can u pls explain this Para, "the conductivity of all electrolytes increases with temperature. The conductivity of a solution varies slightly with pressure due to change in viscosity of the medium . The viscosity of a dilute solution decreases with increasing pressure this is accompanied by an increase in the equivalent conductivity provided the pressure is not too high the effect is most marked in a weak electrolyte than a strong electrolyte because in case of weak electrolyte increase of pressure tends to favour ionization but this factor is not appreciable in case of strong electrolytes."
^m or ^eq is directly proportional to pressure.
The topic about effect of Temperature and Pressure on Conductivity.
As we know, Conductivity of a solution is defined as the conductance of a solution of 1 cm in length and area of cross-section 1 sq. cm. The inverse of resistivity is called conductivity or specific conductance. It is represented by the symbolκ. If ρ is resistivity, then we can write:
The conductivity of a solution at any given concentration is the conductance (G) of one unit volume of solution kept between two platinum electrodes with the unit area of cross-section and at a distance of unit length.
(Since a = 1, l = 1)
Conductivity always decreases with a decrease in concentration, both for weak and strong electrolytes. This is because the number of ions per unit volume that carry the current in a solution decreases with a decrease in concentration.
Molar conductivity of a solution at a given concentration is the conductance of volume V of a solution containing 1 mole of the electrolyte kept between two electrodes with the area of cross-section A and distance of unit length.
Now, l = 1 and A = V (volume containing 1 mole of the electrolyte).
Molar conductivity increases with a decrease in concentration. This is because the total volume V of the solution containing one mole of the electrolyte increases on dilution.
The variation of withfor strong and weak electrolytes is shown in the following plot: