Which one of the following aqueous solutions will exhibit highest boiling point?

Question

Which one of the following aqueous solutions will exhibit highest boiling point? (A)  0.01 M Na2SO4  (B)  0.01 M KNO3  (C)  0.015 M texturea  (D)  0.015 M textglucose

Tardigrade Admin · Accepted Answer

Boiling point =T0(Solvent)+Tb (Elevation in b. p.) Δ Tb=mikb where, m is the molality ie, the van't Hoff factor (i) =[1+(y-1)x] kb= molal elevation constant. Thus, Δ Tb propto im Assume 100% ionization [a] mi(Na2SO4)=0.01× 3=0.03 [b] mi(KNO3)=0.01× 2=0.02 [c] mi(glucose)=0.015

Q. Which one of the following aqueous solutions will exhibit highest boiling point?

$0.01 M N a_{2} S O_{4}$

$0.01 M K N O_{3}$

$0.015 M urea$

$0.015 M glucose$

Q. Which one of the following aqueous solutions will exhibit highest boiling point?

0.01MNa2​SO4​

0.01MKNO3​

0.015Murea

0.015Mglucose

$0.01 M N a_{2} S O_{4}$

$0.01 M K N O_{3}$

$0.015 M urea$

$0.015 M glucose$