Chapter 14.4, Problem 29PP

Consider the following acids and their dissociation constants:
$\begin{array}{r}\hfill {\text{H}}_2{\text{SO}}_3(aq)+{\text{H}}_2\text{O}(l)\rightleftarrows {\text{H}}_3{\text{O}}^{+}(aq)+{\text{HSO}}_3^{-}(aq)\\ \hfill K_{\text{a}}=1.2\times {10}^{-2}\\ \hfill {\text{HS}}^{-}(aq)+{\text{H}}_2\text{O}(l)\rightleftarrows {\text{H}}_3{\text{O}}^{+}(aq)+{\text{S}}^{2-}(aq)\\ \hfill K_{\text{a}}=1.3\times {10}^{-19}\end{array}$
a. Which is the stronger acid, ${\text{H}}_2{\text{SO}}_3$ or ${\text{HS}}^{-}$ ?
b. What is the conjugate base of ${\text{H}}_2{\text{SO}}_3$ ?
c. Which acid has the weaker conjugate base?
d. Which acid has the stronger conjugate base?
e. Which acid produces more ions?