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Chemistry (1)
pH and indicators
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Created by
Leah Murphy
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Cards (12)
K₁
Equilibrium constant for
self-ionisation
of water
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Ionic Product of Water
K₁ = [
H
+][
OH-
]
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Calculate
pH of strong acid
1. Find [H+]
molarity
2. If [H+] = 10^
-5
M,
double
it
3. Find [H+] inverse = 10^
-pH
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Limitations
of pH scale
Only has a range of
0-14
Does not work for
concentrated
solutions
Only works for
aqueous
solutions
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Strong Acid vs Strong Base Titration
1. Find
equivalence
point
2. Use
methyl
orange or
phenolphthalein
indicators
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Acid
Proton
donor
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Base
Proton acceptor
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Bronsted
-Lowry
Acid-base
theory
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Arrhenius
Acid-base
theory
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Weak Acid vs Strong Base Titration
1. Find
equivalence
point
2. No
obvious
equivalence point, no
indicator
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Weak
acid
pH =
-log√
(Ka *
[HA]
)
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Weak
base
pH = 14 - (
-log√
(Kb * [
B
]))
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