Textbook Question
Pick the stronger base from each pair. c. NO2– or NO3–
Ch.17 - Acids and Bases
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Chapter 17, Problem 53a
Calculate [H3O+] and [OH–] for each solution at 25 °C. a. pH = 8.55
Verified step by step guidance1
Identify the relationship between pH and [H3O+]. Use the formula: \([H_3O^+] = 10^{-pH}\).
Substitute the given pH value into the formula to find \([H_3O^+]\).
Use the relationship between [H3O+] and [OH-] at 25 °C, which is given by the ion product of water: \(K_w = [H_3O^+][OH^-] = 1.0 \times 10^{-14}\).
Rearrange the equation to solve for \([OH^-]\): \([OH^-] = \frac{K_w}{[H_3O^+]}\).
Substitute the calculated \([H_3O^+]\) into the equation to find \([OH^-]\).
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
1mWas 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 considered neutral, while values below 7 indicate acidity and values above 7 indicate basicity. The pH is logarithmically related to the concentration of hydrogen ions, [H+], in the solution, where lower pH values correspond to higher [H+] concentrations.
Recommended video:
Guided course
02:33
The pH Scale
Hydronium Ion Concentration
The concentration of hydronium ions, [H3O+], in a solution can be calculated from the pH using the formula [H3O+] = 10^(-pH). This relationship shows that as pH increases, the concentration of hydronium ions decreases, indicating a more basic solution. For a pH of 8.55, this calculation is essential to determine the exact concentration of hydronium ions present.
Recommended video:
Guided course
06:25Hydronium Ion Concentration Example
Water Ion Product
At 25 °C, the product of the concentrations of hydronium ions and hydroxide ions, [H3O+][OH-], is constant and equal to 1.0 x 10^-14, known as the water ion product (Kw). This relationship allows for the calculation of hydroxide ion concentration, [OH-], using the formula [OH-] = Kw / [H3O+]. Understanding this concept is crucial for determining the balance between hydronium and hydroxide ions in a solution.
Recommended video:
Guided course
00:53Production of Hydrogen Example
Related Practice
Textbook Question
Rank the solutions in order of decreasing [H3O+]: 0.10 M HCl; 0.10 M HF; 0.10 M HClO; 0.10 M HC6H5O.
Textbook Question
Calculate [H3O+] and [OH–] for each solution at 25 °C. b. pH = 11.23 c. pH = 2.87
Textbook Question
Complete the table. (All solutions are at 25 °C.)
Textbook Question
Complete the table. (All solutions are at 25 °C.)