Federal regulations set an upper limit of 50 ppm of NH3 in the air in a work environment ( that is, 50molecules of ammonia for every million molecules in the air). Airfrom a manufacturing operation was drawn through a solutioncontaining 1.00 x 102 mL of 0.0105 M HCl. TheNH3 reacts with the HCl to form NH4Cl. After drawing air through the acid solution for10.0 minutes at a rate of 10.0 L/min, the acid was titrated. Theacid left after the reaction with ammonia took 13.1 mL of 0.0588 MNaOH.
a) Write a balanced chemical equation for the reaction.
b) Calculate the grams of ammonia drawn into the solution.
c) If air has a density of 1.20 g/L and an average molar mass of19.0, calculate the ppm of NH3 in theair.
d) Is the manufacturer in compliance with the regulation?