Final answer:
Molality is not temperature-dependent because it is calculated using the mass of the solvent and solute, which do not change with temperature. This makes it a stable unit of measurement for temperature-related properties of solutions compared to molarity, which varies with temperature.
Step-by-step explanation:
Molality is not temperature-dependent because it is defined as the moles of solute per kilograms of solvent, and this relationship does not change with temperature. Since molality is based on masses, which are independent of temperature, unlike volume which can expand or contract with temperature changes affecting the molarity, molality remains constant. This characteristic makes molality a useful unit of concentration for calculating properties such as boiling point elevation and freezing point depression which are directly proportional to the molality of a solution. Molality is particularly vital when significant temperature variation is involved in chemical processes.
Additionally, molality and mole fraction, another temperature-independent concentration measure, are proportional in dilute solutions. However, using molality over mole fraction is often more convenient since molality has larger numerical values that eliminate non-significant zeros, streamlining calculations. Moreover, the mole fraction is limited to a range between zero and one, while molality can exceed this range, providing a more extensive scale for measurement.