Textbook Question
Determine the pH of each solution. a. 0.10 M NH4Cl
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Ch.17 - Acids and Bases
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 17, Problem 104d
Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. d. Li+
Verified step by step guidance1
Identify the nature of the cation: Li^+ is a Group 1 metal cation.
Recall that cations from Group 1 metals, such as Li^+, are typically pH-neutral because they do not react with water to form H^+ ions.
Understand that acidic cations are usually those that can donate a proton (H^+) or increase the concentration of H^+ in solution.
Since Li^+ does not have the ability to donate a proton or increase H^+ concentration, it is considered pH-neutral.
Conclude that Li^+ is a pH-neutral cation and does not act as an acid in aqueous solution.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acidic Cations
Acidic cations are positively charged ions that can donate protons (H+) in solution, thereby lowering the pH. These cations typically come from weak bases or are transition metals that can hydrolyze in water, forming acidic solutions. Understanding whether a cation is acidic involves analyzing its ability to interact with water and affect the concentration of hydrogen ions.
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pH Neutral Cations
pH neutral cations do not significantly affect the pH of a solution. They are usually derived from strong bases and do not hydrolyze in water, meaning they do not release protons. An example of a pH-neutral cation is Li+, which does not react with water to produce H+ ions, thus maintaining a neutral pH.
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Hydrolysis Reactions
Hydrolysis reactions involve the reaction of a cation with water, leading to the formation of an acid or base. In the case of acidic cations, hydrolysis results in the release of H+ ions, which can be represented by an equation. For example, if a cation is acidic, the hydrolysis reaction can be written as: M^n+ + H2O ⇌ MH(n-1)+ + H+, where M^n+ is the cation.
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Related Practice
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