Which Aqueous Solution Will Have the Lowest Freezing Point

Which Aqueous Solution Will Have the Lowest Freezing Point?


The freezing point of a liquid is the temperature at which it changes from a liquid to a solid state. When a solute is dissolved in a solvent, it affects the freezing point of the solution. This phenomenon is known as freezing point depression. In this article, we will explore which aqueous solution will have the lowest freezing point and how different factors contribute to this effect.

Factors Affecting Freezing Point Depression:

1. Concentration of the solute: The more solute dissolved in a solvent, the greater the freezing point depression. This is because the solute particles interfere with the arrangement of the solvent particles, making it harder for them to form a solid structure.

2. Nature of the solute and solvent: Different solutes and solvents have varying abilities to depress the freezing point. Substances with ionic bonds tend to have a greater effect on the freezing point than those with covalent bonds. Similarly, solvents with weaker intermolecular forces are more susceptible to freezing point depression.

3. Van’t Hoff factor: The Van’t Hoff factor (i) represents the number of particles a solute dissociates into when dissolved in a solvent. For example, a solute that dissociates into two ions will have a higher Van’t Hoff factor than a solute that remains as a single molecule. Higher Van’t Hoff factors lead to greater freezing point depression.

4. Colligative properties: Freezing point depression is a colligative property, which means it depends on the number of solute particles rather than their nature. Therefore, the concentration of the solute is the primary factor affecting the freezing point depression, assuming other factors are constant.

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Determining the Solution with the Lowest Freezing Point:

Based on the factors mentioned above, the solution with the lowest freezing point will be the one with the highest concentration of solute particles. In general, ionic compounds, such as salts, tend to dissociate into multiple ions when dissolved in water, resulting in a higher freezing point depression. For example, a solution of sodium chloride (NaCl) will have a lower freezing point than a solution of glucose (C6H12O6) at the same concentration due to the higher Van’t Hoff factor of NaCl.

Frequently Asked Questions:

Q1. Can any solute lower the freezing point of a solvent?

A1. Yes, any solute can lower the freezing point of a solvent to some extent. However, the degree of freezing point depression depends on factors like concentration, nature of solute and solvent, and Van’t Hoff factor.

Q2. Is the freezing point depression always proportional to the concentration of the solute?

A2. Yes, freezing point depression is directly proportional to the concentration of the solute. As the concentration increases, the freezing point depression also increases.

Q3. How does the nature of solute and solvent affect freezing point depression?

A3. The nature of solute and solvent determines the strength of intermolecular forces. Substances with stronger intermolecular forces tend to have a smaller freezing point depression compared to those with weaker forces.

Q4. Can the freezing point of a solution be lower than the freezing point of the pure solvent?

A4. Yes, the freezing point of a solution can be lower than the freezing point of the pure solvent due to freezing point depression caused by the presence of a solute.

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Q5. Are there any practical applications of freezing point depression?

A5. Freezing point depression has various practical applications. For example, it is used in antifreeze solutions for automobiles, allowing the engine coolant to have a lower freezing point and prevent damage from freezing temperatures.


The freezing point of an aqueous solution is determined by various factors, including the concentration of the solute, nature of the solute and solvent, Van’t Hoff factor, and colligative properties. Solutions with higher solute concentrations and ionic compounds tend to have the lowest freezing points. Understanding the factors affecting freezing point depression is crucial in various fields, including chemistry, biology, and engineering, where precise control of freezing points is essential.

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