Hope someone can clear something up for me. I'm working with some dissolved nutrients - Having measures for Nitrate (NO3, µg/l), Nitrite (NO2, µg/l) and Ammonium (NH4, µg/l). Grouping these in a pool called Dissolved Inorganic Nitrogen (DIN)
using µg/l seems to be a straight forward addition. Example:
NO2=0,56 µg/l NO3=12,89µg/l NH4=6,55µg/l => DIN = 20 µg/l
Converting each component into µM (µmoles/l) using the molar weights of each substance (NO2 = 46 µg/µmole, NO3 = 62µg/µmole and NH4 = 18µg/µmole) is all fine - but there is a big difference in taking the DIN µg/l and the collected µg/µmole (126 µg/µmole) and computing a DIN in µM versus
just adding up the individual components...
How is this different?
NO2: 0,56 µg/l = 0,012 µM
NO3: 12,89 µg/l = 0,21 µM ------> added up this gives 0,582 µM DIN
NH4: 6,55 µg/l = 0,36 µM
DIN: 20 µg/l = 0,159 µM (using the collected 126 µg/µmole of all components)... So the results are 0,582 µM DIN vs. 0,159 µM
What is the correct if any and what is the reason this logic does not work. Is there some sort of scientific logic that rules out one of the above methods?
All answers are appreciated