Textbook Question
Write the formula for the conjugate base of each acid. d. HCHO2
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 Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 17, Problem 36b
Write the formula for the conjugate base of each acid. b. HBr
Verified step by step guidance1
Identify the acid in the problem: HBr.
Recall that a conjugate base is formed by removing a proton (H⁺) from the acid.
Remove one hydrogen ion (H⁺) from HBr.
After removing H⁺, the remaining species is Br⁻.
Thus, the conjugate base of HBr is Br⁻.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
33sWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Conjugate Acid-Base Pairs
In acid-base chemistry, a conjugate acid-base pair consists of two species that differ by the presence of a proton (H+). When an acid donates a proton, it transforms into its conjugate base, while the base that accepts the proton becomes its conjugate acid. Understanding this relationship is crucial for identifying the conjugate base of any given acid.
Strong Acids and Their Conjugate Bases
Strong acids, such as HBr, completely dissociate in water, meaning they release all their protons. The conjugate base of a strong acid is typically a weak base, as it has a low tendency to re-accept the proton. Recognizing that HBr is a strong acid helps in determining that its conjugate base, Br-, is relatively stable and does not readily accept protons.
Recommended video:
Guided course
01:09
Strong Acid-Strong Base Titration
Chemical Formulas and Ion Representation
Chemical formulas represent the composition of substances, including ions. The conjugate base of an acid can be represented by its chemical formula, which indicates the remaining species after the acid has lost a proton. For HBr, the conjugate base is Br-, highlighting the importance of understanding how to write and interpret chemical formulas in acid-base reactions.
Recommended video:
Guided course
06:17Ion Formation
Related Practice
Textbook Question
In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. c. CO32–(aq) + H2O(l) ⇌ HCO3–(aq) + OH–(aq)
1099
views
Textbook Question
Write the formula for the conjugate base of each acid. a. H2SO4
Textbook Question
Write the formula for the conjugate acid of each base. c. HCO3–
Textbook Question
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). b. HCl
319
views
Textbook Question
Write the formula for the conjugate base of each acid. c. HI