The boiling point of an aq solution 102.11 C. What is the freezing point?

delta T = Kb*m

Solve for m

delta T = Kf*m
Substitute for m and Kf and solve for delta T, then subtract from zero C to find freezing point.

87.8

To determine the freezing point of an aqueous solution, we need to know the concentration of solute in the solution. The freezing point of a solution is lower than the freezing point of pure water due to the presence of dissolved solute particles.

The relationship between the freezing point depression (ΔTf) and the molality (m) of the solution is given by the equation:

ΔTf = Kf * m

Where:
ΔTf is the freezing point depression,
Kf is the cryoscopic constant specific to the solvent (water in this case),
m is the molality of the solution.

In this case, we don't have the molality or the molar mass of the solute, so we can't directly calculate the freezing point depression. However, if we assume that the solute is a non-volatile, non-electrolyte, we can use the equation:

ΔTf = i * Kf * m

Where:
i is the Van't Hoff factor, which represents the number of particles into which the solute dissociates in the solution.

For a non-electrolyte solute, i = 1.

Next, we need to determine the freezing point depression constant (Kf) for water. The Kf value for water is 1.86 °C/m.

Now, we can use the equation to find the freezing point depression:

ΔTf = Kf * m

Rearranging the equation gives us:

m = ΔTf / Kf

Substituting the given values, the freezing point depression (ΔTf) = 0 °C (pure water freezes at 0 °C), and Kf = 1.86 °C/m, we can calculate the molality (m).

m = 0 °C / 1.86 °C/m = 0 mol/kg

Since the molality (m) is 0 mol/kg, this means that the freezing point depression is also zero. Therefore, the freezing point of the aqueous solution would be the same as the freezing point of pure water, which is 0 °C.