BackChapter 4: Reactions in Aqueous Solution – Solutions and Electrolytes
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Chapter 4: Reactions in Aqueous Solution
Objectives
Define and identify compounds as acids, bases, and electrolytes or nonelectrolytes.
Describe precipitation/double displacement and acid-base neutralization reactions and predict their products.
Calculate solute molarity and relate it to moles and volume.
Perform dilution calculations to achieve a desired molarity.
Use stoichiometry to calculate moles, masses, and volumes of substances in solution.
Solutions
Definition and Components
A solution is a homogeneous mixture of two or more pure substances. The solvent is the substance present in the greatest quantity, and the solute is the substance dissolved in the solvent.
Solvent: The component that dissolves the solute (e.g., water in saltwater).
Solute: The component that is dissolved (e.g., salt in saltwater).
Solution: The resulting homogeneous mixture (e.g., saltwater).
Example: In a sugar-water solution, water is the solvent and sugar is the solute.
Electrolytes
Definition
Electrolyte: A substance whose aqueous solution contains ions and conducts electricity.
Nonelectrolyte: A substance that does not form ions in solution and does not conduct electricity (e.g., sucrose, C12H22O11).
Types of Electrolytes
Strong Electrolytes: Dissociate completely in solution, producing only ions. They are good conductors of electricity.
Weak Electrolytes: Dissociate partially in solution, so both molecules and ions are present. They are poor conductors of electricity.
Nonelectrolytes: Do not dissociate in solution; exist only as molecules and do not conduct electricity.
Classification Table: Electrolyte Strength
Strong Electrolyte | Weak Electrolyte | Nonelectrolyte | |
|---|---|---|---|
Acids | Strong acids (see Table 4.2) | Weak acids (H...) | None |
Bases | Strong bases | Weak bases (NH3) | All other bases |
Other Compounds | Most soluble ionic salts | Some molecular compounds | Most molecular compounds (e.g., sugars) |
Visual Representation
Strong Electrolyte: Solution contains only ions (e.g., NaCl in water).
Weak Electrolyte: Solution contains both molecules and some ions (e.g., acetic acid in water).
Nonelectrolyte: Solution contains only molecules (e.g., sugar in water).
Example: Sodium chloride (NaCl) is a strong electrolyte; ammonia (NH3) is a weak electrolyte; glucose (C6H12O6) is a nonelectrolyte.
Additional info: The degree of dissociation determines the conductivity of the solution. Strong electrolytes are typically soluble ionic compounds and strong acids/bases, while weak electrolytes are weak acids/bases. Nonelectrolytes are usually covalent compounds that do not ionize in water.
