Test 2 & 3 Flashcards
Arrhenius definition
Bases - increase OH- and Acids - increase H+
Bronsted-Lowry definition
Acid: proton donor, Base: proton acceptor
Conjugate-acid base pair
Two species that differ from each other by one H ion
Amphiprotic
Can donate or receive
Kw
Water ionization constant (10^-14)
pH Calculation
-log[H+]
pOH Calculation
-log[OH-]
Large K favors
products
The weaker the acid
the stronger its conjugate base
Massive Ks give clue of
Neutralization: strong acid + strong base
Weak Acid + Strong Base =
Salt with anion of weak acid’s conjugate base
Weak Acid + Strong Base =
Salt whose anion weak acid’s conjugate base
Strong Acid + Weak Base =
Salt whose cation is conjugate acid of weak base
Strong Acid + Weak Base =
Salt whose cation is conjugate acid of weak base
Weak Acid + Weak Base =
Salt: cation is conjugate acid of weak base; anion: conjugate base of weak acid
Weak Acid + Weak Base =
Salt: cation is conjugate acid of weak base; anion: conjugate base of weak acid
Strong Acids
HCl, HNO3, H2SO4, HClO4
Strong Acids
HCl, HNO3, H2SO4, HClO4
Lewis Acid
Substance accepting a pair of electrons
Lewis Base
Substance donating a pair of electrons
Common ion effect
Limiting of acid/base ionization by adding conjugate
the Na ion
has no effect on pH
acetic acid
CH3COOH
acetic acid
CH3COOH
Solubility & Common Ions
Ignore added salt in ICE table
Q=Ksp
Solution saturated
Q
Not saturated
Q>Ksp
Supersaturated (precipitation will occur)
Reaction Quotient
Q (doesn’t consider solids) –> [products]/[reactants]
Reaction Quotient
Q (doesn’t consider solids) –> [products]/[reactants]
Ligands
Molecules/ions that bond to metal ions
Ligands
Molecules/ions that bond to metal ions
Buffer made of
Weak acid and its conjugate base
