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Chemistry
Chemistry unit 1
unit 1.7 simple equilibria and acid based reaction
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Cards (14)
reversible
reaction in which the conversion of
reactants
to
products
and conversion of products to reactants occurs simultaneously
dynamic equilibrium
occurs in a closed system when the rate of the
forward reaction
is equal to the rate of the
reverse reaction
and all
concentration
remain the same
le chateliers principle
states that when a system in
dynamic equilibrium
is subjected to change, the position of equilibrium will shift to
minimise
change
3 factors affecting position of equilibrium
concentration
temperature
pressure (only in reactions involving gases)
temperature
increaes in temperature will always favour
endothermic
as temp will decrease as heat is absorbed
decrease temp will always favour
exothermic
as temp will increase as heat is released
equilibria constant
Kc
=
[
C
]
[
D
]
[
A
]
[
B
]
\frac{\left[C\right]\left[D\right]}{\left[A\right]\left[B\right]}
[
A
]
[
B
]
[
C
]
[
D
]
CD=
products
AB= reactants
Kc= 1
dynamic
equilibrium
pH
measure of how much
hydrogen
is in a
solution
small changes are actually a big difference
pH
=
log
10
\log_{10}
lo
g
10
[
H
+
(
a
q
)
]
\left[H^+(aq)\right]
[
H
+
(
a
q
)
]
[
H
+
(
a
q
)
]
\left[H^+(aq)\right]
[
H
+
(
a
q
)
]
=
1
0
−
p
H
10^{-pH}
1
0
−
p
H
strong acid
any acid thats not a
carboxylic acid
proton
hydrogen ion
monoprotic
acid
with only one
hydrogen
strong acids completely dissociate
concentration of
hydrogen
will be the same as the
original acid concentration
acid dissociation constant
Ka
,
equilibria
constant for acids