Chapter 17

Write chemical equations and corresponding equilibrium expressions for each of the two ionization steps of carbonic acid.

Calculate the concentration of all species in a \(0.155 \mathrm{M}\) solution of \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Based on their molecular structure, pick the stronger acid from each pair of binary acids. Explain your choice. a. \(\mathrm{ HF}\) and \(\mathrm{HCl}\) b. \(\mathrm{H}_{2} \mathrm{O}\) or \(\mathrm{HF}\) c. \(\mathrm{H}_{2}\) Se or \(\mathrm{H}_{2} \mathrm{~S}\)

Based on their molecular structure, pick the stronger acid from each pair of oxyacids. Explain your choice. a. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) or \(\mathrm{H}_{2} \mathrm{SO}_{3}\) b. \(\mathrm{HClO}_{2}\) or \(\mathrm{HClO}\) c. \(\mathrm{HClO}\) or \(\mathrm{HBrO}\) d. \(\mathrm{CCl}_{3} \mathrm{COOH}\) or \(\mathrm{CH}_{3} \mathrm{COOH}\)

Which is a stronger base, \(\mathrm{PO}_{4}^{3-}\) or \(\mathrm{AsO}_{4}^{3-} ?\) Explain.

Classify each species as either a Lewis acid or a Lewis base. a. \(\mathrm{Fe}^{3+}\) b. \(\mathrm{BH}_{3}\) c. \(\mathrm{NH}_{3}\) d. \(\mathrm{F}^{-}\)

Identify the Lewis acid and Lewis base from among the reactants in each equation. a. \(\mathrm{Fe}^{3+}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q)\) b. \(\mathrm{Zn}^{2+}(a q)+4 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}(a q)\) c. \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}(g)+\mathrm{BF}_{3}(g) \rightleftharpoons\left(\mathrm{CH}_{3}\right)_{3} \mathrm{NBF}_{3}(s)\)

Identify the Lewis acid and Lewis base from among the reactants in each equation. a. \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q)\) b. \(\mathrm{AlBr}_{3}+\mathrm{NH}_{3} \rightleftharpoons \mathrm{H}_{3} \mathrm{NAlBr}_{3}\) c. \(\mathrm{F}^{-}(a q)+\mathrm{BF}_{3}(a q) \rightleftharpoons \mathrm{BF}_{4}^{-}(a q)\)

Acid rain over the Great Lakes has a pH of about \(4.5 .\) Calculate the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of this rain and compare that value to the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) of rain over the West Coast that has a pH of \(5.4 .\) How many times more concentrated is the acid in rain over the Great Lakes?

White wines tend to be more acidic than red wines. Find the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in a Sauvignon Blanc with a \(\mathrm{pH}\) of 3.23 and a Cabernet Sauvignon with a pH of \(3.64 .\) How many times more acidic is the Sauvignon Blanc?

Determine the \(\mathrm{pH}\) of each two-component solution. a. \(0.050 \mathrm{M} \mathrm{KOH}\) and \(0.015 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) b. \(0.265 \mathrm{M} \mathrm{NH}_{4} \mathrm{NO}_{3}\) and \(0.102 \mathrm{M} \mathrm{HCN}\) c. \(0.075 \mathrm{M} \mathrm{RbOH}\) and \(0.100 \mathrm{M} \mathrm{NaHCO}_{3}\) d. \(0.088 \mathrm{M} \mathrm{HClO}_{4}\) and \(0.022 \mathrm{M} \mathrm{KOH}\) e. \(0.115 \mathrm{M} \mathrm{NaClO}\) and \(0.0500 \mathrm{M} \mathrm{KI}\)

Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed: a. sodium cyanide and nitric acid b. ammonium chloride and sodium hydroxide c. sodium cyanide and ammonium bromide d. potassium hydrogen sulfate and lithium acetate e. sodium hypochlorite and ammonia

Morphine has the formula \(\mathrm{C}_{17} \mathrm{H}_{19} \mathrm{NO}_{3}\). It is a base and accepts one proton per molecule. It is isolated from opium. A 0.682 -g sample of opium is found to require \(8.92 \mathrm{~mL}\) of a \(0.0116 \mathrm{M}\) solution of sulfuric acid for neutralization. Assuming that morphine is the only acid or base present in opium, calculate the percent morphine in the sample of opium.

A solution of \(0.23 \mathrm{~mol}\) of the chloride salt of protonated quinine \(\left(\mathrm{QH}^{+}\right),\) a weak organic base, in \(1.0 \mathrm{~L}\) of solution has \(\mathrm{pH}=4.58 .\) Find the \(K_{\mathrm{b}}\) of quinine \((\mathrm{Q})\)

A student mistakenly calculates the \(\mathrm{pH}\) of a \(1.0 \times 10^{-7} \mathrm{M} \mathrm{HI}\) solution to be \(7.0 .\) Explain why the student is incorrect and calculate the correct \(\mathrm{pH}\).

Without doing any calculations, determine which solution in each pair is more acidic. a. \(0.0100 \mathrm{M}\) in \(\mathrm{HCl}\) and \(0.0100 \mathrm{M}\) in \(\mathrm{KOH}\) b. \(0.0100 \mathrm{M}\) in HF and \(0.0100 \mathrm{M}\) in \(\mathrm{KBr}\) c. \(0.0100 \mathrm{M}\) in \(\mathrm{NH}_{4} \mathrm{Cl}\) and \(0.0100 \mathrm{M}\) in \(\mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{Br}\) d. \(0.100 \mathrm{M}\) in \(\mathrm{NaCN}\) and \(0.100 \mathrm{M}\) in \(\mathrm{CaCl}_{2}\)

Rank the acids in order of increasing acid strength. \(\mathrm{CH}_{3} \mathrm{COOH} \quad \mathrm{CH}_{2} \mathrm{ClCOOH} \quad \mathrm{CHCl}_{2} \mathrm{COOH} \quad \mathrm{CCl}_{3} \mathrm{COOH}\)

Without using a calculator, determine the \(\mathrm{pH}\) and \(\mathrm{pOH}\) of each solution. Rank the solutions from most acidic to most basic. a. \(1.0 \times 10^{-2} \mathrm{M} \mathrm{HCl}\) b. \(1.0 \times 10^{-4} \mathrm{M} \mathrm{HCl}\) c. \(1.0 \times 10^{-2} \mathrm{M} \mathrm{NaOH}\) d. \(1.0 \times 10^{-4} \mathrm{M} \mathrm{NaOH}\)

Without referring to the text, have each member of your group mention a different property of either an acid or a base, such as “Acids turn blue litmus paper red." Record as many properties as your group can recall without the text.

Have each group member make two flashcards with an acid or base on one side and its conjugate on the other side. Check each other's cards and quiz each other until each group member is proficient at identifying conjugate pairs.

Answer the following questions in a complete sentence or two: a. How do you know if an acid is strong or weak? b. How do you calculate the \(\mathrm{pH}\) of a strong acid solution? c. How do you calculate the \(\mathrm{pH}\) of a weak acid solution? d. If you know the \(K_{\mathrm{a}}\) of an acid, how do you determine the \(K_{\mathrm{b}}\) of its conjugate base? e. If you know [OH \(^{-}\) ] for a solution, how do you determine \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right] ?\)