If the freezing point of a pure solvent is 6.00 degrees Celsius, will the solvent which is contaminated with a soluble material have a freezing point (higher than, lower than or same as) 6.00 degrees Celsius? Explain.

delta T = kf*m

The freezing point of a solvent is affected by the presence of a soluble material. The presence of a soluble material results in a phenomenon known as colligative properties. One of these colligative properties is called the freezing point depression.

When a soluble material is added to a solvent, the particles of the material disrupt the crystal lattice structure that forms during freezing. The solute particles occupy space between solvent particles, making it more difficult for the solvent particles to arrange themselves into an ordered, solid structure. As a result, the solvent requires a lower temperature to freeze, and its freezing point is depressed.

So, if the pure solvent has a freezing point of 6.00 degrees Celsius, the solvent contaminated with a soluble material will have a freezing point lower than 6.00 degrees Celsius. The degree of depression depends on the concentration or amount of solute present in the solvent. The more solute there is, the greater the depression of the freezing point.