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Chapter 8: Aqueous Solutions

  • Page ID
    19089
    • Anonymous
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    Aqueous solutions are solutions in which the solvent is water, which is an excellent solvent and is also naturally abundant, it is a ubiquitous solvent in chemistry. Substances that are hydrophobic ('water-fearing') often do not dissolve well in water, whereas those that are hydrophilic ('water-loving') do. Reactions in aqueous solutions are usually double-displacement reactions. Aqueous solutions that conduct electric current efficiently contain strong electrolytes, while ones that conduct poorly are considered to have weak electrolytes. Those strong electrolytes are substances that are completely ionized in water, whereas the weak electrolytes exhibit only a small degree of ionization in water. Nonelectrolytes are substances that dissolve in water yet maintain their molecular integrity (do not dissociate into ions).

    • Chapter 8.01: Aqueous Solutions
      This page covers the nature of aqueous solutions, highlighting water's role as a polar solvent that facilitates the dissolution of ionic and some organic compounds by forming hydrated ions. It categorizes substances into strong and weak electrolytes based on their dissociation in water, alongside nonelectrolytes, which remain neutral.
    • Chapter 8.02: Solution Concentrations
      This page covers solution concentration in chemistry, focusing on molarity and various measurement methods like mass-to-mass and parts per million. It explains solution preparation, emphasizing the importance of accounting for solute volume, and details practical calculations for making solutions of specific concentrations, including dilution from stock solutions.
    • Chapter 8.03: Stoichiometry of Reactions in Solution
      This page covers stoichiometric calculations for reactions in solution, emphasizing the importance of balancing equations and understanding limiting reactants. It includes examples, such as gold recovery from cyanide and reactions involving potassium dichromate and ethanol. Key steps involve calculating moles using solution volumes and concentrations, as illustrated through various problems.
    • Chapter 8.04: Ionic Equations
      The chemical equation for a reaction in solution can be written in three ways. The overall chemical equation shows all the substances present in their undissociated forms; the complete ionic equation shows all the substances present in the form in which they actually exist in solution; and the net ionic equation is derived from the complete ionic equation by omitting all spectator ions, ions that occur on both sides of the equation with the same coefficients.
    • Chapter 8.05: Precipitation Reactions
      This page provides an overview of precipitation reactions, detailing how soluble ionic compounds can lead to insoluble products upon mixing. It includes definitions, examples, and guidelines for predicting solubility and identifying potential reactions, complemented by exercises on calculating ionic reactions and discussing economic implications, particularly in silver recovery from photographic waste.
    • Chapter 8.06: Acids and Bases
      The page provides an educational overview of acid and base nomenclature, focusing on the ability to identify and name common acids and bases. It explains the differences between oxoacids, which have the H+ ion attached to oxygen atoms, and other acids. Additionally, it covers carboxylic acids and bases like ammonia and amines. The information includes naming rules, examples of common acids and bases, and related conceptual and numerical exercises to reinforce learning.
    • Chapter 8.07: Acid Base Reactions
      This page provides an overview of acids and bases, detailing their definitions, properties, and historical context. It covers the distinctions between strong and weak acids and bases, introduces the concept of amphoteric substances, and discusses neutralization reactions, particularly with antacids. The pH scale and its significance in measuring acidity and basicity are explained, alongside the nature of pH calculations and hydrogen ion concentration.
    • Chapter 8.08: The Chemistry of Acid Rain
      This page addresses the environmental consequences of acid rain, caused by human-induced acid-base reactions from fossil fuel combustion. It details its detrimental effects on natural waters, buildings, and ecosystems, including damage from carbonate reactions and increased aluminum toxicity, harming aquatic life and forest health.
    • Chapter 8.09: Quantitative Analysis Using Titration
      This page explains quantitative analysis through titration techniques in chemistry to determine the concentration of unknown solutions. It covers the titration of oxalic acid with potassium permanganate, detailing the importance of chemical equations and stoichiometry to calculate the mass percentage of calcium oxalate in rhubarb.
    • Chapter 8.10: Oxidation-Reduction Reactions
      This page provides a comprehensive overview of balancing oxidation-reduction (redox) reactions in aqueous solutions, highlighting the process of assigning oxidation states, formulating half-reactions, and ensuring charge and atom balance. It covers both acidic and basic conditions, the activity series of metals for predicting reaction outcomes, and examples of reactions involving metals, acids, and gases.
    • Chapter 8.11: Essential Skills 3
      This page covers base-10 logarithms and their applications in chemistry, detailing how to determine exponents, calculate logarithms using calculators, and the importance of significant figures. It explains properties of logarithms related to multiplication, division, and inverse numbers.
    • Chapter 8.12: End of Chapter Material
      This page covers application problems in chemistry, emphasizing topics like molarity, stoichiometry, and environmental ramifications of chemical reactions. Examples include acetaminophen, lead compounds, and wastewater treatment. It also details titration, baking powder's role in baking, and methods for bromide removal from brine. Furthermore, it discusses marble dissolution in acid rain and lake neutralization with slaked lime.


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