Why is the actual van\'t Hoff factor for a strong electrolyte not necessarily eq

Question

Why is the actual van't Hoff factor for a strong electrolyte not necessarily equal to the expected van't Hoff factor?

Sometimes ions will associate with one another in solution, which effectively reduces the number of dissolved particles. Sometimes, the strong electrolyte does not dissolve well in aqueous solution. This reduces the number of particles in solution, reducing the van't Hoff factor. Sometimes, the molality of the ions from the electrolyte cannot be predicted by the expected van't Hoff term. The solution may be too concentrated to accurately determine a van't Hoff factor, resulting in a deviation from the expected value.

Explanation / Answer

Because,

Sometimes ions will associate with one another in solution, which effectively reduces the number of dissolved particles.

Because,

Sometimes ions will associate with one another in solution, which effectively reduces the number of dissolved particles.

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