Acid Base Chemistry
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Arrhenius acid
Acids that produce H+
Arrhenius Base
Bases that produce OH-
Lewis acids
Atom or compounds that accept a pair of electrons to form a covalent bond
Lewis bases
Atom or compound that donates a pair of electrons to form a covalent bond
Lowry-Bronsted Acid
are proton donors
Lowry-Bronsted Bases
are proton acceptors
Amphoteric
Molecules that donate or accept protons in response to whatever else is in solution
Strong acid and bases
Completely dissociates in solution
Strong acids
HCl, HBr, HI, HNO3, H2SO4, HClO4
Strong Bases
LiOH, NaOH, KOH
Weak acids and bases
Acids that undergo partial, reversible dissociation
Weak acids
An acid that isn’t one of the six strong acids
Weak base
A base that isn’t one of the strong bases
Conjugate acid base pair
A conjugate pair is made up of two molecules that have identical molecular formulas, except that one of them has an additional H+
Conjugate acid
A member of a conjugate pair having an extra H+
Conjugate base
A member of a conjugate pair having one fewer H+
The conjugate acid of a strong base is:
Neutral
The conjugate base of a strong acid is:
Neutral
The conjugate acid of a weak base is:
An acid
The conjugate base of a weak acid is:
A base
Buffer
A buffer must consist of a conjugate pair of a weak acid and weak base
Henderson-Hasselbalch Equation
pH = pKa + log([A-]/[HA]) pOH = pKb + log([HA]/[A-])
Important rule about buffers
Diluting or concentration a buffered solution DOES NOT change its pH
Titrant
Strong base or acid of known identity and concentration that is added to an unknown acid or base solution