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Chapter 16: Problem 102

Indicate whether each of the following statements is correct or incorrect. For those that are incorrect, explain why they are wrong. (a) Every Bronsted-Lowry acid is also a Lewis acid. (b) Every Lewis acid is also a Bronsted-Lowry acid. (c) Conjugate acids of weak bases produce more acidic solutions than conjugate acids of strong bases. (d) \(\mathrm{K}^{+}\) ion is acidic in water because it causes hydrating water molecules to become more acidic. (e) The percent ionization of a weak acid in water increases as the concentration of acid decreases.

Short Answer

Expert verified
(a) Correct - All Bronsted-Lowry acids can be classified as Lewis acids as they donate protons and involve transfer of electron pairs. (b) Incorrect - Not all Lewis acids are Bronsted-Lowry acids. Some accept an electron pair without donating a proton, such as boron trifluoride (BF3). (c) Correct - Conjugate acids of weak bases produce more acidic solutions than conjugate acids of strong bases as they more readily donate protons. (d) Incorrect - \(\mathrm{K}^{+}\) ion is not acidic or basic in water; it doesn't react with water and doesn't affect the pH significantly. (e) Correct - The percent ionization of a weak acid increases as the concentration of acid decreases due to fewer acid molecules impeding dissociation and maintaining equilibrium.

Step by step solution

01

Statement (a)

Every Bronsted-Lowry acid is also a Lewis acid. This statement is correct. The definition of a Bronsted-Lowry acid is a substance that donates a proton (H+) in a reaction, while a Lewis acid is a substance that accepts an electron pair. Since proton donation involves the transfer of an electron pair, all Bronsted-Lowry acids can be classified as Lewis acids.
02

Statement (b)

Every Lewis acid is also a Bronsted-Lowry acid. This statement is incorrect. While all Bronsted-Lowry acids are indeed Lewis acids, not all Lewis acids are Bronsted-Lowry acids. Some Lewis acids can accept an electron pair without donating a proton. For example, boron trifluoride (BF3) is a Lewis acid because it can accept an electron pair, but it is not a Bronsted-Lowry acid since it does not donate a proton.
03

Statement (c)

Conjugate acids of weak bases produce more acidic solutions than conjugate acids of strong bases. This statement is correct. In a solution, weak bases are less likely to accept protons, so their conjugate acids will more readily donate protons, making the solution more acidic. On the other hand, strong bases readily accept protons, making their conjugate acids less likely to donate protons and the solution less acidic.
04

Statement (d)

\(\mathrm{K}^{+}\) ion is acidic in water because it causes hydrating water molecules to become more acidic. This statement is incorrect. The \(\mathrm{K}^{+}\) ion is not acidic or basic in water, but rather it is a spectator ion. It doesn't react with water nor cause the formation of acidic or basic species. The presence of this ion in water doesn't affect the pH significantly.
05

Statement (e)

The percent ionization of a weak acid in water increases as the concentration of acid decreases. This statement is correct. The percent ionization or dissociation of a weak acid in water is the ratio of dissociated acid to the initial concentration of the acid. As the concentration of a weak acid decreases, the degree of ionization increases since there are fewer acid molecules to impede the dissociation process and maintain the equilibrium. In other words, at lower concentration, more acid molecules dissociate in an attempt to achieve equilibrium, leading to a higher percentage of ionization.

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Most popular questions from this chapter

Calculate the \(\mathrm{pH}\) of each of the following strong acid solutions: (a) \(8.5 \times 10^{-3} \mathrm{MHBr}\), (b) \(1.52 \mathrm{~g}\) of \(\mathrm{HNO}_{3}\) in \(575 \mathrm{~mL}\) of solution, (c) \(5.00 \mathrm{~mL}\) of \(0.250 \mathrm{M} \mathrm{HClO}_{4}\) diluted to \(50.0 \mathrm{~mL}\), (d) a solution formed by mixing \(10.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{HBr}\) with \(20.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HCl}\)

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) \(\mathrm{HCO}_{3}^{-}, (\mathrm{c}) \mathrm{O}^{2-}, (\mathrm{d}) \mathrm{Cl}^{-} ,(\mathrm{e}) \mathrm{NH}_{3}\)

Although \(\mathrm{HCl}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) have very different properties as pure substances, their aqueous solutions possess many common properties. List some general properties of these solutions, and explain their common behavior in terms of the species present.

(a) What is the difference between the Arrhenius and the Bronsted-Lowry definitions of an acid? (b) \(\mathrm{NH}_{3}(g)\) and \(\mathrm{HCl}(g)\) react to form the ionic solid \(\mathrm{NH}_{4} \mathrm{Cl}(s) .\) Which substance is the Bronsted-Lowry acid in this reaction? Which is the Bronsted-Lowry base?

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) In general, the acidity of binary acids increases from left to right in a given row of the periodic table. (b) In a series of acids that have the same central atom, acid strength increases with the number of hydrogen atoms bonded to the central atom. (c) Hydrotelluric acid \(\left(\mathrm{H}_{2} \mathrm{Te}\right)\) is a stronger acid than \(\mathrm{H}_{2} \mathrm{~S}\) because Te is more electronegative than \(\mathrm{S}\).
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