Domanda del libro di testo
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)
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Ch.17 - Acids and Bases
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- 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
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 17, Problema 35c
Write the formula for the conjugate acid of each base. c. HCO3–
Guida verificata passo dopo passo1
Identify the base in the problem: \( \text{HCO}_3^- \).
Recall that a conjugate acid is formed by adding a proton (\( \text{H}^+ \)) to the base.
Add a proton to the base \( \text{HCO}_3^- \) to form the conjugate acid.
The addition of \( \text{H}^+ \) to \( \text{HCO}_3^- \) results in \( \text{H}_2\text{CO}_3 \).
Write the formula for the conjugate acid: \( \text{H}_2\text{CO}_3 \).
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Conjugate Acid-Base Pair
In acid-base chemistry, a conjugate acid is formed when a base accepts a proton (H+). This relationship is part of the Brønsted-Lowry theory, which defines acids as proton donors and bases as proton acceptors. Each acid-base pair differs by one proton, illustrating the dynamic nature of proton transfer in chemical reactions.
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Percorso guidato
01:30
Conjugate Acid-Base Pairs
Bicarbonate Ion (HCO3–)
The bicarbonate ion (HCO3–) is an important buffer in biological systems and plays a crucial role in maintaining pH balance. It can act as a base by accepting a proton to form carbonic acid (H2CO3), which is essential in processes like respiration and metabolic regulation. Understanding its behavior is key to identifying its conjugate acid.
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Percorso guidato
06:17Ion Formation
Protonation
Protonation is the process by which a molecule gains a proton (H+), resulting in the formation of a conjugate acid. This process is fundamental in acid-base reactions, as it alters the charge and reactivity of the molecule. For the bicarbonate ion, protonation leads to the formation of carbonic acid, illustrating how bases can transform into acids through protonation.
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Percorso guidato
01:38Neutron-to-Proton Plot
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