46 Cards in this Set
| Front | Back |
|---|---|
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is Kc really small or really big when the equation is reactant favored?
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really small
|
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if x (change) is less than 5% of the smallest starting concentration then the assumption is?
|
zero
|
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acid
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H+ donor
|
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base
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H+ acceptor
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acid-base reaction
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proton transfer
|
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neutralization reaction
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mix acid and base
|
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every acid has a
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conjugate base
|
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every base has a
|
conjugate acid
|
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conjugate base
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what's left over when the acid is done
|
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strongest base in H20
|
OH-
|
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amphoteric
|
can be an acid or a base
|
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which side is favored? the weaker or the stronger?
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weaker
|
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when Kc is really small does the reaction lay far to the left or far to the right?
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far to the left
|
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in H2O solution, all strong acids are
|
the "same"
H30+
|
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is water an acid or a base?
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can be both
|
|
Kc for water
|
[H30+][OH-]
= 1.0 x 10^-14
= Kw
|
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pH =
|
-log[H+]
|
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pOH =
|
-log[OH-]
|
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[H+]=[OH-]
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neutral
|
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pH + pOH =
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14
|
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do strong acids completely ionize?
|
yes
|
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are strong acids every involved in equilibrium?
|
no
|
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6 strong acids
|
HCl
HBr
HI
HClO4
HNO3
H2SO4
|
|
incomplete dissociation
strengths are not leveled in H2O
equilibrium
|
weak acids
|
|
molecular form
|
acid before it gives up H+
|
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pH depends on these 2 things
|
concentration and Ka
|
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are acid-base reactions very fast or very slow?
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very fast
|
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diluted weak acids become more generous
|
have less H+ to give but still give a greater percentage
|
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does a weak acid go to the right a lot?
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no
|
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polyprotic acid
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donates 2 or more protons
|
|
strong bases
|
strong electrolytes
ionize completely
group 1 metal hydroxide and group 2a hydroxides
|
|
8 strong bases
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LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Ba(OH)2
Sr(OH)2
|
|
every base has to have?
|
lone pair(s)
|
|
lewis base
|
electron pair donor
|
|
lewis acid
|
electron pair acceptor
|
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there is an inverse relationship between a weak base and
|
conjugate acid
|
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which is the stronger base? F- or Cl-?
|
F-
|
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which is the stronger acid? NH4+ or H2O?
|
NH4+
|
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2 options for a buffer
|
a weak acid with added conjugate base
a weak base with added conjugate acid
|
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do buffers resist changes in pH?
|
yes
|
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more ions =
|
more soluable
|
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the more ion pairs you form,
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the more soluble the salt gets
|
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Q > K
|
reaction runs left
|
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Q < K
|
reaction runs right
|
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supersaturated
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holding more ions than it can
|
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unsaturated
|
solution could dissolve some more
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CHM 104: EXAM 4