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Chapter 15: Problem 193

Write a chemical equation for the reaction between each pair of reactants, using single or double arrows as appropriate: (a) \(\mathrm{HCO}_{3}^{-}\) and \(\mathrm{OH}^{-}\) (b) \(\mathrm{HCl}\) and \(\mathrm{F}^{-}\) (c) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) and \(\mathrm{OH}^{-}\) (d) \(\mathrm{HCN}\) and \(\mathrm{H}_{2} \mathrm{O}\)

Short Answer

Expert verified
(a) \(\mathrm{HCO}_3^- + \mathrm{OH}^- \rightarrow \mathrm{CO}_3^{2-} + \mathrm{H}_2\mathrm{O}\) (b) \(\mathrm{HCl} + \mathrm{F}^- \rightarrow \mathrm{HF} + \mathrm{Cl}^-\) (c) \(\mathrm{H}_2\mathrm{CO}_3 + \mathrm{OH}^- \rightarrow \mathrm{HCO}_3^- + \mathrm{H}_2\mathrm{O}\) (d) \(\mathrm{HCN} + \mathrm{H}_2\mathrm{O} \rightleftharpoons \mathrm{CN}^- + \mathrm{H}_3\mathrm{O}^+\)

Step by step solution

01

(a) HCO3- and OH- reaction

The given reactants are the bicarbonate ion (HCO₃⁻) and the hydroxide ion (OH⁻). This is a reaction between a weak acid (HCO₃⁻) and a strong base (OH⁻). The acid will donates a proton (H⁺) to the base, resulting in the formation of water (H₂O) and the carbonate ion (CO₃²⁻). Since the reaction involves a weak acid and a strong base, the equilibrium will lie strongly to the right, and we can use a single arrow to represent the reaction: \[\mathrm{HCO}_3^- + \mathrm{OH}^- \rightarrow \mathrm{CO}_3^{2-} + \mathrm{H}_2\mathrm{O}\]
02

(b) HCl and F- reaction

The given reactants are hydrogen chloride (HCl) and the fluoride ion (F⁻). This is an acid-base reaction between a strong acid (HCl) and a weak base (F⁻). The acid donates a proton (H⁺) to the base, resulting in the formation of water (or hydronium ion) and hydrogen fluoride (HF). Since the reaction involves a strong acid and a weak base, the equilibrium will lie strongly to the right. We can use a single arrow to represent the reaction: \[\mathrm{HCl} + \mathrm{F}^- \rightarrow \mathrm{HF} + \mathrm{Cl}^-\]
03

(c) H2CO3 and OH- reaction

The given reactants are carbonic acid (H₂CO₃) and the hydroxide ion (OH⁻). This is a reaction between a weak acid (H₂CO₃) and a strong base (OH⁻). The acid will donates a proton (H⁺) to the base, resulting in the formation of water (H₂O) and bicarbonate ion (HCO₃⁻). Since the reaction involves a weak acid and a strong base, the equilibrium will lie strongly to the right. We can use a single arrow to represent the reaction: \[\mathrm{H}_2\mathrm{CO}_3 + \mathrm{OH}^- \rightarrow \mathrm{HCO}_3^- + \mathrm{H}_2\mathrm{O}\]
04

(d) HCN and H2O reaction

The given reactants are hydrogen cyanide (HCN) and water (H₂O). This is an acid-base reaction between a weak acid (HCN) and a weak base (H₂O). The acid donates a proton (H⁺) to the water, resulting in the formation of the hydronium ion (H₃O⁺) and the cyanide ion (CN⁻). Since the reaction involves a weak acid and a weak base, the equilibrium will be around the center. Consequently, we can use double arrows to represent the reaction: \[\mathrm{HCN} + \mathrm{H}_2\mathrm{O} \rightleftharpoons \mathrm{CN}^- + \mathrm{H}_3\mathrm{O}^+\]

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Most popular questions from this chapter

Suppose \(2.0\) moles of sodium acetate, \(\mathrm{NaO}_{2} \mathrm{CCH}_{3}\), are dissolved in some water and then \(1.0 \mathrm{~L}\) of a \(1.0 \mathrm{M} \mathrm{HCl}\) solution is added. (a) Write the chemical reaction that occurs. (b) After the reaction, what are the predominant species in solution? How many moles of each species are there? (c) Is the resulting solution a buffer? If yes, explain why.

How many moles of \(\mathrm{Ba}(\mathrm{OH})_{2}\) does it take to neutralize \(2.5\) moles of \(\mathrm{HNO}_{3}\) ?

Acrylic acid, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{COOH}\), is a weak monoprotic acid. Write a balanced equation for the reaction that occurs when \(25.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{KOH}\) is added to \(50.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{COOH}\). Besides water, what species are present in the solution? Is this solution a buffer? Why or why not?

Aniline, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\), is a weak base, with a lone pair of electrons on the nitrogen atom. (a) According to Bronsted and Lowry, what must aniline do to act as a base? (b) Why can aniline act as a base? (c) What are the molecular formula and charge of the conjugate acid of aniline?

Is it possible to obtain water at \(25{ }^{\circ} \mathrm{C}\) that contains absolutely no ions of any sort? Explain.
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