Question

Which of the following statements regarding solubility is incorrect? a. A polar compound dissolves an ionic compound due to ion-dipole interactions. b. A nonpolar solvent will not interact strongly enough with ions to dissolve an ionic compound. c. Nonpolar liquids will dissolve in one another because the intermolecular forces in the pure liquids are weak, and there is an increase in entropy. d. Most ionic solids are more soluble in water at higher temperatures than at lower temperatures. e. Most gases are more soluble in water at higher temperatures than at lower temperatures.

Answer 1

The incorrect statement about solubility is that gases are more soluble at higher temperatures; in truth, gases are typically less soluble in water as the temperature increases. Ionic compounds tend to be more soluble at higher temperatures, while nonpolar liquids are miscible due to similar intermolecular forces. The inncorect option is e. Most gases are more soluble in water at higher temperatures than at lower temperatures.

Step-by-step explanation:

The statement that is incorrect regarding solubility is 'Most gases are more soluble in water at higher temperatures than at lower temperatures.' This is because, in general, the solubility of gases in liquids decreases with an increase in temperature. Conversely, most ionic solids are indeed more soluble in water at higher temperatures.

When a polar solvent such as water encounters an ionic compound, ion-dipole interactions occur, leading to the dissolution of the ionic compound. On the other hand, a nonpolar solvent like hexane, which does not have a dipole moment, does not effectively interact with ions and therefore cannot dissolve ionic compounds.

Regarding miscibility, nonpolar liquids tend to dissolve in each other due to their similar weak intermolecular dispersion forces and the increase in entropy upon mixing. This principle is often summarized as 'like dissolves like.'