In the context of boiling point elevation, what does the "i" in the equation represent?

In the context of boiling point elevation, what does the "i" in the equation represent?

• A. Impermeability factor
• B. Ideal gas constant
• C. Van't Hoff factor
• D. Ionic strength

Answer: (C)

In the context of boiling point elevation, the "i" in the equation represents the Van't Hoff factor. This factor is crucial because it accounts for the degree of dissociation or ionization of a solute in a solution. When a solute dissolves in a solvent, it may dissociate into multiple particles (ions or molecules). The Van't Hoff factor quantifies how many particles result from the dissociation. For instance, a substance that dissociates into two ions, such as sodium chloride (NaCl), has a Van't Hoff factor of 2, while a non-dissociating substance, like glucose, has a factor of 1. The presence of more particles in the solution leads to a greater elevation of the boiling point, as described by the boiling point elevation equation: ΔT_b = i * K_b * m, where ΔT_b is the change in boiling point, K_b is the ebullioscopic constant of the solvent, and m is the molality of the solution. Understanding the Van't Hoff factor is essential in predicting how solutes behave in solution, particularly in applications involving colligative properties, which rely on the number of solute particles rather than their identity.

In the context of boiling point elevation, the "i" in the equation represents the Van't Hoff factor. This factor is crucial because it accounts for the degree of dissociation or ionization of a solute in a solution. When a solute dissolves in a solvent, it may dissociate into multiple particles (ions or molecules). The Van't Hoff factor quantifies how many particles result from the dissociation.

For instance, a substance that dissociates into two ions, such as sodium chloride (NaCl), has a Van't Hoff factor of 2, while a non-dissociating substance, like glucose, has a factor of 1. The presence of more particles in the solution leads to a greater elevation of the boiling point, as described by the boiling point elevation equation: ΔT_b = i * K_b * m, where ΔT_b is the change in boiling point, K_b is the ebullioscopic constant of the solvent, and m is the molality of the solution.

Understanding the Van't Hoff factor is essential in predicting how solutes behave in solution, particularly in applications involving colligative properties, which rely on the number of solute particles rather than their identity.