⁻¹
• Concentration (C) = 0.20 M

Calculating Molar Conductivity

Now, we can substitute the given values into the formula:

Λ = 0.0248 S cm⁻¹ / 0.20 mol/L

Performing the Calculation

Let's do the math:

Λ = 0.0248 / 0.20 = 0.124 S cm²/mol

Final Result

The molar conductivity of the 0.20 M KCl solution at 298 K is 0.124 S cm²/mol.

Understanding Molar Conductivity

Molar conductivity gives us insight into how well ions in a solution can conduct electricity. In the case of KCl, which dissociates into K⁺ and Cl⁻ ions, the value we calculated indicates the efficiency of these ions in conducting electric current. Higher molar conductivity values generally suggest better ionic mobility and higher ion concentration in the solution.

This concept is crucial in various applications, including electrochemistry and understanding the behavior of electrolytes in different solutions. If you have any further questions or need clarification on any part of this topic, feel free to ask!