Final answer:
Methanol is more soluble in water than 1-octanol due to its smaller size, more polar nature, and ability to form extensive hydrogen bonds with water molecules, whereas 1-octanol's longer nonpolar carbon chain reduces these interactions, thus reducing its solubility in water.
Step-by-step explanation:
The question is focused on why methanol is more soluble in water than 1-octanol. To answer this, we compare the molecular structures of both compounds. Methanol has one carbon with an OH group, making it highly polar and allowing it to create hydrogen bonds with water molecules. 1-Octanol, however, has a longer carbon chain which makes its nonpolar part dominant over its polar OH group, leading to weaker interactions with water and less solubility.
Hydrogen bonding is crucial in the solubility of substances in water. Smaller alcohols like methanol can engage in extensive hydrogen bonding due to their small size, which makes them miscible in water in all proportions. In contrast, as the carbon chain length increases in alcohols like 1-octanol, the nonpolar influence becomes greater, diminishing their ability to dissolve in water significantly.
The polarity of the molecules plays a significant role in solubility. Methanol, being highly polar due to its short carbon chain and OH group, is highly soluble in water. On the other hand, the long carbon chain of 1-octanol limits its polarity, making it less soluble in water.