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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: (a) \(\mathrm{CH}_{3} \mathrm{COO}^{-},\) (b) \(\mathrm{HCO}_{3}^{-}, (\mathrm{c}) \mathrm{O}^{2-}, (\mathrm{d}) \mathrm{Cl}^{-} ,(\mathrm{e}) \mathrm{NH}_{3}\)

Short Answer

Expert verified
(a) \(\mathrm{CH}_{3}\mathrm{COO}^{-}\) is a weak base. Its conjugate acid is \(\mathrm{CH}_{3}\mathrm{COOH}\), a weak acid. (b) \(\mathrm{HCO}_{3}^{-}\) is a weak base. Its conjugate acid is \(\mathrm{H}_{2}\mathrm{CO}_{3}\), a weak acid. (c) \(\mathrm{O}^{2-}\) is a strong base. Its conjugate acid is \(\mathrm{OH}^{-}\), a weak acid. (d) \(\mathrm{Cl}^{-}\) has negligible basicity. Its conjugate acid is \(\mathrm{HCl}\), a strong acid. (e) \(\mathrm{NH}_{3}\) is a weak base. Its conjugate acid is \(\mathrm{NH}_{4}^{+}\), a weak acid.

Step by step solution

01

Identify nature of species

This species \(\mathrm{CH}_{3}\mathrm{COO}^{-}\) is the conjugate base of acetic acid (\(\mathrm{CH}_{3}\mathrm{COOH}\)). It is a weak base because it is the conjugate base of a weak acid.
02

Conjugate acid and its nature

The conjugate acid of this species is \(\mathrm{CH}_{3}\mathrm{COOH}\), which is a weak acid. (b) \(\mathrm{HCO}_{3}^{-}\)
03

Identify nature of species

Bicarbonate ion (\(\mathrm{HCO}_{3}^{-}\)) is a weak base, as it is the conjugate base of carbonic acid (\(\mathrm{H}_{2}\mathrm{CO}_{3}\)).
04

Conjugate acid and its nature

The conjugate acid of this species is \(\mathrm{H}_{2}\mathrm{CO}_{3}\), which is a weak acid. (c) \(\mathrm{O}^{2-}\)
05

Identify nature of species

This species is a strong base. It is the oxide ion, formed when the stronger acid water (\(\mathrm{H}_{2}\mathrm{O}\)) loses two protons.
06

Conjugate acid and its nature

The conjugate acid of this species is \(\mathrm{OH}^{-}\), which is a weak acid. (d) \(\mathrm{Cl}^{-}\)
07

Identify nature of species

This species is the chloride ion and is considered to have negligible basicity, as it is the conjugate base of a strong acid (\(\mathrm{HCl}\)).
08

Conjugate acid and its nature

The conjugate acid of this species is \(\mathrm{HCl}\), which is a strong acid. (e) \(\mathrm{NH}_{3}\)
09

Identify nature of species

Ammonia (\(\mathrm{NH}_{3}\)) is a weak base because the nitrogen atom has a lone pair of electrons that it can use to bind a proton.
10

Conjugate acid and its nature

The conjugate acid of this species is \(\mathrm{NH}_{4}^{+}\), which is a weak acid.

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Most popular questions from this chapter

(a) The hydrogen oxalate ion \(\left(\mathrm{HC}_{2} \mathrm{O}_{4}^{-}\right)\) is amphiprotic. Write a balanced chemical equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water. (b) What is the conjugate acid of \(\mathrm{HC}_{2} \mathrm{O}_{4}\) ? What is its conjugate base?

(a) Given that \(K_{b}\) for ammonia is \(1.8 \times 10^{-5}\) and that for hydroxylamine is \(1.1 \times 10^{-8}\), which is the stronger base? (b) Which is the stronger acid, the ammonium ion or the hydroxylammonium ion? (c) Calculate \(K_{a}\) values for \(\mathrm{NH}_{4}^{+}\) and \(\mathrm{H}_{3} \mathrm{NOH}^{+}\)

Designate the Bronsted-Lowry acid and the Bronsted-Lowry base on the left side of each equation, and also designate the conjugate acid and conjugate base of each on the right side. (a) \(\mathrm{HBrO}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{BrO}^{-}(a q)\) (b) \(\mathrm{HSO}_{4}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{SO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q)\) (c) \(\mathrm{HSO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)

Write the chemical equation and the \(K_{b}\) expression for the reaction of each of the following bases with water: (a) propylamine,\(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{NH}_{2} ;\) (b) monohydrogen phosphate ion, \(\mathrm{HPO}_{4}^{2-}\); (c) benzoate ion, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2}^{-}\).

(a) What is a strong base? (b) A solution is labeled \(0.035 \mathrm{M}\) \(\mathrm{Sr}(\mathrm{OH})_{2} .\) What is \(\left[\mathrm{OH}^{-}\right]\) for the solution? (c) Is the following statement true or false? Because \(\mathrm{Mg}(\mathrm{OH})_{2}\) is not very soluble, it cannot be a strong base. Explain.
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