Chapter 4, Problem 116AE

When organic compounds containing sulfur are burned,sulfur dioxide is produced. The amount of ${\text{SO}}_{\text{2}}$ formedcan be determined by the reaction with hydrogenperoxide:

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

The resulting sulfuric acid is then titrated with a standardNaOH solution. A 1.302-g sample of coal isburned and the ${\text{SO}}_{\text{2}}$ is collected in a solution of hydrogenperoxide. It took 28.44 mL of a 0.1000-M NaOHsolution to titrate the resulting sulfuric acid. Calculatethe mass percent of sulfur in the coal sample. Sulfuricacid has two acidic hydrogens.