Textbook Question
Which of the following solutions is the most acidic? (a) 0.2 M Ba(OH)2, (b) 0.2 M H2SO3, (c) 1.0 M glucose 1C6H12O6).
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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 Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 16, Problem 32
Which of the following solutions is the most basic?(a) 0.6 M NaCl, (b) 0.150 M CsOH, (c) 0.100 M Sr1OH22.
Verified step by step guidance1
Identify the nature of each compound: NaCl is a neutral salt, CsOH is a strong base, and Sr(OH)2 is a strong base.
Recognize that the basicity of a solution is determined by the concentration of hydroxide ions (OH⁻) it produces.
Calculate the concentration of OH⁻ ions for each solution: NaCl does not produce OH⁻ ions, CsOH produces OH⁻ ions equal to its concentration, and Sr(OH)2 produces twice the concentration of OH⁻ ions because it dissociates into two OH⁻ ions per formula unit.
Compare the OH⁻ ion concentrations: 0 M for NaCl, 0.150 M for CsOH, and 0.200 M for Sr(OH)2.
Determine which solution has the highest OH⁻ concentration, indicating it is the most basic.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
pH and Basicity
pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. A pH value above 7 signifies a basic solution, while a value below 7 indicates acidity. Basic solutions contain higher concentrations of hydroxide ions (OH-) compared to hydrogen ions (H+), which is crucial for determining the most basic solution among the options provided.
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The pH Scale
Strong Bases
Strong bases are substances that completely dissociate in water to produce hydroxide ions. Examples include alkali metal hydroxides like CsOH and alkaline earth metal hydroxides like Sr(OH)2. The strength of a base is determined by its ability to increase the concentration of OH- ions in solution, which directly affects the pH and basicity of the solution.
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Concentration and Dilution
Concentration refers to the amount of solute present in a given volume of solution, typically expressed in molarity (M). In this context, higher concentrations of strong bases will lead to a greater production of hydroxide ions, thus increasing the basicity of the solution. Understanding how concentration affects pH is essential for comparing the basicity of the given solutions.
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Related Practice
Textbook Question
Deuterium oxide 1D2O, where D is deuterium, the hydrogen-2 isotope) has an ion-product constant, Kw, of 8.9 * 10-16 at 20 °C. Calculate 3D+4 and 3OD-4 for pure (neutral) D2O at this temperature.
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Textbook Question
Write the expression for the ion product constant for water, Kw.
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Textbook Question
Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) 3H+4 = 0.0505 M
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Textbook Question
By what factor does [H+] change for a pH change of (a) 2.00 units? (b) 0.50 units?
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