Which sample, when dissolved in 1.0 liter of water, produces a solution with the lowest freezing point

Freezing point depression of a solution, when a nonvolatile solute is dissolved in a solvent, is a colligative property, which means that it depends on the number of particles of solute dissolved.

The equation is:

[tex]\Delta T_f=m\times k_f\times i[/tex]

Where:

ΔTf is the decrease in the freezing point
m is the molal concentration
kf is the molal freezing point depression constant, which depends on the solvent
i is the nan't Hoff factor, which accounts for the dissociation of ionic compounds.

Since the volume is the same for all the solutoins, the molal concentration will be higher for those solutions with more number of moles. Then, cross out the first two choices.

Since CaCl₂, in ideal conditions, dissociates into 1 Ca²⁺ ion and 2 Cl⁻ ions, the van't Hoff factor is 3, while for the molcecular C₆H₁₂O₆ it is 1.

Thus, the lowest freezing point will be produced by the sample of 0.2 mol of CaCl₂.

aliasger2709 aliasger2709 · Answer 2 · 2022-03-19T10:22:06+01:00

The freezing point is the temperature at which the substance freezes. The lowest freezing point will be produced by the sample of calcium chloride.

What is the Freezing point?

The freezing point is a colligative property that depends on the number of non-volatile solute particles dissolved in the solution.

Freezing point depression is given as:

[tex]\rm \Delta T_{f} = \rm m\times k_{f}\times i[/tex]

Here,

The decrease in the freezing point = [tex]\rm \Delta T_{f}[/tex]

Molal concentration = m

Molal freezing point depression constant = Kf

Van't Hoff factor = i

More the number of the moles of the substance higher will be the molal concentration. Therefore, 0.1 mol of ethanol and Lithium bromide will not have the lowest freezing point.

The van't Hoff factor (i) for glucose is 1 while calcium chloride dissociates into one calcium ion and 2 chloride ions and hence the i = 3.

Therefore, option 4. 0.2 mol of calcium chloride will have the lowest freezing point.

Learn more about a freezing point here:

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