Acid rain results from the reaction of nitrogen dioxide with water in the air. Unbalanced equation: NO2(g) + H2O(l) --> HNO3(aq) + NO(g)

A water spray is sometimes used in exhaust stacks at coal-fired power plants to help prevent acid rain. Given the following parameters, calculate the concentration of the nitric acid in 8L of wastewater (assume no evaporation ... I know this is not reality but let's make the calculation a bit easier!).

1000L/min vented through the exhaust stack
assume a constant concentration of the nitrogen dioxide is entering the water spray at 0.19mg/L
The scrubber sprays 0.500L/min
Assume 100% of the nitrogen dioxide reacts with the water. Assume water is present in excess so the nitrogen dioxide is the limiting reactant.
Because of the large excess of water, you do not need to adjust the volume of water for the amount consumed in the reaction. That would make for a sneaky question!

This is a multi-step stoichiometry problem that requires you make multiple conversions. You must first balance the equation!

Report your answer to two significant figures.