Question

What is the millimolar solubility of oxygen gas, o2, in water at 16 ∘c, if the pressure of oxygen is 1.00 atm?

Answer 1

`C=42.2mM`

Step-by-step explanation:

Hello,

By using the ideal gas equation, one could find the molar solubility for the given pressure as shown below:

`PV=nRT\\(n)/(V) =C=(P)/(RT)=(1.00atm)/(0.082 (atm*L)/(mol*K) * (16+273.15)K) \\C=0.0422mol/L=C=0.0422M`

Finally, as it is required in millimolar units, mM, one applies the following conversion:

`C=0.0422M*(1000mM)/(1M) \\C=42.2mM`

Best regards.

Answer 2

Partial pressure is the amount of pressure or force that is exerted by the atoms into the outer environment. it is dependent on the temperature and pressure of the present surroundings. in this case, we are asked in this problem to determine the partial pressure of oxygen at 16oC and 1 atm. We have to look into a solubility data table commonly found in handbooks and determined via experiments and correlations. According to literature, the value of the partial pressure is equal to 0.617 mM.This is under the assumption that the salinity of the water in which oxygen is dissolved is equal to zero.