Final answer:
Aldehydes and ketones' ability to form hydrogen bonds with water through the carbonyl oxygen atom affects their solubility and boiling points, making them more soluble in water and having higher boiling points than alkanes but lower than alcohols.
Step-by-step explanation:
The consequence of the ability of aldehydes and ketones to form hydrogen bonds with water is seen in their physical properties. While they cannot hydrogen bond with themselves, the polar carbon-to-oxygen double bond allows them to engage in dipole-dipole interactions with water, which increases their solubility in water, especially for those with short carbon chains. Furthermore, these interactions result in boiling points that are higher than nonpolar molecules like alkanes but lower than alcohols, which form stronger hydrogen bonds. For instance, when comparing ethane, ethanal, and ethanol, we observe boiling points of -89°C, 20°C, and 78°C, respectively, highlighting how the presence of the functional group affects boiling points.