Molar conductivity

The molar conductivity of an <a href="/facts/Electrolyte/4YE8bIVa">electrolyte</a> solution is defined as its <a href="/facts/Conductivity_(electrolytic)/tLb0N5Be">conductivity</a> divided by its molar concentration:

Λ
          
            m
          
        
        =
        
          
            κ
            c
          
        
        ,
      
    
    {\displaystyle \Lambda _{\text{m}}={\frac {\kappa }{c}},}

where

κ is the measured conductivity (formerly known as specific conductance),<a class="footnote-ref" id="fnref:3" href="#fn:3">3</a>
c is the <a href="/facts/Molar_concentration/P2WL5b9q">molar concentration</a> of the electrolyte.
The <a href="/facts/International_System_of_Units/S7YLglNz">SI unit</a> of molar conductivity is <a href="/facts/Siemens_(unit)/kLUHhcCj">siemens</a> metres squared per mole (S m2 mol−1). However, values are often quoted in S cm2 mol−1. In these last units, the value of Λm may be understood as the <a href="/facts/Electrical_resistance_and_conductance/hxSt0UAj">conductance</a> of a volume of solution between parallel plate electrodes one centimeter apart and of sufficient area so that the solution contains exactly one mole of electrolyte.

Molar conductivity open-in-new

Molar conductivity