## Chemistry and Chemical Reactivity (9th Edition)

$1.526\times10^{-6}\ g/mL$
Vapor pressure of water: $23.8\ torr\times 1.0\ bar/750.06\ torr=0.032\ bar$ The partial pressure of Hydrogen: $1.00-0.032=0.968\ bar$ Henry's Law: $S=k_HP$ $S=7.8\times10^{-4}\ mol/kg.bar\times0.968\ bar$ $S=7.55\times10^{-4}\ mol/kg$ Assuming that the mass of the mixture is approximately the mass of water and that it has a density of 0.001 kg/mL $7.55\times10^{-4}\ mol/kg\times 2.02\ g/mol\times0.001\ kg/mL=1.526\times10^{-6}\ g/mL$