For a uni - univalent electrolyte such as NaCl, the Kohlrausch's law is expressed as
\({ ({ \Lambda }_{ m }^{ o }) }_{ NaCl }=({ { \lambda }_{ m }^{ o })_{ { Na }^{ + } }+{ ({ \lambda }_{ m }^{ o }) }_{ { Cl }^{ - } } }\)

\(\alpha =\frac { { \Lambda }_{ m } }{ { \Lambda }_{ m }^{ o } } \)

Conductivity, molar conductance and equivalent conductance increases with dilution whereas Conductance (C) decreases.

Yes, the above given statement is true.
When the dilution increases, the ions are far apart and the attractive forces decrease. At infinite dilution the ions are so far apart, the interaction between them becomes insignificant and hence, the molar conductivity increases and reaches a maximum value at infinite dilution

(i) For a strong electrolyte, at high concentration, the number of constituent ions of the electrolyte in a given volume is high and hence the attractive force between the oppositely charged ions is also high.
(ii) Moreover the ions also experience a viscous drag due to greater solvation.
(iii) These factors attribute for the low molar conductivity at high concentration.

Kohlrausch deduced the following empirical relationship between the molar conductance (\({ \Lambda }_{ m }\)) and the concentration of the electrolyte (C).
\(​​{ \Lambda }_{ m }={ \Lambda }_{ m }^{ o }-k\sqrt { C } \)

\({ \Lambda }_{ m }={ \Lambda }_{ m }^{ o }-(-A+B{ \Lambda }_{ m }^{ o })\sqrt { C } \)

Unit of x
\(k=\frac { 1 }{ \rho } .\frac { l }{ A } \left( \frac { 1 }{ ohm } .\frac { m }{ { m }^{ 2 } } \right) \)
= ohm^-1 m^-1 = mho m^-1 (or) Sm^-1

k = \(\frac{1}{R}.\frac{1}{a}=\frac{1}{ρ}\)
Where K is specific conductance
R is resistance and \(\frac1a\) is cell constant.
ρ is specific resistance.

The specific conductance is defined as the conductance of a cube of an electrolytic solution of unit dimensions.

The reciprocal of the resistance \((\frac{l}{R})\) gives the conductance of an electrolytic solution. The SI unit of conductance is Siemen (S).

The ratio \((\frac{l}{A})\) is called the cell constant.

Resistivity is defined as the resistance of an electrolyte confined between to electrodes having unit cross sectional area and are separated by a unit distance. The ratio \((\frac{l}{A})\) is called the cell constant, Unit of resistivity is ohm metre (Ωm).

The resistance of such an electrolytic solution is also directly proportional to the length (l) and inversely proportional to the cross sectional area (A)
R α \(\frac{l}{A}\)
R = ρ \(\frac{l}{A}\)

i.e., I α V (or) I = \(\frac{V}{R}\) ⇒ V = IR
Where 'R' is the resistance of the solution in ohm (Ω)
Here the resistance is the opposition that a cell offers to the flow of electric current through it.