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Chapter 16: Problem 4

Which of the following species are amphiprotic in aqueous solution? For such a species, write one equation showing it acting as an acid, and another equation showing it acting as a base. \(\mathrm{OH}^{-}, \mathrm{NH}_{4}^{+}, \mathrm{H}_{2} \mathrm{O}, \mathrm{HS}^{-}\) \(\mathrm{NO}_{2}^{-}, \mathrm{HCO}_{3}^{-}, \mathrm{HBr}\)

Short Answer

Expert verified
The amphiprotic species are: \(OH^-\), \(H_2O\), \(HS^-\) and \(HCO_3^-\). As acids, their reactions are: \(OH^- + H^+ \rightarrow H_2O\), \(H_2O + H^+ \rightarrow H_3O^+\), \(HS^- + H^+ \rightarrow H_2S\), and \(HCO_3^- + H^+ \rightarrow H_2CO_3\). As bases, their reactions are: \(OH^- + H_2O \rightarrow HO^- + H_2O\), \(H_2O + H_2O \rightarrow OH^- + H_3O^+\), \(HS^- + H_2O \rightarrow OH^- + H_2S\), and \(HCO_3^- + H_2O \rightarrow OH^- + H_2CO_3\)

Step by step solution

01

Amphiprotic Identification

The amphiprotic species are: \(OH^-\), \(H_2O\), \(HS^-\) and \(HCO_3^-\). They have the ability to both accept and donate a proton.
02

Action as Acids

As acids, these species donate a proton (H+). The equations describing this are: \(OH^- + H^+ \rightarrow H_2O\), \(H_2O + H^+ \rightarrow H_3O^+\), \(HS^- + H^+ \rightarrow H_2S\), and \(HCO_3^- + H^+ \rightarrow H_2CO_3\)
03

Action as Bases

As bases, these species accept a proton (H+). The equations describing this are: \(OH^- + H_2O \rightarrow HO^- + H_2O\), \(H_2O + H_2O \rightarrow OH^- + H_3O^+\), \(HS^- + H_2O \rightarrow OH^- + H_2S\), and \(HCO_3^- + H_2O \rightarrow OH^- + H_2CO_3\)

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Most popular questions from this chapter

Show that when \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) is reduced to half its original value, the \(\mathrm{pH}\) of a solution increases by 0.30 unit, regardless ofthe initial \(p H .\) Is it also true that when any solution is diluted to half its original concentration, the pH increases by 0.30 unit? Explain.

What is the \(\mathrm{pH}\) of the solution obtained when \(125 \mathrm{mL}\) of \(0.606 \mathrm{M} \mathrm{NaOH}\) is diluted to \(15.0 \mathrm{L}\) with water?

The solubility of 1 -naphthylamine, \(\mathrm{C}_{10} \mathrm{H}_{7} \mathrm{NH}_{2}, \mathrm{a}\) substance used in the manufacture of dyes, is given in a handbook as 1 g per \(590 \mathrm{g} \mathrm{H}_{2} \mathrm{O}\). What is the approximate \(\mathrm{pH}\) of a saturated aqueous solution of 1-naphthylamine? $$\begin{array}{r} \mathrm{C}_{10} \mathrm{H}_{7} \mathrm{NH}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{C}_{10} \mathrm{H}_{7} \mathrm{NH}_{3}^{+}+\mathrm{OH}^{-} \\ \mathrm{p} K_{\mathrm{b}}=3.92 \end{array}$$

In \(0.10 \mathrm{M} \quad \mathrm{CH}_{3} \mathrm{NH}_{2}(\mathrm{aq}), \quad\) (a) \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=0.10 \mathrm{M}\) (b) \(\left[\mathrm{OH}^{-}\right]=0.10 \mathrm{M} ;(\mathrm{c}) \mathrm{pH}<7 ;(\mathrm{d}) \mathrm{pH}<13\).

For the ionization of phenylacetic acid, $$\begin{array}{r} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{2} \mathrm{CO}_{2} \\\ K_{\mathrm{a}}=4.9 \times 10^{-5} \end{array}$$ (a) What is \(\left[\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{2} \mathrm{CO}_{2}^{-}\right]\) in \(0.186 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H} ?\) (b) What is the \(\mathrm{pH}\) of \(0.121 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H} ?\)
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