Assuming that the concentration determined in the previous

Reference no: EM13635023

Ammonia NH3 with Kb = 1.8 x 10^05 is added to 100 mL of waterat room temperature and the vapor pressure of water above thesoultion drops to P = 0.03 atm. What is the pH of the solution inthe limit that any gas phase NH3 is negliglble.

a) Calculate the vapor pressure above room temperature waterwhere delta H vapor = 40.7 kj/mol
I got .815 atm not sure if it's right

b) Calculate the mole fraction of the solvent from Raoult'slaw from part a.

c) Calculate the total number of moles of the solute from thesolvent mole fraction.

d) What is the total solute concentration assuming a constant100 mL volume?

e) Assuming that the concentration determined in the previousstep corresponds to the inital amount of added NH3 (aq), what is the pH of the solution?

Reference no: EM13635023

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