Transcript Acids And Bases

Acids And Bases
By: Spenser Oriot and Sam Ready
Acids
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pH <7
[H+]> 10-7M
10-6M pH 6
10-5 pH5…
Arrhenius Definition
– HyX where Xy- is an anion
– Releases H+ into solution
Acids (continued)
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Bronsted-Lowrey
– “proton donor”
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Lewis
– “electron acceptor”
Acids (continued)
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Ide (hydro______ic)
– HCl
– H2S
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hyrdrochloric
hyrdosulfuric
Ate (______ic)
– HClO3
– H2SO4
– H3PO4
– HNO3
Chloric
Sulfuric
Phosporic
Nitric
Acids (continued)
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Ite (_____ous)
HClO2
Chlorous
H2SO3
Sulfurous
HNO2
Nitrous
Six Strong Acids
HCl HNO3
HBr
H2SO4
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HI
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acid)
HClO4
H2SeO4(next
strongest
Bases
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pH> 7
[OH-]<10-7M
Arrhenius Definition
– M(OH)x where Mx+ is cation
– Releases OH- into solution
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Bronsted-Lowrey
– “proton acceptor”
Bases (continued)
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Lewis
– “electron donor”
Amphiprotic Substances
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Polyprotic acids
Many protons
Amphiprotic
Can accept and donate protons
Base and Acid
Ex: H3PO4 + H2O <> H3O+ + H2PO4A
B
CA
CB
Amphiprotic substances
(cont)
 H2PO4B
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+ HCl <> H3PO4 +ClA
 H2PO4- + NaOH <>
A
B
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 Ka= [CA][CB]/[A]
 pH + pOH = 14
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Kb=[CA][CB]/[B]
pH =-log(H+)
CA
CB
H2O + HPO42- + Na+
CA
CB
Buffers
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HA + H2O <> H3O+ + AKa= [H3O+][A-]/{HA]
-log([H3O+]) + (-log{[A-]/[HA]}) = -logKa
pH = pka + log [A-]/[HA]
Henderson- Hasselbach equation
pH = Pka + log [A-]/[HA]
pOH= Pkb + log [HB]/[B-]