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Chapter 17: Problem 17

State which of the following ions or compounds has the strongest conjugate base and briefly explain your choice. (a) \(\mathrm{HSO}_{4}^{-}\) (b) \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\) (c) HClO

Short Answer

Expert verified
The strongest conjugate base is \( \mathrm{ClO}^- \), from \( \mathrm{HClO} \).

Step by step solution

01

Understand the Concept of Conjugate Bases

A conjugate base is what remains after an acid donates a proton (H鈦�). The strength of a conjugate base is inversely related to the strength of its acid. The weaker the acid, the stronger its conjugate base will be.
02

Identify the Parent Acids

Determine the parent acids for each given ion or compound.- \( \mathrm{HSO}_4^{-} \) is the conjugate base of \( \mathrm{H}_2\mathrm{SO}_4 \) (sulfuric acid).- \( \mathrm{CH}_3 \mathrm{CO}_2 \mathrm{H} \) is acetic acid, so its conjugate base would be \( \mathrm{CH}_3 \mathrm{CO}_2^- \).- \( \mathrm{HClO} \) is hypochlorous acid, so its conjugate base is \( \mathrm{ClO}^- \).
03

Assess the Acid Strengths

Identify the relative strengths of the parent acids:- \( \mathrm{H}_2\mathrm{SO}_4 \) is a strong acid, meaning it dissociates completely in solution.- \( \mathrm{CH}_3 \mathrm{CO}_2 \mathrm{H} \) is a weak acid.- \( \mathrm{HClO} \) is also a weak acid, but weaker than \( \mathrm{CH}_3 \mathrm{CO}_2 \mathrm{H} \).
04

Determine the Strongest Conjugate Base

Since \( \mathrm{HClO} \) is the weakest acid among the options, its conjugate base \( \mathrm{ClO}^- \) will be the strongest of the conjugate bases provided.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acid Strength
Understanding acid strength is crucial when exploring conjugate bases. Acid strength refers to an acid's ability to donate a proton ( H鈦� ). Strong acids dissociate completely in water, releasing all their protons. For example, sulfuric acid ( H_2SO_4 ) is a strong acid. It fully dissociates in solution, meaning it is highly effective at donating protons.

In contrast, weak acids do not fully dissociate. They release fewer protons, demonstrating a lower tendency to give up their hydrogen ions. Understanding the strength of an acid helps to predict the strength of its conjugate base. Strong acids produce weak conjugate bases, and weak acids produce stronger conjugate bases. This inverse relationship is key in predicting and comparing conjugate base strengths.
Weak Acids
Weak acids only partially dissociate in water, which means they release some, but not all, of their hydrogen ions. Because they don't fully give up their protons, their conjugate bases are stronger than those of strong acids.

Examples of weak acids include acetic acid ( CH_3CO_2H ) and hypochlorous acid ( HClO ). Between these two, hypochlorous acid is even weaker than acetic acid. This lower dissociation ability results in a stronger conjugate base. The weak nature of HClO , for instance, makes its conjugate base, ClO^- , relatively strong, which is an important feature in acid-base chemistry.
Conjugate Acid-Base Pairs
In any acid-base reaction, there are always conjugate acid-base pairs involved. A conjugate base is the species that remains after an acid has donated a proton. Conversely, a conjugate acid is formed when a base accepts a proton.

Take sulfuric acid ( H_2SO_4 ), for example. After losing a proton, it transforms into its conjugate base, HSO_4^- . Since H_2SO_4 is a strong acid, HSO_4^- is a weak conjugate base. In general, when comparing conjugate bases, the weaker the parent acid, the stronger the conjugate base. This principle helps identify that ClO^- , derived from the weakest acid amongst the choices, HClO , is the strongest conjugate base in this scenario.

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Most popular questions from this chapter

In each of the following acid-base reactions, identify the Bronsted acid and base on the left and their conjugate partners on the right. $$\begin{aligned}&\text { (a) } \mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}(\mathrm{aq})+\mathrm{CH}_{3} &\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{NH}^{+}(\mathrm{aq})+\mathrm{CH}_{3} \mathrm{CO}_{2}^{-}(\mathrm{aq})\end{aligned}$$ (b) \(\mathrm{N}_{2} \mathrm{H}_{4}(\mathrm{aq})+\mathrm{HSO}_{4}^{-}(\mathrm{aq}) \rightleftarrows \mathrm{N}_{2} \mathrm{H}_{5}^{+}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})\). (c) \(\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \rightleftarrows\) \(\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{OH}\right]^{2+}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)\).

Perchloric acid behaves as an acid, even when it is dissolved in sulfuric acid. (a) Write a balanced equation showing how perchloric acid can transfer a proton to sulfuric acid. (b) Draw a Lewis electron dot structure for sulfuric acid. How can sulfuric acid function as a base?

Arrange the following \(0.10 \mathrm{M}\) solutions in order of increasing pH. (a) \(\mathrm{NaCl}\) (b) \(\mathrm{NH}_{4} \mathrm{Cl}\) (c) \(\mathrm{HCl}\) $$\begin{aligned} &\text { (d) } \mathrm{NaCH}_{3} \mathrm{CO}_{2}\\\ &\text { (e) } \mathrm{KOH} \end{aligned}$$

Decide whether each of the following substances should be classified as a Lewis acid or a Lewis base. (a) \(\mathrm{BCl}_{3}\) (Hint: Draw the electron dot structure.) (b) \(\mathrm{H}_{2} \mathrm{NNH}_{2},\) hydrazine (Hint: Draw the electron dot structure. (c) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) (Hint: Draw the electron dot structure.)

The base ethylamine \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)\) has a \(K_{\mathrm{b}}\) of \(4.3 \times 10^{-4}\) A closely related base, ethanolamine (HOCH,CH \(_{2} \mathrm{NH}_{2}\) ), has a \(K_{\mathrm{b}}\) of \(3.2 \times 10^{-5}\) (a) Which of the two bases is stronger? (b) Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M}\) solution of the stronger base.
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