Electrolytes
Compounds such as: Acids, Bases, and Salts. Which when they are dissolved break into the individual ions, allowing for electrical conductivity.
Arrhenius Acids
When dissolved in water it will release H⁺ ions into the solution, increasing the concentration of H⁺ ions.
Arrhenius Bases
When dissolved in water it will release OH⁻ ions (Hydroxide Ions) increasing their concentration in a solution.
Alkalinity
Another term for Bases.
Bronsted-Lowry Acids
Any substance that will donate a Hydrogen Ion. (H+)
Proton(H⁺) Donor
Bronsted-Lowry Bases
Any substance that will accept a Hydrogen Ion. (H+)
Proton(H⁺) Acceptor
Conjugate Acid-Base pairs
When an acid gives up a H⁺ ion, it will form a conjugate Base. And Vise Versa.
Neutralization Reaction
Acid + Base → Salt + Water (SWAB)
Titration
The procedure used to find the unknown molarity of an acid or base, by adding an acid or base of a known molarity until the solution is neutral, then solving for the unknown.
Titration equation
(MA)(VA) = (MB)(VB) (The A’s and B’s are subscripts)
Monoprotic
Acids or bases with only one H⁺ or OH⁻ ions.
Diprotic
Acids or Bases with only two H⁺ or OH⁻ ions.
The pH scale
Expression of how many H+ ions are in a solution. (The Acidity)
pH formula
-log[H⁺]
[ ]
Means concentration
0-6 pH
Acidic pH
7 pH
Neutral pH
8-14 pH
Basic pH
The pOH scale
Expression of how many OH- ions are in a solution. (The Alkalinity)
pOH formula
-log[OH⁻]
0-6 pOH
Basic pOH
7 pOH
Neutral pOH
8-14 pOH
Acidic pOH