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Four liters of water are equilibrated with a gas mixture containing carbon dioxide at a partial pressure of .3 atm. Henry's law constant for H2CO3* solubility is 2.0 g/L-atm.
a. How many grams of Co2 are dissolved in the water? What is the pH of this water? (Neglect the 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 the secondary dissociation). Find the PH of this solution and compare it to the result obtained in (a).
How many moles of each are present in the eq mixture b)Calculate the equilibrium constant
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