Define specific conductivity and molar conducticity. What is the effect of dilution on them ?

Explanation

Specific Conductivity The inverse of resistivity is called conductivity, k, also known as specific conductance. It can be defined as the conductance of a solution of 1m length with area of cross-section equal to `1m^(2)`.
i.e. G = k (when, l = 1m and `A = 1m^(2)`)
`k = (1)/(rho)`
Units of conductivity `(kappa) = (1)/("ohm.m")`
`= "ohm"^(-1) cm^(-1)` or `S^(-1) cm^(-1)`
Molar Conductivity `(Lambda_(m))` Molar conductivity of a solution is the conductance of all ions produced by one gram mole of electrolyte kept between two electrodes having unit length between them and large cross-sectional area, so as to contain the electrolyte.
It is denoted by `Lambda_(m)`.
`Lambda_(m) = (kappa)/(C) xx 1000`
If `kappa` is expressed in `Omega^(-1)m^(-1)` or `Sm^(-1)` unit and the concentration C in mol `m^(-3)`, then the unit of `Lambda_(m)` will be `Omega^(-1) m^(2) mol^(-1)` or `Sm^(2) mol^(-1)`.
`Lambda_(m) = (kappa xx 1000)/(M)`
where, M is the molarity of the electrolytic solution. Effect of Dilution Condutivity always decreases with decreases in concentration (i.e. with dilution) of both string and weak electrolytes. This is due to the fact that the number of ions that carry current in a unit volume of solution always decreases with decrease in concentration.
Molar conductivity increases with decrease in concentration. This is because the total volume V of solution containing one mole of electrolyte also increases.