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Chapter 14: Problem 43

Classify each of the following as a strong acid or a weak acid.

Short Answer

Expert verified
In the example list of acids, HCl and H2SO4 are strong acids because they completely ionize in water, while H3PO4 and CH3COOH are weak acids as they only partially ionize in water.

Step by step solution

01

Classify HCl

Hydrochloric acid, HCl, is a strong acid because it completely ionizes (dissociates) in water, producing H+ and Cl- ions.
02

Classify H3PO4

Phosphoric acid, H3PO4, is a weak acid because it only partially ionizes in water. It produces H+ ions and phosphate ions (H2PO4-, HPO4^2-, PO4^3-) in different extents.
03

Classify H2SO4

Sulfuric acid, H2SO4, is a strong acid because it has high dissociation in water, producing H+ ions and sulfate ions (SO4^2-).
04

Classify CH3COOH

Acetic acid, CH3COOH, is a weak acid because it only partially ionizes in water, producing H+ ions and acetate ions (CH3COO-). Conclusion: In our example list of acids, HCl and H2SO4 are strong acids, while H3PO4 and CH3COOH are weak acids.

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Key Concepts

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

Strong Acids
Strong acids are acids that completely dissociate in water. This means that when placed in water, they fully split into their constituent ions. For example, hydrochloric acid (HCl) breaks down entirely into hydrogen ions (H\(^+\)) and chloride ions (Cl\(^-\)). This complete dissociation allows strong acids to conduct electricity well in aqueous solutions, a property that is useful in various industrial applications.

When you encounter an acid, and it is labeled as strong, you can expect it to:
  • Release a large amount of H\(^+\) ions in water
  • Have a low pH, typically below 3
  • React quickly and completely with bases
Understanding the behavior of strong acids is crucial in predicting their reactivity and the outcomes of acid-base reactions.
Weak Acids
Unlike strong acids, weak acids only partially dissociate in water. This partial dissociation means that weak acids remain largely undissociated, and only a small fraction of the acid molecules release hydrogen ions (H\(^+\)). An example of a weak acid is acetic acid (CH\(_3\)COOH), which partially dissociates into H\(^+\) and acetate ions (CH\(_3\)COO\(^-\)) in an aqueous solution.

Characteristics of weak acids include:
  • Higher pH values, usually ranging from 3 to 7
  • Less electrical conductivity compared to strong acids
  • Equilibrium between undissociated acid and ions
These properties of weak acids result in slower reactions when neutralizing bases, making them ideal in applications where gradual pH changes are required.
Dissociation in Water
Dissociation in water refers to the process where acid molecules split into ions when dissolved. In strong acids, this dissociation is complete, while in weak acids, it is only partial. Understanding this process is key to predicting how an acid will behave in a solution.

When acids dissociate in water:
  • Hydrogen ions (H\(^+\)) are released, influencing the solution's acidity
  • Acids interact with water, breaking into their respective anions
  • Equilibrium exists in weak acids between dissociated ions and undissociated molecules
The degree of dissociation impacts the acid strength, affecting properties such as pH and reactivity in chemical processes.
Ionization
Ionization is the process by which molecules convert into ions. It is a fundamental concept for understanding how acids behave in aqueous solutions. For both strong and weak acids, ionization is the reason they release hydrogen ions (H\(^+\)) into their environments.

Key points about ionization include:
  • Strong acids ionize completely, leading to high H\(^+\) concentration
  • Weak acids partially ionize, maintaining an equilibrium
  • Ionization influences properties such as electrical conductivity and reaction speed
Grasping the concept of ionization helps in understanding how acids interact with various substances, predicting the behavior of solutions during chemical reactions.

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Most popular questions from this chapter

A \(1.0 \times 10^{-2}-M\) solution of cyanic acid (HOCN) is 17\(\%\) dissociated. Calculate \(K_{\mathrm{a}}\) for cyanic acid.

Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced equations for the reactions causing the solution to be acidic or basic. The relevant \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values are found in Tables 14.2 and \(14.3 .\) \(\begin{array}{ll}{\text { a. } \operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}} & {\text { d. } \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{ClO}_{2}} \\ {\text { b. } \mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}} & {\text { e. } \mathrm{NH}_{4} \mathrm{F}} \\ {\text { c. } \mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{O} \mathrm{l}} & {\text { f. } \mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{CN}}\end{array}\)

Calculate the mass of sodium hydroxide that must be added to 1.00 \(\mathrm{L}\) of \(1.00-M \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) to double the pH of the solution (assume that the added NaOH does not change the volume of the solution).

One mole of a weak acid HA was dissolved in 2.0 \(\mathrm{L}\) of solution. After the system had come to equilibrium, the concentration of HA was found to be 0.45 \(\mathrm{M} .\) Calculate \(K_{\mathrm{a}}\) for \(\mathrm{HA}\) .

The pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium reactions: $$ \mathrm{CO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}^{+}(a q) $$ Acids formed during normal cellular respiration react with the \(\mathrm{HCO}_{3}^{-}\) to form carbonic acid, which is in equilibrium with \(\mathrm{CO}_{2}(a q)\) and \(\mathrm{H}_{2} \mathrm{O}(l) .\) During vigorous exercise, a person's \(\mathrm{H}_{2} \mathrm{CO}_{3}\) blood levels were \(26.3 \mathrm{mM},\) whereas his \(\mathrm{CO}_{2}\) levels were 1.63 \(\mathrm{mM}\) . On resting, the \(\mathrm{H}_{2} \mathrm{CO}_{3}\) levels declined to 24.9 \(\mathrm{m} M\) . What was the \(\mathrm{CO}_{2}\) blood level at rest?
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