The freezing point depression constant (\( K_f \)) for water is \( 1.86 \, {°C·kg/mol} \). If 0.5 moles of a non-volatile solute is dissolved in 1 kg of water, calculate the freezing point depression.
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The freezing point depression depends on the molality of the solution. For non-volatile solutes, the freezing point of the solvent decreases by \( \Delta T_f = K_f \times m \).