Chapter 8 Review

Solution

A homogeneous mixture that has two components, (solute/solvent)

Solute

The dissolved substance in a solution (smaller amount)

Solvent

The major component in a solution

Molarity (M)

moles of a solute/liters of solution

Mass percent

m/m

Volume Percent

v/v

Mass/Volume Percent

m/v

Electrolytes

Substances which dissolve in water to produce conducting solutions of ions

Nonelectrolytes

Substances which do not produce ions in aqueous solutions (do not conduct electricity)

Strong Electrolytes

Compounds that dissociate to a large extent into ions when dissolved in water

Weak Electrolytes

Compounds that dissociate to a small extent into ions when dissolved in water

Electrolytes in Aqueous Solution (Strong Acids)

• Hydrochloric Acid (HCl)

• Hydrobromic Acid (HBr)

• Hydroiodic Acid (HI)

• Perchloric Acid (HClO₄)

• Nitric Acid (HNO₃)

• Sulfuric Acid (H₂SO₄)

Electrolytes in Aqueous Solutions (Weak Electrolytes)

• Acetic Acid (CH₃CO₂H)

• Hydrofluoric Acid (HF)

• Phosphoric Acid (H₃PO₄)

Nonelectrolytes

• Water (H₂O)

• Methyl Alcohol (CH₃OH)

• Ethyl alcohol (C₂H₅OH)

• Sucrose (C₁₂H₂₂O₁₁)

• Most compound of carbon (organic compounds)

Precipitation Reactions

Processes in which soluble ionic reactant yield an insoluble solid product that falls out of solution

Precipitate

Solid product formed from a reaction in soluiton.

Solubility

States how much of a compound will dissolve in a given amount of solvent at a given temperature

Molecular Equation

All substances in the chemical equation are written using their complete formulas as if they were molecules

Ionic Equation

All of the strong electrolytes are written as ions

Spectator ions

Ions that undergo no change during the reaction and appear on both sides of the reaction arrow

Molecular Equation

Chemcial equation showing the complete, neutral formulas for every compound in a reaction

Complete ionic equation

Chemical equation showing all of the species as they are actually present in solution

Net Ionic Equation

Only the ions undergoing change are shown

Acid (Arrhenius)

A substance that dissociates in water to produce hydrogen ions, H¹⁺

Base (Arrhenius)

A substance that dissociates in water to produce hydroxide ions, OH^1-

Strong Electrolytes

Strong acids and strong bases are ____________

Weak Electrolytes

Weak acids and weak bases are ________

Oxidation

The loss of one or more electrons by a substance, whether element, compound, or ion

Reduction

The gain of one or more electrons by a substance, whether element, compound, or ion

Oxidation Number (State)

A value which indicates whether an atom is neutral, electron-rich, or electron poor

Zero

The sum of the oxidation numbers is ___ for a neutral compound and is equal to the net charge for a polyatomic ion.

Reducing Agent

• Causes reduction of some other substance

• Itself loses one or more electrons

• Itself undergoes oxidation

• Oxidation number of atom increases

Oxidizing Agent

• Causes oxidation of some other substance

• Itself gains one or more electrons

• Itself undergoes reduction

• Oxidation number of atom decreases

Monoprotic

1 dissociable hydrogen

Diprotic

2 dissociable H

Triprotic

3 dissociable H