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Chapter 16: Problem 21

Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: $(\mathbf{a}) \mathrm{F}^{-}(\mathbf{b}) \mathrm{Br}^{-}(\mathbf{c}) \mathrm{HS}^{-}(\mathbf{d}) \mathrm{ClO}_{4}^{-}(\mathbf{e}) \mathrm{HCOO}^{-}$

Short Answer

Expert verified
In summary: 1. F- is a weak base, and its conjugate acid HF is a weak acid. 2. Br- has negligible basicity, and its conjugate acid HBr is a strong acid. 3. HS- is a weak base, and its conjugate acid H2S is a weak acid. 4. ClO₄- has negligible basicity, and its conjugate acid HClO₄ is a strong acid. 5. HCOO- is a weak base, and its conjugate acid HCOOH is a weak acid.

Step by step solution

01

(a) Fluoride Ion - F-

Fluoride ion (F-) acts as a weak base in solution. Its conjugate acid would be the result of the base accepting a proton (H+). So, the conjugate acid of F- is HF (hydrogen fluoride). HF is a weak acid.
02

(b) Bromide Ion - Br-

Bromide ion (Br-) has negligible basicity because it is the conjugate base of a strong acid, HBr (hydrogen bromide). Its conjugate acid would be HBr. HBr is a strong acid.
03

(c) HS- Ion

HS- ion is a weak base, as it is the conjugate base of H2S (hydrogen sulfide). Its conjugate acid would be H2S. H2S is a weak acid.
04

(d) Perchlorate Ion - ClO₄-

Perchlorate ion (ClO₄-) has negligible basicity because it is the conjugate base of a strong acid, HClO₄ (perchloric acid). Its conjugate acid would be HClO₄. HClO₄ is a strong acid.
05

(e) Formate Ion - HCOO-

Formate ion (HCOO-) is a weak base, which is the conjugate base of formic acid (HCOOH). Its conjugate acid would be HCOOH. HCOOH is a weak acid. In summary: 1. F- is a weak base, and its conjugate acid HF is a weak acid. 2. Br- has negligible basicity, and its conjugate acid HBr is a strong acid. 3. HS- is a weak base, and its conjugate acid H2S is a weak acid. 4. ClO₄- has negligible basicity, and its conjugate acid HClO₄ is a strong acid. 5. HCOO- is a weak base, and its conjugate acid HCOOH is a weak acid.

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Most popular questions from this chapter

The active ingredient in aspirin is acetylsalicylic acid \(\left(\mathrm{HC}_{9} \mathrm{H}_{7} \mathrm{O}_{4}\right),\) a monoprotic acid with \(K_{a}=3.3 \times 10^{-4}\) at \(25^{\circ} \mathrm{C}\) What is the \(\mathrm{pH}\) of a solution obtained by dissolving one regular aspirin tablet, containing \(100 \mathrm{mg}\) of acetylsalicylic acid, in $200 \mathrm{~mL}$ of water?

Calculate the \(\mathrm{pH}\) of each of the following strong acid solutions: (a) \(8.3 \times 10^{-4} \mathrm{MHCl},(\mathbf{b}) 1.20 \mathrm{~g}\) of \(\mathrm{HNO}_{3}\) in \(500 \mathrm{~mL}\) of solution, $(\mathbf{c}) 2.0 \mathrm{~mL}\( of \)0.250 \mathrm{M} \mathrm{HClO}_{4}\( diluted to \)40.0 \mathrm{~mL}\(, (d) a solution formed by mixing \)25.0 \mathrm{~mL}\( of \)0.100 \mathrm{M} \mathrm{HBr}\( with \)25.0 \mathrm{~mL}\( of \)0.200 \mathrm{M} \mathrm{HCl}$.

(a) Write a chemical equation that illustrates the autoionization of water. (b) Write the expression for the ionproduct constant for water, $K_{w} .(\mathbf{c})$ If a solution is described as basic, which of the following is true: (i) \(\left[\mathrm{H}^{+}\right]>\left[\mathrm{OH}^{-}\right]\), (ii) \(\left[\mathrm{H}^{+}\right]=\left[\mathrm{OH}^{-}\right],\) or (iii) \(\left[\mathrm{H}^{+}\right]<\left[\mathrm{OH}^{-}\right] ?\)

For each of these reactions, identify the acid and base among the reactants, and state if the acids and bases are Lewis, Arrhenius, and/or Brønsted-Lowry: (a) \(\mathrm{PCl}_{4}^{+}+\mathrm{Cl}^{-} \longrightarrow \mathrm{PCl}_{5}\) (b) $\mathrm{NH}_{3}+\mathrm{BF}_{3} \longrightarrow \mathrm{H}_{3} \mathrm{NBF}_{3}$ (c) $\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+\mathrm{H}_{2} \mathrm{O} \longrightarrow\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{OH}\right]^{2+}+\mathrm{H}_{3} \mathrm{O}^{+}$

A solution is made by adding $1.000 \mathrm{~g} \mathrm{Ca}(\mathrm{OH})_{2}(s), 100.0 \mathrm{~mL}$ of \(0.10 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\), and enough water to make a final volume of \(350.0 \mathrm{~mL}\). Assuming that all of the solid dissolves, what is the \(\mathrm{pH}\) of the final solution?
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