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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

(a) Give the conjugate base of the following BronstedLowry acids: (i) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\). (ii) \(\mathrm{HPO}_{4}{ }^{2-}\). (b) Give the conjugate acid of the following Bronsted-Lowry bases: (i) \(\mathrm{CO}_{3}^{2-}\) (ii) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{2}\)

Identify the Lewis acid and Lewis base among the reactants in each of the following reactions: (a) \(\mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{3}(s)+6 \mathrm{H}_{2} \mathrm{O}(I) \rightleftharpoons\) \(\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q)+3 \mathrm{ClO}_{4}^{-}(a q)\) (b) \(\mathrm{CN}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q)\) (c) \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}(\mathrm{~g})+\mathrm{BF}_{3}(g) \rightleftharpoons\left(\mathrm{CH}_{3}\right)_{3} \mathrm{NBF}_{3}(\mathrm{~s})\) (d) \(\mathrm{HIO}(\mathrm{lq})+\mathrm{NH}_{2}^{-(l q)} \rightleftharpoons \mathrm{NH}_{3}(l q)+\mathrm{IO}^{-}(l q)\) (Iq denotes liquid ammonia as solvent)

(a) The hydrogen oxalate ion \(\left(\mathrm{HC}_{2} \mathrm{O}_{4}{ }^{-}\right)\) is amphiprotic. Write a balanced chemical equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water. (b) What is the conjugate acid of \(\mathrm{HC}_{2} \mathrm{O}_{4}^{-} ?\) What is its conjugate base?

Label each of the following as being a strong acid, a weak acid, or a species with negligible acidity. In each case write the formula of its conjugate base, and indicate whether the conjugate base is a strong base, a weak base, or a species with negligible basicity: (a) \(\mathrm{HNO}_{2}\), (b) \(\mathrm{H}_{2} \mathrm{SO}_{4},(\mathrm{c}) \mathrm{HPO}_{4}{ }^{2-}\), (d) \(\mathrm{CH}_{4}\) (e) \(\mathrm{CH}_{3} \mathrm{NH}_{3}{ }^{+}\) (an ion related to \(\mathrm{NH}_{4}{ }^{+}\) ).

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.
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