Answer: [tex]-1.960^o C[/tex].
Explanation:
[tex]\Delta T_f=i\times K_f\times m[/tex]
[tex]\Delta T_f[/tex] = depression in freezing point
[tex]K_f[/tex] = freezing point constant =[tex]1.86^0C/m[/tex]
i= vant hoff factor = number of ions produced on complete dissociation
[tex]LiBr\rightarrow Li^++Br^-[/tex]
For [tex]LiBr[/tex] , i= 2
m= molality = 0.527
[tex]\Delta T_f=T_f^0-T_f=(0-T_f)^0C[/tex]
[tex]0-T_f=2\times 1.86\times 0.527[/tex]
[tex]T_f=-1.960^0C[/tex]
The freezing point of the solution is [tex]-1.960^o C[/tex].
