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Boiling Points of Carboxylic Acids
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✔ https://StudyForce.com • ✔ https://Biology-Forums.com • ✔ Ask questions here: https://Biology-Forums.com/index.php?... • Follow us: • ▶ Facebook: / studyforceps • ▶ Instagram: / studyforceonline • ▶ Twitter: / studyforceps • Q1. Match each of the compounds 2-butanol, pentane, propanoic acid with a boiling point of 141 °C, 100 °C, or 36 °C. (They have about the same molar mass.) • Q2. Why would methanoic acid (molar mass 46, bp 101 °C) have a higher boiling point than ethanol (molar mass 46, • bp 78 °C)? • The boiling point increases when the molecules of a compound can form hydrogen bonds or have dipole–dipole attractions. Pentane has the lowest boiling point, 36 °C, because alkanes cannot form hydrogen bonds or dipole–dipole attractions. 2-Butanol has a higher boiling point, 100 °C, than pentane because an alcohol can form hydrogen bonds. Propanoic acid has the highest boiling point, 141 °C, because carboxylic acids can form stable dimers through hydrogen bonding to increase their effective molar mass and therefore their boiling points. • Two methanoic acid molecules form a dimer, which gives an effective molar mass that is double that of a single acid molecule. Thus, a higher boiling point is required than for ethanol.
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