Chapter 10

Identify the following as cither an acid or a base: (a) \(\mathrm{NH}_{3}\) (b) \(\mathrm{HCl}\); (c) \(\mathrm{NaOH}\); (d) \(\mathrm{H}_{2} \mathrm{SO}_{4}\); (e) \(\mathrm{Ba}(\mathrm{OH})_{2}\).

Complete and write the overall equation, the complete ionic equation, and the net ionic equation for the following acid-base reactions. If the substance is a weak acid or base, leave it in its molecular form in writing the equations. (a) \(\mathrm{HCl}\) (aq) \(+\mathrm{NaOH}\) (aq) \(\rightarrow\) (b) \(\mathrm{NH}_{3}\) (aq) \(+\mathrm{HNO}_{3}\) (aq) \(\rightarrow\) (c) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) (aq) \(+\mathrm{Hl}\) (aq) \(\rightarrow\)

Select an acid and a base for a neutralization reaction that results in the formation of (a) potassium bromide; (b) zinc nitrite; (c) calcium cyanide, \(\mathrm{Ca}(\mathrm{CN})_{2}\); (d) potassium phosphate. Write the overall and net ionic equations for each reaction.

Identify the acid and the base in the following reactions: (a) \(\mathrm{CH}_{3} \mathrm{NH}_{2}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}) \rightarrow\) \(\mathrm{CH}_{3} \mathrm{NH}_{3}{ }^{*}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})\) (b) \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{NH}_{2}\) (aq) \(+\mathrm{HCl}\) (aq) \(\rightarrow\) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3}{ }^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})\) (c) \(\mathrm{CaO}\) (s) \(+2 \mathrm{HI}(\mathrm{aq}) \rightarrow \mathrm{CaI}_{2}\) (aq) \(+\mathrm{H}_{2} \mathrm{O}\) (l)

Identify the acid and the base in the following reactions: (a) \(\mathrm{CH}_{3} \mathrm{COOH}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \rightarrow\) \(\mathrm{NH}_{4}{ }^{+}(\mathrm{aq})+\mathrm{CH}_{3} \mathrm{CO}_{2}{ }^{-}(\mathrm{aq})\) (b) \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \rightarrow\) \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{NH}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})\) (c) \(\mathrm{O}^{2-}\) (aq) \(+\mathrm{H}_{2} \mathrm{O}\) (1) \(\rightarrow 2 \mathrm{OH}^{-}\)(aq)

Use the periodic table to determine which oxides form acidic solutions in water and which form basic solutions: (a) \(\mathrm{CaO}\); (b) \(\mathrm{SO}_{3}\); (c) \(\mathrm{N}_{2} \mathrm{O}_{3}\); (d) \(\mathrm{Tl}_{2} \mathrm{O}\).

Use the periodic rable to determine which oxides form acidic solutions in water and which form basic solutions: (a) \(\mathrm{P}_{4} \mathrm{O}_{105}\) (b) \(\mathrm{Na}_{2} \mathrm{O}\); (c) \(\mathrm{CO}_{2}\); (d) \(\mathrm{MgO}\).