The Henry's Law constant for hydrogen sulfide (H2S), a flammable gas with a rotten egg mol smell, is 0.1 When hydrogen sulfide gas dissolves in water, it acts as a weak acid with L atm a pka of 7.04 that reversibly dissociates according to: H2S 4 H+ + HS- If you bubble pure hydrogen sulfide gas through a solution of water and measure a pH of 4.7, what is the mass concentration of HS-, in units of mg/L? Hints: Yes, you do need to use the Henry's Law constant -- this question combines an old topic with a new one. Molar mass of sulfur is 32.07 g/mol When bubbling a gas through water you can assume the bubbles are at atmospheric pressure. Think about what "pure" means with respect to the mixing ratio