For each conjugate acid-base pair, identify the first species as an acid or base and the second species as its conjugate acid or conjugate base. In addition, draw Lewis structures for each species, showing all valence electrons and any formal charges. (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{HSO}_{4}{ }^{-}\) (b) \(\mathrm{NH}_{3}, \mathrm{NH}_{2}{ }^{-}\) (c) \(\mathrm{CH}_{3} \mathrm{OH}, \mathrm{CH}_{3} \mathrm{O}^{-}\)

(a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{HSO}_{4}{ }^{-}\) In this pair, \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is the acid (donates \(\mathrm{H}^{+}\)) and \(\mathrm{HSO}_{4}{ }^{-}\) is the conjugate base (accepts \(\mathrm{H}^{+}\)). Lewis structure for \(\mathrm{H}_{2} \mathrm{SO}_{4}\): ``` O || S - O - H || O - H ``` Lewis structure for \(\mathrm{HSO}_{4}{ }^{-}\): ``` O- | S - O - H || O ``` (b) \(\mathrm{NH}_{3}\) and \(\mathrm{NH}_{2}{ }^{-}\) In this pair, \(\mathrm{NH}_{3}\) is the base (accepts \(\mathrm{H}^{+}\)) and \(\mathrm{NH}_{2}{ }^{-}\) is the conjugate acid (donates \(\mathrm{H}^{+}\)). Lewis structure for \(\mathrm{NH}_{3}\): ``` H | N - H | H ``` Lewis structure for \(\mathrm{NH}_{2}{ }^{-}\): ``` H | N - H | : ``` (c) \(\mathrm{CH}_{3} \mathrm{OH}\) and \(\mathrm{CH}_{3} \mathrm{O}^{-}\) In this pair, \(\mathrm{CH}_{3} \mathrm{OH}\) is the acid (donates \(\mathrm{H}^{+}\)) and \(\mathrm{CH}_{3} \mathrm{O}^{-}\) is the conjugate base (accepts \(\mathrm{H}^{+}\)). Lewis structure for \(\mathrm{CH}_{3} \mathrm{OH}\): ``` H | O - H | C - H | H ``` Lewis structure for \(\mathrm{CH}_{3} \mathrm{O}^{-}\): ``` O- | C - H | H ```