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15 Cards in this Set

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Bronsted-Lowry Acid
Lewis Acid
Arrhenius Acid
proton donor
e- pair acceptor
produces H+
Bronsted-Lowry Base
Lewis Base
Arrhenius Base
proton acceptor
e- pair donor
produces OH-
If the anion ends in -ite, it has ____ oxygen atoms and its acid should end with ___

If the anion ends in -ate, it has ____ oxygen atoms and its acid should end with ___
1 or 2, -ous acid

more than 2, -ic acid
definition of pH and its generic equation

definition of pOH and its generic equation
a measure of H+ concentration
pH=-log[H+]

a measure of OH- concentration
pOH==log[OH-]
Kw definition and equation
water dissociation constant, a constant that describes an equilibrium reaction.

Kw=[H+][OH-]=10^-14
Rewrite the Kw equation in logarithmic form

and another form
pH+pOH=14

Kw=Ka x Kb= 1 x 10^-14
Log x^n = _____

Log 10^x = _____

-Log 10^-x = _____
nLog x

x

x
Common strong Acids
Hydrogen halides:HCl,HBr,HI
Oxyacids of halogens:HClO3,HClO4,HBrO3,HBrO4 ,HIO3,HIO4
Sulfuric acid:H2SO4
Nitric acid:HNO3
Common strong Bases
NaOH
KOH
CsOH
Ca(OH)2
*mostly from the alkali group and some alkaline group
the difference b/n strong acids/bases and weak acid/bases
strong acids and bases dissociate completely into their component ions in aq solution.
weaker species partially dissociate.
common weak acids
Formic HCOOH
Acetic CH3COOH
Trichloroacetic CCl3COOH
Hydrofluoric HF
Hydrocyanic HCN
Hydrogen
sulfide H2S
Water H2O
Conjugate acids
of weak bases NH4+
common weak bases
ammonia NH3
trimethyl
ammonia N(CH3)3
pyridine C5H5N
ammonium
hydroxide NH4OH
water H2O
HS- ion HS-
conjugate bases
of weak acids e.g.:
HCOO-
HA+H20->H30+ + A-

Ka equation
[H30+][A-]/[HA]

*only for aq molecules
define conjugate acid

define conjugate base
the acid formed when a base gains a proton

formed when an acid loses a proton
Neutralization reaction

The reverse of this is called _____
HA + BOH -> BA + H20

hydrolysis