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Acids, Bases and PH
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Some Properties of Acids
Produce H+ (as H3O+) ions in water (the hydronium ion is a
hydrogen ion attached to a water molecule)
Taste sour
Corrode metals
Electrolytes
React with bases to form a salt and water
pH is less than 7
Turns blue litmus paper to red “Blue to Red A-CID”
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Some Properties of Bases
Produce OHProduce OH-- ions in water ions in water
Taste bitter, chalkyTaste bitter, chalky
Are electrolytesAre electrolytes
Feel soapy, slipperyFeel soapy, slippery
React with acids to form salts and waterReact with acids to form salts and water
pH greater than 7pH greater than 7
Turns red litmus paper to blue “Turns red litmus paper to blue “BBasic asic BBlue”lue”
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Acid/Base definitions• Definition #1: Arrhenius
Acids:– produce H+ ions (or hydronium ions H3O+)
Bases:– produce OH- ions
(problem: some bases don’t have hydroxide ions!)
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55Arrhenius acid is a substance that produces H+ (H3O+) in water
Arrhenius base is a substance that produces OH- in water
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• Definition #2: Brønsted – Lowry
Acids:– proton donor
Bases:– proton acceptor
A “proton” is really just a hydrogen atom that has lost it’s electron!
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A Brønsted-Lowry acid is a proton donorA Brønsted-Lowry base is a proton acceptor
acidconjugate
basebase conjugate
acid
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The Brønsted definition means NHThe Brønsted definition means NH33 is a is a BASEBASE in in water — and water is itself anwater — and water is itself an ACIDACID
BaseAcidAcidBaseNH4
+ + OH-NH3 + H2OBaseAcidAcidBase
NH4+ + OH-NH3 + H2O
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Conjugate PairsConjugate Pairs
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Learning Check!
Label the acid, base, conjugate acid, and Label the acid, base, conjugate acid, and conjugate base in each reaction:conjugate base in each reaction:
HCl + OHHCl + OH-- Cl Cl-- + H + H22OO HCl + OHHCl + OH-- Cl Cl-- + H + H22OO
HH22O + HO + H22SOSO44 HSO HSO44-- + H + H33OO
++ HH22O + HO + H22SOSO44 HSO HSO44-- + H + H33OO
++
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Lewis acid:- a substance that Lewis acid:- a substance that accepts an electron pair.accepts an electron pair.
Lewis base:- a substance that Lewis base:- a substance that donates an electron pair.donates an electron pair.
Definition #3 – Lewis
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Formation ofFormation of hydronium ion hydronium ion is also an excellent is also an excellent example.example.
Lewis Acids & BasesLewis Acids & Bases
•Electron pair of the new O-H bond Electron pair of the new O-H bond originates on the Lewis base.originates on the Lewis base.
HH
H
BASE
••••••
O—HO—H
H+
ACID
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HNO3, HCl, H2SO4 and HClO4 are strong acids.
Strong and Weak Acids/BasesStrong and Weak Acids/Bases
The strength of an acid (or base) is determined by the amount of IONIZATION.
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• Weak acidsWeak acids are much less than 100% ionized in water. are much less than 100% ionized in water.
One of the best known is acetic acid = CHOne of the best known is acetic acid = CH33COOHCOOH
Strong and Weak Acids/BasesStrong and Weak Acids/Bases
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• Strong Base:Strong Base: 100% dissociated in water.100% dissociated in water.
NaOH (aq) ---> NaNaOH (aq) ---> Na+ + (aq) + OH(aq) + OH- - (aq)(aq)
Strong and Weak Acids/BasesStrong and Weak Acids/Bases
• Weak base:Weak base: less than 100% ionized in waterless than 100% ionized in water
One of the best known weak bases is One of the best known weak bases is ammoniaammonia
NHNH3 3 (aq) + H(aq) + H22O (l) O (l) NH NH44+ + (aq) + OH(aq) + OH- - (aq)(aq)
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Equilibria Involving Equilibria Involving Weak Acids and BasesWeak Acids and Bases
Consider acetic acid, HCConsider acetic acid, HC22HH33OO22 (HOAc) (HOAc)
HCHC22HH33OO22 + H + H22O O H H33OO++ + C + C22HH33OO22 --
AcidAcid Conj. base Conj. base
Ka [H3O+][OAc- ]
[HOAc] 1.8 x 10-5Ka
[H3O+][OAc- ][HOAc]
1.8 x 10-5
(K is designated K(K is designated Kaa for ACID) for ACID)
K gives the ratio of ions (split up), to molecules K gives the ratio of ions (split up), to molecules
(don’t split up).(don’t split up).
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1717Ionization Constants for Acids/Bases Ionization Constants for Acids/Bases
AcidsAcids ConjugateConjugateBasesBases
Increase strength
Increase strength
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The The pH scalepH scale is a way of is a way of expressing the strength of expressing the strength of acids and bases. acids and bases.
Under 7 = acidUnder 7 = acid 7 = neutral 7 = neutral
Over 7 = base Over 7 = base
The pH scale The pH scale
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pH of Common SubstancespH of Common Substances
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2020Calculating the pH
pH = - log [H+](Remember that the [ ] mean Molarity)
Example:
If [H+] = 1 X 10-10
pH = - log 1 X 10-10
pH = - (- 10)
pH = 10
Example:
If [H+] = 1.8 X 10-5
pH = - log 1.8 X 10-5
pH = - (- 4.74)
pH = 4.74
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More Examples:More Examples:
Find the pH of:Find the pH of:
1) A 0.15 M solution of Hydrochloric acid .1) A 0.15 M solution of Hydrochloric acid .
2) A 3.00 X 102) A 3.00 X 10-7-7 M solution of Nitric acid . M solution of Nitric acid .
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More About WaterMore About WaterHH22O can function as both an ACID and a BASE.O can function as both an ACID and a BASE.
In pure water there can beIn pure water there can be AUTOIONIZATIONAUTOIONIZATION
Equilibrium constant for water = KEquilibrium constant for water = Kww
KKww = [H = [H33OO++] [OH] [OH--] =] = 1.00 x 101.00 x 10-14-14 at 25 at 25 ooCC
OH-
H3O+
OH-
H3O+
In a In a neutral neutral solution [Hsolution [H33OO++] = [OH] = [OH--] = 1.00 x 10] = 1.00 x 10-7-7 M M
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2424pOH
• pOH does not really exist, but it is useful for pOH does not really exist, but it is useful for changing bases to pH.changing bases to pH.
pOH = - log [OHpOH = - log [OH--]]Since pH and pOH are on opposite ends,Since pH and pOH are on opposite ends,
pH + pOH = 14pH + pOH = 14
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pHpH [H+][H+] [OH-][OH-] pOHpOH
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2626Examples:Examples:
1- What is the pH of :1- What is the pH of :
0.0010 M NaOH solution?0.0010 M NaOH solution?
soln:soln:
[OH-] = 0.0010 (or 1.0 X 10[OH-] = 0.0010 (or 1.0 X 10-3-3 M) M)
pOH = - log 0.0010pOH = - log 0.0010
pOH = 3pOH = 3
pH = 14 – 3 = 11pH = 14 – 3 = 11
OR:OR:
KKww = [H = [H33OO++] [OH] [OH--]]
[H[H3OO++] = 1.0 x 10] = 1.0 x 10-11-11 M M
pH = - log (1.0 x 10pH = - log (1.0 x 10-11-11) = 11.00) = 11.00
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[OH[OH--]]
[H[H++]] pOHpOH
pHpH
1010 -pOH
-pOH
1010 -pH-pH-Log[H
-Log[H++]]
-Log[OH
Log[OH
--]]
14 -
pOH
14 -
pOH
14 -
pH
14 -
pH
1.0
x 10
1.0
x 10-1
4-14
[OH[O
H-- ]]
1.0
x 10
1.0
x 10-1
4-14
[H[H
++ ]]
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The OH- ion concentration of a blood sample is 2.5 x 10-7 M. What is the pH of the blood?
More Examples:
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