Chapter 16

According to the Bronsted-Lowry theory, label each of the following as an acid or a base. (a) \(\mathrm{HNO}_{2}\) (b) \(\mathrm{OCl}^{-} ;(\mathrm{c}) \mathrm{NH}_{2}^{-} ;\) (d) \(\mathrm{NH}_{4}^{+} ;\) (e) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\)

Write the formula of the conjugate base in the reaction of each acid with water. (a) \(\mathrm{HIO}_{3} ;\) (b) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\) (c) \(\mathrm{HPO}_{4}^{2-} ;\) (d) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\)

For each of the following, identify the acids and bases involved in both the forward and reverse directions. (a) \(\mathrm{HOBr}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{OBr}^{-}+\mathrm{H}_{3} \mathrm{O}^{+}\) (b) \(\mathrm{HSO}_{4}^{-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{SO}_{4}^{2-}+\mathrm{H}_{3} \mathrm{O}^{+}\) (c) \(\mathrm{HS}^{-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{2} \mathrm{S}+\mathrm{OH}^{-}\) (d) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}+\mathrm{OH}^{-} \rightleftharpoons \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}+\mathrm{H}_{2} \mathrm{O}\)

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. \(\mathrm{OH}^{-}, \mathrm{NH}_{4}^{+}, \mathrm{H}_{2} \mathrm{O}, \mathrm{HS}^{-}\) \(\mathrm{NO}_{2}^{-}, \mathrm{HCO}_{3}^{-}, \mathrm{HBr}\)

With which of the following bases will the ionization of acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH},\) proceed furthest toward completion (to the right): (a) \(\mathrm{H}_{2} \mathrm{O} ;\) (b) \(\mathrm{NH}_{3} ;\) (c) \(\mathrm{Cl}^{-}\) (d) \(\mathrm{NO}_{3}^{-} ?\) Explain your answer.

Calculate \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) for each solution:(a) \(0.00165 \mathrm{M} \mathrm{HNO}_{3} ;\) (b) \(0.0087 \mathrm{M} \mathrm{KOH} ;\) (c) \(0.00213 \mathrm{M}\) \(\operatorname{Sr}(\mathrm{OH})_{2} ;(\mathrm{d}) 5.8 \times 10^{-4} \mathrm{M} \mathrm{HI}\)

What is the pH of each of the following solutions? (a) \(0.0045 \mathrm{M} \mathrm{HCl} ;\) (b) \(6.14 \times 10^{-4} \mathrm{M} \mathrm{HNO}_{3} ;\) (c) 0.00683 \(\mathrm{M} \mathrm{NaOH} ;\) (d) \(4.8 \times 10^{-3} \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\)

Calculate \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) and \(\mathrm{pH}\) in saturated \(\mathrm{Ba}(\mathrm{OH})_{2}(\mathrm{aq})\) which contains \(3.9 \mathrm{g} \mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}\) per \(100 \mathrm{mL}\) of solution.

A saturated aqueous solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\) has a pH of 12.35. What is the solubility of \(\mathrm{Ca}(\mathrm{OH})_{2}\), expressed in milligrams per 100 mL of solution?

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?

How many milliliters of concentrated HCl(aq) \((36.0 \%\) HCl by mass, \(d=1.18 \mathrm{g} / \mathrm{mL}\) ) are required to produce \(12.5 \mathrm{L}\) of a solution with \(\mathrm{pH}=2.10 ?\)

What volume of \(6.15 \mathrm{M} \mathrm{HCl}(\mathrm{aq})\) is required to exactly neutralize 1.25 L of \(0.265 \mathrm{M} \mathrm{NH}_{3}(\text { aq }) ?\) $$\mathrm{NH}_{3}(\mathrm{aq})+\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}) \longrightarrow \mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}$$

A 28.2 L volume of \(\mathrm{HCl}(\mathrm{g}),\) measured at \(742 \mathrm{mmHg}\) and \(25.0^{\circ} \mathrm{C},\) is dissolved in water. What volume of \(\mathrm{NH}_{3}(\mathrm{g}),\) measured at \(762 \mathrm{mmHg}\) and \(21.0^{\circ} \mathrm{C},\) must be absorbed by the same solution to neutralize the HCl?

\(50.00 \mathrm{mL}\) of \(0.0155 \mathrm{M} \mathrm{HI}(\mathrm{aq})\) is mixed with \(75.00 \mathrm{mL}\) of 0.0106 M KOH(aq). What is the pH of the final solution?

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 \(0.121 \mathrm{M} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H} ?\)

A 625 mL sample of an aqueous solution containing 0.275 mol propionic acid, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H},\) has \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]=0.00239 \mathrm{M} .\) What is the value of \(K_{\mathrm{a}}\) for propionic acid? $$\begin{aligned} &\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2}\\\ &&K_{\mathrm{a}}=? \end{aligned}$$

Fluoroacetic acid occurs in gifblaar, one of the most poisonous of all plants. A 0.318 M solution of the acid is found to have a \(\mathrm{pH}=1.56 .\) Calculate \(K_{\mathrm{a}}\) of fluoroacetic acid. $$\mathrm{CH}_{2} \mathrm{FCOOH}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \quad\mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{CH}_{2} \mathrm{FCOO}^{-}(\mathrm{aq}) \quad K_{\mathrm{a}}=?$$

Caproic acid, \(\mathrm{HC}_{6} \mathrm{H}_{11} \mathrm{O}_{2},\) found in small amounts in coconut and palm oils, is used in making artificial flavors. A saturated aqueous solution of the acid contains \(11 \mathrm{g} / \mathrm{L}\) and has \(\mathrm{pH}=2.94 .\) Calculate \(K_{\mathrm{a}}\) for the acid. $$\mathrm{HC}_{6} \mathrm{H}_{11} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{C}_{6} \mathrm{H}_{11} \mathrm{O}_{2}^{-} \quad K_{\mathrm{a}}=?$$

What mass of benzoic acid, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\), would you dissolve in \(350.0 \mathrm{mL}\) of water to produce a solution with a \(\mathrm{pH}=2.85 ?\) $$\begin{aligned} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-} & \\ K_{\mathrm{a}}=6.3 \times 10^{-5} \end{aligned}$$

What must be the molarity of an aqueous solution of trimethylamine, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{N},\) if it has a \(\mathrm{pH}=11.12 ?\) $$\begin{aligned} \left(\mathrm{CH}_{3}\right)_{3} \mathrm{N}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons\left(\mathrm{CH}_{3}\right)_{3} \mathrm{NH}^{+} &+\mathrm{OH}^{-} \\ K_{\mathrm{b}}=6.3 \times 10^{-5} \end{aligned}$$

What are \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right],\left[\mathrm{OH}^{-}\right], \mathrm{pH},\) and \(\mathrm{pOH}\) of \(0.55 \mathrm{M}\) \(\mathrm{M} \mathrm{HClO}_{2} ?\)

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? $$\begin{array}{r} \mathrm{C}_{10} \mathrm{H}_{7} \mathrm{NH}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{C}_{10} \mathrm{H}_{7} \mathrm{NH}_{3}^{+}+\mathrm{OH}^{-} \\ \mathrm{p} K_{\mathrm{b}}=3.92 \end{array}$$

A saturated aqueous solution of \(o\) -nitrophenol, \(\mathrm{HOC}_{6} \mathrm{H}_{4} \mathrm{NO}_{2},\) has \(\mathrm{pH}=4.53 .\) What is the solubility of \(o\) -nitrophenol in water, in grams per liter? $$\begin{aligned} &\mathrm{HOC}_{6} \mathrm{H}_{4} \mathrm{NO}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+-\mathrm{OC}_{6} \mathrm{H}_{4} \mathrm{NO}_{2}\\\ &&\mathrm{p} K_{\mathrm{a}}=7.23 \end{aligned}$$

A 275 mL sample of vapor in equilibrium with 1-propylamine at \(25.0^{\circ} \mathrm{C}\) is removed and dissolved in \(0.500 \mathrm{L} \mathrm{H}_{2} \mathrm{O} .\) For 1 -propylamine, \(\mathrm{p} K_{\mathrm{b}}=3.43\) and v.p. \(=316\) Torr. (a) What should be the pH of the aqueous solution? (b) How many \(\mathrm{mg}\) of \(\mathrm{NaOH}\) dissolved in \(0.500 \mathrm{L}\) of water give the same pH?

One handbook lists a value of 9.5 for \(\mathrm{p} \mathrm{K}_{\mathrm{b}}\) of quinoline, \(\mathrm{C}_{9} \mathrm{H}_{7} \mathrm{N},\) a weak base used as a preservative for anatomical specimens and to make dyes. Another handbook lists the solubility of quinoline in water at \(25^{\circ} \mathrm{C}\) as \(0.6 \mathrm{g} / 100 \mathrm{mL} .\) Use this information to calculate the \(\mathrm{pH}\) of a saturated solution of quinoline in water.

What is the (a) degree of ionization and (b) percent ionization of propionic acid in a solution that is \(0.45 \mathrm{M}\) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H} ?\) $$\begin{aligned} &\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2} \mathrm{H}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CO}_{2}^{-}\\\ &&\mathrm{p} K_{\mathrm{a}}=4.89 \end{aligned}$$

Explain why \(\left[\mathrm{PO}_{4}^{3-}\right]\) in \(1.00 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}\) is not simply \(\frac{1}{3}\left[\mathrm{H}_{3} \mathrm{O}^{+}\right],\) but much, much less than \(\frac{1}{3}\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\)

Adipic acid, \(\mathrm{HOOC}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{COOH},\) is among the top 50 manufactured chemicals in the United States (nearly 1 million metric tons annually). Its chief use is in the manufacture of nylon. It is a diprotic acid having \(K_{\mathrm{a}_{1}}=3.9 \times 10^{-5}\) and \(K_{\mathrm{a}_{2}}=3.9 \times 10^{-6} .\) A saturated solution of adipic acid is about \(0.10 \mathrm{M}\) \(\mathrm{HOOC}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{COOH} .\) Calculate the concentration of each ionic species in this solution.

The antimalarial drug quinine, \(\mathrm{C}_{20} \mathrm{H}_{24} \mathrm{O}_{2} \mathrm{N}_{2},\) is a diprotic base with a water solubility of \(1.00 \mathrm{g} / 1900 \mathrm{mL}\) of solution. (a) Write equations for the ionization equilibria corresponding to \(\mathrm{p} K_{\mathrm{b}_{1}}=6.0\) and \(\mathrm{p} K_{\mathrm{b}_{2}}=9.8\) (b) What is the \(\mathrm{pH}\) of saturated aqueous quinine?

Codeine, \(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{O}_{3} \mathrm{N},\) is an opiate, has analgesic and antidiarrheal properties, and is widely used. In water, codeine is a weak base. A handbook gives \(\mathrm{p} K_{\mathrm{a}}=6.05\) for protonated codeine, \(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{O}_{3} \mathrm{NH}^{+} .\) Write the reaction for \(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{O}_{3} \mathrm{NH}^{+}\) and calculate \(\mathrm{p} K_{\mathrm{b}}\) for codeine.

Approximately 4 metric tons of quinoline, \(\mathrm{C}_{9} \mathrm{H}_{7} \mathrm{N},\) is produced annually. The principal source of quinoline is coal tar. Quinoline is a weak base in water. A handbook gives \(K_{\mathrm{a}}=6.3 \times 10^{-10}\) for protonated quinoline, \(\mathrm{C}_{9} \mathrm{H}_{7} \mathrm{NH}^{+} .\) Write the ionization reaction for \(\mathrm{C}_{9} \mathrm{H}_{7} \mathrm{NH}^{+}\) and calculate \(\mathrm{p} \bar{K}_{\mathrm{b}}\) for quinoline.

Complete the following equations in those instances in which a reaction (hydrolysis) will occur. If no reaction occurs, so state. (a) \(\mathrm{NH}_{4}^{+}(\mathrm{aq})+\mathrm{NO}_{3}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (b) \(\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{NO}_{2}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (c) \(\mathrm{K}^{+}(\mathrm{aq})+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (d) \(\mathrm{K}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{I}^{-}(\mathrm{aq})+\) (e) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{2} \mathrm{O} \longrightarrow\)

Predict whether a solution of each of the following salts is acidic, basic, or pH neutral: (a) KCl; (b) KF; (c) \(\mathrm{NaNO}_{3} ;\) (d) \(\mathrm{Ca}(\mathrm{OCl})_{2} ;\) (e) \(\mathrm{NH}_{4} \mathrm{NO}_{2}\)

Arrange the following 0.010 M solutions in order of increasing \(\mathrm{pH}: \mathrm{NH}_{3}(\mathrm{aq}), \mathrm{HNO}_{3}(\mathrm{aq}), \mathrm{NaNO}_{2}(\mathrm{aq})\) \(\mathrm{CH}_{3} \mathrm{COOH}(\mathrm{aq}), \quad \mathrm{NaOH}(\mathrm{aq}), \quad \mathrm{NH}_{4} \mathrm{CH}_{3} \mathrm{COO}(\mathrm{aq})\) \(\mathrm{NH}_{4} \mathrm{ClO}_{4}(\mathrm{aq})\)

Pyridine, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}\left(\mathrm{p} K_{\mathrm{b}}=8.82\right),\) forms a salt, pyridinium chloride, as a result of a reaction with HCl. Write an ionic equation to represent the hydrolysis of the pyridinium ion, and calculate the \(\mathrm{pH}\) of \(0.0482 \mathrm{M} \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+} \mathrm{Cl}^{-}(\mathrm{aq})\).

Suppose you wanted to produce an aqueous solution of \(\mathrm{pH}=8.65\) by dissolving one of the following salts in water. Which salt would you use, and at what molarity? (a) \(\mathrm{NH}_{4} \mathrm{Cl} ;\) (b) \(\mathrm{KHSO}_{4} ;\) (c) \(\mathrm{KNO}_{2}\); (d) \(\mathrm{NaNO}_{3}\).

Predict which is the stronger acid: (a) \(\mathrm{HClO}_{2}\) or \(\mathrm{HClO}_{3} ;(\mathrm{b}) \mathrm{H}_{2} \mathrm{CO}_{3}\) or \(\mathrm{HNO}_{2} ;(\mathrm{c}) \mathrm{H}_{2} \mathrm{SiO}_{3}\) or \(\mathrm{H}_{3} \mathrm{PO}_{4}\) Explain.

Explain why trichloroacetic acid, \(\mathrm{CCl}_{3} \mathrm{COOH},\) is a stronger acid than acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH}\).

Which is the stronger acid of each of the following pairs of acids? Explain your reasoning. (a)\( HBr or HI;\) (b\() HOClO or HOBr; (c) I_SCCH_CH_COOH\) or \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CCl}_{2} \mathrm{COOH}\).

For each reaction draw a Lewis structure for each species and indicate which is the acid and which is the base: (a) \(\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{2} \mathrm{CO}_{3}\) (b) \(\mathrm{H}_{2} \mathrm{O}+\mathrm{BF}_{3} \longrightarrow \mathrm{H}_{2} \mathrm{OBF}_{3}\) (c) \(\mathrm{O}^{2-}+\mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{OH}^{-}\) (d) \(\mathrm{S}^{2-}+\mathrm{SO}_{3} \longrightarrow \mathrm{S}_{2} \mathrm{O}_{3}^{2-}\)

In the following reactions indicate which is the Lewis acid and which is the Lewis base: (a) \(\mathrm{SOI}_{2}+\mathrm{BaSO}_{3} \longrightarrow \mathrm{Ba}^{2+}+2 \mathrm{I}^{-}+2 \mathrm{SO}_{2}\) (b) \(\mathrm{HgCl}_{3}^{-}+\mathrm{Cl}^{-} \longrightarrow \mathrm{HgCl}_{4}^{2}\)

Indicate whether each of the following is a Lewis acid or base. (a) \(\mathrm{OH}^{-} ;\) (b) \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{3} \mathrm{B} ;\) (c) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\)

Each of the following is a Lewis acid-base reaction. Which reactant is the acid, and which is the base? Explain. (a) \(\mathrm{SO}_{3}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}\) (b) \(\operatorname{Zn}(\mathrm{OH})_{2}(\mathrm{s})+2 \mathrm{OH}^{-}(\mathrm{aq}) \longrightarrow\left[\mathrm{Zn}(\mathrm{OH})_{4}\right]^{2-}(\mathrm{aq})\)

The three following reactions are acid-base reactions according to the Lewis theory. Draw Lewis structures, and identify the Lewis acid and Lewis base in each reaction. (a) \(\mathrm{B}(\mathrm{OH})_{3}+\mathrm{OH}^{-} \longrightarrow\left[\mathrm{B}(\mathrm{OH})_{4}\right]^{-}\) (b) \(\mathrm{N}_{2} \mathrm{H}_{4}+\mathrm{H}_{3} \mathrm{O}^{+} \longrightarrow \mathrm{N}_{2} \mathrm{H}_{5}^{+}+\mathrm{H}_{2} \mathrm{O}\) (c) \(\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{O}+\mathrm{BF}_{3} \longrightarrow\left(\mathrm{C}_{2} \mathrm{H}_{5}\right)_{2} \mathrm{OBF}_{3}\)

\(\mathrm{CO}_{2}(\mathrm{g})\) can be removed from confined quarters (such as a spacecraft) by allowing it to react with an alkali metal hydroxide. Show that this is a Lewis acid-base reaction. For example, $$\mathrm{CO}_{2}(\mathrm{g})+\mathrm{LiOH}(\mathrm{s}) \longrightarrow \mathrm{LiHCO}_{3}(\mathrm{s})$$

The molecular solid \(\mathrm{I}_{2}(\mathrm{s})\) is only slightly soluble in water but will dissolve to a much greater extent in an aqueous solution of \(\mathrm{KI}\), because the \(\mathrm{I}_{3}^{-}\) anion forms. Write an equation for the formation of the \(I_{3}^{-}\) anion, and indicate the Lewis acid and Lewis base.

The following very strong acids are formed by the reactions indicated: $$ \mathrm{HF}+\mathrm{SbF}_{5} \longrightarrow \mathrm{HSb} \mathrm{F}_{6} $$ (called "super acid," hexafluoroantimonic acid) $$ \mathrm{HF}+\mathrm{BF}_{3} \longrightarrow \mathrm{HBF}_{4} $$ (tetrafluoroboric acid) (a) Identify the Lewis acids and bases. (b) To which atom is the H atom bonded in each acid?

Use Lewis structures to diagram the following reaction in the manner of reaction (16.20) $$\mathrm{H}_{2} \mathrm{O}+\mathrm{SO}_{2} \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{3}$$ Identify the Lewis acid and Lewis base.

Use Lewis structures to diagram the following reaction in the manner of reaction (16.19) $$2 \mathrm{NH}_{3}+\mathrm{Ag}^{+} \longrightarrow\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}$$ Identify the Lewis acid and Lewis base.

The pH of saturated \(\operatorname{Sr}(\text { OH })_{2}(\text { aq })\) is found to be 13.12 A \(10.0 \mathrm{mL}\) sample of saturated \(\operatorname{Sr}(\mathrm{OH})_{2}(\mathrm{aq})\) is diluted to \(250.0 \mathrm{mL}\) in a volumetric flask. A \(10.0 \mathrm{mL}\) sample of the diluted \(\operatorname{Sr}(\mathrm{OH})_{2}(\mathrm{aq})\) is transferred to a beaker, and some water is added. The resulting solution requires \(25.1 \mathrm{mL}\) of a \(\mathrm{HCl}\) solution for its titration. What is the molarity of this HCl solution?