Questions: What were the differences between solvents that dissolved aspirin the best/worst? Explain with structural comparisons and intermolecular forces.

What were the differences between solvents that dissolved aspirin the best/worst? Explain with structural comparisons and intermolecular forces.
Transcript text: What were the differences between solvents that dissolved aspirin the best/worst? Explain with structural comparisons and intermolecular forces.
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Solution

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Solution Steps

Step 1: Identify the Solvents

To determine the differences between solvents that dissolved aspirin the best and the worst, we first need to identify the solvents in question. Common solvents for aspirin include water, ethanol, acetone, and hexane.

Step 2: Analyze Structural Properties

Aspirin (acetylsalicylic acid) has both polar (carboxyl and ester groups) and non-polar (benzene ring) regions. Solvents can be categorized based on their polarity:

  • Polar solvents: Water, ethanol
  • Non-polar solvents: Hexane
  • Intermediate polarity: Acetone
Step 3: Intermolecular Forces

The solubility of aspirin in these solvents depends on the intermolecular forces:

  • Water: Strong hydrogen bonding due to its high polarity.
  • Ethanol: Moderate hydrogen bonding and dipole-dipole interactions.
  • Acetone: Dipole-dipole interactions, but no hydrogen bonding.
  • Hexane: London dispersion forces (weakest).
Step 4: Compare Solubility

Aspirin is more soluble in solvents that can engage in hydrogen bonding and dipole-dipole interactions:

  • Best solvents: Ethanol (moderate polarity, hydrogen bonding) and acetone (dipole-dipole interactions).
  • Worst solvent: Hexane (non-polar, only London dispersion forces).

Final Answer

The differences between solvents that dissolved aspirin the best and the worst are primarily due to their polarity and the types of intermolecular forces they can engage in. Polar solvents like ethanol and acetone dissolve aspirin better due to hydrogen bonding and dipole-dipole interactions, while non-polar solvents like hexane dissolve aspirin poorly due to weak London dispersion forces.

\(\boxed{\text{Best solvents: Ethanol, Acetone}}\)

\(\boxed{\text{Worst solvent: Hexane}}\)

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