Question

At a depth of 100 ft in water, the external pressure is 4.0 atm. What is the solubility of N2 from air in blood at this pressure

Answer 1

Answer:

Solubility  = 2.142 x  $10^{-4}$ M

Explanation:

Solution:

Note: This question is incomplete and lacks necessary data to solve this question. But I have found similar question on the internet and fetched the necessary data to solve:

Missing Data:

Number of Moles of N2 dissolved per litre of blood = 5.357 x $10^{-4}$ M

As we know that, the air is approximately. 78 mol % of N2

N2 = 0.78

Partial pressure of the N2 at 100 ft:

Partial Pressure = 0.78 x (4.0)

Partial Pressure = 3.12 atm

Now, this is 4 times the pressure of nitrogen at 1 atm air pressure.

SO,

According to the Henry's Law, we have:

Solubility = k x $P_{g}$

Here, k = 4 times

So,

Solubility = 4 x (5.357 x $10^{-4}$)

Solubility  = 2.142 x  $10^{-4}$ M