Determine the freezing point (°C)of a 0.015 molal aqueous solution of MgSO₄. Assume i = 2.0 for MgSO₄. The molal freezing-point-depression constant of water is 1.86 °C/m. A)-0.056 B)-0.028 C)-0.17 D)-0.084 E)0.000

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The freezing point depression is given by the equation:$$\Delta T_f = iK_fm$$where:* $\Delta T_f$ is the freezing point depression in °C* $i$ is the van't Hoff factor* $K_f$ is the molal freezing-point-depression constant of the solvent in °C/m* $m$ is the molality of the solution in mol/kgIn this case, we have:* $i = 2.0$* $K_f = 1.86 °C/m$* $m = 0.015 mol/kg$Substituting these values into the equation, we get:$$\Delta T_f = (2.0)(1.86 °C/m)(0.015 mol/kg) = 0.0558 °C$$The freezing point of the solution is therefore:$$T_f = 0.0 °C - 0.0558 °C = -0.056 °C$$Therefore, the correct choice is A.

Determine the Freezing Point (°C)of a 0