Hyperbaric chambers, which provide high pressures (up to 6 atm) of either air or pure oxygen, are used to treat a variety of conditions, ranging from decompression sickness in deep-sea divers to carbon monoxide poisoning. Look up the solubility of O 2 , N 2 , CO, and CO 2 in water at standard temperature and pressure (1 atm, 25 °C). b. Explain how elevated pressures in a hyperbaric chamber be used to treat decompression sickness (excess N 2 in blood) and carbon monoxide poisoning.

Welcome back, everyone. We need to explain how high pressure allows for the successful production of sparkling water. Note that the solubility of carbon dioxide in water is 0.1 69 g per 100 mL at standard temperature and pressure 1 a.m. and 25 Celsius. We have choice A which states that high pressure increases the solubility of carbon dioxide in water to form carbonic acid. Choice B which states that high pressure decreases the solubility of carbon dioxide in water so that gasses stay in the head space of the tightly sealed container. Choice C which states that high pressure maintains the solubility of carbon dioxide at its standard level and choice D which states that high pressure is not an important factor in the successful production of sparkling water. Let's begin by recalling our Henry's law and within Henry's law, we would recall that with an increase of pressure, we will have the correspondence of an increase in solubility of our gas. So in this case, in order to create sparkling water, we would have the reaction between carbon dioxide co two in gaseous form which reacts with water in liquid form. Note that this is an equilibrium reaction in which we would form one mole of a proton H plus as a product, as well as our anion of hydrogen carbonate. HCO +31 minus. Now, because hydrogen carbonate is formed, we would have its ionization which is followed where we would form our product, carbonic acid H two co three note that we're given our solubility of carbon dioxide equal to 0.169 g of CO2 per 100 mL of water. And based on Henry's law, we would imagine that if we increase our pressure of carbon dioxide gas, this will correspond to an increase in its solubility in water and the greater the solubility of our carbon dioxide. The more carbon carbonic acid H two co three is formed, meaning we have sparkling water as our product. And so we can understand that our high pressure of carbon dioxide is going to be maintained through a tight seal of the can of sparkling water. Now, looking at our answer choices, we would already based on what we've outlined, be able to rule out choice B since it states that high pressure decreases the solubility of carbon dioxide. And we would disagree with that statement, high pressure would increase its solubility. We would also be able to rule out choice C because it states that high pressure maintains the solubility of carbon dioxide at its standard level where we know that the high pressure would be exponentially increasing our solubility of carbon dioxide to form even more carbonic acid. And then choice D we can also rule out because it says that high pressure is not an important factor in the production of sparkling water when we know that it is. And so our final answer will be choice. A which states that high pressure increases the solubility of carbon dioxide in water to form carbonic acid. So I hope that this made sense and let us know if you have any questions.

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9. Solutions

Intro to Henry's Law

GOB Chemistry

9. Solutions

Intro to Henry's Law

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Problem 96b

Textbook Question

Hyperbaric chambers, which provide high pressures (up to 6 atm) of either air or pure oxygen, are used to treat a variety of conditions, ranging from decompression sickness in deep-sea divers to carbon monoxide poisoning. Look up the solubility of O₂, N₂, CO, and CO₂ in water at standard temperature and pressure (1 atm, 25 °C).
b. Explain how elevated pressures in a hyperbaric chamber be used to treat decompression sickness (excess N₂ in blood) and carbon monoxide poisoning.

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Decompression sickness occurs when nitrogen (N₂) gas, which is dissolved in the blood under high pressure (e.g., during a deep-sea dive), forms bubbles as the pressure decreases too quickly. This can cause pain and other serious symptoms.

According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. Mathematically, this is expressed as:

C = k P

, where

C

is the concentration of the gas,

k

is the solubility constant, and

P

is the partial pressure of the gas.

In a hyperbaric chamber, the pressure is increased to several atmospheres, which increases the solubility of nitrogen in the blood. This helps dissolve nitrogen gas bubbles back into the blood, alleviating the symptoms of decompression sickness.

Carbon monoxide (CO) poisoning occurs because CO binds to hemoglobin in red blood cells with a much higher affinity than oxygen (O₂), reducing the blood's ability to carry oxygen to tissues.

In a hyperbaric chamber, the high pressure of pure oxygen increases the partial pressure of O₂ in the blood. This promotes the displacement of CO from hemoglobin and increases the oxygen supply to tissues, helping to treat carbon monoxide poisoning.

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Key Concepts

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

Henry's Law

Henry's Law states that the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of that gas above the liquid. In the context of hyperbaric chambers, increasing the pressure allows more oxygen and nitrogen to dissolve in the blood, which is crucial for treating conditions like decompression sickness and carbon monoxide poisoning.

Decompression Sickness

Decompression sickness, also known as 'the bends,' occurs when nitrogen dissolved in the blood forms bubbles as pressure decreases during ascent from deep water. Hyperbaric treatment helps by increasing pressure, allowing excess nitrogen to dissolve back into the blood, thus preventing bubble formation and alleviating symptoms.

Carbon Monoxide Poisoning

Carbon monoxide poisoning occurs when CO binds to hemoglobin in red blood cells more effectively than oxygen, reducing oxygen transport. Hyperbaric oxygen therapy increases the amount of dissolved oxygen in the blood, displacing carbon monoxide from hemoglobin and facilitating its elimination from the body.

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