Textbook Question
Determine the pH of each solution. a. 0.10 M NH4Cl
1140
views
Ch.17 - Acids and Bases
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
Not the one you use?Change textbookSelect a different textbook
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 107
Arrange the solutions in order of increasing acidity. NaCl, NH4Cl, NaHCO3, NH4ClO2, NaOH
Verified step by step guidance1
Identify the nature of each compound: NaCl is a neutral salt, NH4Cl is an acidic salt, NaHCO3 is a basic salt, NH4ClO2 is an acidic salt, and NaOH is a strong base.
Consider the ions produced in solution: NaCl dissociates into Na+ and Cl-, NH4Cl into NH4+ and Cl-, NaHCO3 into Na+ and HCO3-, NH4ClO2 into NH4+ and ClO2-, and NaOH into Na+ and OH-.
Evaluate the acidic or basic nature of the ions: NH4+ is a weak acid, Cl- is neutral, HCO3- is a weak base, ClO2- is a weak acid, and OH- is a strong base.
Rank the solutions based on the strength of their acidic or basic ions: NaOH (strong base) < NaHCO3 (weak base) < NaCl (neutral) < NH4ClO2 (weak acid) < NH4Cl (stronger acid).
Arrange the solutions in order of increasing acidity: NaOH, NaHCO3, NaCl, NH4ClO2, NH4Cl.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acidity and pH
Acidity refers to the concentration of hydrogen ions (H+) in a solution, which determines its pH level. A lower pH indicates a more acidic solution, while a higher pH indicates a more basic solution. Understanding the pH scale is essential for comparing the acidity of different solutions.
Salt Hydrolysis
Salt hydrolysis occurs when a salt dissolves in water and reacts with water to produce an acidic or basic solution. For example, ammonium chloride (NH4Cl) can release H+ ions, making the solution acidic, while sodium bicarbonate (NaHCO3) can produce OH- ions, making the solution basic. This concept is crucial for determining the acidity of the given salts.
Recommended video:
Guided course
00:50
Ionic Salts
Strong vs. Weak Acids and Bases
Strong acids and bases completely dissociate in water, while weak acids and bases only partially dissociate. For instance, NaOH is a strong base that fully dissociates, leading to a higher pH, whereas NH4Cl is derived from a weak acid (NH4+) and a strong base (Cl-), resulting in a more acidic solution. This distinction is vital for ranking the acidity of the solutions.
Recommended video:
Guided course
02:22Strong vs Weak Bases
Related Practice
Textbook Question
Calculate the concentration of all species in a 0.15 M KF solution.
1727
views
1
rank
Textbook Question
Calculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.
1638
views
Textbook Question
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+
1241
views
Textbook Question
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. Al(NO3)3
609
views