Chapter 4: Ionic Theory of Solution and Solubility Roles Flashcards
Electrolyte
A substance that dissolves in water to give an electrically conducting solution. Ionic solids that dissolve in water are electrolytes.
Nonelectrolyte
A substance that dissolves in water to give a nonconducting or very poorly conducting solution.
Strong electrolyte
A solute that completely, or almost completely, ionizes or dissociates in a solution. These ions are good conductors of electric current in the solution.
Example: NaCl –> Na+(aq) + Cl-(aq)
Weak electrolyte
An electrolyte that dissolves in water to give a relatively small percentage of ions. Generally are molecular substances
Example: NH3(aq)+H2O(l) –> NH4^+(aq) + OH-(aq)
Molecular Equation
Which is a chemical equation in which the reactants and products are written as if they were molecular substances, even though they may actually exist in solution as ions.
Complete Ionic Equation
Written in stand-alone ionic form.
Spectator Ions
An ion in an ionic equation that does not take part in the reaction. You can cancel such ions from both sides to express essential reactions that occur.
Strong acid
An acid that ionizes completely ion water and is also a strong electrolyte.
Strong base
Base that is present in aqueous solution entirely as ions, one of which is OH-. A strong electrolyte
Weak base
A base that is only partly ionized in water; it is a weak electrolyte.
Common Strong Acids
HClO4 H2SO4 HI HBr HCl HNO3
Strong Bases
LiOH NaOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Ba(OH)2
Weak Acids
CO(2)H (Carboxylic Acids.)
Rules for Assigning Oxidation Numbers: Elements
Oxidation = 0
Rules for Assigning Oxidation Numbers: Monoatomic Ions
Oxidation number always = 0
Rules for Assigning Oxidation Numbers: Oxygen
Oxidation # = -2 in most compounds. Except in H2O2 and other peroxides, it is 1.
Rules for Assigning Oxidation Numbers: Hydrogen
Oxidation # = 1 unless it is in a binary compound with metal, it is -1.
Rules for Assigning Oxidation Numbers: Halogens
Flourine always = 1
Chlorine, Bromine, Iodine, Astitine = -1 in binary compounds, except when the other element is another halogen above it on PT or is O.
Rules for Assigning Oxidation Numbers: Compounds and Ions
- The sum of the Ox# = 0.
- The sum of the Ox# of polyatomic ion equals the charge on the ion.
Ease of Oxidation
Bottom-Up on PT
Calculating Molarity:
Molarity: Moles of Solute/Liters of the Solution
Concentration
Moles/Volume in Liters
Same as molarity
Monoprotic
One ionizable acid
Diprotic
Two ionizable acids
Intensive property
Bulk property, not depending on the system size or amount of material in the system. Properties include temperature, refractive index, density, hardness. I.e., maintained properties
Extensive properties
Proportional to the amount of material in the system, e.g., energy, entropy, length, mass, particle number, momentum, moles, volume.
Dissociation reaction
Reversible
Decomposition reaction
Irreversible
Titration
Neutralization, often indicated by a color change.
Carbonates and HCO3 with acids produce…
…H2O!
Examples:
CaCO3 + HCl –> CaCl2 + CO2 + H2O
NaHCO3 + HBr –> NaBr + CO2 + H2O
The CO2 and H2O in these equations creates Hydrogen Carbonate (HCO3).
Gas forming reactions for
NH4OH –>
NH3 + H2O
Ammonium, salt + strong base = NH4OH
Example
NH4Cl + NaOH –> H2O + NH3 + NaCl
Gas forming reactions of
H2SO3 –>
SO2 + H2O
Decomposes to create H2SO3
Example
SrSO3 + 2HI –> SrI2 + SO2 + H2O
Gas forming reactions for
H2CO3 –>
CO2 + H2O Produces Hydrogen Carbonates (H2CO3) when added with acid. Examples: CaCO3 + HCl --> CaCl2 + CO2 + H2O NaHCO3 + HBr --> NaBr + CO2 + H2O
Ionic equations
An equation in which ions are specifically shown
Spectator Ion
An ion that appears unchanged on both sides of a reaction arrow
Net ionic equation
An equation that does not include spectator ions.
The gas-forming compounds
NH4OH
H2SO3
H2CO3
Naming acids: SO4^2-
-ate = -ic
Sulfate –> H2SO4 = Sulfuric Acic
Naming acids: NO2^-
-ite = -ous
Nitrite –> HNO2^- = Nitrous acid
Naming acids: Cl^-
-ide = hydro- -ic
Chloride –> HCl^- = Hydrochloric acid
