Four liters of water are equilibrated with a gas mixture containing carbon dioxide at a partial pressure of 0.3 atm. Henry's law constant for H2CO3* solubility is 2.0g/L-atm.
a) How many grams of CO2 are dissolved in the water? What is the pH of this water? (neglect secondary dissociation of carbonic acid.)
b) Assume that H2CO3* dissolves first without dissociating, achieving equilibrium with the atmosphere, and then the solution is closed to the atmosphere. H2CO3* then dissociates (neglect secondary dissociation). Find the pH of this solution and compare it to the result obtained in (a).