91Ó°ÊÓ

What are some physical properties that historically led chemists to classify various substances as acids and bases?

Write an equation showing how \(\mathrm{HCl}(g)\) behaves as an Arrhenius acid when dissolved in water. Write an equation showing how \(\mathrm{NaOH}(s)\) behaves as an Arrhenius base when dissolved in water.

According to the Bronsted-Lowry model, an acid is a "proton donor" and a base is a "proton acceptor." Explain.

How do the components of a conjugate acid-base pair differ from one another? Give an example of a conjugate acid-base pair to illustrate your answer.

Given the general equation illustrating the reaction of the acid HA in water, $$ \mathrm{HA}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{A}^{-}(a q) $$ explain why water is considered a base in the Bronsted-Lowry model.

Which of the following do not represent a conjugate acid-base pair? For those pairs that are not conjugate acid-base pairs, write the correct conjugate acid-base pair for each species in the pair. a. HI \(, \mathrm{I}^{-}\) b. \(\mathrm{HClO}, \mathrm{HClO}_{2}\) c. \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{PO}_{4}^{3-}\) d. \(\mathrm{H}_{2} \mathrm{CO}_{3}, \mathrm{CO}_{3}^{2-}\)

Which of the following do \(n o t\) represent a conjugate acid-base pair? For those pairs that are not conjugate acid-base pairs, write the correct conjugate acid-base pair for each species in the pair. a. \(\mathrm{H}_{2} \mathrm{SO}_{4}, \mathrm{SO}_{4}^{2-}\) b. \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}, \mathrm{HPO}_{4}^{2-}\) c. \(\mathrm{HClO}_{4}, \mathrm{Cl}^{-}\) d. \(\mathrm{NH}_{4}^{+}, \mathrm{NH}_{2}^{-}\)

In each of the following chemical equations, identify the conjugate acid-base pairs. a. \(\mathrm{HF}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{F}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)\) b. \(\mathrm{CN}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q)\) c. \(\mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{OH}^{-}(a q)\)

In each of the following chemical equations, identify the conjugate acid-base pairs. a. \(\mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{NH}_{4}^{+}(a q)+\mathrm{OH}^{-}(a q)\) b. \(\mathrm{PO}_{4}^{3-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HPO}_{4}^{2-}(a q)+\mathrm{OH}^{-}(a q)\) c. \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{OH}^{-}(a q)\)

Write the conjugate acid for each of the following bases: a. \(\mathrm{PO}_{4}^{3-}\) b. \(\mathrm{IO}_{3}^{-}\) c. \(\mathrm{NO}_{3}^{-}\) d. \(\mathrm{NH}_{2}^{-}\)