Acids and Bases

Lewis Theory

Lewis Theory

An acid is an electron pair acceptor and a base is an electron pair donor

Arrhenius Theory

Acids are substances that produce H+ ions when dissolved and bases produce OH- ions when dissolved

Bronsted-Lowry Theory

acids donate H+ (protons) and bases accept H+

amphoteric substance

a substance that can behave either as an acid or as a base depending on the situation

strong acids

HCl HBr HI H2SO4 HCLO4 HNO3

strong bases

LiOH NaOH KOH RbOH CsOH (alkali metals)

Ca(OH)2 Sr(OH)2 Ba(OH)2 (castro bear)

partially

weak acids and bases (fully/partially) dissociate in solution

Ka of a weak acid

Ka<1

Ka of a strong acid

greater than 1

Kb of a weak base

Kb<1

conjugates are (opposite/same) in strength

opposite

pH

a measure of hydronium ion concentration

buffer solution

a solution made from a weak acid and its conjugate base that neutralizes small amounts of acids or bases added to it

titration

a measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is complete

equivalence point

point where moles H+ and mole OH- are equal

end point

point where indicator changes color to indicate the rxn in complete

per-______-ate

+1 oxygen

________-ite

-1 oxygen

polyatomic ion mneumonic

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