Textbook Question
Which of the following solutions is the most basic?(a) 0.6 M NaCl, (b) 0.150 M CsOH, (c) 0.100 M Sr1OH22.
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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 30a
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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Identify the given concentration: \([H^+] = 0.0505\, \text{M}\).
Use the relationship between \([H^+]\) and \([OH^-]\) in water: \([H^+][OH^-] = 1.0 \times 10^{-14}\, \text{at 25°C}\).
Rearrange the equation to solve for \([OH^-]\): \([OH^-] = \frac{1.0 \times 10^{-14}}{[H^+]}\).
Substitute the given \([H^+]\) value into the equation: \([OH^-] = \frac{1.0 \times 10^{-14}}{0.0505}\, \text{M}\).
Determine if the solution is acidic, basic, or neutral by comparing \([H^+]\) and \([OH^-]\): If \([H^+] > [OH^-]\), the solution is acidic; if \([H^+] < [OH^-]\), it is basic; if \([H^+] = [OH^-]\), it is neutral.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
pH and pOH
pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. The pOH is similarly a measure of hydroxide ion concentration. The relationship between pH and pOH is defined by the equation pH + pOH = 14 at 25°C. Understanding these concepts is essential for determining the nature of a solution.
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pH and pOH Calculations
Acidic, Basic, and Neutral Solutions
A solution is considered acidic if its pH is less than 7, basic if its pH is greater than 7, and neutral if its pH is exactly 7. The concentration of hydrogen ions (H+) and hydroxide ions (OH-) in a solution determines its classification. For example, a higher concentration of H+ indicates acidity, while a higher concentration of OH- indicates basicity.
Calculating pOH from pH
To find the pOH from a given concentration of H+, one first calculates the pH using the formula pH = -log[H+]. Once the pH is determined, pOH can be calculated using the relationship pOH = 14 - pH. This calculation is crucial for determining the hydroxide ion concentration and the overall nature of the solution.
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Related Practice
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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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
Write a chemical equation that illustrates the autoionization of water.
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