Solubility Chemistry Example 4

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Example 4

hard
Explain why a scuba diver must ascend slowly, using the concept of gas solubility and Henry's Law. What happens to the dissolved nitrogen in the diver's blood as pressure decreases?

Solution

  1. 1
    Henry's Law states that gas solubility is directly proportional to the pressure of the gas above the liquid: C=kHƗPC = k_H \times P. At depth, high pressure increases nitrogen solubility in blood.
  2. 2
    If the diver ascends too quickly, the pressure drops rapidly, and dissolved nitrogen comes out of solution as bubbles in the bloodstream (decompression sickness or 'the bends').
  3. 3
    Ascending slowly allows nitrogen to gradually leave the blood through the lungs as pressure decreases, preventing dangerous bubble formation.

Answer

RapidĀ ascentĀ ā†’Ā pressureĀ dropĀ ā†’Ā N2Ā bubblesĀ inĀ bloodĀ (theĀ bends)\text{Rapid ascent ā†’ pressure drop ā†’ N}_2\text{ bubbles in blood (the bends)}
This is a life-threatening application of gas solubility principles. Henry's Law governs how gases dissolve under pressure, and decompression sickness demonstrates the consequences of violating these principles.

About Solubility

The maximum amount of a solute that can dissolve in a given quantity of solvent at a specific temperature and pressure, typically expressed as grams.

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