Final answer:
At the top of Mount Everest, the reduced atmospheric pressure and lower boiling point of water due to high elevation lead to a decrease in the solubility of gaseous solutes like oxygen in water.
Step-by-step explanation:
At the top of Mount Everest, the elevation is about 29,000 feet above sea level, which significantly impacts atmospheric conditions including pressure and temperature. Generally, the solubility of gases in liquids, such as the solubility of oxygen in water, is directly related to pressure — higher pressure increases the solubility of a gas. At Everest's summit, atmospheric pressure is much lower compared to sea level, which means the partial pressure of oxygen is also lower.
Consequently, the solubility of oxygen in water at the top of Mount Everest would decrease due to this reduced pressure. Furthermore, the boiling point of water decreases as elevation increases, which at the summit of Everest, can be as low as around 70°C, much lower than the 100°C boiling point at sea level. This combination of lower temperature and pressure would result in significantly lower amounts of dissolved oxygen in water at high altitudes.