Textbook Question
Calculate Kb values for CH3COO- and ClO-.
1705
views
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 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 78b
Which is the stronger acid, the ammonium ion or the hydroxylammonium ion?
Verified step by step guidance1
Identify the chemical formulas for the ammonium ion and the hydroxylammonium ion. The ammonium ion is \( \text{NH}_4^+ \) and the hydroxylammonium ion is \( \text{NH}_3\text{OH}^+ \).
Understand that the strength of an acid is determined by its ability to donate a proton (\( \text{H}^+ \)). The more readily an ion donates a proton, the stronger the acid.
Consider the conjugate bases of each ion. The conjugate base of the ammonium ion is ammonia (\( \text{NH}_3 \)), and the conjugate base of the hydroxylammonium ion is hydroxylamine (\( \text{NH}_2\text{OH} \)).
Compare the stability of the conjugate bases. A more stable conjugate base corresponds to a stronger acid. Factors affecting stability include electronegativity and resonance.
Research or recall the \( pK_a \) values of the acids. The \( pK_a \) value is inversely related to acid strength: a lower \( pK_a \) indicates a stronger acid. Compare the \( pK_a \) values of ammonium ion and hydroxylammonium ion to determine which is the stronger acid.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
3mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid Strength
Acid strength refers to the ability of an acid to donate protons (H+) in a solution. Stronger acids dissociate more completely in water, resulting in a higher concentration of H+ ions. The strength of an acid can be quantified using the acid dissociation constant (Ka), where a larger Ka value indicates a stronger acid.
Recommended video:
Guided course
03:51
Binary Acid Strengths
Ammonium Ion (NH4+)
The ammonium ion (NH4+) is a positively charged ion formed when ammonia (NH3) accepts a proton. It acts as a weak acid in aqueous solutions, capable of donating a proton to form ammonia. Understanding its behavior in acid-base reactions is crucial for comparing its strength to other acids.
Recommended video:
Guided course
06:17Ion Formation
Hydroxylammonium Ion (NH3OH+)
The hydroxylammonium ion (NH3OH+) is derived from hydroxylamine and can also donate a proton, functioning as an acid. Its strength relative to the ammonium ion can be assessed by comparing their respective Ka values. The presence of the hydroxyl group in hydroxylammonium can influence its acidity due to potential resonance stabilization.
Recommended video:
Guided course
06:17Ion Formation
Related Practice
Textbook Question
Which is the stronger base, the acetate ion or the hypochlorite ion?
524
views
Textbook Question
Using data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (b) 0.035 M Na2S
616
views
Textbook Question
Pyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (b) Using Appendix D, calculate the Ka for pyridinium bromide.
577
views
Textbook Question
Given that Kb for ammonia is 1.8 × 10-5 and that for hydroxylamine is 1.1 × 10-8, which is the stronger base?
1115
views