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.
Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
Not the one you use?Change textbookSelect a different textbook
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 33
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 \( 10^2 \).
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
2mWas this helpful?
Key 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.
Recommended video:
Guided course
02:33
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.
Recommended video:
Guided course
01:22Hydrogenation Reactions
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.
Recommended video:
Guided course
04:56Logarithmic Operations
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).
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.