What is the molality of a 0.142 M Na₃PO₄(aq) solution that has a density of 1.015 g/mL A) 0.113 m B) 0.133 m C) 0.153 m D) 0.173 m E) None of the above

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Molality (m) is defined as the number of moles of solute per kilogram of solvent. To find the molality from molarity (M), we need the density of the solution to convert volume to mass and then to determine the mass of the solvent. The formula to convert molarity to molality is: $ m = \frac{M \times \text{Density} \times 1000}{1000 \times \text{Density} - M \times \text{MW of solute}} $, where MW is the molecular weight of the solute. However, the molecular weight of Na₃PO₄ cannot be calculated as it is not a real chemical compound. Therefore, without the molecular weight of the solute, the molality cannot be accurately calculated from the given information.

What Is the Molality of a 0