91Ó°ÊÓ

Define (a) an Arrhenius acid and (b) an Arrhenius base.

Write an equation for the reaction that takes place when each acid is added to water. (a) \(\mathrm{HNO}_{3}\) (b) \(\quad \mathrm{HBr}\) (c) \(\mathrm{HCO}_{3}^{-}\) (d) \(\quad \mathrm{NH}_{4}^{+}\)

Write an equation for the reaction that takes place when each base is added to water. (a) LiOH (b) \(\quad\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH}\) \((\mathrm{c}) \quad \mathrm{Sr}(\mathrm{OH})_{2}\) (d) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}\)

For each of the following, tell whether the acid is strong or weak. (a) Acetic acid (b) \(\mathrm{HCl}\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (d) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (e) HCN (f) \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

For each of the following, tell whether the base is strong or weak. (a) \(\mathrm{NaOH}\) (b) Sodium acetate (c) KOH (d) Ammonia (e) Water

Which of these acids are monoprotic, which are diprotic, and which are triprotic? Which are amphiprotic? (a) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (b) \(\mathrm{HBO}_{3}^{2-}\) (c) \(\mathrm{HClO}_{4}\) (d) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) (e) \(\mathrm{HSO}_{3}^{-}\) (f) HS" \((\mathrm{g}) \mathrm{H}_{2} \mathrm{CO}_{3}\)

Define (a) a Bronsted-Lowry acid and (b) a Bronsted-Lowry base.

Write the formula for the conjugate base of each acid. (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (b) \(\mathrm{H}_{3} \mathrm{BO}_{3}\) (c) HI (d) \(\mathrm{H}_{3} \mathrm{O}^{+}\) (e) \(\mathrm{NH}_{4}^{+}\) (f) \(\mathrm{HPO}_{4}^{2-}\)

Write the formula for the conjugate base of each acid. (a) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (b) \(\mathrm{H}_{2} \mathrm{S}\) (c) \(\mathrm{HCO}_{3}^{-}\) (d) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) (e) \(\mathrm{H}_{2} \mathrm{O}\)

Write the formula for the conjugate acid of each base. (a) \(\mathrm{OH}^{-}\) (b) \(\mathrm{HS}^{-}\) (c) \(\mathrm{NH}_{3}\) (d) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}^{-}\) (e) \(\mathrm{CO}_{3}^{2-}\) (f) \(\mathrm{HCO}_{3}^{-}\)