A 500 mL sample of an equilibrium mixture of gaseous N2O4 and NO2 at 25°C and 753 mm of Hg was allowed to react with enough water to make 250.0 mL of solution at 25°C. Assume that all the dissolved N2O4 is converted to NO2 which disproportionates in water yielding a solution of nitrous acid and nitric acid. Assume further that disproportionation reaction goes to completion and that none of the nitrous acid disproportionates. The equilibrium constant ( Kp ) for N2O4(g)⇌2NO2(g) is 0.113 at 25°C. Ka for HNO2 is 4.5×10−4 at 25°C.
(1) Write balanced equation for disproportionation.
(2) What is molar concentration of NO2− and pH of the solution?
(3) What is osmotic pressure of solution?
(4) How many grams of lime ( CaO ) would be required to neutralize the solution?