Domanda del libro di testo
The hydrogen sulfite ion 1HSO3-2 is amphiprotic. Write a balanced chemical equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water.
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Ch.16 - Acid-Base Equilibria
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 20b
Give the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-.
Guida verificata passo dopo passo1
Identify the Brønsted–Lowry acid in each case. A Brønsted–Lowry acid is a substance that can donate a proton (H⁺).
For each acid, remove one proton (H⁺) to find the conjugate base. This involves subtracting an H⁺ from the chemical formula of the acid.
For (i) HCOOH, remove an H⁺ to form the conjugate base. The resulting formula will be HCOO⁻.
For (ii) HPO₄²⁻, remove an H⁺ to form the conjugate base. The resulting formula will be PO₄³⁻.
Verify that the charge of the conjugate base is one unit more negative than the original acid, as losing a proton (H⁺) decreases the charge by one.
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Brønsted–Lowry Acid-Base Theory
The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. This framework emphasizes the transfer of protons (H+) in chemical reactions, allowing for a broader understanding of acid-base behavior beyond just the presence of hydroxide ions. In this context, identifying conjugate bases involves recognizing the species formed when an acid donates a proton.
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Percorso guidato
02:08
Bronsted-Lowry Acid-Base Theory
Conjugate Acid-Base Pairs
Conjugate acid-base pairs consist of two species that differ by the presence of a single proton. When an acid donates a proton, it transforms into its conjugate base, while the base that accepts the proton becomes its conjugate acid. Understanding these pairs is crucial for predicting the outcome of acid-base reactions and determining the strength of acids and bases.
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01:30Conjugate Acid-Base Pairs
Dissociation of Acids
The dissociation of acids refers to the process by which an acid releases protons into solution. For example, when formic acid (HCOOH) dissociates, it loses a proton to form its conjugate base, formate (HCOO-). Similarly, the dissociation of hydrogen phosphate (HPO4^2-) results in the formation of its conjugate base, phosphate (PO4^3-). This concept is essential for identifying conjugate bases in acid-base reactions.
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00:54Acid-Base Dissociation Example
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Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+.
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Give the conjugate acid of the following Brønsted–Lowry bases: (i) SO42-, (ii) CH3NH2.
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Identify the Lewis acid and Lewis base in each of the following reactions:
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Identify the Brønsted–Lowry acid and the Brønsted– Lowry base on the left side of each equation, and also identify the conjugate acid and conjugate base of each on the right side.
(a) HBrO(aq) + H2O(l) ⇌ H3O+(aq) + BrO-(aq)
(b) HSO4-(aq) + HCO3-(aq) ⇌ SO42-(aq) + H2CO3(aq)
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