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Chapter 16: Problem 95

Based on their compositions and structures and on conjugate acid-base relationships, select the stronger base in each of the following pairs: (a) \(\mathrm{BrO}^{-}\) or \(\mathrm{ClO}^{-}\), (b) \(\mathrm{BrO}^{-}\) or \(\mathrm{BrO}_{2}^{-},(\mathrm{c}) \mathrm{HPO}_{4}^{2-}\) or \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)

Short Answer

Expert verified
The stronger bases for each pair are: (a) BrO鈦�, (b) BrO鈦�, and (c) HPO鈧劼测伝.

Step by step solution

01

(a) Comparing BrO鈦� and ClO鈦�

First, let's identify the conjugate acids of these two bases: BrOH for BrO鈦� and ClOH for ClO鈦�. In general, the more electronegative the element, the more stable the conjugate acid will be. Here, Cl is more electronegative than Br, which means that the conjugate acid ClOH is stronger than BrOH. Since the stronger the conjugate acid, the weaker the conjugate base, the stronger base in this case is BrO鈦�.
02

(b) Comparing BrO鈦� and BrO鈧傗伝

First, we need to identify the conjugate acids: BrOH for BrO鈦� and BrO鈧侶 for BrO鈧傗伝. Both bases have Br as the central atom, but BrO鈧傗伝 has more oxygen atoms than BrO鈦�. Generally, the presence of more oxygen atoms increases the stability of the conjugate acid due to the electron-donating effect of oxygen atoms, which can help dissipate the charge. Since the conjugate acid of BrO鈧傗伝 is more stable than the conjugate acid of BrO鈦�, BrO鈧傗伝 is the weaker base. Therefore, BrO鈦� is the stronger base.
03

(c) Comparing HPO鈧劼测伝 and H鈧侾O鈧勨伝

The conjugate acids for these bases are H鈧侾O鈧勨伝 for HPO鈧劼测伝 and H鈧働O鈧� for H鈧侾O鈧勨伝. We can see that H鈧働O鈧� has more hydrogen atoms (meaning it is more acidic) compared to H鈧侾O鈧勨伝, which indicates a stronger conjugate acid. Since the stronger the conjugate acid, the weaker the conjugate base, H鈧侾O鈧勨伝 would be a weaker base compared to HPO鈧劼测伝. Thus, the stronger base is HPO鈧劼测伝.

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Most popular questions from this chapter

The amino acid glycine \(\left(\mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH}\right)\) can participate in the following equilibria in water: \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH}+\mathrm{H}_{2} \mathrm{O}=\) \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COO}^{-}+\mathrm{H}_{3} \mathrm{O}^{+} \quad K_{a}=4.3 \times 10^{-3}\) \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons\) \({ }^{+} \mathrm{H}_{3} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH}+\mathrm{OH}^{-} \quad K_{b}=6.0 \times 10^{-5}\) (a) Use the values of \(K_{a}\) and \(K_{b}\) to estimate the equilibrium constant for the intramolecular proton transfer to form a zwitterion: \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COOH} \rightleftharpoons{ }^{+} \mathrm{H}_{3} \mathrm{~N}-\mathrm{CH}_{2}-\mathrm{COO}^{-}\) What assumptions did you need to make? (b) What is the pH of a \(0.050 \mathrm{M}\) aqueous solution of glycine? (c) What would be the predominant form of glycine in a solution with pH 13? With pH 1?

(a) What is a strong base? (b) A solution is labeled \(0.035 \mathrm{M} \mathrm{Sr}(\mathrm{O} \mathrm{H})_{2}\). 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.

(a) Identify the Bronsted-Lowry acid and the Br酶nstedLowry base in the following reaction: (b) Identify the Lewis acid and the Lewis base in the reaction. [Sections \(16.2\) and \(16.11]\)

(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 \(\mathrm{Cl} \mathrm{O}^{-}\)

Although the acid-dissociation constant for phenol \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\right)\) is listed in Appendix \(\mathrm{D}\), the base - \(\mathrm{d}\) issociation constant for the phenolate ion \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}\right)\) is not. (a) Explain why it is not necessary to list both \(K_{a}\) for phenol and \(K_{b}\) for the phenolate ion. (b) Calculate \(K_{b}\) for the phenolate ion. (c) Is the phenolate ion a weaker or stronger base than ammoria?
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