Textbook Question
Identify each of the following as an acid or a base:
d. HI
Ch.10 Acids and Bases and Equilibrium
Timberlake14th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249
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Table of contents
- Ch.1 Chemistry in Our Lives19
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy53
- Ch.4 Atoms and Elements58
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions38
- Ch.8 Gases30
- Ch.9 Solutions50
- Ch.10 Acids and Bases and Equilibrium64
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons77
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones82
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides91
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis86
- Ch.18 Metabolic Pathways and ATP Production73
Timberlake14th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249Not the one you use?Change textbook
Chapter 10, Problem 72a
Identify each of the following as an acid or a base:
b. H2SO3
Verified step by step guidance1
Step 1: Recall the definition of acids and bases. Acids are substances that donate protons (H⁺ ions) in aqueous solutions, while bases are substances that accept protons or produce hydroxide ions (OH⁻) in aqueous solutions.
Step 2: Examine the chemical formula of the given compound, H₂SO₃. This is sulfurous acid, which contains hydrogen atoms that can potentially be donated as H⁺ ions.
Step 3: Recognize that the presence of hydrogen atoms at the beginning of the formula (H₂) is a common indicator of an acid. These hydrogens are ionizable and can dissociate in water to release H⁺ ions.
Step 4: Consider the context of the compound in water. When H₂SO₃ dissolves in water, it dissociates partially to form H⁺ ions and HSO₃⁻ ions, confirming its behavior as an acid.
Step 5: Conclude that H₂SO₃ is an acid because it donates H⁺ ions in aqueous solutions, which aligns with the definition of an acid.
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Video duration:
1mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acids and Bases
Acids are substances that can donate protons (H⁺ ions) in a solution, while bases are substances that can accept protons. This definition is rooted in the Brønsted-Lowry theory, which emphasizes the transfer of protons in acid-base reactions. Understanding this distinction is crucial for classifying compounds like H₂SO₃.
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Arrhenius Acids & Bases Concept 1
Sulfurous Acid (H₂SO₃)
H₂SO₃, or sulfurous acid, is a weak acid formed when sulfur dioxide (SO₂) dissolves in water. It can dissociate in solution to release H⁺ ions, which is characteristic of acids. Recognizing H₂SO₃ as an acid is essential for understanding its behavior in chemical reactions and its role in various environmental processes.
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pH Scale
The pH scale measures the acidity or basicity of a solution, ranging from 0 (strongly acidic) to 14 (strongly basic), with 7 being neutral. A solution with a pH less than 7 indicates the presence of more H⁺ ions, typical of acids like H₂SO₃. Familiarity with the pH scale helps in predicting the properties and reactions of acids and bases.
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Related Practice
Textbook Question
Sometimes, during stress or trauma, a person can start to hyperventilate. Then the person might breathe into a paper bag to avoid fainting.
a. What changes occur in the blood pH during hyperventilation?
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Textbook Question
Determine if each of the following diagrams represents a strong acid or a weak acid. The acid has the formula HX.
Textbook Question
Write the balanced chemical equation for the neutralization reaction of stomach acid HCl with Al(OH)3, an ingredient in some antacids.
Textbook Question
Sometimes, during stress or trauma, a person can start to hyperventilate. Then the person might breathe into a paper bag to avoid fainting.
b. How does breathing into a paper bag help return blood pH to normal?
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Textbook Question
How many grams of Al(OH)3 are required to neutralize 150. mL of stomach acid with a pH of 1.5?