Which property of solutions is affected by the presence of a solute?

The presence of a solute in a solution has a significant impact on the boiling point, a phenomenon known as boiling point elevation. When a non-volatile solute is added to a solvent, the resulting solution has a higher boiling point compared to the pure solvent. This occurs because the solute particles disrupt the ability of solvent molecules to escape into the gas phase. Consequently, more energy (in the form of heat) is required to bring the vapor pressure of the solution up to the atmospheric pressure needed for boiling.

The extent of boiling point elevation can be quantitatively described using the formula:

ΔT_b = i * K_b * m

where ΔT_b is the increase in boiling point, i is the van 't Hoff factor (which accounts for the number of particles the solute breaks into), K_b is the ebullioscopic constant of the solvent, and m is the molality of the solution. This illustrates how the addition of solute influences the boiling point due to colligative properties.

While factors such as color, temperature, and pressure can be influenced by various conditions, they do not change in a systematic way due to solute presence in the same way that boiling point does. The color of a solution may