In higher altitudes the temperature is very low so conceptually the solubility should be high, but it is not so why in this example only pressure is taken into consideration? why not temperature?

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Solution

Dissolved oxygen concentration in water is dependant of water temperature but also of the partial pressure of oxygen (so of air) above the water. This is the Henry's law. If the partial pressure increases, then the Dissolved Oxygen concentration in water will also increase. When the altitude is increasing, the total atmospheric pressure decreases, and then the partial pressure of oxygen is also decreasing (assuming a constant proportion of O2 in air). You will then obtain a decrease of Dissolved Oxygen concentration with altitude elevation (at constant temperature and constant water composition of course). hence solubility decreases.

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