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.
Ch.16 - Acid-Base Equilibria
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 16, Problem 37
By what factor does [H+] change for a pH change of (a) 2.00 units? (b) 0.50 units?
Verified step by step guidance1
pH is a measure of the hydrogen ion concentration in a solution, given by the formula: \( \text{pH} = -\log[\text{H}^+] \).
A change in pH of 2.00 units means the pH has either increased or decreased by 2.00.
If the pH decreases by 2.00 units, the concentration of \( \text{H}^+ \) ions increases. Conversely, if the pH increases by 2.00 units, the concentration of \( \text{H}^+ \) ions decreases.
The relationship between pH change and \( \text{H}^+ \) concentration change is logarithmic. A change of 1 pH unit corresponds to a tenfold change in \( \text{H}^+ \) concentration.
Therefore, a change of 2.00 pH units corresponds to a change in \( \text{H}^+ \) concentration by a factor of \( 10^2 \).
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2mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
pH Scale
The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is neutral, below 7 is acidic, and above 7 is basic. Each unit change in pH represents a tenfold change in hydrogen ion concentration, meaning that a decrease in pH indicates an increase in acidity.
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The pH Scale
Hydrogen Ion Concentration
Hydrogen ion concentration, denoted as [H+], is a measure of the amount of hydrogen ions present in a solution. It is directly related to pH, where a lower pH corresponds to a higher concentration of H+. For example, a change of 2.00 units in pH results in a change in [H+] by a factor of 10^2, or 100 times.
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Logarithmic Relationship
The relationship between pH and hydrogen ion concentration is logarithmic, meaning that pH is the negative logarithm of the hydrogen ion concentration: pH = -log[H+]. This implies that small changes in pH can lead to significant changes in [H+], which is crucial for understanding how acidity affects chemical reactions and biological processes.
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Related Practice
Textbook Question
Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (c) a solution in which 3H+4 is 1000 times greater than 3OH-4.
Textbook Question
Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3H+4 = 2.5 * 10-10 M