Hydrogen chloride (HCl) gas is much more soluble than propane gas \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) in water, even though \(\mathrm{HCl}\) has a lower boiling point. Explain.

Polar molecules have areas of positive and negative charge, which means they have a dipole moment. This happens because the electrons in the molecule are not evenly distributed. Water (H₂O) and hydrogen chloride (HCl) are both examples of polar molecules.
In polar molecules, one end of the molecule is slightly positive, while the other end is slightly negative. This difference in charge allows polar molecules to interact strongly with each other and with other polar substances.
For example:

• Oxygen in H₂O is more electronegative than hydrogen, causing a partial negative charge on the oxygen atom.
• Similarly, chlorine in HCl is more electronegative than hydrogen, causing a partial negative charge on the chlorine atom.

In the case of solubility, water is a polar solvent, which makes it great at surrounding and interacting with other polar molecules like HCl, but it is less effective with nonpolar molecules such as propane (C₃H₈).

Hydrogen bonding is a strong type of dipole-dipole interaction that occurs between molecules where hydrogen is directly bonded to a more electronegative atom like oxygen, nitrogen, or fluorine. This bond causes hydrogen to have a slightly positive charge.
In water, hydrogen bonds play a crucial role in its properties. Each hydrogen atom of a water molecule can form a hydrogen bond with the oxygen atoms of neighboring water molecules.
Molecules like HCl can form hydrogen bonds with water because they have a hydrogen atom and a highly electronegative element (chlorine). These hydrogen bonds are stronger than other types of intermolecular forces, making the molecule highly soluble in polar solvents like water.
However, C₃H₈ cannot form such bonds due to its nonpolar nature, which makes it much less soluble in water. Thus, the ability to form hydrogen bonds significantly increases the solubility of substances in water.

Dipole-dipole interactions occur between polar molecules, where the positive end of one molecule is attracted to the negative end of another. These interactions are weaker than hydrogen bonds but stronger than Van der Waals forces.
When considering solubility, these interactions are critical. Water, being polar, has a high ability to interact with other polar molecules through dipole-dipole forces.
For example, because hydrogen chloride (HCl) is a polar molecule, it experiences strong dipole-dipole interactions with water molecules. As a result, it is highly soluble in water.
In contrast, propane (C₃H₈) is nonpolar and does not have a permanent dipole. Instead, it only exhibits weak dispersion forces, which do not interact strongly with water molecules. This is why propane is much less soluble in water compared to hydrogen chloride.
To summarize, dipole-dipole interactions significantly enhance the solubility of polar substances in polar solvents like water.