Suppose 95.0 mL of HCl gas at 25 ºC and 707 torr is bubbled into 298 mL of pure water. What will be the pH of the resulting solution, assuming all the HCl dissolves in the water?

Answer 1

Use PV = nRT and solve for n = number mols HCl.
The M HCl = mols HCl/L solution.
Then pH = -log(HCl)

Answer 2

(0.930atm*0.393L)/(0.0821*298)= 0.0149mol
0.0149mol/0.393L= 0.038
-log(0.038)= 1.42
what did I do wrong?