The boiling point elevation is a colligative property, which depends on the number of solute particles in the solution:
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Since strong electrolytes like KNO3 and NaCl produce more particles in solution compared to weak electrolytes like CH3COOH and non-electrolytes like sucrose, the order of boiling points is: 1 N KNO3 = 1 N NaCl>1 N CH3COOH>1 N sucrose.
If \(A_2B \;\text{is} \;30\%\) ionised in an aqueous solution, then the value of van’t Hoff factor \( i \) is:
1.24 g of \(AX_2\) (molar mass 124 g mol\(^{-1}\)) is dissolved in 1 kg of water to form a solution with boiling point of 100.105°C, while 2.54 g of AY_2 (molar mass 250 g mol\(^{-1}\)) in 2 kg of water constitutes a solution with a boiling point of 100.026°C. \(Kb(H)_2\)\(\text(O)\) = 0.52 K kg mol\(^{-1}\). Which of the following is correct?