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15 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Acid = Proton Donor
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The definition of a Bronstead-Lowry Acid is a Proton Donor
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Base = Proton Acceptor
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The definition of a Bronstead-Lowry base is a Proton Acceptot
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Acid-Base reaction = Transfer of a Proton
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The definition of a Bronstead-Lowry acid-base reaction is the transfer of a proton from one species to another
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Monoprotic Acid
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Donates one proton - e.g. HCl or HNO3
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Diprotic Acid
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Donates 2 protons e.g. H2SO4
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Definition of pH:
pH = -log [H+] |
Always give to 2 Decimal Places
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[H+] = 10(-pH)
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Give to 3 Significant Figures
E.g. pH = 1 so 10 (-1) = 0.1 so [H+] is 0.1 |
Round brackets mean to the power of
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Dilution of a strong acid
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Work out number of moles in original solution. Use this to work out the new concentration using the new volume
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Number of moles = concentration x volume
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pH of a strong base
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1. Work out concentration of [OH-]
2. Use Kw ^ [OH-] to work out concentration of [H+] 3. Put [H+] into pH expression |
pH should be between 12-14 approximately
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Work out [OH-] concentration in a strong base
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1. Get [H+] from [H+] = 10 (-pH)
2. Put into [OH-] Kw ^ [H+] |
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Dilution of a strong base
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1. Work out moles in original solution
2. Work out new concentration by moles ^ new volume 3. Work out [H+] from [H+] = Kw ^ [OH-] 4. Put into pH expression |
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Reaction between a strong acid and a strong base
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1. Calculate moles of [H+] and [OH-]
2. Calculate moles in excess ( biggest number) 3. Convert excess moles back into concentration using the combined volume of H+ and OH- 4. Calculate pH |
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Weak Acids
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Ka = [H+](2) ^ [HA]
[H+] = square route of Ka x [HA] |
HA is the original concentration of the acid as dissociation is negligible.
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Bigger Ka = stronger acid
Bigger pKa = weaker acid |
pKa = -log(Ka)
Ka = 10 (-pKa) |
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Strong acids fully dissociate
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Weak acids partially dissociate
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Weak acids between pH 3-4
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