Ch.16 - Acid-Base Equilibria

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.16 - Acid-Base Equilibria

Problem 84a

Chapter 16, Problem 84a

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (a) AlCl3

Verified step by step guidance

Step 1: Identify the type of compound. AlCl3 is a salt, which is formed from the reaction of an acid and a base. In this case, AlCl3 is formed from the reaction of Al(OH)3, a weak base, and HCl, a strong acid.

Step 2: Determine the potential hydrolysis reactions. Since AlCl3 is a salt, it can undergo hydrolysis, a reaction with water. The potential hydrolysis reactions are Al3+ + H2O -> Al(OH)2+ + H+ and Cl- + H2O -> HCl + OH-.

Step 3: Evaluate the likelihood of the hydrolysis reactions. The Al3+ ion can react with water to produce H+, making the solution acidic. The Cl- ion, however, is the conjugate base of a strong acid (HCl), so it will not react with water to produce OH-.

Step 4: Combine the results of the hydrolysis reactions. Since the Al3+ ion can react with water to produce H+ and the Cl- ion will not react with water to produce OH-, the solution will be acidic.

Step 5: Make the final prediction. Therefore, an aqueous solution of AlCl3 will be acidic.

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Key Concepts

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

Acid-Base Theory

Acid-base theory explains how substances can donate or accept protons (H+ ions). According to the Brønsted-Lowry theory, acids are proton donors, while bases are proton acceptors. Understanding this concept is crucial for predicting the behavior of substances in solution, particularly how they affect the pH of the solution.

Hydrolysis of Salts

When salts dissolve in water, they can undergo hydrolysis, where the ions react with water to produce acidic or basic solutions. For example, cations from weak bases or anions from strong acids can lead to acidic solutions. In the case of AlCl3, the aluminum ion can hydrolyze to form H+ ions, contributing to acidity.

pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 (very acidic) to 14 (very basic), with 7 being neutral. A solution with a pH less than 7 is considered acidic, while a pH greater than 7 is basic. Understanding the pH scale is essential for predicting the nature of solutions formed by different substances, including salts like AlCl3.

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Related Practice

Textbook Question

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (e) Na2SO3.

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Textbook Question

Pyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (c) A solution of pyridinium bromide has a pH of 2.95. What is the concentration of the pyridinium cation at equilibrium, in units of molarity?

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Textbook Question

An unknown salt is either NaF, NaCl, or NaOCl. When 0.050 mol of the salt is dissolved in water to form 0.500 L of solution, the pH of the solution is 8.08. What is the identity of the salt?

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Textbook Question

Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (b) NaBr

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Textbook Question

Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral: (c) Na₂CO₃

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Textbook Question

Pyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (b) Using Appendix D, calculate the Ka for pyridinium bromide.

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