Acid-Base Equilibria

Which of the following are Arrhenius bases? 

(a) ${\mathbf{H}}_{\mathbf{3}}{\mathbf{AsO}}_{\mathbf{4}}$

(b) $\mathbf{Ba}{\mathbf{\left(}\mathbf{OH}\mathbf{\right)}}_{\mathbf{2}}$

(c) $\mathbf{HCIO}$

(d) $\mathbf{KOH}$

Write the ${\text{K}}_{\text{a}}$expression for each of the following in water: 

(a) $\text{HCN}$

(b) ${\text{HCO}}_{\text{3}}^{\text{-}}$

(c) $\text{HCOOH}$

Write the  expression for each of the following in water: 

(a) ${\mathbf{\text{CH}}}_{\mathbf{\text{3}}}{\mathbf{\text{NH}}}_{\mathbf{\text{3}}}^{\mathbf{\text{+}}}$

(b)  $\mathbf{\text{HClO}}$

(c)  ${\text{H}}_{\text{2}}\text{S}$

Write the expression for each of the following in water: 

(a) ${\mathbf{\text{HNO}}}_{\mathbf{\text{2}}}$

(b) ${\mathbf{\text{CH}}}_{\mathbf{\text{3}}}\mathbf{\text{COOH}}$

(c) ${\mathbf{\text{HBrO}}}_{\mathbf{\text{2}}}$

Question: Which of the following are Arrhenius bases? 

(a) ${\mathbf{\text{H}}}_{\mathbf{\text{3}}}{\mathbf{\text{AsO}}}_{\mathbf{\text{4}}}$

(b) ${\mathbf{\text{Ba(OH)}}}_{\mathbf{\text{2}}}$

(c) $\mathbf{\text{HClO}}$

(d) $\mathbf{\text{KOH}}$

Question: Write the ${\mathbf{\text{K}}}_{\mathbf{\text{a}}}$ expression for each of the following in water: 

(a) ${\mathbf{\text{H}}}_{\mathbf{\text{2}}}{\mathbf{\text{PO}}}_{\mathbf{\text{4}}}^{\mathbf{\text{ - }}}$

(b) ${\mathbf{\text{H}}}_{\mathbf{\text{3}}}{\mathbf{\text{PO}}}_{\mathbf{2}}$

(c) ${\mathbf{\text{HSO}}}_{\mathbf{\text{4}}}^{\mathbf{\text{ - }}}$

Question: Use Appendix C to rank the following in order of increasing acid strength: ${\mathbf{\text{HIO}}}_{\mathbf{\text{3}}}{\mathbf{\text{, HI, CH}}}_{\mathbf{\text{3}}}\mathbf{\text{COOH, HF}}$ .

What is the difference between  ${\mathbf{\text{K}}}_{\mathbf{\text{c}}}$ and ${\mathbf{\text{K}}}_{\mathbf{\text{w}}}$ for the autoionization of water?

Question: which solution has the higher pH  ? Explain.

(a) A 0.1 M  solution of an acid with ${\mathit{K}}_{\mathbf{a}}\mathbf{=}\mathbf{1}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{4}}$  or one with ${\mathit{K}}_{\mathbf{a}}\mathbf{=}\mathbf{4}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{5}}$

(b) A 0.1 M solution of an acid with  ${\mathbf{\text{pK}}}_{\mathbf{\text{a}}}\mathbf{\text{ = 3.0}}$or one with ${\mathbf{\text{pK}}}_{\mathbf{\text{a}}}\mathbf{\text{ = 3.5}}$

(c) A 0.1 M  solution or a 0.01 M  solution of a weak acid

(d) A 0.01 M   solution of a weak acid or a 0.01 M solution of a strong acid

(e) A 0.01 M solution of an acid or a 0.01 m  solution of a base

(f) A solution of pOH 6.0  or one of pOH 8.0

(a) What is the pH of $\mathbf{0}.\mathbf{0111}\mathbf{M}\mathbf{NaOH}$? Is the solution neutral, acidic, or basic? (b) What is the pOH of $\mathbf{1}\mathbf{.}\mathbf{35}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{ }\mathit{M}\mathbf{ }\mathit{H}\mathit{C}\mathit{l}$? Is the solution neutral, acidic, or basic?

(a) What is the ph of ${\mathbf{\text{0.0333 M HNO}}}_{\mathbf{\text{3}}}$? Is the solution neutral, acidic, or basic? 

(b) What is the pOH of $\mathbf{\text{0.0347 M KOH}}$? Is the solution neutral, acidic, or basic?

What is the difference between  ${\mathbf{K}}_{\mathbf{c}}$ and ${\mathbf{K}}_{\mathbf{w}}$ for the autoionization of water?

(a) What is the pH of $\mathbf{6}\mathbf{.}\mathbf{14}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{3}}$ M HI? Is the solution neutral, acidic, or basic? 

(b) What is the pOH of 2.55 M Ba ${\left(\mathrm{OH}\right)}_{\mathbf{2}}$? Is the solution neutral, acidic, or basic?

The two molecular scenes below depict the relative concentrations of   (purple) in solutions of the same volume (with counter ions and solvent molecules omitted for clarity). If the pH in scene A is 4.8, what is the pH in scene B?

(a) A Brønsted-Lowry acid-base reaction proceeds in the net direction in which a stronger acid and stronger base form a weaker acid and weaker base. Explain

(b) The molecular scene at the right depicts an aqueous solution of two conjugate acid-base pairs: HA/A and HB/B. The base in the first pair is represented by red spheres and the base in the second pair by green spheres; solvent molecules are omitted for clarity. Which is the stronger acid? Stronger base? Explain.

Use Appendix to calculate the percent dissociation of $\mathbf{\text{0.55 M}}$ benzoic acid, ${\mathbf{\text{C}}}_{\mathbf{\text{6}}}{\mathbf{\text{H}}}_{\mathbf{\text{5}}}\mathbf{\text{COOH}}$.

Use Appendix to calculate $\left[{\text{H}}_{\text{2}}\text{S}\right]\mathbf{\text{, }}\left[{\text{HS}}^{\text{-}}\right]\mathbf{\text{, }}\left[{\text{S}}^{\text{2-}}\right]\mathbf{\text{, }}\left[{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\right]\mathbf{\text{, pH, }}\left[{\text{OH}}^{\text{-}}\right]$ and $\mathbf{\text{pOH}}$ in a $\mathbf{\text{0.10 M}}$ solution of the diprotic acid hydro sulfuric acid.

Hypochlorous acid, $\mathbf{\text{HClO}}$, has a ${\mathbf{\text{pK}}}_{\mathbf{\text{a}}}$ of $\mathbf{\text{7.54}}$. What are $\left[{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\right]$, $\mathbf{\text{pH}}$, $\left[{\text{ClO}}^{\text{-}}\right]$, and $\left[\text{HClO}\right]$ in $\mathbf{\text{0.115 M}}$ $\mathbf{\text{HClO}}$ ?

Nitrous acid, ${\mathbf{\text{HNO}}}_{\mathbf{\text{2}}}$, has a ${\mathbf{\text{K}}}_{\mathbf{\text{a}}}$ of ${\mathbf{\text{7.1 × 10}}}^{\mathbf{\text{-4}}}$. What are ${\mathbf{\text{[H}}}_{\mathbf{\text{3}}}{\mathbf{\text{O}}}^{\mathbf{\text{+}}}{\mathbf{\text{], [NO}}}_{\mathbf{\text{2}}}^{\mathbf{\text{-}}}\mathbf{\text{],}}$ and in ${\mathbf{\text{0.60 M HNO}}}_{\mathbf{\text{2}}}$?

In which of the following solutions will $\left[{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\right]$ be approximately equal to $\left[{\text{CH}}_{\text{3}}{\text{COO}}^{\text{-}}\right]$ :

 $\begin{array}{l}{\mathbf{\text{(a) 0.1 MCH}}}_{\mathbf{\text{3}}}{\mathbf{\text{COOH}}}_{\mathbf{\text{; }}}\\ {\mathbf{\text{(b) 1×10}}}^{\mathbf{\text{-J}}}{\mathbf{\text{ MCH}}}_{\mathbf{\text{3}}}\mathbf{\text{COOH }}\\ {\mathbf{\text{(c) a solution containing both 0.1 MCH}}}_{\mathbf{\text{3}}}{\mathbf{\text{COOH}}}_{\mathbf{\text{; }}}{\mathbf{\text{ and 0.1 MCH}}}_{\mathbf{\text{3}}}{\mathbf{\text{COOH}}}_{\mathbf{\text{; }}}\mathbf{\text{? Explain.}}\end{array}$

Why are most anions basic in ${\mathbf{\text{H}}}_{\mathbf{\text{2}}}\mathbf{\text{O}}$ ? Give formulas of four anions that are not basic.

Explain with equations and calculations, when necessary, whether an aqueous solution of each of these salts is acidic, basic, or neutral: (a) KBr; (b)NH4I; (c) KCN

The NH⁺₄ ion forms acidic solutions, and the CH₃COO^- ion forms basic solutions. However, a solution of ammonium acetate is almost neutral. Do all of the ammonium salts of weak acids form neutral solutions? Explain your answer.

What is the pH of  0.070 M dimethylamine?

Which are Lewis acids and which are Lewis bases? 

$$\begin{gathered} \left(a\right)\mathbf{ }\mathit{C}{\mathit{u}}^{\mathbf{2}\mathbf{+}} \\ \left(b\right)\mathbf{ }\mathit{C}{\mathit{l}}^{\mathbf{-}} \\ \left(c\right)\mathbf{ }\mathit{S}\mathit{n}\mathit{C}{\mathit{l}}_{\mathbf{2}} \\ \left(d\right)\mathbf{ }\mathit{O}{\mathit{F}}_{\mathbf{2}} \end{gathered}$$

Explain the differing extents of dissociation of ${\mathit{H}}_{\mathbf{2}}\mathit{S}{\mathit{O}}_{\mathbf{4}}$ in $\mathit{C}{\mathit{H}}_{\mathbf{3}}\mathit{C}\mathit{O}\mathit{O}\mathit{H}\mathbf{,}\mathbf{ }{\mathit{H}}_{\mathbf{2}}\mathit{O}\mathbf{,}$ and $\mathit{N}{\mathit{H}}_{\mathbf{3}}$.

Explain with equations and calculations, when necessary, whether an aqueous solution of each of these salts is acidic, basic, or neutral: $\left(a\right)\mathit{C}\mathit{r}{\left(N{O}_3\right)}_{\mathbf{3}}\mathit{C}\mathit{r}{\left(N{O}_2\right)}_{\mathbf{3}}\mathbf{ }\mathbf{;}$ $\mathbf{\left(}\mathbf{b}\mathbf{\right)}\mathit{N}\mathit{A}\mathit{H}\mathit{S}\mathit{N}\mathit{a}\mathit{H}\mathit{S}\mathbf{ }\mathbf{;}$ $\mathbf{\left(}\mathbf{c}\mathbf{\right)}\mathit{Z}\mathit{n}{\mathbf{\left(}{\mathbf{CH}}_{\mathbf{3}}\mathbf{COO}\mathbf{\right)}}_{\mathbf{2}}$

Chloral  $\mathbf{\left(}{\mathbf{\text{Cl}}}_{\mathbf{\text{3}}}\mathbf{\text{C-CH=O}}\mathbf{\right)}$forms a monohydrate, chloral hydrate, the sleep-inducing depressant called “knockout drops” in old movies. 

(a) Write two possible structures for chloral hydrate, one involving hydrogen bonding and one that is a Lewis adduct. 

(b) What spectroscopic method could be used to identify the real structure? Explain

The disinfectant phenol, ${\mathbf{\text{C}}}_{\mathbf{6}}{\mathbf{\text{H}}}_{\mathbf{5}}\mathbf{\text{OH,}}$, has a${\mathbf{\text{p K}}}_{\mathbf{\text{a}}}$ of$\mathbf{\text{10.0}}$ in water, but$\mathbf{\text{14.4}}$ in methanol. 

(a) Why are the values different? 

(b) Is methanol a stronger or weaker base than water? 

(c) Write the dissociation reaction of phenol in methanol. 

(d) Write an expression for the autoionization constant of methanol.

The beakers shown contain 0.300 Lof aqueous solutions of a moderately weak acid HY. Each particle represents 0.010 mol; solvent molecules are omitted for clarity. 

(a) The reaction in beaker Ais at equilibrium. Calculate Q for B, C, and D to determine which, if any, is also at equilibrium. 

(b) For any not at equilibrium, in which direction does the reaction proceed? 

(c) Does dilution affect the extent of dissociation of a weak acid? Explain.

Seashells are mostly calcium carbonate, which reacts with $\left[{\text{H}}_{\text{3}}{\text{O}}^{\text{ + }}\right]$ according to the equation

${\mathbf{\text{CaCO}}}_{\mathbf{\text{3}}}{\mathbf{\text{(s) + H}}}_{\mathbf{\text{3}}}{\mathbf{\text{O}}}^{\mathbf{\text{ + }}}\mathbf{\text{(aq)}}\mathbf{\rightleftharpoons }{\mathbf{\text{Ca}}}^{\mathbf{\text{2 + }}}{\mathbf{\text{(aq) + HCO}}}_{\mathbf{\text{3}}}^{\mathbf{\text{ - }}}{\mathbf{\text{(aq) + H}}}_{\mathbf{\text{2}}}\mathbf{\text{O(l)}}$

If  ${\mathbf{\text{K}}}_{\mathbf{\text{w}}}$ increases at higher pressure, will seashells dissolve more rapidly near the surface of the ocean or at great depths? Explain.

Many molecules with central atoms from Period 3 or higher take part in Lewis acid-base reactions in which the central atom expands its valence shell. SnCl4 reacts with (CH₃)₃N as follows:

(a) Identify the Lewis acid and the Lewis base in the reaction.  

(b) Give the nl designation of the sublevel of the central atom in the acid before it accepts the lone pair.

The strength of an acid or base is related to its strength as an electrolyte. (a) Is the electrical conductivity of $\mathbf{\text{0.1MHCl}}$ electrical conductivity of  $\mathbf{1}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{7}}$MHCl higher, lower, or the same as that of ${\mathbf{\text{0.1MCH}}}_{\mathbf{\text{3}}}\mathbf{\text{COOH}}$ ? Explain.

(b) Is the electrical conductivity of $\mathbf{1}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{7}}$MHCl higher, lower, or the same as that of $\mathbf{1}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{7}}{\mathbf{\text{MCH}}}_{\mathbf{\text{3}}}\mathbf{\text{COOH}}$? Explain

Human urine has a normal pH of 6.2. If a person eliminates an average of 1250 mL of urine per day, how many ${\mathbf{\text{H}}}^{\mathbf{\text{ + }}}$  ions are eliminated per week?

Auto ionization occurs in methanol $\left({\text{CH}}_{\text{3}}\text{OH}\right)$  and in ethylenediamine                               (${\mathbf{\text{NH}}}_{\mathbf{\text{2}}}{\mathbf{\text{CH}}}_{\mathbf{\text{2}}}{\mathbf{\text{CH}}}_{\mathbf{\text{2}}}{\mathbf{\text{NH}}}_{\mathbf{\text{2}}}$). 

(a) The auto ionization constant of methanol  $\left({\text{K}}_{\text{met }}\right)$is $\mathbf{\text{2}}\mathbf{\times }{\mathbf{\text{10}}}^{\mathbf{\text{ - 17}}}$. What is $\left[{\text{CH}}_{\text{3}}{\text{O}}^{\text{ - }}\right]$ in pure $\left({\text{CH}}_{\text{3}}\text{OH}\right)$ ?

(b) The concentration of ${\mathbf{\text{NH}}}_{\mathbf{\text{2}}}{\mathbf{\text{CH}}}_{\mathbf{\text{2}}}{\mathbf{\text{CH}}}_{\mathbf{\text{2}}}{\mathbf{\text{NH}}}_{\mathbf{\text{2}}}$  in pure ${\mathbf{\text{NH}}}_{\mathbf{\text{2}}}{\mathbf{\text{CH}}}_{\mathbf{\text{2}}}{\mathbf{\text{CH}}}_{\mathbf{\text{2}}}{\mathbf{\text{NH}}}_{\mathbf{\text{2}}}$ is $\mathbf{\text{2}}\mathbf{\times }{\mathbf{\text{10}}}^{\mathbf{\text{ - 8}}}\mathbf{\text{M}}$ . What is the auto ionization constant of ethylenediamine $\left({\text{K}}_{\text{en}}\right)$?

Acetic acid has a Ka of,${\mathbf{\text{1.8×10}}}^{\mathbf{\text{-3}}}$ and ammonia has a Kb of.${\mathbf{\text{1.8×10}}}^{\mathbf{\text{-3}}}$ Find $\mathbf{\left[}{\mathbf{\text{H}}}_{\mathbf{\text{3}}}{\mathbf{\text{O}}}^{\mathbf{\text{+}}}\mathbf{\right]}$ ,[OH], pH, and pOH for 

(a) $\mathbf{\text{0.240}}$M acetic acid and 

(b)$\mathbf{\text{0.240}}$ M ammonia. 

A site in Pennsylvania receives a total annual deposition of $\mathbf{\text{2.688}}$g/m2 of sulfate from fertilizer and acid rain. The ratio by mass of ammonium sulfate/ammonium bisulfate/sulfuric acid is.$\mathbf{\text{3.0/5.5/1.0}}$

 (a) How much acid, expressed as kg of sulfuric acid, is deposited over an area of ${\mathbf{\text{10.km}}}^{\mathbf{\text{2}}}$

(b) How many pounds of${\mathbf{\text{CaCO}}}_{\mathbf{\text{3}}}$ are needed to neutralize this acid?

 (c) If ${\mathbf{\text{10.km}}}^{\mathbf{\text{2}}}$is the area of an unpolluted lake$\mathbf{3}$ m deep and there is no loss of acid, what pH would be attained in the year? (Assume constant volume.) 

Putrescine,$\mathbf{\left[}{\mathbf{\text{NH}}}_{\mathbf{\text{2}}}{\mathbf{\left(}{\mathbf{\text{CH}}}_{\mathbf{\text{2}}}\mathbf{\right)}}_{\mathbf{\text{4}}}{\mathbf{\text{NH}}}_{\mathbf{\text{2}}}\mathbf{\right]}$ found in rotting animal tissue, is now known to be in all cells and essential for normal and abnormal (cancerous) growth. It also plays a key role in the formation of GABA, a neurotransmitter. A aqueous solution of putrescine has[ $\mathbf{\text{O}}{\mathbf{\text{H}}}^{\mathbf{\text{-}}}\mathbf{]}$=${\mathbf{\text{2.1×10}}}^{\mathbf{\text{-3}}}$. What is the${\mathbf{\text{K}}}_{\mathbf{\text{b}}}$? 

In his acid-base studies, Arrhenius discovered an important fact involving reactions like the following:

$$\begin{gathered} {\mathbf{\text{KOH(aq) + HNO}}}_{\mathbf{\text{3}}}\mathbf{\text{(aq)n?}} \\ \mathbf{\text{NaOH(aq) + HCl(aq)n?}} \end{gathered}$$

(a) Complete the reactions and use the data for the individual ions in Appendix B to calculate each$\mathbf{∆}{\mathit{H}}_{\mathbf{r}\mathbf{\times }{\mathbf{n}}^{\mathbf{*}}}$

(b) Explain your results and use them to predict $\mathbf{∆}{\mathit{H}}_{\mathbf{r}\mathbf{\times }{\mathbf{n}}^{\mathbf{*}}}$for $\mathbf{\text{KOH(aq) + HCl(aq)}}\mathbf{\to }\mathbf{\text{?}}$

Calcium propionate$\mathbf{\text{Ca}}({\text{CH}}_3{\text{CH}}_2\text{COO}{\mathbf{)}}_{\mathbf{2}}$; calcium propionate] is a mold inhibitor used in food, tobacco, and pharmaceuticals. 

(a) Use balanced equations to show whether aqueous calcium propionate is acidic, basic, or neutral. 

(b) Use Appendix C to find the resulting pH when 8.75g of $\mathbf{\text{Ca}}({\text{CH}}_3{\text{CH}}_2\text{COO}{\mathbf{)}}_{\mathbf{2}}$dissolves in enough water to give 0.500L of solution. 

The beakers below depict the aqueous dissociations of weak acids HA (blue and green) and HB (blue and yellow); solvent molecules are omitted for clarity. If the HA solution is0.50 L, and the HB solution is 0.25 L, and each particle represents mol, find the Ka of each acid. Which acid, if either, is stronger?

Tris(hydroxymethyl)aminomethane, known as TRIS or THAM, is a water-soluble base used to synthesize surfactants and pharmaceuticals, as an emulsifying agent in cosmetics, and in cleaning mixtures for textiles and leather. In biomedical research, solutions of TRIS are used to maintain nearly constant pH for the study of enzymes and other cellular components. Given that the pKb is 5.91, calculate the pH of 0.075 M TRIS.

When ${\mathbf{\text{Fe}}}^{\mathbf{\text{3 + }}}$ salts are dissolved in water, the solution becomes acidic due to formation of $\mathbf{\text{Fe}}{\left({\text{H}}_{\text{2}}\text{O}\right)}_{\mathbf{\text{5}}}{\mathbf{\text{OH}}}^{\mathbf{\text{2 + }}}$ and ${\mathbf{\text{H}}}_{\mathbf{\text{3}}}{\mathbf{\text{O}}}^{\mathbf{\text{ + }}}$.The overall process involves both Lewis and Brønsted-Lowry acid-base reactions. Write the equations for the process.

What is the pH of a vinegar with  5.0 % (w/v) acetic acid in water?

How would you differentiate between a strong and a weak monoprotic acid from the results of the following procedures? 

(a) Electrical conductivity of an equimolar solution of each acid is measured.

 (b) Equal molarities of each are tested with pH paper. 

(c) Zinc metal is added to solutions of equal concentration

HX ( $\mathbf{\mu }\mathbf{=}\mathbf{150}\mathbf{ }\mathbf{g}\mathbf{/}\mathbf{mol}$ and HY( $\mathbf{\mu }\mathbf{=}\mathbf{50}\mathbf{ }\mathbf{g}\mathbf{/}\mathbf{mol}$) are weak acids. A solution of 12.0 g/Lof HX has the same pH as one containing 6.00 g/Lof HY. Which is the stronger acid? Why

A solution of propanoic acid $\left({\text{CH}}_{\text{3}}{\text{CH}}_{\text{2}}\text{COOH}\right)$,made by dissolving $\mathbf{7}\mathbf{.500}\mathbf{ }\mathbf{\text{g}}$ in sufficient water to make $\mathbf{100}\mathbf{.}\mathbf{0}\mathbf{ }\mathbf{\text{mL}}$, has a freezing point of $\mathbf{-}\mathbf{1}\mathbf{.}\mathbf{890}{\mathbf{ }}^{\mathbf{\text{0}}}\mathbf{\text{C}}$. 

(a) Calculate the molarity of the solution. 

(b) Calculate the molarity of the propanoate ion. (Assume the molarity of the solution equals the molality.) 

(c) Calculate the percent dissociation of propanoic acid

The antimalarial properties of quinine (${\mathbf{\text{C}}}_{\mathbf{\text{20}}}{\mathbf{\text{H}}}_{\mathbf{\text{24}}}{\mathbf{\text{N}}}_{\mathbf{\text{2}}}{\mathbf{\text{O}}}_{\mathbf{\text{2}}}$) saved thousands of lives during construction of the Panama Canal. This substance is a classic example of the medicinal wealth of tropical forests. Both N atoms are basic, but the N (coloured) of the 3amine group is far more basic (pKb =5.1 ) than the N within the aromatic ring system (pKb =9.7).

 (a) A saturated solution of quinine in water is only $\mathbf{1}\mathbf{.}\mathbf{6}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{ }\mathbf{\text{M}}$. What is the pH of this solution?

 (b) Show that the aromatic N contributes negligibly to the pH of the solution. 

(c) Because of its low solubility, quinine is given as the salt quinine hydrochloride $(C_{20}{H}_{24}{N}_2{O}_2\times \mathrm{HCl})$,which is 120 times more soluble than quinine. What is the pH of M quinine hydrochloride?

(d) An antimalarial concentration in water is 15 % quinine hydrochloride by mass (d 1.0 g/mL). What is the pH?

Drinking water is often disinfected with ${\mathbf{\text{CI}}}_{\mathbf{\text{2}}}$, which hydrolyzes to form HClO, a weak acid but powerful disinfectant:

${\mathbf{C}}_{\mathbf{2}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathbf{2}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{l}\mathbf{\right)}\mathbf{nHClO}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}{\mathbf{H}}_{\mathbf{3}}{\mathbf{O}}^{\mathbf{+}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}{\mathbf{Cl}}^{\mathbf{-}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$

The fraction of HClO in solution is defined as
$\frac{\mathbf{\left[}\mathbf{HClO}\mathbf{\right]}}{\mathbf{\left[}\mathbf{HClO}\mathbf{\right]}\mathbf{+}\mathbf{\left[}{\mathbf{ClO}}^{\mathbf{-}}\mathbf{\right]}}$

(a) What is the fraction of HClO at pH 7.00 (Ka of HClO=$\mathbf{(}\mathbf{2}\mathbf{.}\mathbf{9}\mathbf{\times }{\mathbf{10}}^{\mathbf{-}\mathbf{8}}\mathbf{)}$?

(b) What is the fraction at pH 10.00?

The following scenes represent three weak acids HA

(a) Rank the acids in order of increasing Ka.

 (b) Rank the acids in order of increasing ${\mathbf{pK}}_{\mathbf{a}}.$

c) Rank the conjugate bases in order of increasing ${\mathbf{pK}}_{\mathbf{b}}$. 

(d) What is the percent dissociation of HX? 

(e) If equimolar amounts of the sodium salts of the acids (NaX, NaY, and NaZ) were dissolved in water, which solution would have the highest pOH? The lowest pH?