Two solutions 'A' and 'B' are taken and diluted. On dilution, it was seen that the limiting molar conductivity of 'B' increases to a smaller extent while that of 'A' increases to a much larger extent comparatively, which of the two is a strong electrolyte?

B

The correct answer is option 1. \(B\).

Strong electrolytes dissociate almost completely into ions even at high concentrations. Their molar conductivity is already high due to this extensive dissociation, and further dilution results in a relatively smaller increase in Λ°m.

Weak electrolytes dissociate only partially into ions at high concentrations. Their molar conductivity starts lower due to limited dissociation. Upon dilution, a significant fraction of undissociated molecules dissociate, leading to a larger increase in Λ°m compared to strong electrolytes.

In the given scenario, solution B shows a smaller increase in Λ°m than solution A upon dilution. This suggests that B is already more extensively dissociated at moderate concentrations, even before dilution. This characteristic behavior points towards B being a strong electrolyte. In contrast, solution A, whose Λ°m increases to a larger extent, has more room for increased dissociation upon dilution, suggesting its nature as a weak electrolyte.

Therefore, based on the principle that strong electrolytes experience smaller increases in Λ°m with dilution due to their near-complete dissociation at moderate concentrations, the answer should be B.