We’re going to use the equation for Freezing Point Depression.
∆Tf = change in freezing point = Tf pure solvent –Tf solution
Kf = freezing point depression constant
i = van' t Hoff factor of the solute = no. of ions
m = molality
The higher the i, the stronger it is to lower the freezing point.
The highest number of i per gram should be the most cost-effective.
Molar mass = 62.08 g/mol
Molar mass =58.44
Molar mass =74.55
Molar mass =95.21
Molar mass =158.52
If each substance listed here costs the same amount per kilogram, which would be most cost-effective as a way to lower the freezing point of water? (Assume complete dissociation for all ionic compounds.)
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