Can someone please explain where and how they got the 1.15 *10^-3 mol/L in this problem?

Thermal Pollution and Oxygen Solubility A certain species of freshwater trout requires a dissolved oxygen concentration of 7.5mg/L. Could these fish thrive in a thermally polluted mountain stream (water temperature is 30.0C, partial whes - . of atmospheric oxygen is 0.17atm) ? Firsi, compute the Henry's law constant for oxygen in water at the specified temperature of 30.0C (see Eigure 11.19). k=PgCg=1.15103mol/L/1.00atm=1.15103mol/Latm Then, use thic \& value to compute the oxygen solubility at the specified oxygen partial pressure, 0.17 atm. Ck=kPk=(1.15103mol/Latm)(0.17atm)=1.95104mol/L Finally, convert this dissolved oxygen concentration from mol/L to mg/L. (1.95104mol/L)(32.0g/lmol)(1000mg/g)=6.2mg/L. This concentration is lesser than the required minimum value of 7.5mg/h, and so these trout would likely not thrive in the polluted stream. Check Your Learning What dissolved oxygen concentration is expected for the stream above when it returns to a normal summer time temperature of 15C