Textbook Question
Calculate the concentration of all species in a 0.155 M solution of H2CO3.
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Ch.17 - Acids and Bases
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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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 122
Based on molecular structure, arrange the binary compounds in order of increasing acid strength. Explain your choice. H2Te, HI, H2S, NaH
Verified step by step guidance1
Identify the type of acids involved: Binary acids are typically composed of hydrogen and one other element.
Consider the periodic trends: Acid strength in binary acids generally increases across a period and down a group in the periodic table.
Analyze the molecular structure: The strength of an acid is influenced by the bond strength between hydrogen and the other element. Weaker bonds typically result in stronger acids.
Apply the concept to the given compounds: Compare the bond strengths and electronegativities of the elements in H2Te, HI, H2S, and NaH.
Arrange the compounds: Based on the analysis, order the compounds from weakest to strongest acid.
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 a compound to donate protons (H+) in a solution. Strong acids completely dissociate in water, while weak acids only partially dissociate. The strength of binary acids, which consist of hydrogen and one other element, often increases with the size and electronegativity of the non-hydrogen element.
Recommended video:
Guided course
03:51
Binary Acid Strengths
Binary Acids
Binary acids are compounds formed from hydrogen and one other nonmetal element. The general formula is HA, where A is a nonmetal. The strength of binary acids typically increases down a group in the periodic table due to the decreasing bond strength between hydrogen and the nonmetal, making it easier for the acid to release a proton.
Recommended video:
Guided course
01:03Binary Acids
Electronegativity and Bond Strength
Electronegativity is the tendency of an atom to attract electrons in a bond. In binary acids, higher electronegativity of the nonmetal can lead to stronger H-A bonds, but as you move down a group, larger atomic size results in weaker bonds. This interplay affects the acid's ability to dissociate and thus its strength, with larger, less electronegative atoms generally leading to stronger acids.
Recommended video:
Guided course
02:10Electronegativity Trends
Related Practice
Textbook Question
Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2 given here.
a. Ka1 = 1.0 × 10–4; Ka2 = 5.0 × 10–5
Calculate the contributions to [H3O+] from each ionization step. At what point can the contribution of the second step be neglected?
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Textbook Question
Which is a stronger base, S2– or Se2–? Explain.
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Textbook Question
Based on molecular structure, arrange the oxyacids in order of increasing acid strength. Explain your choice. HClO3, HIO3, HBrO3
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