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Chapter 16: Problem 25

Explain what is meant by the strength of an acid.

Short Answer

Expert verified
The strength of an acid is determined by its degree of ionization in water, which refers to how completely it dissociates to form hydrogen ions or hydronium ions. The more completely an acid ionizes, releasing more \(H^+\) ions, the stronger it is. It can also be measured using the pH scale, with lower values indicating stronger acids.

Step by step solution

01

Define an Acid

An acid can be defined as a compound that donates a hydrogen ion (\(H^+\)) to another compound called a base. In aqueous solutions, it forms hydronium ions (\(H_3O^+\)).
02

Discuss the Ionization of Acids

The process of ionization refers to the separation of an acid into ions when it comes into contact with water. Thus, it gives off hydrogen ions. The more completely an acid produces these ions, the stronger it is.
03

Define Acid Strength

The strength of an acid is based on the degree of ionization. A strong acid is one that almost completely ionizes in water, denoted by releasing more \(H^+\) ions, whereas a weak acid only partially ionizes.
04

Discuss the pH scale

The strength of an acid can also be measured using the pH scale. Acids have a pH value less than 7. The lower the pH value, the stronger the acid is.

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Most popular questions from this chapter

Classify each of these species as a Bronsted acid or base, or both: (a) \(\mathrm{H}_{2} \mathrm{O},\) (b) \(\mathrm{OH}^{-},\) (c) \(\mathrm{H}_{3} \mathrm{O}^{+}\), (d) \(\mathrm{NH}_{3}\) (e) \(\mathrm{NH}_{4}^{+},\) (f) \(\mathrm{NH}_{2}^{-},(\mathrm{g}) \mathrm{NO}_{3}^{-},\) (h) \(\mathrm{CO}_{3}^{2-}\) (i) HBr, (j) HCN.

Why do we normally not quote \(K_{\mathrm{a}}\) values for strong acids such as \(\mathrm{HCl}\) and \(\mathrm{HNO}_{3}\) ? Why is it necessary to specify temperature when giving \(K_{\mathrm{a}}\) values?

Classify each of these species as a weak or strong acid: (a) \(\mathrm{HNO}_{3}\) (b) HF, (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (d) \(\mathrm{HSO}_{4}^{-}\) (e) \(\mathrm{H}_{2} \mathrm{CO}_{3},\) (f) \(\mathrm{HCO}_{3}^{-},(\mathrm{g}) \mathrm{HCl}\) (h) HCN, (i) \(\mathrm{HNO}_{2}\)

Prove the statement that when the concentration of a weak acid HA decreases by a factor of 10 , its percent ionization increases by a factor of \(\sqrt{10}\). State any assumptions.

Novocaine, used as a local anesthetic by dentists, is a weak base \(\left(K_{\mathrm{b}}=8.91 \times 10^{-6}\right)\). What is the ratio of the concentration of the base to that of its acid in the blood plasma \((\mathrm{pH}=7.40)\) of a patient?
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