We’re being asked to determine the freezing point of an aqueous K_{2}SO_{4}solution. Aqueous means that K_{2}SO_{4} was dissolved in water.

When calculating the freezing point of a solution, we’re going to use the **Freezing Point Depression **equation

**Freezing Point Depression****:**

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

where

ΔT_{f} = change in freezing point = T_{f pure solvent } - T_{f solvent}

K_{f} = freezing point depression constant

i = van't Hoff factor of the solute = no. of ions

m = molality

Calculate the freezing point of a aqueous solution of K_{2}SO_{4},

Calculate the freezing point of a 0.100 m aqueous solution of K_{2}SO_{4}, taking interionic attractions into consideration by using the vant Hoff factor (i for 0.100 m K_{2}SO_{4} = 2.32).

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