Ch.4 - Reactions in Aqueous Solution

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.4 - Reactions in Aqueous Solution

Problem 33b

Chapter 4, Problem 33b

State whether each of the following statements is true or false. Justify your answer in each case. (b) HCl is a weak acid.

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Identify the nature of HCl in terms of acid strength. Hydrochloric acid (HCl) is commonly known and used in chemistry.

Recall the definition of a strong acid. A strong acid is one that completely dissociates into its ions in solution.

Consider the dissociation of HCl in water. When HCl is dissolved in water, it dissociates completely into hydrogen ions (H+) and chloride ions (Cl-).

Compare the behavior of HCl with the characteristics of strong acids. Since HCl completely dissociates in solution, it exhibits the key characteristic of a strong acid.

Conclude the classification of HCl based on its dissociation. Given that HCl fully dissociates in water, it should be classified as a strong acid, not a weak acid.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid Strength

Acid strength refers to the ability of an acid to donate protons (H+) in a solution. Strong acids, like hydrochloric acid (HCl), completely dissociate in water, releasing all their protons, while weak acids only partially dissociate. Understanding this distinction is crucial for evaluating the nature of acids.

Dissociation in Water

Dissociation in water is the process by which an acid separates into its constituent ions when dissolved. For strong acids, this process is complete, leading to a high concentration of H+ ions. In contrast, weak acids result in a dynamic equilibrium between the undissociated acid and its ions, which is essential for determining their strength.

pH Scale

The pH scale measures the acidity or basicity of a solution, with lower values indicating higher acidity. Strong acids typically have low pH values due to their complete dissociation, while weak acids have higher pH values because they do not fully dissociate. This concept helps in understanding the behavior of acids in various chemical contexts.

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Related Practice

Textbook Question

You know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO3, CaCl2, or Al21SO423. A friend suggests that you test a portion of the solution with Ba1NO322 and then with NaCl solutions. According to your friend's logic, which of these chemical reactions could occur, thus helping you identify the solution in the bottle? (a) Barium sulfate could precipitate. (b) Silver chloride could precipitate. (c) Silver sulfate could precipitate. (d) More than one, but not all, of the reactions described in answers a–c could occur. (e) All three reactions described in answers a–c could occur.

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State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid.

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Three solutions are mixed together to form a single solution; in the final solution, there are 0.2 mol Pb1CH3COO)2, 0.1 mol Na2S, and 0.1 mol CaCl2 present. What solid(s) will precipitate?

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Textbook Question

State whether each of the following statements is true or false. Justify your answer in each case. (a) NH3 contains no OH- ions, and yet its aqueous solutions are basic

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State whether each of the following statements is true or false. Justify your answer in each case. (b) HF is a strong acid.

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