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Chapter 45: Problem 9

The nitrate ion is the conjugate base of nitric acid, \(\mathrm{HNO}_{3}\). Explain why \(\mathrm{NO}_{3}^{-}\) does not produce a basic solution when dissolved in water.

Short Answer

Expert verified
The nitrate ion \(\mathrm{NO}_{3}^{-}\) does not produce a basic solution when dissolved in water because it is the conjugate base of a strong acid, nitric acid \(\mathrm{HNO}_{3}\). Conjugate bases of strong acids do not act as bases, hence they do not react with water to produce a hydroxide ion.

Step by step solution

01

Understanding the Nitrate Ion

In acid-base chemistry, the nitrate ion \(\mathrm{NO}_{3}^{-}\) is the conjugate base of the nitric acid \(\mathrm{HNO}_{3}\). Conjugate bases are formed by the loss of a proton (\(\mathrm{H}^{+}\)) from the acid.
02

Interpreting Acid-Base reactions

A commonly understood principle of acid-base chemistry states that the conjugate base of a strong acid doesn't act as a base. When nitrate ion is formed from nitric acid (which is a strong acid), even though it's technically a base, it doesn’t behave as a typical base - reacting with water to produce a hydroxide ion (\(\mathrm{OH}^{-}\)).
03

Understanding Non-Basic Behavior

The non-basic behavior of the nitrate ion can be explained by examining its reaction with water. When nitrate ion \(\mathrm{NO}_{3}^{-}\) is added to water, it doesn't react to form a hydroxide ion (\(\mathrm{OH}^{-}\)). Instead, it remains quite stable and does not accept a proton from water (it doesn’t act as a base). Therefore, the pH of the solution remains neutral and does not become basic.

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Most popular questions from this chapter

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 \(K_{\mathrm{b}}\) ? c) Provide a qualitative description of the relationship between the relative strength of an acid and the relative strength of its conjugate base. d) Assume that \(K_{\mathrm{a}}\) of \(\mathrm{HA}\) is \(1.0 \times 10^{-5}\) and \(K_{\mathrm{a}}\) of \(\mathrm{HX}\) is \(3.5 \times 10^{-7}\). Calculate the \(K_{\mathrm{b}}\) for \(\mathrm{A}^{-}\) and for \(\mathrm{X}^{-}\) and confirm that your answers to parts \(\mathrm{b}\) and \(\mathrm{c}\) are correct.

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

\(\mathrm{HNO}_{3}\) is considered to be the weakest of the strong acids. Explain why the conjugate bases of all strong acids do not produce basic solutions when dissolved in water.

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

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) \(\mathrm{H}_{2} \mathrm{O}\)
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