Chapter 4, Problem 4.149MP

Compound X contains only the elements C, H, O, and S. A5.00 g sample undergoes complete combustion to give 4.83 gof ${\text{CO}}_{\text{2}}$ , 1.48 g of ${\text{H}}_{\text{2}}\text{O}$ , and a certain amount of ${\text{SO}}_{\text{2}}$ that is further oxidized to ${\text{SO}}_{\text{3}}$ and dissolved in water to form sulfuric acid, ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ . On titration of the ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ , 109.8 mLof 1.00 M NaOH is needed for complete reaction. (Both Hatoms in sulfuric acid are acidic and react with NaOH.)
(a) What is the empirical formula of X?
(b) When 5.00 g of X is titrated with NaOH, it is found that X has two acidic hydrogens that react with NaOH and that54.9 mL of 1.00 M NaOH is required to completely neutralize the sample. What is the molecular formula of X?