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Chapter 15: Problem 30

\(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid, but \(\mathrm{HSO}_{4}^{-}\) is a weak acid. Account for the difference in strength of these two related species.

Short Answer

Expert verified
\(\mathrm{H}_{2}\mathrm{SO}_{4}\) is a strong acid because it fully ionizes, spontaneously donating its two \(H^+\) in the solution. The \(\mathrm{HSO}_{4}^{-}\), produced after the first ionization, is less likely to donate its remaining proton due to a higher energy of ionization, hence it's a weak acid.

Step by step solution

01

Understanding Acid Strength

Acid strength can be characterized by the degree of ionization, specifically how completely an acid donates its protons (\(H^+\)). An acid is strong if it fully ionizes (donates its protons) in a solution, while a weak acid does not completely ionize.
02

Analyzing \(\mathrm{H}_{2}\mathrm{SO}_{4}\)

\(\mathrm{H}_{2}\mathrm{SO}_{4}\) or Sulfuric Acid is a strong acid. This is largely due to its ability to donate two protons (\(H^+\)) to the solution. In the first ionization, \(\mathrm{H}_{2}\mathrm{SO}_{4}\) loses one \(H^+\) to form \(\mathrm{HSO}_{4}^{-}\) and releases a fair amount of energy which makes the process spontaneous and therefore, it fully ionizes.
03

Analyzing \(\mathrm{HSO}_{4}^{-}\)

\(\mathrm{HSO}_{4}^{-}\), on the other hand, is a weak acid. After the first ionization of \(\mathrm{H}_{2}\mathrm{SO}_{4}\), the production of the remaining \(\mathrm{HSO}_{4}^{-}\) species is less likely to donate its remaining proton because it has a relatively higher energy of ionization. This higher energy of ionization implies less spontaneous ionization in solution, earning it the classification of a weak acid.

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Most popular questions from this chapter

Henry's law constant for \(\mathrm{CO}_{2}\) at \(38^{\circ} \mathrm{C}\) is \(2.28 \times 10^{-3}\) \(\mathrm{mol} / \mathrm{L} \cdot \mathrm{atm} .\) Calculate the \(\mathrm{pH}\) of a solution of \(\mathrm{CO}_{2}\) at \(38^{\circ} \mathrm{C}\) in equilibrium with the gas at a partial pressure of 3.20 atm.

In terms of orbitals and electron arrangements, what must be present for a molecule or an ion to act as a Lewis acid (use \(\mathrm{H}^{+}\) and \(\mathrm{BF}_{3}\) as examples)? What must be present for a molecule or ion to act as a Lewis base (use \(\mathrm{OH}^{-}\) and \(\mathrm{NH}_{3}\) as examples)?

Which would be considered a stronger Lewis acid: (a) \(\mathrm{BF}_{3}\) or \(\mathrm{BCl}_{3}\), (b) \(\mathrm{Fe}^{2+}\) or \(\mathrm{Fe}^{3+}\) ? Explain.

\(\mathrm{Al}(\mathrm{OH})_{3}\) is an insoluble compound. It dissolves in excess \(\mathrm{NaOH}\) in solution. Write a balanced ionic equation for this reaction. What type of reaction is this?

Write the equation relating \(K_{\mathrm{a}}\) for a weak acid and \(K_{\mathrm{b}}\) for its conjugate base. Use \(\mathrm{NH}_{3}\) and its conjugate acid \(\mathrm{NH}_{4}^{+}\) to derive the relationship between \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\).
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