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Question

What will be the elevation in boiling point for 13.44 g of CuCl2 dissolved in 1 kg of water as solvent if CuCl2 is fully ionised?
(Kb=0.52 K kg mol1
Molar mass of CuCl2=134.4 g/mol)

A
0.05
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B
0.10
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C
0.16
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D
0.20
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Solution

The correct option is C 0.16
Given,
CuCl2 is an electrolytic solute and it is fully ionised

CuCl2Cu2++2Cl
Thus, the number of ions in the solution is 3
i = 3, assuming complete ionization of CuCl2
We know,
Corrected boiling point elevation of solution is,
Tb=i×Kb×m
where,
Tb is the elevation in boiling point.
Kb is molal elevation constant.
m is molality of solution.
i is van't Hoff factor

Tb=i×Kb×wB×1000mB×wA
where,
wB is mass of solute
mB is molar mass of solute
wA is mass of solvent
Tb=3×0.52×13.44×1000134.4×1000=0.1560.16 K

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