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Chapter 16: Problem 100

If a substance is a Lewis acid, is it necessarily a Br酶nsted-Lowry acid? Is it necessarily an Arrhenius acid? Explain.

Short Answer

Expert verified
A substance being a Lewis acid, which is an electron-pair acceptor, does not necessarily mean it is a Br酶nsted-Lowry acid or an Arrhenius acid. The key differences are that Br酶nsted-Lowry acids donate protons in reactions, and Arrhenius acids increase the concentration of H鈦� ions in aqueous solutions. Some Lewis acids may not exhibit these behaviors, making it possible for a substance to be a Lewis acid without being a Br酶nsted-Lowry or Arrhenius acid.

Step by step solution

01

Defining Lewis, Br酶nsted-Lowry, and Arrhenius acids

A Lewis acid is a substance that can accept an electron pair from a Lewis base to form a coordinate covalent bond. In other words, it is an electron-pair acceptor. A Br酶nsted-Lowry acid is a substance that can donate a proton (H鈦�) to a Br酶nsted-Lowry base in a reaction. So, it is a proton donor. An Arrhenius acid is a substance that, when dissolved in water, increases the concentration of H鈦� ions (or H鈧僌鈦�, hydronium ions) in the solution. These are typically compounds containing hydrogen, such as hydrogen halides (e.g., HCl, HBr, HI).
02

Comparing Lewis acids to Br酶nsted-Lowry acids

Now that we have defined each type of acid, let's compare Lewis acids to Br酶nsted-Lowry acids. While both types of acids can accept electron pairs to form coordinate covalent bonds, the key difference is that Br酶nsted-Lowry acids include the donation of a proton in the reaction. It is possible for a substance to be a Lewis acid without being a Br酶nsted-Lowry acid, as it may not necessarily donate a proton during the reaction. Therefore, a substance being a Lewis acid does not necessarily mean it is a Br酶nsted-Lowry acid.
03

Comparing Lewis acids to Arrhenius acids

Next, let's compare Lewis acids to Arrhenius acids. Arrhenius acids specifically increase the concentration of H鈦� ions in an aqueous solution. Some Lewis acids may not necessarily do this, as they may accept electron pairs from Lewis bases without releasing H鈦� ions into the solution. Therefore, a substance being a Lewis acid does not necessarily mean it is an Arrhenius acid.
04

Conclusion

In conclusion, a substance being a Lewis acid is not sufficient to guarantee that it is also a Br酶nsted-Lowry or an Arrhenius acid. The key differences lie in whether the substance donates a proton (for Br酶nsted-Lowry) or increases the concentration of H鈦� ions in an aqueous solution (for Arrhenius).

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Most popular questions from this chapter

Caproic acid \(\left(\mathrm{C}_{5} \mathrm{H}_{11} \mathrm{COOH}\right)\) is found in small amounts in coconut and palm oils and is used in making artificial flavors. A saturated solution of the acid contains \(11 \mathrm{~g} / \mathrm{L}\) and has a pH of 2.94. Calculate \(K_{a}\) for the acid.

(a) Given that \(K_{a}\) for acetic acid is \(1.8 \times 10^{-5}\) and that for hypochlorous acid is \(3.0 \times 10^{-8}\), which is the stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) Calculate \(K_{b}\) values for \(\mathrm{CH}_{2} \mathrm{COO}^{-}\) and \(\mathrm{Cl} \mathrm{O}^{-}\)

Designate the Br酶nsted-Lowry acid and the BronstedLowry base on the left side of each of the following equations, and also designate the conjugate acid and conjugate base on the right side: (a) \(\mathrm{NH}_{4}{ }^{+}(a q)+\mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{NH}_{3}(a q)\) (b) \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}(a q)+\mathrm{H}_{2} \mathrm{O}(I) \rightleftharpoons\) (c) \(\mathrm{HCHO}_{2}(a q)+\mathrm{PO}_{4}{ }^{3-}(a q) \stackrel{\left(\mathrm{CH}_{3}\right)_{3} \mathrm{NH}^{+}(a q)+\mathrm{OH}^{-}(a q)}{\mathrm{CHO}_{2}^{-}(a q)+\mathrm{HPO}_{4}{ }^{2-}(a q)}\)

Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) Acid strength in a series of \(\mathrm{H}-\mathrm{X}\) molecules increases with increasing size of \(X .\) (b) For acids of the same general structure but differing electronegativities of the central atoms, acid strength decreases with increasing electronegativity of the central atom. (c) The strongest acid known is HF because fluorine is the most electronegative element.

Write the chemical equation and the \(K_{b}\) expression for the ionization of each of the following bases in aqueous solution: (a) dimethylamine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NH} ;\) (b) carbonate ion, \(\mathrm{CO}_{3}{ }^{2-} ;(\mathrm{c})\) formate ion, \(\mathrm{CHO}_{2}{ }^{-}\).
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