Answer
a. $H_2SO_3$ is the stronger acid.
b. $HS{O_3}^-$ is the conjugate base of $H_2SO_3$
c. $H_2SO_3$ has the weaker conjugate base.
d. $HS^-$ has the stronger conjugate base.
e. $H_2SO_3$ produces more ions.
Work Step by Step
a. Since $H_2SO_3$ has a larger $K_a$ value than $HS^-$, it is a stronger acid.
$$1.2 \times 10^{-2} \gt 1.3 \times 10^{-19}$$
b. As we can see by the reaction, when $H_2SO_3$ loses a proton, it produces $HS{O_3}^-$.
c. The stronger the acid, the weaker its conjugate base. Therefore, $H_2SO_3$ has the weaker conjugate base.
d. The weaker the acid, the stronger its conjugate base. Thus, $HS^-$ has the stronger conjugate base.
e. The stronger acid produces more ions. So, $H_2SO_3$ produces more ions.
