state four limitations of depression of freezing point ?
I need answers pls
av been searching through google for the answers...buh still confused
So what did you find that confuses you?
they are not straight to the point
that's why I need the answer
https://www.coursehero.com/file/p4db1qf/Limitations-The-limitations-in-this-experiment-is-that-it-is-not-completely/
Sure! Let me explain the concept of depression of freezing point and then provide you with four limitations of this phenomenon.
Depression of freezing point is a colligative property of solutions, meaning it depends on the concentration of solute particles rather than the specific nature of the solute. When a solute is added to a solvent, it disrupts the orderly arrangement of solvent particles and reduces the freezing point of the solution compared to the pure solvent.
Now, let's discuss four limitations of depression of freezing point:
1. Presence of impurities: The depression of freezing point is based on the assumption that the solute is a non-volatile and non-ionizing substance. If the solute is contaminated with impurities or if it chemically reacts with the solvent, the observed depression of freezing point may not solely depend on the concentration of solute particles.
2. Association and dissociation of solute: Some solutes, like certain molecular compounds or ionic substances, can associate or dissociate in solution. This affects the number of solute particles present and can lead to deviations from the expected depression of freezing point calculations.
3. Electrolytes and ion pairing: In the presence of electrolytes, the ions can form ion pairs or complexes, which alters the behavior of the solution. This can result in higher or lower depression of freezing point than would be expected based on the concentration of the solute particles.
4. Concentration dependence: The depression of freezing point assumes ideal behavior. However, at high concentrations or in concentrated solutions, the solvent-solute interactions can become significant, deviating from ideal behavior. As a result, the depression of freezing point may not strictly follow the expected linear relationship with solute concentration.
Remember, these limitations are important to consider when applying the concept of depression of freezing point to real-life situations.