The concentration of a KCl solution can be measured in different ways, including molarity, molality, and molar conductivity:

 The concentration of a KCl solution can be measured in different ways, including molarity, molality, and molar conductivity: 

Molarity

The concentration of a solution in terms of moles per liter. For example, a 1.00 M KCl solution is made by diluting 74.6 grams of KCl to one liter with water. 

Molality

The concentration of a solution in terms of moles of solute per kilogram of solvent. For example, an imolkg−1 KCl solution means that there are i moles of KCl for every 1 kg of solvent. 

Molar conductivity

A measure of how well a solution conducts electricity. The molar conductivity of a KCl solution increases as the solution is diluted, because the ions become more mobile. 

Here are some examples of molar conductivity for KCl solutions at different concentrations: 

0.000198 molL−1: ∧m = 48.610 S cm2mol−1

0.000309 molL−1: ∧m = 48.290 S cm2mol−1

0.000521 molL−1: ∧m = 47.810 S cm2mol−1

0.000989 molL−1: ∧m = 47.090 S cm2mol−1