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Chapter 16: Problem 89

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 \(\mathrm{ClO}^{-},(\mathbf{b}) \mathrm{BrO}^{-}\) or \(\mathrm{BrO}_{2}^{-}\) (c) \(\mathrm{HPO}_{4}^{2-}\) or \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}.\)

Short Answer

Expert verified
Based on their compositions and structures and on conjugate acid-base relationships, the stronger bases in each pair are: (a) ClO⁻, (b) BrO⁻, and (c) HPO₄²⁻.

Step by step solution

01

Understand the concept of conjugate acid-base pairs

A conjugate acid-base pair consists of two species that differ by the presence of a proton (H+ ion). The species which can donate a proton is known as the conjugate acid and the species which can accept a proton is called the conjugate base. When comparing the basic strength of two given species, the stronger base will be the one that can donate its proton more readily.
02

Analyze the basic strength of (a) BrO⁻ or ClO⁻

First, let's compare the basic strength of BrO⁻ and ClO⁻. Both of these species are in the same period and have the same charge. The only difference is in the central atom, where the Br atom is larger and less electronegative than the Cl atom. As a result, the negative charge on the BrO⁻ ion is more dispersed over a larger atom, making it less reactive, thus the BrO⁻ ion is a weaker base. In comparison, ClO⁻ has a more localized negative charge on the smaller, more electronegative Cl atom, which makes it a stronger base. Therefore, the stronger base is ClO⁻.
03

Analyze the basic strength of (b) BrO⁻ or BrO₂⁻

Next, let's compare the basic strength of BrO⁻ and BrO₂⁻. Both of these species have the same central atom, bromine. However, they differ in the number of oxygen atoms present. The BrO₂⁻ ion has one more oxygen atom than BrO⁻, which spreads the negative charge over more atoms. This makes BrO₂⁻ less reactive and hence a weaker base compared to BrO⁻. So, the stronger base is BrO⁻.
04

Analyze the basic strength of (c) HPO₄²⁻ or H₂PO₄⁻

Finally, let's compare the basic strength of HPO₄²⁻ and H₂PO₄⁻. Both of these species have the same central atom, phosphorus, and the same composition in terms of P, H, and O atoms. However, they differ in the degree of protonation (number of hydrogen ions attached). H₂PO₄⁻ has one more H+ ion than HPO₄²⁻, which means HPO₄²⁻ has a greater negative charge associated with it. This greater charge on HPO₄²⁻ makes it more eager to accept a proton, thus making it a stronger base. Therefore, the stronger base is HPO₄²⁻.

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Most popular questions from this chapter

The active ingredient in aspirin is acetylsalicylic acid \(\left(\mathrm{HC}_{9} \mathrm{H}_{7} \mathrm{O}_{4}\right),\) a monoprotic acid with \(K_{a}=3.3 \times 10^{-4}\) at \(25^{\circ} \mathrm{C} .\) What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 500 \(\mathrm{mg}\) of acetylsalicylic acid each, in 250 \(\mathrm{mL}\) of water?

(a) Give the conjugate base of the following Bronsted-Lowry acids: (i) \(\mathrm{HIO}_{3},(\mathbf{i} \mathbf{i}) \mathrm{NH}_{4}^{+} .(\mathbf{b})\) Give the conjugate acid of the following Bronsted-Lowry bases: (i) \(\mathrm{O}^{2-},(\mathbf{i} \mathbf{i}) \mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)

Ammonia, \(\mathrm{NH}_{3},\) acts as an Arrhenius base, a Bronsted-Lowry base, and a Lewis base, in aqueous solution. Write out the reaction \(\mathrm{NH}_{3}\) undergoes with water and explain what properties of ammonia correspond to each of the three definitions of "base."

Is each of the following statements true or false? (a) All strong acids contain one or more H atoms. (b) A strong acid is a strong electrolyte. (c) A \(1.0-M\) solution of a strong acid will have \(\mathrm{pH}=1.0 .\)

Calculate the \(\mathrm{pH}\) of each of the following strong acid solutions: \((\mathbf{a}) 8.5 \times 10^{-3} \mathrm{M} \mathrm{HBr},(\mathbf{b}) 1.52 \mathrm{g}\) of \(\mathrm{HNO}_{3}\) in 575 \(\mathrm{mL}\) of solution, \((\mathbf{c}) 5.00 \mathrm{mL}\) of 0.250 \(\mathrm{M} \mathrm{ClO}_{4}\) 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 \(\mathrm{M} \mathrm{HCl} .\)
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