Henry's Law and the Relative Concentrations of Dissolved Gasses in Water or the Blood at Sea Level
Relative partial pressures at sea level (mm Hg)**
Relative concentrations of
dissolved gases at sea level:
[N2]:[O2]:[CO2]= 3:1:8
water
[N2]:[O2]:[CO2] = 3:65:165
blood

pN2 (572)  / pO2 (107) / pCO2 (36) / pH2O (45)
Dalton's Law:  Total pressure (P) of a gas mixture approximately equals to the sum of the partial pressures of the individual gases in the mixture. to the mole fractions of each gas.
P = pN2 + pO2 + pCO2 + pH2O
Raoult's Law:  The partial pressure (pN2 etc.) of one gas in a mixture of gases approximately equals the mole fraction (fN2, etc.) of that gas times the total pressure, P.
At sea level, P1 atm = 760 mm Hg.
fN2  =  pN2/P (= 36)       fO2  =  PO2/P (= 0.1)
fCO2  =  pCO2/P (= 36)     fH20  =  POH2O/P (= 0.06)
Henry's Law:  The dissolved concentration of a gas is approximately proportional to its partial pressure by a unique empirically-determined constant called Henry's constant:  KN2, KO2, KCO2, or KH20.
At sea level, P1 atm = 760 mm Hg.
[N2] = pN2/KN2 [O2] = pO2/KO2  [CO2] = pCO2/KCO2   [H2O] = pH2O/KH20
KN2/KO2 = 3/2    KN2/KCO2 = 1/50 [N2]/[O2] = 5/2 [N2]/[CO2] = 1/3
Water at sea level: [N2]/[O2]/[CO2] = 3/1/8
Blood at sea level: [N2]/[O2]/[CO2] = 3/65/165
** Based on D. Freifelder Physical Chemistry for Students of Biology and Chemistry Science Books International (1982), pp. 210-211 © January 27, 2021