Textbook Question
An unknown salt is either KBr, NH4Cl, KCN, or K2CO3. If a 0.100 M solution of the salt is neutral, what is the identity of the salt?
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Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 16, Problem 84e
Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (e) Na2SO3.
Verified step by step guidance1
Identify the ions produced when \( \text{Na}_2\text{SO}_3 \) dissolves in water: \( \text{Na}^+ \) and \( \text{SO}_3^{2-} \).
Recognize that \( \text{Na}^+ \) is a spectator ion and does not affect the pH of the solution.
Consider the behavior of the \( \text{SO}_3^{2-} \) ion in water. It can react with water to form \( \text{HSO}_3^- \) and \( \text{OH}^- \), indicating a basic solution.
Write the hydrolysis reaction: \( \text{SO}_3^{2-} + \text{H}_2\text{O} \rightarrow \text{HSO}_3^- + \text{OH}^- \).
Conclude that the presence of \( \text{OH}^- \) ions makes the solution basic.
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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 the behavior of substances in terms of their ability to donate protons (H+) or accept protons. According to the Brønsted-Lowry theory, acids are proton donors and bases are proton acceptors. Understanding this theory is essential for predicting the acidity or basicity of a solution based on the ions produced when a substance dissolves in water.
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Bronsted-Lowry Acid-Base Theory
Salt Hydrolysis
Salt hydrolysis occurs when an ionic compound dissolves in water and its constituent ions interact with water molecules, potentially affecting the pH of the solution. In the case of Na2SO3, the sodium ions (Na+) are neutral, while the sulfite ions (SO3^2-) can react with water to produce hydroxide ions (OH-), leading to a basic solution. This concept is crucial for determining the resulting pH of the solution.
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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 pH less than 7 indicates an acidic solution, while a pH greater than 7 indicates a basic solution. Understanding the pH scale is important for interpreting the results of acid-base reactions and predicting the nature of solutions formed from various substances.
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Related Practice
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 substances are acidic, basic, or neutral: (c) NaClO
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Textbook Question
Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (d) 3CH3NH34NO3
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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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