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Chapter 16: Problem 96

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

Short Answer

Expert verified
A substance being a Lewis acid does not necessarily mean it is a Bronsted-Lowry acid or an Arrhenius acid. While a Lewis acid accepts an electron pair, a Bronsted-Lowry acid donates a proton, and an Arrhenius acid increases hydrogen ion concentrations when dissolved in water. These definitions involve specific chemical interactions or conditions that may not apply to all Lewis acids.

Step by step solution

01

1. Defining Lewis Acids

A Lewis acid is a substance that can act as an electron-pair acceptor. It accepts a pair of electrons from another species, typically a Lewis base, to form a new bond.
02

2. Defining Bronsted-Lowry Acids

A Bronsted-Lowry acid is a substance that can donate a proton (H+) to another species, which is the Bronsted-Lowry base. The Bronsted-Lowry acid/base reaction involves the transfer of a proton from the acid to the base.
03

3. Defining Arrhenius Acids

An Arrhenius acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions (H+) or hydronium ions (H3O+) in the solution. This means that the substance must dissociate in water to produce hydrogen ions.
04

4. Comparing Lewis Acids to Bronsted-Lowry Acids

While both Lewis acids and Bronsted-Lowry acids involve the interaction between two species, the key difference is the type of interaction. A Lewis acid accepts an electron pair, while a Bronsted-Lowry acid donates a proton. A substance being a Lewis acid may or may not involve proton transfer, so it is not necessarily a Bronsted-Lowry acid.
05

5. Comparing Lewis Acids to Arrhenius Acids

Arrhenius acids specifically involve substances that increase hydrogen ion concentrations when dissolved in water. This definition is more restrictive than that of a Lewis acid since it requires the substance to be in an aqueous solution and produce hydrogen ions. A Lewis acid may not necessarily increase hydrogen ion concentrations or need to be in an aqueous solution, so it is not necessarily an Arrhenius acid. In conclusion, a substance being a Lewis acid does not necessarily mean it is a Bronsted-Lowry acid or an Arrhenius acid, as the definitions for each acid involve specific types of chemical interactions or conditions that may not apply to all Lewis acids.

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Most popular questions from this chapter

Using data from Appendix \(\mathrm{D},\) calculate \(\left[\mathrm{OH}^{-}\right]\) and \(\mathrm{pH}\) for each of the following solutions: (a) \(0.10 \mathrm{M} \mathrm{NaBrO},\) (b) \(0.080 \mathrm{MNaHS}\), (c) a mixture that is \(0.10 \mathrm{M}\) in \(\mathrm{NaNO}_{2}\) and \(0.20 \mathrm{M}\) in \(\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2}\)

(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.

Calculate \(\left[\mathrm{OH}^{-}\right]\) for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) \(\left[\mathrm{H}^{+}\right]=0.0505 \mathrm{M} ;\) (b) \(\left[\mathrm{H}^{+}\right]=2.5 \times 10^{-10} \mathrm{M} ;(\mathrm{c})\) a solution in which \(\left[\mathrm{H}^{+}\right]\) is 1000 times greater than \(\left[\mathrm{OH}^{-}\right] .\)

Calculate the percent ionization of propionic acid \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{COOH}\right)\) in solutions of each of the following concentrations \(\left(K_{a}\right.\) is given in Appendix \(\left.D\right):\) (a) \(0.250 \mathrm{M}\), (b) \(0.0800 \mathrm{M}\), (c) \(0.0200 \mathrm{M}\).

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) \(\mathrm{HSO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)
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