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 112
Calculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.
Verified step by step guidance1
Identify the components of the solution: C6H5NH3Cl is an ionic compound that dissociates into C6H5NH3+ (anilinium ion) and Cl- (chloride ion) in water.
Recognize that C6H5NH3+ is a weak acid, which can donate a proton to water, forming C6H5NH2 (aniline) and H3O+ (hydronium ion).
Write the equilibrium expression for the dissociation of C6H5NH3+ in water: C6H5NH3+ + H2O ⇌ C6H5NH2 + H3O+.
Use the acid dissociation constant (Ka) for C6H5NH3+ to set up an ICE (Initial, Change, Equilibrium) table to find the concentrations of C6H5NH2 and H3O+ at equilibrium.
Calculate the concentration of Cl- ions, which is equal to the initial concentration of C6H5NH3Cl, since it fully dissociates in water.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Chemistry
C6H5NH3Cl, or phenylammonium chloride, is a salt formed from the weak base aniline (C6H5NH2) and hydrochloric acid (HCl). In solution, it dissociates into C6H5NH3+ (the conjugate acid) and Cl-. Understanding the behavior of weak acids and bases is crucial for determining the concentrations of species in solution.
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Arrhenius Acids and Bases
Dissociation of Salts
When salts dissolve in water, they dissociate into their constituent ions. For C6H5NH3Cl, it dissociates completely into C6H5NH3+ and Cl-. The concentration of each ion in the solution can be directly derived from the initial concentration of the salt, which is 0.225 M in this case.
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Equilibrium and Concentration Calculations
In solutions involving weak acids or bases, equilibrium plays a significant role. The concentration of the conjugate acid (C6H5NH3+) will influence the pH of the solution. To calculate the concentrations of all species, one must consider both the initial concentration and any changes due to dissociation and equilibrium shifts.
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