Scientists determine the quantity of atmospheric sulfur dioxide ( SO2 ), a large contributor to acid rain, by an indirect titration. First, a scientist collects a sample of air and reacts it with hydrogen peroxide ( H2O2 ) to form a solution of sulfuric acid ( H2SO4 ). Then, the amount of H2SO4 produced is determined by titration with a sodium hydroxide solution ( NaOH ) of known concentration. H2O2(aq)+SO2(g)⟶H2SO4(aq) H2SO4(aq)+2NaOH(aq)⟶2H2O(l)+Na2SO4( aq) Suppose Lane collects a 658.0 g sample of air that is known to contain SO2 and reacts it with excess H2O2 . A volume of 22.4 mL of 0.025 M NaOH is required to neutralize the H2SO4 produced. Calculate the mass percent of SO2 in the air sample.