posted by Linda .
A sample of 8.00 L of NH3 (ammonia) gas at 22 degree Celsius and 735 torr is bubbled into a 0.500 L solution of 0.400 M (hydrochloric acid).
The kb value for NH3 is 1.8 x 10^-5.
Assuming all the dissolves and that the volume of the solution remains at 0.500L , calculate the pH of the resulting solution.
Use PV = nRT to determine n for NH3 at the conditions listed. Write the equation for NH3 + HCl==>
the prepare an ICE chart. I suspect, but I've not worked the problem, that there will be an excess of NH3 for the reaction which will lead to a solution of NH3 and NH4Cl. Use the Henderson-Hasselbalch equation to solve for pH. If my assumption is wrong about being left with a buffer solution, another approach must be used.