Textbook Question
Calculate the pH of 100.0 mL of 0.30 M NH3 before and after the addition of 4.0 g of NH4NO3, and account for the change. Assume that the volume remains constant.
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Ch.16 - Aqueous Equilibria: Acids & Bases
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 16, Problem 63a
Identify the weakest acid in each of the following sets. Explain your reasoning. (a) H2SO3, HClO3, HClO4
Verified step by step guidance1
Identify the structure and stability of the conjugate bases of each acid. The stability of the conjugate base often determines the strength of the acid.
Consider the oxidation state of the central atom in each oxyacid. Higher oxidation states generally correlate with stronger acids because they stabilize the negative charge on the conjugate base more effectively.
Examine the electronegativity and electron withdrawing effects of the atoms surrounding the central atom. More electronegative atoms or groups that are better at withdrawing electrons will generally stabilize the conjugate base, leading to a stronger acid.
Compare the number of oxygen atoms bonded to the central atom in each acid. More oxygen atoms usually indicate stronger acids due to better stabilization of the conjugate base through resonance and inductive effects.
Based on the above considerations, determine which acid has the least effective stabilization of its conjugate base, indicating it is the weakest acid among the given options.
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. Strong acids completely dissociate in water, while weak acids only partially dissociate. The strength of an acid is often determined by its dissociation constant (Ka), with larger values indicating stronger acids.
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03:51
Binary Acid Strengths
Oxidation States
The oxidation state of an element in a compound indicates its degree of oxidation or reduction. In oxyacids, the oxidation state of the central atom can influence acid strength; higher oxidation states typically lead to stronger acids due to increased positive charge, which stabilizes the conjugate base after proton donation.
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02:42Oxidation Numbers
Comparative Analysis of Oxyacids
When comparing oxyacids, the number of oxygen atoms bonded to the central atom plays a crucial role in determining acid strength. More oxygen atoms generally lead to stronger acids because they stabilize the negative charge on the conjugate base through resonance. Thus, in a set of oxyacids, the one with fewer oxygen atoms is often the weakest.
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01:15Oxyacids
Related Practice
Textbook Question
Calculate the percent dissociation of 0.10 M hydrazoic acid (HN3, Ka = 1.9 X 10^-5). Recalculate the percent dissociation of 0.10 M HN3 in the presence of 0.10 M HCl, and explain the change.
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Textbook Question
Arrange each group of compounds in order of increasing acid strength. Explain your reasoning. (a) HCl, H2S, PH3
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Textbook Question
Identify the stronger acid in each of the following pairs.Explain your reasoning.(b) H3PO4 or H3AsO4
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Textbook Question
Identify the weakest acid in each of the following sets. Explain your reasoning. (c) B(OH)3, Al(OH)3, Ga(OH)3
Textbook Question
Identify the weakest acid in each of the following sets. Explain your reasoning. (b) NH3, H2O, H2S
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