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Chapter 45: Problem 7

Indicate which of the following are potential acids, potential bases, or both (potential acid and potential base). a) \(\mathrm{Al}^{3+}\) b) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) c) \(\mathrm{HPO}_{4}{ }^{2-}\) d) \(\quad \mathrm{F}^{-}\) e) \(\mathrm{NH}_{4}^{+}\) f) \(\mathrm{H}_{2} \mathrm{O}\)

Short Answer

Expert verified
a) base, b) acid, c) both (acid and base), d) base, e) acid, f) both (acid and base)

Step by step solution

01

Identify potential acids

A potential acid is a substance which can donate H+. \(\mathrm{Al}^{3+}\) cannot donate H+ meaning it's not an acid. \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) can release an H+ to form \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) so it's an acid. \(\mathrm{HPO}_{4}{ }^{2-}\) can donate an H+ to form \(\mathrm{PO}_{4}{ }^{3-}\) so it's an acid. \(\mathrm{NH}_{4}^{+}\) can donate an H+ to form \(\mathrm{NH}_{3}\) so it's an acid.
02

Identify potential bases

A potential base is a substance which can accept H+. \(\mathrm{Al}^{3+}\) can accept three H+ to form \(\mathrm{Al(H_{2}O)_{6}}^{3+}\) so it's a base. \(\mathrm{F}^{-}\) can accept an H+ to form HF so it's a base. \(\mathrm{H}_{2} \mathrm{O}\) can accept an H+ to form \(\mathrm{H}_{3} \mathrm{O}^{+}\) so it's a base.
03

Identify substances that are both potential acids and potential bases

A substance that can both accept and donate H+ is an amphoteric substance. \(\mathrm{HPO}_{4}{ }^{2-}\) can also accept an H+ to form \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) so it's both an acid and a base. \(\mathrm{NH}_{4}^{+}\) cannot accept H+. \(\mathrm{H}_{2} \mathrm{O}\) can also donate an H+ to form \(\mathrm{OH}^{-}\) so it's both an acid and a base

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Most popular questions from this chapter

To 2 significant figures, predict the \(\mathrm{pH}\) of a \(1.00\) molar solution of \(\mathrm{NaBr}\). Explain your reasoning carefully.

\(\mathrm{HNO}_{3}\) is considered to be the weakest of the strong acids. Explain why the conjugate bases of all strong acids do not produce basic solutions when dissolved in water.

Provide an expression relating \(K_{\mathrm{w}}\) to \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) of a conjugate acid-base pair.

Consider two acids, HA and HX, with HA being a stronger acid than HX. a) Which acid has a larger value of \(K_{\mathrm{a}}\) ? b) Which conjugate base, \(\mathrm{A}^{-}\) or \(\mathrm{X}^{-}\), has a larger value of \(K_{\mathrm{b}}\) ? c) Provide a qualitative description of the relationship between the relative strength of an acid and the relative strength of its conjugate base. d) Assume that \(K_{\mathrm{a}}\) of \(\mathrm{HA}\) is \(1.0 \times 10^{-5}\) and \(K_{\mathrm{a}}\) of \(\mathrm{HX}\) is \(3.5 \times 10^{-7}\). Calculate the \(K_{\mathrm{b}}\) for \(\mathrm{A}^{-}\) and for \(\mathrm{X}^{-}\) and confirm that your answers to parts \(\mathrm{b}\) and \(\mathrm{c}\) are correct.

For each of the following, describe the common features: a) all \(K_{\mathrm{a}}\) expressions b) all \(K_{\mathrm{b}}\) expressions c) all \(K_{\mathrm{a}} \times K_{\mathrm{b}}\) products
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