Originally Posted by pop
NOTE: POPíS OPINION IS NOT ASSOCIATED WITH ANY FACT OR RESEARCH, IF THERE IS ANY RELATIONSHIP WITH A KNOWN FACT OR TRUTH OR SCIENCE THAT RELATIONSHIP IS ACCIDENTAL.
So what you are saying is that this is purely fictional...
Originally Posted by pop
is it possible that atmosphere nitrogen dissolves in water and maybe pressure is related to how fast organic nitrogen is dissolved and saturation levels reached. Organic nitrogen may be important to the micro ecology of the water column. By gassing out do you mean evaporation into the atmosphere?
It does dissolve in water to somewhere around 20ppm at 1 atmosphere at around room temperature.
Ammonia, nitrite and nitrate are far more readily dissolved in water so the N2 will not affect their respective concentrations in any easily measurable way. Seeing as air is always about 78% N2 this is a constant factor and not something that we can change and even if we bumped it up to 100% the water will not absorb much more than the atmospheric air baseline.
By off gassing I am suggesting that the concentration of N2 dissolved in the water will not increase past the approximate 20ppm level from the air. If there is a source of N2 from within the tank it will form micro bubbles of undissolved gas and escape to the surface. This is what happens when divers get the "bends" as the nitrogen gas comes out of solution in the blood stream and cannot be off gassed fast enough through respiration. It only builds up due to the increased pressure under the water. As the air is breathed (with it's 78% N2 content) it diffuses into the blood. At depth, say 90 feet, the pressure is equivalent to 4 atmospheres (this affects the air breathed by compressing it) which means that there is just more N2 per breath which will dissolve into the blood that much more readily due to the pressure.
NH3 concentration can be as high as 500,000ppm (yes that is the same as half of the water being ammonia) but this cannot happen in a natural setting as there would never be that much ammonia to be dissolved in the water. The point being that ammonia is so readily dissolved that a little N2 won't affect it.
For reference, CO2 can be as high as 1,500ppm, but again, this is not possible as a 100% pure CO2 atmosphere would be needed to do this.
There are some charts that reference gas solubility in water at this link
. I knew the reasoning but didn't realize the numbers would be so large for CO2 and NH3.
Sorry, no proof reading time this time.