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Chapter 16: Problem 23

(a) Which of the following is the stronger Bronsted-Lowry acid, HBrO or HBr? (b) Which is the stronger BronstedLowry base, \(\mathrm{F}^{-}\) or \(\mathrm{Cl}^{-} ?\)

Short Answer

Expert verified
(a) HBr is a stronger Bronsted-Lowry acid than HBrO. (b) F⁻ is a stronger Bronsted-Lowry base than Cl⁻.

Step by step solution

01

(a) Compare acid strengths of HBrO and HBr

Consider the following reactions: HBrO ⇌ BrO⁻ + H⁺ (1) HBr ⇌ Br⁻ + H⁺ (2) To determine the stronger acid, we need to compare the stability of the conjugate bases (BrO⁻ and Br⁻) produced in the reactions.
02

(a) Stability of conjugate bases

BrO⁻ is a halogen-containing anion with a negative charge on the oxygen atom, whereas Br⁻ is a simple halide anion. Halogens are generally more electronegative than oxygen, so Br⁻ is significantly more stable due to electron distribution. Therefore, Br⁻ is more stable than BrO⁻.
03

(a) Stronger acid

As Br⁻ is a more stable conjugate base than BrO⁻, this implies that HBr is a stronger Bronsted-Lowry acid than HBrO.
04

(b) Compare base strengths of F⁻ and Cl⁻

To determine the stronger base between F⁻ and Cl⁻, we need to compare the stabilities of the conjugate acids produced from these bases: F⁻ + H⁺ ⇌ HF (3) Cl⁻ + H⁺ ⇌ HCl (4)
05

(b) Stability of conjugate acids

HF and HCl are both hydrogen halides. Since fluorine is more electronegative than chlorine, the H-F bond is more polar. This means that the HF molecule is less stable and has a weaker H-F bond compared to HCl.
06

(b) Stronger base

As HF is less stable as a conjugate acid than HCl, it implies that F⁻ is a stronger Bronsted-Lowry base than Cl⁻. In conclusion: (a) HBr is the stronger Bronsted-Lowry acid between HBrO and HBr. (b) F⁻ is the stronger Bronsted-Lowry base between F⁻ and Cl⁻.

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Most popular questions from this chapter

Identify the Brønsted-Lowry acid and the BrønstedLowry base on the left side of each equation, and also identify the conjugate acid and conjugate base of each on the right side. $$ \begin{array}{l} \text { (a) } \mathrm{HBrO}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{BrO}^{-}(a q) \\\ \text { (b) } \mathrm{HSO}_{4}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{SO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q) \\ \text { (c) } \mathrm{HSO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \end{array} $$

How many milliliters of concentrated hydrochloric acid solution \((36.0 \%\) HCl by mass, density \(=1.18 \mathrm{~g} / \mathrm{mL}\) ) are required to produce \(10.0 \mathrm{~L}\) of a solution that has a pH of \(2.05 ?\)

Saccharin, a sugar substitute, is a weak acid with \(\mathrm{p} K_{a}=2.32\) at \(25^{\circ} \mathrm{C}\). It ionizes in aqueous solution as follows: $$ \mathrm{HNC}_{7} \mathrm{H}_{4} \mathrm{SO}_{3}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{NC}_{7} \mathrm{H}_{4} \mathrm{SO}_{3}^{-}(a q) $$ What is the pH of a \(0.25 \mathrm{M}\) solution of this substance?

Calculate the number of \(\mathrm{H}^{+}(a q)\) ions in \(1.0 \mathrm{~mL}\) of pure water at \(25^{\circ} \mathrm{C}\).

The odor of fish is due primarily to amines, especially methylamine \(\left(\mathrm{CH}_{3} \mathrm{NH}_{2}\right)\). Fish is often served with a wedge of lemon, which contains citric acid. The amine and the acid react forming a product with no odor, thereby making the less-than-fresh fish more appetizing. Using data from Appendix \(D\), calculate the equilibrium constant for the reaction of citric acid with methylamine, if only the first proton of the citric acid \(\left(K_{a 1}\right)\) is important in the neutralization reaction.
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