Chapter 15, Problem 143CP

When organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of SO₂formed can be determined by the reaction with hydrogen peroxide:

${\text{H}}_{\text{2}}{\text{O}}_{\text{2}}\left(\text{aq}\right)+{\text{SO}}_{\text{2}}\left(\text{g}\right){\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}\left(\text{aq}\right)$

The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1 .302-g sample of coal is burned, and the SO₂is collected in a solution of hydrogen peroxide. It took 28.44 mL of a 0.1000 M NaOH solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.