Chapter 9, Problem 9.69P

For each pair of acids: $[1]$ Label the stronger acid. $[2]$ Draw the conjugate bases. $[3]$ Label the
stronger conjugate base.
a. $\begin{array}{c}{\text{HSO}}_{\text{4}}{}^{\text{-}}\\ \text{bisulfate}\\ K_a=1.2\times {10}^{-2}\end{array}$ or $\begin{array}{c}{\text{H}}_2{\text{PO}}_{\text{4}}{}^{\text{-}}\\ \text{dihydrogen phosphate}\\ K_a=6.2\times {10}^{-8}\end{array}$
b. $\begin{array}{c}{K}_a=1.2\times {10}^{-2}\\ {\text{CH}}_{\text{3}}{\text{CH}}_{\text{2}}\text{COOH}\\ \text{Propanoic acid}\\ K_a=1.3\times {10}^{-5}\end{array}$ or $\begin{array}{c}{K}_a=6.2\times {10}^{-8}\\ {\text{CH}}_{\text{3}}\text{COOH}\\ \text{acetic acid}\\ K_a=1.8\times {10}^{-5}\end{array}$