Why Ammonia is a deviation from the Henry's Law,when it is dissolved in water?
Does that has anything to do with Ammonia having Hydrogen bonds? Or what could be the reason?
To understand why ammonia is a deviation from Henry's Law when dissolved in water, we first need to revisit Henry's Law itself. Henry's Law states that at a constant temperature, the amount of gas dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid.
However, ammonia (NH3) deviates from Henry's Law when it dissolves in water due to the formation of hydrogen bonds. Hydrogen bonding occurs when the hydrogen atom in a molecule, in this case, ammonia, forms a bond with an electronegative atom, such as oxygen or nitrogen. In water, hydrogen bonding is especially prevalent.
When ammonia dissolves in water, some of the ammonia molecules attract water molecules, and hydrogen bonds are formed between them. These hydrogen bonds cause the ammonia-water solution to deviate from Henry's Law because the presence of hydrogen bonding affects the solubility of ammonia.
The hydrogen bonding in the ammonia-water solution leads to stronger intermolecular interactions, making it more difficult for ammonia molecules to escape from the solution and enter the gas phase. As a result, the solubility of ammonia in water is higher than what would be expected based on Henry's Law.
In summary, the deviation of ammonia from Henry's Law when dissolved in water is primarily due to the formation of hydrogen bonds between ammonia and water molecules. This leads to stronger intermolecular interactions and a higher solubility of ammonia in water than predicted by Henry's Law.