Problem: For each compound, would you expect greater solubility in water or in hexane? Indicate the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble.

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We're being asked to determine whether each compound has a greater solubility in water or in hexane and determine the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble.

Recall that the main idea in dissolution is like dissolves like, which means compounds with the same polarity and intermolecular force can dissolve each other.

Let's first determine the intermolecular forces present in water and hexane:

• Water (H2O) is a polar molecule that exhibits hydrogen bonding, so the best solute is another polar compound that also exhibits hydrogen bonding.

• Hexane is an example of a hydrocarbon, a compound composed only of carbons and hydrogens. Hydrocarbons are nonpolar compounds. This means that hexane is a nonpolar molecule that exhibits dispersion forces.

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Problem Details

For each compound, would you expect greater solubility in water or in hexane? Indicate the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Solutions, Molarity and Intermolecular Forces concept. You can view video lessons to learn Solutions, Molarity and Intermolecular Forces. Or if you need more Solutions, Molarity and Intermolecular Forces practice, you can also practice Solutions, Molarity and Intermolecular Forces practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Gerard Domanski's class at OAKLAND.