Answer: The freezing point of solution is [tex]-24^0C[/tex]
Explanation:
Formula used for elevation in boiling point is,
[tex]\Delta T_b=k_b\times m[/tex]
where,
[tex]T_b[/tex] = change in boiling point
[tex]k_b[/tex] = boiling point constant= [tex]0.512^0Ckg/mol[/tex]
m = molality
Given: Boiling point of solution =[tex]106.6^0C[/tex]
Boiling point of water= [tex]100^0C[/tex]
thus [tex]6.6^0C=0.512^0Ckg/mol\times m[/tex]
[tex]m=12.8[/tex]
Formula used for lowering in freezing point is,
[tex]\Delta T_f=k_f\times m[/tex]
where,
[tex]T_f[/tex] = change in freezing point
[tex]k_f[/tex] = freezing point constant =[tex]1.86^0Ckg/mol[/tex]
m = molality
Freezing point of water=[tex]0^0C[/tex]
[tex]0^0C-T_f=1.86\times 12.8[/tex]
[tex]T_f=-24^0C[/tex]
