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Chapter 47: Problem 11

Explain why the conjugate bases of the strong acids do not produce basic solutions when dissolved in water.

Short Answer

Expert verified
The conjugate bases of strong acids do not produce basic solutions when dissolved in water because they do not have a high tendency to accept protons from water. They will not react with water to form hydroxide ions (OH-), a process necessary to make the solution basic.

Step by step solution

01

Understand Conjugate Base

First, we need to understand what a conjugate base is. In acid-base chemistry, a conjugate base refers to what is left over after an acid has donated a proton during a chemical reaction.
02

Recognize Strong Acids

Second, it is important to recognize common strong acids. They include Hydrochloric acid (HCl), Sulfuric acid (H2SO4), Nitric acid (HNO3), Perchloric acid (HClO4), Hydriodic acid (HI), and Hydrobromic acid (HBr). When these acids dissolve in water, they completely ionize, producing their conjugate bases and H+ ions.
03

Explain the Behavior of Conjugate Bases

Lastly, we explain the behavior of this conjugate base in water. Because the strong acids completely ionize, their conjugate bases do not have a tendency to accept protons (H+ ions). This means they will not remove H+ ions from water to form hydroxide ions (OH-), they remain in their form and do not make the solution basic.

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Most popular questions from this chapter

Provide an expression relating \(K_{\mathrm{w}}\) to \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) of a conjugate acid-base pair.

Describe how to determine the value of \(K_{\mathrm{b}}\) for a base-given the value of \(K_{\mathrm{a}}\) for its conjugate acid.

For each of the following, describe the common features: a) all \(K_{\mathrm{a}}\) expressions b) all \(K_{\mathrm{b}}\) expressions c) all \(K_{\mathrm{a}} \times K_{\mathrm{b}}\) products

Indicate which of the following are potential acids, potential bases, or both (potential acid and potential base). a) \(\mathrm{Al}^{3+}\) b) \(\mathrm{CH}_{3} \mathrm{NH}_{3}{ }^{+}\) c) \(\mathrm{HPO}_{4}^{2-}\) d) \(\quad \mathrm{F}^{-}\) e) \(\mathrm{NH}_{4}^{+}\) f) \(\mathrm{H}_{2} \mathrm{O}\)

The chloride ion is the conjugate base of hydrochloric acid. Explain why \(\mathrm{Cl}^{-}\) does not produce a basic solution when dissolved in water.
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