We have to calculate the freezing point of an aqueous solution that boils at 104.6 °C.

When a nonvolatile solute is dissolved in a solvent, the freezing point of the resulting solution is always lower than the freezing point of pure solvent. This property of solutions is called the **freezing point depression**.

**The formula for freezing point depression is:**

$\overline{){\mathbf{\u2206}}{{\mathbf{T}}}_{{\mathbf{f}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{i}}{\mathbf{\xb7}}{{\mathbf{K}}}_{{\mathbf{f}}}{\mathbf{\xb7}}{\mathbf{m}}}$

**Where,**

ΔT_{f} = change in freezing point

i = van ‘t Hoff constant (i = 1 for nonelectrolytes)

K_{f} =freezing point depression constant

m = molality of solution

When a nonvolatile solute is dissolved in a solvent, the boiling point of the resulting solution is always higher than the boiling point of pure solvent. This property of solutions is called the **boiling point elevation**.

**The formula for boiling point elevation is:**

$\overline{){\mathbf{\u2206}}{{\mathbf{T}}}_{{\mathbf{b}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{i}}{\mathbf{\xb7}}{{\mathbf{K}}}_{{\mathbf{b}}}{\mathbf{\xb7}}{\mathbf{m}}}$

**Where,**

ΔT_{b} = change in boiling point

i = van ‘t Hoff constant (i = 1 for nonelectrolytes)

K_{b} = boiling point elevation constant

m = molality of solution

What is the freezing point of an aqueous solution that boils at 104.6 °C?

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