Textbook Question
Indicate whether aqueous solutions of each of the following solutes contain only ions, only molecules, or mostly molecules and a few ions:
a. acetic acid, HC2H3O2, a weak electrolyte
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Ch.9 Solutions
Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353
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Table of contents
- Ch.1 Chemistry in Our Lives11
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy54
- Ch.4 Atoms and Elements51
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions41
- Ch.8 Gases29
- Ch.9 Solutions51
- Ch.10 Acids and Bases and Equilibrium65
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons78
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones83
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides90
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis83
- Ch.18 Metabolic Pathways and ATP Production67
Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353Not the one you use?Change textbook
Chapter 9, Problem 9d
Write a balanced equation for the dissociation of each of the following strong electrolytes in water:
d. Fe(NO3)3
Verified step by step guidance1
Identify the strong electrolyte: Fe(NO₃)₃ is iron(III) nitrate, a strong electrolyte that dissociates completely in water into its constituent ions.
Determine the ions produced: Iron(III) nitrate dissociates into Fe³⁺ (iron(III) ion) and NO₃⁻ (nitrate ion).
Write the unbalanced dissociation equation: Fe(NO₃)₃ → Fe³⁺ + NO₃⁻.
Balance the equation: Since there are three nitrate ions (NO₃⁻) in one formula unit of Fe(NO₃)₃, the balanced equation is Fe(NO₃)₃ → Fe³⁺ + 3NO₃⁻.
Verify the charge balance: The total positive charge from Fe³⁺ (3+) is balanced by the total negative charge from 3NO₃⁻ (3 × 1−), ensuring the equation is correctly balanced.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Dissociation of Electrolytes
Dissociation refers to the process by which an ionic compound separates into its constituent ions when dissolved in water. Strong electrolytes, such as salts, completely dissociate in solution, meaning that all of the solute breaks apart into ions. This is crucial for understanding how compounds like Fe(NO₃)₃ behave in aqueous solutions.
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Electrolytes (Simplified) Concept 3
Ionic Compounds
Ionic compounds are formed from the electrostatic attraction between positively charged cations and negatively charged anions. In the case of Fe(NO₃)₃, iron (Fe) acts as the cation, while the nitrate ion (NO₃) serves as the anion. Recognizing the structure of ionic compounds is essential for predicting their behavior in solution, including their dissociation.
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Balanced Chemical Equations
A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. For the dissociation of Fe(NO₃)₃, it is important to write the equation correctly to reflect the stoichiometry of the ions produced. This ensures that the law of conservation of mass is upheld in the reaction.
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Related Practice
Textbook Question
Indicate whether aqueous solutions of each of the following solutes contain only ions, only molecules, or mostly molecules and a few ions: c. fructose, C6H12O6, a nonelectrolyte
Textbook Question
Indicate whether aqueous solutions of each of the following solutes contain only ions, only molecules, or mostly molecules and a few ions:
b. NaBr, a strong electrolyte
Textbook Question
KF is a strong electrolyte, and HF is a weak electrolyte. How is the solution of KF different from that of HF?
Textbook Question
Water is a polar solvent and carbon tetrachloride (CCl4) is a nonpolar solvent. In which solvent is each of the following, which is found or used in the body, more likely to be soluble?
d. cholesterol (lipid), nonpolar
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Textbook Question
Describe the formation of an aqueous KI solution, when solid KI dissolves in water.
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