Textbook Question
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. d. CH2NH3+
Ch.17 - Acids and Bases
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Chapter 17, Problem 100d
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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1mKey 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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Cation Acidity in Salts
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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Textbook Question
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. e. C6H5NH3NO2