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Chapter 16: Problem 86

The \(\mathrm{pH}\) of a \(0.0642 \mathrm{M}\) solution of a monoprotic acid is \(3.86 .\) Is this a strong acid?

Short Answer

Expert verified
No, this is not a strong acid.

Step by step solution

01

Calculate the concentration of \(H^{+}\)

Determine the concentration of \(H^{+}\) in the solution using the expression \( [H^{+}]=10^{-\mathrm{pH}}\). Here, \(\mathrm{pH}=3.86\). So, \( [H^{+}]=10^{-3.86}\). The calculation yields \( [H^{+}]\) equals approximately \(1.37 \times 10^{-4} \mathrm{M}\).
02

Compare \(HA\) and \(H^{+}\)

Compare the concentration of the original acid (\(HA=0.0642 \mathrm{M}\)) with that of the H+ ions (\(H^{+}=1.37 \times 10^{-4} \mathrm{M}\)). It is evident that \(HA >> H^{+}\). This means that only a small fraction of the original acid has ionized into \(H^{+}\) ions.
03

Determine acid strength

Based on the comparison in Step 2, it can be concluded that this is not a strong acid. Strong acids ionize completely and would have a \(H^{+}\) concentration that is equal to the starting concentration of the acid.

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Most popular questions from this chapter

About half of the hydrochloric acid produced annually in the United States \((3.0\) billion pounds \()\) is used for metal pickling. This process involves the removal of metal oxide layers from metal surfaces to prepare them for coating. (a) Write the overall and net ionic equations for the reaction between iron(III) oxide, which represents the rust layer over iron, and HCl. Identify the Bronsted acid and base. (b) Hydrochloric acid is also used to remove scale (which is mostly \(\mathrm{CaCO}_{3}\) ) from water pipes. Hydrochloric acid reacts with calcium carbonate in two stages; the first stage forms the bicarbonate ion, which then reacts further to form carbon dioxide. Write equations for these two stages and for the overall reaction. (c) Hydrochloric acid is used to recover oil from the ground. It dissolves rocks (often \(\mathrm{CaCO}_{3}\) ) so that the oil can flow more easily. In one process, a 15 percent (by mass) HCl solution is injected into an oil well to dissolve the rocks. If the density of the acid solution is \(1.073 \mathrm{~g} / \mathrm{mL}\), what is the \(\mathrm{pH}\) of the solution?

Which of these statements is/are true regarding a 1.0 \(M\) solution of a strong acid HA? (a) \(\left[\mathrm{A}^{-}\right]>\left[\mathrm{H}^{+}\right]\) (b) The \(\mathrm{pH}\) is 0.00 . (c) \(\left[\mathrm{H}^{+}\right]=1.0 \mathrm{M}\) (d) \([\mathrm{HA}]=1.0 \mathrm{M}\).

Hemoglobin (Hb) is a blood protein that is responsible for transporting oxygen. It can exist in the protonated form of \(\mathrm{HbH}^{+}\). The binding of oxygen can be represented by the simplified equation $$\mathrm{HbH}^{+}+\mathrm{O}_{2} \rightleftharpoons \mathrm{HbO}_{2}+\mathrm{H}^{+}$$ (a) What form of hemoglobin is favored in the lungs where oxygen concentration is highest? (b) In body tissues, where carbon dioxide is released as a result of metabolism, the medium is more acidic because of the formation of carbonic acid. What form of hemoglobin is favored under this condition? (c) When a person hyperventilates, the concentration of \(\mathrm{CO}_{2}\) in his or her blood decreases. How does this action affect the above equilibrium? Frequently a person who is hyperventilating is advised to breathe into a paper bag. Why does this action help the individual?

For a species to act as a Bronsted base, an atom in the species must possess a lone pair of electrons. Explain why this is so.

Describe this reaction according to the Lewis theory of acids and bases: $$\mathrm{AlCl}_{3}(s)+\mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{AlCl}_{4}^{-}(a q)$$
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