Question

in denver, colorado the elevation is about 5,280 feet above sea level. explain what potential effects this may have on the solubility of a gaseous solute in a liquid solution.

Explanation:

Denver has high elevation, so atmospheric pressure is lower than at sea level. For gaseous solutes in liquid solutions, solubility depends on pressure (Henry's Law: $C = kP$, where $C$ is concentration, $k$ is Henry's constant, $P$ is partial pressure of gas). Lower atmospheric pressure means lower partial pressure of the gaseous solute above the liquid. According to Henry's Law, as the partial pressure of the gas decreases, its solubility in the liquid also decreases. So the gaseous solute's solubility in the liquid solution will be lower in Denver compared to at sea level.

Answer:

The solubility of a gaseous solute in a liquid solution will decrease in Denver (high elevation) because atmospheric pressure is lower there. By Henry's Law ($C = kP$), lower partial pressure of the gas (due to lower atmospheric pressure) leads to lower solubility of the gaseous solute in the liquid.