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Chapter 14: Problem 48

Based on formulas alone, which is the stronger acid? (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) or \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (b) \(\mathrm{HNO}_{3}\) or \(\mathrm{HNO}_{2}\) (c) \(\mathrm{HClO}_{4}\) or \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (d) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) or \(\mathrm{HClO}_{3}\) (e) \(\mathrm{H}_{2} \mathrm{SO}_{2}\) or \(\mathrm{H}_{2} \mathrm{SO}\)

Short Answer

Expert verified
(a) \( \mathrm{H}_{2} \mathrm{SO}_{4} \); (b) \( \mathrm{HNO}_{3} \); (c) \( \mathrm{HClO}_{4} \); (d) \( \mathrm{HClO}_{3} \); (e) \( \mathrm{H}_{2} \mathrm{SO}_{2} \).

Step by step solution

01

Understanding Acid Strength

The strength of an acid is determined by its ability to donate protons (H鈦� ions) in water, which is often linked to its chemical structure and the stability of the conjugate base. Generally, stronger acids dissociate more completely in water.
02

Comparison of \( \mathrm{H}_{2} \mathrm{CO}_{3} \) and \( \mathrm{H}_{2} \mathrm{SO}_{4} \)

Sulfuric acid ( \( \mathrm{H}_{2} \mathrm{SO}_{4} \)) is significantly stronger than carbonic acid ( \( \mathrm{H}_{2} \mathrm{CO}_{3} \)) because \( \mathrm{H}_{2} \mathrm{SO}_{4} \) fully dissociates into \( \mathrm{H}^{+} \) ions and \( \mathrm{HSO}_{4}^{-} \) while carbonic acid only partially dissociates, producing \( \mathrm{HCO}_{3}^{-} \).
03

Comparison of \( \mathrm{HNO}_{3} \) and \( \mathrm{HNO}_{2} \)

Nitric acid ( \( \mathrm{HNO}_{3} \)) is stronger than nitrous acid ( \( \mathrm{HNO}_{2} \)) due to its ability to fully dissociate into \( \mathrm{H}^{+} \) and \( \mathrm{NO}_{3}^{-} \) ions, compared to the partial dissociation of nitrous acid into \( \mathrm{NO}_{2}^{-} \).
04

Comparison of \( \mathrm{HClO}_{4} \) and \( \mathrm{H}_{2} \mathrm{SO}_{4} \)

Perchloric acid ( \( \mathrm{HClO}_{4} \)) is among the strongest acids and stronger than sulfuric acid ( \( \mathrm{H}_{2} \mathrm{SO}_{4} \)) as it fully dissociates in solution to give \( \mathrm{H}^{+} \) ions and \( \mathrm{ClO}_{4}^{-} \).
05

Comparison of \( \mathrm{H}_{3} \mathrm{PO}_{4} \) and \( \mathrm{HClO}_{3} \)

Chloric acid ( \( \mathrm{HClO}_{3} \)) is stronger than phosphoric acid ( \( \mathrm{H}_{3} \mathrm{PO}_{4} \)) due to chloric acid's greater ability to dissociate and provide \( \mathrm{H}^{+} \) ions.
06

Comparison of \( \mathrm{H}_{2} \mathrm{SO}_{2} \) and \( \mathrm{H}_{2} \mathrm{SO} \)

Sulfurous acid ( \( \mathrm{H}_{2} \mathrm{SO}_{2} \)) is the stronger acid compared to hypothetical \( \mathrm{H}_{2} \mathrm{SO} \), which is less likely to have the same stability or strength of dissociation as sulfurous acid.

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Key Concepts

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

Proton Donation
Proton donation is a key indicator of acid strength. When an acid donates a proton (H鈦� ion) in water, it undergoes a reaction that contributes to its acidity. The ease with which an acid gives up this proton determines whether it is classified as a strong or weak acid. Strong acids dissociate completely, releasing all their available protons in water, hence showing higher acidity. On the other hand, weak acids only partially dissociate, meaning they donate fewer protons. This difference in dissociation is crucial in comparing the strengths of acids like sulfuric acid and carbonic acid, where sulfuric acid exhibits almost complete dissociation.
Conjugate Base Stability
Once an acid donates a proton, the remaining part of the molecule becomes the conjugate base. The stability of this conjugate base heavily influences the acid's strength. More stable conjugate bases correspond to stronger acids. This stability can be affected by several factors, including the electronegativity of atoms involved and the distribution of charge across the molecule. For example, the conjugate base of nitric acid (NO鈧冣伝) is more stable than that of nitrous acid (NO鈧傗伝), which directly contributes to nitric acid's greater strength. A highly stable conjugate base is less reactive, thus making the original acid more willing to dissociate.
Acid Dissociation
Acid dissociation refers to the process where an acid breaks apart in water to yield protons and its conjugate base. The degree of dissociation is a primary determinant of acid strength. Strong acids like sulfuric acid and perchloric acid dissociate fully into their components, while weaker acids like phosphoric acid only partially dissociate. This concept is represented by the acid dissociation constant ( K_a ), which quantifies how readily an acid donates its protons. A larger K_a value indicates a stronger acid capable of more complete dissociation.
Sulfuric Acid
Sulfuric acid ( H鈧係O鈧� ) is a highly strong and widely used acid. It is a diprotic acid, meaning it has the ability to donate two protons. Its first dissociation in water is complete, making it highly conductive and acidic. Sulfuric acid's ability to completely dissociate into HSO鈧勨伝 and H鈦� ensures its place among the strongest acids, making it well-suited for numerous industrial applications. In comparison exercises, sulfuric acid often stands out due to its strong proton donation capabilities and the stability of its conjugate base, HSO鈧勨伝 .
Nitric Acid
Nitric acid ( HNO鈧� ) is another prominent example of strong acid. It dissociates fully into H鈦� and NO鈧冣伝 ions. This complete dissociation is indicative of its strength and efficiency as an acid. The conjugate base, NO鈧冣伝 , is highly stable because the negative charge is delocalized over the oxygen atoms, making it less reactive and confirming nitric acid's high level of acidity. This makes nitric acid stronger than its counterpart, nitrous acid ( HNO鈧� ), which does not dissociate completely. The total dissociation ability of nitric acid supports its usage in applications requiring a strong oxidizing agent.

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Most popular questions from this chapter

Write the formula for the conjugate base of \(\left[\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}(\mathrm{OH})\right]^{1+}\).

Write ionization equations and ionization constant expressions for these acids and bases. (a) \(\mathrm{CH}_{3} \mathrm{COOH}\) (b) \(\mathrm{HCN}\) (c) \(\mathrm{SO}_{3}^{2-}\) (d) \(\mathrm{PO}_{4}^{3-}\) (e) \(\mathrm{NH}_{4}^{+}\) (f) \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

Trimethylamine, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}:\), reacts readily with diborane, \(\mathrm{B}_{2} \mathrm{H}_{6}\). The diborane dissociates to two \(\mathrm{BH}_{3}\) fragments, each of which can react with trimethylamine to form a complex, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{~N}: \mathrm{B} \mathrm{H}_{3}\). Write an equation for this reaction and interpret it in terms of Lewis acid-base theory.

Identify the Lewis acid and the Lewis base in each reaction. (a) \(\mathrm{I}_{2}(\mathrm{~s})+\mathrm{I}^{-}(\mathrm{aq}) \longrightarrow \mathrm{I}_{3}^{-}(\mathrm{aq})\) (b) \(\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{BF}_{3}(\mathrm{~g}) \longrightarrow \mathrm{O}_{2} \mathrm{SBF}_{3}(\mathrm{~s})\) (c) \(\mathrm{Au}^{+}(\mathrm{aq})+2 \mathrm{CN}^{-}(\mathrm{aq}) \longrightarrow\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})\) (d) \(\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\ell) \longrightarrow \mathrm{H}_{2} \mathrm{CO}_{3}(\mathrm{aq})\)

Write a chemical equation to describe the proton transfer that occurs when each of these bases is added to water. (a) \(\mathrm{PO}_{4}^{3-}\) (b) \(\mathrm{SO}_{3}^{2-}\) (c) \(\mathrm{HPO}_{4}^{2-}\)
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