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Chapter 4: Problem 35

Consider the following generic equation: $$ \mathrm{H}^{+}(a q)+\mathrm{B}^{-}(a q) \longrightarrow \mathrm{HB}(a q) $$ For which of the following pairs would this be the correct prototype equation for the acid-base reaction in solution? If it is not correct, write the proper equation for the acid-base reaction between the pair. (a) nitric acid and calcium hydroxide (b) hydrochloric acid and \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) (c) hydrobromic acid and aqueous ammonia (d) perchloric acid and barium hydroxide (e) sodium hydroxide and nitrous acid

Short Answer

Expert verified
Answer: No, the reactions in Pair (a) and Pair (d) do not follow the generic equation for acid-base reactions. The correct equations are provided in the solution above, showcasing that additional products are formed in these reactions.

Step by step solution

01

Pair (a): Nitric acid and calcium hydroxide

Nitric acid (\(\mathrm{HNO}_3\)) will act as an acid, donating \(\mathrm{H}^+\) ions, and calcium hydroxide (\(\mathrm{Ca(OH)}_2\)) will act as a base, providing \(\mathrm{OH}^-\) ions. The prototype equation provided does not describe the reaction between these substances. The correct equation is: $$ \mathrm{HNO}_3 (aq) + \mathrm{Ca(OH)}_2 (aq) \longrightarrow \mathrm{Ca(NO}_3)_2 (aq) + 2\mathrm{H}_2\mathrm{O} (l) $$
02

Pair (b): Hydrochloric acid and \(\mathrm{CH}_{3} \mathrm{NH}_{2}\)

Hydrochloric acid (\(\mathrm{HCl}\)) will act as an acid, donating \(_H^+\) ions, and \(\mathrm{CH_3NH_2}\) (methylamine) will act as a base. This pair matches the generic equation. The correct equation is: $$ \mathrm{H}^+ (aq) + \mathrm{CH}_{3} \mathrm{NH}_{2}^{-}(aq) \longrightarrow \mathrm{CH}_3\mathrm{NH}_3\mathrm{Cl} (aq) $$
03

Pair (c): Hydrobromic acid and aqueous ammonia

Hydrobromic acid (\(\mathrm{HBr}\)) will act as an acid, donating \(\mathrm{H}^+\) ions, and aqueous ammonia (\(\mathrm{NH}_3\)) will act as a base. This pair matches the generic equation. The correct equation is: $$ \mathrm{H}^+ (aq) + \mathrm{NH}_{3}(aq) \longrightarrow \mathrm{NH}_{4} \mathrm{Br}(aq) $$
04

Pair (d): Perchloric acid and barium hydroxide

Perchloric acid (\(\mathrm{HClO}_4\)) will act as an acid, donating \(\mathrm{H}^+\) ions, and barium hydroxide (\(\mathrm{Ba(OH)}_2\)) will act as a base, providing \(\mathrm{OH}^-\) ions. The prototype equation provided does not describe the reaction between these substances. The correct equation is: $$ \mathrm{HClO}_4 (aq) + \mathrm{Ba(OH)}_2 (aq) \longrightarrow \mathrm{Ba(ClO}_4)_2 (aq) + 2\mathrm{H}_2\mathrm{O} (l) $$
05

Pair (e): Sodium hydroxide and nitrous acid

Sodium hydroxide (\(\mathrm{NaOH}\)) will act as a base, providing \(\mathrm{OH}^-\) ions, and nitrous acid (\(\mathrm{HNO}_2\)) will act as an acid, donating \(\mathrm{H}^+\) ions. The prototype equation provided does not describe the reaction between these substances. The correct equation is: $$ \mathrm{NaOH}(aq) + \mathrm{HNO}_2(aq) \longrightarrow \mathrm{NaNO}_2(aq) + \mathrm{H}_2\mathrm{O}(l) $$

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Most popular questions from this chapter

Write balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus \(\left(P_{4}\right)\) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate \(\left(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\right)\) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.

Consider the following generic equation $$ \mathrm{OH}^{-}(a q)+\mathrm{HB}(a q) \longrightarrow \mathrm{B}^{-}(a q)+\mathrm{H}_{2} \mathrm{O} $$ For which of the following pairs would this be the correct prototype equation for the acid-base reaction in solution? If it is not correct, write the proper equation for the acid-base reaction between the pair. (a) hydrochloric acid and pyridine, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{~N}\) (b) sulfuric acid and rubidium hydroxide (c) potassium hydroxide and hydrofluoric acid (d) ammonia and hydriodic acid (e) strontium hydroxide and hydrocyanic acid

A capsule of vitamin \(\mathrm{C}\), a weak acid, is analyzed by titrating it with \(0.425 M\) sodium hydroxide. It is found that \(6.20 \mathrm{~mL}\) of base is required to react with a capsule weighing \(0.628 \mathrm{~g}\). What is the percentage of vitamin \(\mathrm{C}\) \(\left(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{6}\right)\) in the capsule? (One mole of vitamin \(\mathrm{C}\) reacts with one mole of hydroxide ion.)

Solid iron(III) hydroxide is added to \(625 \mathrm{~mL}\) of \(0.280 \mathrm{M} \mathrm{HCl}\). The resulting solution is acidic and titrated with \(238.2 \mathrm{~mL}\) of \(0.113 \mathrm{M} \mathrm{NaOH}\). What mass of iron(III) hydroxide was added to the HCl?

An artificial fruit beverage contains \(12.0 \mathrm{~g}\) of tartaric acid, \(\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{O}_{6}\) to achieve tartness. It is titrated with a basic solution that has a density of \(1.045 \mathrm{~g} / \mathrm{cm}^{3}\) and contains \(5.00\) mass percent \(\mathrm{KOH}\). What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
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