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Chemistry
Acids and bases
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Created by
Lauren Chritmas
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Cards (73)
Topics
covered
Bronsted-Lowry acid base equilibria
Definition and determination of pH
Kw (ion product of water)
Ka for weak acids and bases
pH curves, titrations and indicators
Buffers
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Bronsted-Lowry acids
Proton donors
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Bronsted-Lowry bases
Proton acceptors
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Acids produce hydronium ions (
H3O+
) which make the solution
acidic
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Bases
produce hydroxide ions (OH-) which make the solution
basic
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Examples of strong acids
Hydrochloric
acid
Sulfuric
acid
Nitric
acid
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Examples of weak acids
Carboxylic acids
(e.g. ethanoic acid)
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Examples
of strong bases
Sodium
hydroxide
Potassium
hydroxide
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Examples of
weak
bases
Ammonia
(
NH3
)
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Strong
acids
and
bases dissociate
/ionise almost completely
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Weak acids and bases
dissociate
/
ionise
poorly
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Acid
-base reactions
1.
Protons
are
exchanged
2. Forms a
salt
(
BH+
and A-)
3.
Equilibrium
can shift based on amounts of
reactants
/products added
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Water behaves as a
base
when an
acid
is added to it
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Ionic product of
water
(
Kw
)
Equilibrium constant for the
dissociation
of
water
into H+ and OH- ions
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Kw
= [H+][OH-] = 1 x 10^-14 at
25°C
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In
pure water,
[H
+] = [OH-]
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pH
Logarithmic scale that measures the
concentration
of
H+
ions in solution
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pH
= -log[
H+
]
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pH 0 is very
acidic
, pH 7 is
neutral
, pH 14 is very basic
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Calculating
pH of hydrochloric acid: pH = -log[
H+
]
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pH
A logarithmic scale that measures the
concentration
of
H+
ions in solution
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pH scale ranges from 0 (very
acidic
) to 14 (very basic), with 7 being
neutral
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Calculating
pH
pH = -log[
H+
]
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Calculating [H+] from pH
[H+] = 10^(
-pH
)
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Strong
acids
Fully
dissociate
in
water
, [H+] = [acid]
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Calculating
pH of strong acid
pH =
-log
[
acid
]
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Diprotic
acids
Produce 2 H+ per acid molecule, [H+] =
2
[acid]
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Strong
bases
Fully dissociate in water,
[OH
-
]
= [base]
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Calculating
pH of strong base
Use Kw = [H+][OH-] to find [H+], then pH =
-log[H+]
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Ka
Acid dissociation
constant, used for
weak
acids
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For weak acids, [
H+
] ≠ [acid] so
Ka
must be used
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Calculating pH of weak acid
Use
Ka
expression:
Ka
= [H+]^2 / [acid]
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Calculating [acid] from pH and Ka
Rearrange Ka expression
to solve for [acid]
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Concentration
of methanoic acid
We need to bring up our
k expression
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Rearranging
the equation
Concentration of
methanoic
acid =
h+ squared
/ ka
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ka
Value of
1.77
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Concentration of weak acid is
2.96
x
10
^-3
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To calculate ka, we just put the figures in and work it out, no need to rearrange
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pH
Measure of
acidity
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pKa
Another way of measuring the strength of an acid, using
ka
instead of
concentration
of H+
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