The molar conductivity for electrolytes A and B are plotted against $$C^{1/2}$$ as shown below. Electrolytes A and B respectively are 

Curve B is a straight line with a small negative slope. This behaviour is characteristic of a strong electrolyte.

Strong electrolytes dissociate completely at all concentrations. The slight decrease in molar conductivity with increasing concentration is due to inter-ionic attractions (as described by the Debye-Hückel-Onsager equation).

Examples: KCl, NaCl, HCl.

Based on the graph of molar conductivity (Λm​) versus the square root of concentration (C1/2), we can identify the nature of electrolytes A and B by looking at how they behave as they approach infinite dilution (C→0).

Curve A shows a steep, non-linear increase in molar conductivity as the concentration approaches zero. This is characteristic of a weak electrolyte.Weak electrolytes do not dissociate completely. As the solution is diluted, the degree of dissociation increases rapidly (Ostwald’s Dilution Law), leading to a sharp spike in the number of ions available to carry current.

Examples: CH3​COOH (Acetic acid), NH4​OH.