Respuesta :
The freezing point of a solution is -1.16°C
Calculation,
The equation which give relation between freezing point depletion and molality is,
Δ[tex]T_{f} = K_{f} .m[/tex] ... (i)
- Δ[tex]T_{f}[/tex] is change in the freezing point of the solvent .
- [tex]K_{f}[/tex] of benzene = 5.12°C/m
- m is molality of the solution
Moles of the solute = 22.0 g / 114.23 g/mole = 0.193 mole
Mass of the solvent in g = 148 g
Mass of the solvent in kg = 0.148 kg
Molality = 0.193 mole/ 0.148 kg = 1.3 m
Now, after putting the value of [tex]K_{f}[/tex] and m in equation (i) we get
Δ[tex]T_{f} = K_{f} .m[/tex]
Δ[tex]T_{f}[/tex]= 5.12°C/m×1.3 m = 6.66°C
Δ[tex]T_{f}[/tex]= [tex]T_{f}[/tex] (solvent) - [tex]T_{f}[/tex] (solution)
[tex]T_{f}[/tex] (solution) = [tex]T_{f}[/tex] (solvent) -Δ[tex]T_{f}[/tex]= 5.5 °C - 6.66°C = -1.16°C
The freezing point of a is -1.16°C
To learn about freezing point
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