The freezing Point of a solution : -1.661 °C(no option)
Further explanation
Solution properties are the properties of a solution that don't depend on the type of solute but only on the concentration of the solute.
The term is used in the Solution properties
1. molal
that is, the number of moles of solute in 1 kg of solvent
[tex]\tt m=\dfrac{mol~solute}{mass~1~kg~solvent}[/tex]
2. freezing point
Solutions from volatile substances have a higher boiling point and lower freezing points than the solvent
[tex]\tt \Delta Tf=Kf\times m[/tex]
ΔTf = Tf solvent - Tf solution
Kf = The molal freezing point depression constant
m = molal solution
Given
1.25 mol CaCl₂
1400 g water = 1.4 kg
Required
The freezing point
Solution
molal of the solution :
= mol : kg solvent(water)
= 1.25 mol : 1.4 kg
= 0.893
The freezing point :
Tf solvent = 0 °C(for water)
Kf water = 1.86 °C/m
Input the value :
ΔTf = Tf solvent - Tf solution = Kf . m
0 - Tf solution = 1.86 °C/m . 0.893
0 - Tf solution = 1.661
Tf solution = - 1.661 °C
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