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Nitric acid can be prepared by bubbling dinitrogen pentoxide into water.
N2O5(g) + H2O -> 2H+(aq) + 2NO3-(aq)
a) How many moles of H+ are obtained when 1.50 L of N2O5 at 25 degrees C and 1.00 atm pressure is bubbled into water?
b) The solution obtained in (a) after reaction is complete has a volume of 437 mL. What is the molarity of the nitric acid obtained?

Here is my work for (a)- does it look ok?
n= PV/RT
(1.00 atm x 1.50 L/ .08206 L x atm/mol x K x 298.15 K)= .0613 mol N2O5 x 2= .123 mol H+

If this is correct [I don't know if I made assumptions that I shouldn't have made], how do I do (b)? I know I need to get an answer in mol/L but I'm not sure how to do that.

Your work looks ok to me, Dave. You are also correct that molarity must come out in mols/L so mols/L =
0.123 mols/1.5 L = ??

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