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Chapter 12: Problem 168

Draw pictures illustrating the solute-solvent interactions and the solvent- solvent interactions for methanol, \(\mathrm{CH}_{3} \mathrm{OH}\), in water. Is this a case of like dissolves like? Explain.

Short Answer

Expert verified
In the case of methanol (\(\mathrm{CH}_{3}\mathrm{OH}\)) dissolving in water, both solute and solvent have similar intermolecular forces, which is hydrogen bonding. The favorable solute-solvent interactions between methanol and water, as well as the solvent-solvent interactions within water and methanol, confirm that the "like dissolves like" principle applies in this scenario.

Step by step solution

01

Understand the "like dissolves like" principle

The "like dissolves like" principle states that polar solvents will dissolve polar solutes, and nonpolar solvents will dissolve nonpolar solutes. This is primarily due to the similarity in intermolecular forces within the solute and solvent, allowing them to interact favorably and dissolve one another.
02

Draw and label the structures of methanol and water

Methanol (\(\mathrm{CH}_{3}\mathrm{OH}\)) has a structure where three hydrogen atoms are attached to a central carbon atom, which is connected to an oxygen atom that has a hydrogen atom attached to it. Water (\(\mathrm{H}_{2}\mathrm{O}\)) has a structure where two hydrogen atoms are attached to a central oxygen atom.
03

Identify the dominant intermolecular forces in both molecules

In both methanol and water, the dominant intermolecular force is hydrogen bonding. Hydrogen bonding occurs when a hydrogen atom bonded to a highly electronegative atom (such as oxygen) is attracted to another highly electronegative atom. In this case, oxygen attracts hydrogen atoms in both molecules.
04

Analyze solute-solvent and solvent-solvent interactions

When methanol and water mix, the hydrogen bonding between the molecules allows for favorable solute-solvent interactions. Methanol can form hydrogen bonds with water molecules, so the methanol-water (solute-solvent) interaction is favorable. In the solvent-solvent interactions (water-water and methanol-methanol), hydrogen bonding is again the dominant force. This means that the solvent-solvent interactions are also favorable.
05

Determine if "like dissolves like" applies in this case

In the case of methanol dissolving in water, the principles of "like dissolves like" apply because both solute and solvent have similar intermolecular forces (hydrogen bonding). This allows the solute (methanol) to dissolve in the solvent (water), as favorable solute-solvent interactions exist. In conclusion, methanol dissolves in water following the "like dissolves like" principle, as both molecules exhibit hydrogen bonding as their primary intermolecular force, supporting favorable solute-solvent and solvent-solvent interactions.

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