Scuba divers breathing air at increased pressure can suffer from oxygen toxicity—too much oxygen in their bloodstream— when the partial pressure of oxygen exceeds about 1.4 atm. What happens to the amount of oxygen in a diver's bloodstream when he or she breathes oxygen at elevated pressures? How can this be reversed?

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Understand that the amount of a gas dissolved in a liquid is described by Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

Recognize that when a diver breathes air at increased pressure, the partial pressure of oxygen increases, leading to more oxygen dissolving in the bloodstream.

Identify that oxygen toxicity occurs when the partial pressure of oxygen in the bloodstream exceeds safe levels, causing harmful effects.

To reverse oxygen toxicity, the diver should reduce the partial pressure of oxygen by ascending to a lower depth, thereby decreasing the pressure and the amount of oxygen dissolved in the blood.

Consider using a gas mixture with a lower oxygen concentration, such as nitrox or trimix, to prevent oxygen toxicity during deep dives.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Partial Pressure

Partial pressure refers to the pressure exerted by a single component of a gas mixture. In the context of scuba diving, as a diver descends, the total pressure increases, which also raises the partial pressure of the gases they breathe, including oxygen. This relationship is described by Dalton's Law, which states that the total pressure of a gas mixture is the sum of the partial pressures of its individual gases.

Oxygen Toxicity

Oxygen toxicity occurs when the partial pressure of oxygen in the bloodstream becomes excessively high, leading to harmful physiological effects. Symptoms can include visual disturbances, seizures, and lung damage. This condition is particularly relevant for divers, as breathing oxygen at pressures above 1.4 atm can overwhelm the body's ability to process oxygen safely, resulting in toxicity.

Reversal of Oxygen Toxicity

Reversing oxygen toxicity primarily involves reducing the partial pressure of oxygen in the diver's environment. This can be achieved by ascending to shallower depths where the pressure is lower, thereby decreasing the partial pressure of oxygen in the lungs and bloodstream. Additionally, administering pure oxygen in a controlled environment can help manage symptoms and facilitate recovery.

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Textbook Question

An aqueous NaCl solution is made using 102 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the molality of the solution. (Assume a density of 1.08 g>mL for the solution.)

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Textbook Question

A KNO3 solution containing 35 g of KNO3 per 100.0 g of water is cooled from 40 °C to 0 °C. What happens during cooling? (Use Figure 14.11.)

Textbook Question

An aqueous NaCl solution is made using 102 g of NaCl diluted to a total solution volume of 1.00 L. Calculate the molarity of the solution. (Assume a density of 1.08 g>mL for the solution.)

Textbook Question

A KNO3 solution containing 35 g of KNO3 per 100.0 g of water is cooled from 40°C to 0°C. What happens during cooling? (Use Figure 14.11.)