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Chapter 47: Problem 10

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

Short Answer

Expert verified
Cl- does not produce a basic solution when dissolved in water because it is the conjugate base of a strong acid (HCl), which makes it a weak base. As such, it does not significantly accept H+ ions when in water, and thus does not significantly increase the solution's pH.

Step by step solution

01

Understand Conjugate Acid-Base Pairs

This involves both the Bronsted-Lowry theory of acids and bases and the principles of chemical equilibrium. An acid is a substance that donates hydrogen ions, H+, and its conjugate base is the substance that remains after the acid has lost the H+ ion. Similarly, a base is a substance that accepts H+ ions, and its conjugate acid is the substance that results once the base has gained an H+ ion. Hydrochloric acid (HCl) is a strong acid. When it donates its H+ ion, it becomes its conjugate base, Cl-.
02

Analyze the Behaviour of Cl- in Water

In order to determine if Cl- would act as a base in water, we have to consider whether it would accept an H+ ion. If it did, it would form HCl, according to the following reaction: Cl- + H2O 鈫� HCl + OH-. This reaction would proceed to the right only if Cl- were a strong base. But Cl- is the conjugate base of a strong acid, HCl. As such, it is a weak base, and this reaction would not proceed to any significant extent. Instead, the vast majority of the Cl- ions would remain as Cl- ions.
03

Understand the pH Impact

The lack of significant reaction between Cl- and H2O to form OH- means that adding Cl- to water does not significantly increase the concentration of OH- ions in the solution. Therefore, it does not increase the pH, meaning it does not create a basic solution when dissolved in water.

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Most popular questions from this chapter

Which of the following ions are potential bases: \(\mathrm{Fe}^{3+} ; \mathrm{NH}_{4}^{+} ; \mathrm{F}^{-} ?\)

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

Consider two acids, HA and HX, with HA being a stronger acid than HX. a) Which acid has a larger value of \(K_{\mathrm{a}}\) ? b) Which conjugate base, \(\mathrm{A}^{-}\) or \(\mathrm{X}^{-}\), has a larger value of \(\mathrm{K}_{\mathrm{b}}\) ? c) Provide a qualitative description of the relationship between the relative strength of an acid and the relative strength of its conjugate base.

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

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