Domanda del libro di testo
Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+.
415
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Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 14
Which of the following statements is false? (a) An Arrhenius base increases the concentration of OH- in water. (b) A Brønsted-Lowry base is a proton acceptor. (c) Water can act as a Brønsted–Lowry acid. (d) Water can act as a Brønsted–Lowry base. (e) Any compound that contains an –OH group acts as a Brønsted-Lowry base.
Guida verificata passo dopo passo1
Identify the definitions of Arrhenius and Brønsted-Lowry acids and bases.
Recall that an Arrhenius base increases the concentration of OH^- ions in water.
Understand that a Brønsted-Lowry base is defined as a proton (H^+) acceptor.
Recognize that water (H2O) can act as both a Brønsted-Lowry acid (proton donor) and a Brønsted-Lowry base (proton acceptor).
Evaluate the statement that any compound with an –OH group acts as a Brønsted-Lowry base, and consider exceptions such as alcohols, which do not typically act as bases.
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Arrhenius Theory of Acids and Bases
The Arrhenius theory defines acids as substances that increase the concentration of hydrogen ions (H+) in aqueous solution, while bases increase the concentration of hydroxide ions (OH-). This theory is foundational in understanding the behavior of acids and bases in water, particularly in identifying how they dissociate and interact in solution.
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Percorso guidato
02:00
Arrhenius Acids and Bases
Brønsted-Lowry Theory of Acids and Bases
The Brønsted-Lowry theory expands the definition of acids and bases beyond aqueous solutions. According to this theory, an acid is a proton donor and a base is a proton acceptor. This concept allows for a broader understanding of acid-base reactions, including those that occur in non-aqueous environments.
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Percorso guidato
02:08Bronsted-Lowry Acid-Base Theory
Amphoteric Substances
Amphoteric substances are those that can act as either an acid or a base depending on the context of the reaction. Water is a prime example, as it can donate a proton (acting as an acid) or accept a proton (acting as a base). Understanding this dual behavior is crucial for analyzing reactions involving water and other amphoteric compounds.
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Percorso guidato
03:03Amphoteric Species
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Give the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-.
511
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361
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