# ACIDS, BASES AND BUFFERS

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• Created by: abc
• Created on: 21-12-17 00:34
Molarity
M = g/L / g/mol
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Normality
N = Eq/L
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Equivalence
Eq = mol x valence
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pH of a strong acid
pH = -log[H+/H3O+]
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pOH of a strong base
pOH = -log[OH-]
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Degree of ionisation (qualitative)
α = [ionised]/([unionised] + [ionised])
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Degree of ionisation of weak acids
α (%)=100/((1+〖10〗^(pKa-pH) ) )
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Degree of ionisation of weak bases
α (%)=100/((1+〖10〗^(pH-pKa) ) )
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pH of a weak acid
pH = 1/2 pKa - 1/2 log[HA]
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pH of a weak base
pH = 1/2 pKa + 1/2 log[B] + 1/2 pKw
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Dissociation of water
pKw = pH + pOH = 14 (at 25℃)
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Henderson-Hasselbalch equation (pH of acidic buffer)
pH = pKa + log([salt] / [acid])
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pH of a basic buffer
pH=pKw-pKb+ log⁡〖[Base]/[Salt] 〗
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Buffer capacity
β=∆B/∆pH
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Slyke's equation
β = 2.303 × C × (Ka×[H3O+])/(Ka+H3O+ ] )^2 where C is the total buffer concentration
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Maximum buffer capacity
βmax=0.576C
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## Other cards in this set

Normality

N = Eq/L

### Card 3

Equivalence

#### Back ### Card 4

#### Front

pH of a strong acid

#### Back ### Card 5

#### Front

pOH of a strong base

#### Back 