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Question

1.0 molal aqueous solution of an electrolyte A2B3 is 60% ionized. The boiling point of the solution at 1 atm is:

[Kb(H2O)=0.52 K kg mol1]

A
274.76 K
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B
377 K
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C
376.4 K
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D
374.72 K
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Solution

The correct option is D 374.72 K
The vant Hoff factor (i) is

i=n(obsrved)n(theoretical)=(2+3)×0.61=3

The expression for the elevation in boiling point is

ΔTb=kb×m×i=0.52×1.0×3=1.56K

The boiling point of 1.0 molal aqueous solution is 373.15K+1.56=374.72 K

Hence, the correct option is D

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