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Chapter 15: Problem 85

True or false? Because carbonic acid, \(\mathrm{H}_{2} \mathrm{CO}_{3}\), is diprotic, it is a stronger acid than \(\mathrm{HCl}\), which is only monoprotic. Explain your answer.

Short Answer

Expert verified
The statement is false. Although carbonic acid (\(\mathrm{H}_{2}\mathrm{CO}_{3}\)) is diprotic, it is a weaker acid than hydrochloric acid (\(\mathrm{HCl}\)), which is monoprotic. The strength of an acid depends on its acidity constant (K_a) rather than the number of protons it can donate. In this case, the K_a of the first dissociation step of carbonic acid is smaller than that of hydrochloric acid, making carbonic acid a weaker acid.

Step by step solution

01

Understand diprotic and monoprotic acids

A diprotic acid is an acid that has two hydrogen ions (protons) available for donation, while a monoprotic acid has only one hydrogen ion available for donation. In this case, carbonic acid, \(\mathrm{H}_{2}\mathrm{CO}_{3}\), is diprotic because it has two hydrogen atoms in its chemical formula, while hydrochloric acid, \(\mathrm{HCl}\), is monoprotic because it only has one hydrogen atom in its formula.
02

Compare the acidity constants

To determine the strength of an acid, we need to look at the acidity constants. A larger acidity constant (K_a) indicates a stronger acid. The K_a values for the first dissociation step of carbonic acid (\(\mathrm{H}_{2}\mathrm{CO}_{3}\)) and hydrochloric acid (\(\mathrm{HCl}\)) are: \[\mathrm{H}_{2}\mathrm{CO}_{3}\:K_{a1} = 4.3 \times 10^{-7}\] \[\mathrm{HCl}\: K_{a} = 1.3 \times 10^{6}\]
03

Compare the acid strengths

Since the acidity constant for the first dissociation step of carbonic acid (\(\mathrm{H}_{2}\mathrm{CO}_{3}\), K_a1) is smaller than the acidity constant of hydrochloric acid (\(\mathrm{HCl}\), K_a), it indicates that carbonic acid is a weaker acid than hydrochloric acid. The fact that carbonic acid is diprotic does not necessarily make it stronger than monoprotic hydrochloric acid.
04

Conclusion

The statement is false. Although carbonic acid (\(\mathrm{H}_{2}\mathrm{CO}_{3}\)) is diprotic, it is a weaker acid than hydrochloric acid (\(\mathrm{HCl}\)), which is monoprotic. The strength of an acid depends on its acidity constant (K_a) rather than the number of protons it can donate.

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Most popular questions from this chapter

A solution is formed by mixing \(50.0 \mathrm{~mL}\) of \(0.015 \mathrm{M} \mathrm{NaOH}(a q)\) with \(50.0 \mathrm{~mL}\) of \(0.010 \mathrm{M}\) \(\mathrm{HNO}_{3}(a q)\) (a) Is the solution acidic or basic? (b) Draw a beaker and show all species present in the solution. (c) What is the pH of the solution?

Aniline, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\), is a weak base, with a lone pair of electrons on the nitrogen atom. (a) According to Bronsted and Lowry, what must aniline do to act as a base? (b) Why can aniline act as a base? (c) What are the molecular formula and charge of the conjugate acid of aniline?

A solution has an \(\mathrm{OH}\) concentration of \(10^{-11} \mathrm{M}\). (a) Is this solution basic or acidic? Explain how you know. (b) Without using a calculator, explain how you could quickly determine the \(\mathrm{H}_{3} \mathrm{O}\) concentration of this solution. What is that concentration?

A solution is prepared by dissolving \(2.50\) moles of \(\mathrm{LiOH}\) in enough water to get \(4.00 \mathrm{~L}\) of solution. What are the \(\mathrm{OH}^{-}\) and the \(\mathrm{H}_{3} \mathrm{O}^{+}\) molar concentrations?

Does pure liquid water have any buffering ability? Explain.
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