9 ch110 acids & bases
TRANSCRIPT
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9 - 1CH110: Chpt 9
Acids and Bases
Acids & Bases
Ionization of Water
pH
Acid-Base Reactions
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9 - 2CH110: Chpt 9
Remember Electrolytes
Na+
NaCl
Na+Cl-
Cl-
C6H12O6
C6H12O6
C6H12O6
Ionic Covalent
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9 - 3CH110: Chpt 9
Acids
H+
HC2H3O2
H+C2H3O21-
C2H3O21-
H+
H-Cl
H+Cl
-
Cl-
Weak Strong
Lots of IonsOnly a few Ions
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9 - 4CH110: Chpt 9
Acids
Acid = gives hydrogenionsin water
H+
H-Cl
H
+
Cl-
Cl-
HCl
H+ + Cl-
hydrogen ion
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9 - 5CH110: Chpt 9
Acids
H-Cl + H-O-H
+ Cl-
hydronium ion
H O H
H
+H
OH
H
+ Cl-
H-Cl
Acid = gives hydrogenionsin water
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9 - 6CH110: Chpt 9
CommonAcids
Battery AcidStomach Acid
Coca Cola
Carbonated WaterVinegar
Citrus fruitsVitamin C
Grapes
Aspirin
H2SO4HCl
H3PO4
H2CO3HC2H3O2H
3C
6O
7H
8
HC6O6H7H2C4O6H4H2C9O4H8
SulfuricAcidHydrochloricAcid
PhosphoricAcid
CarbonicAcid
AceticAcidCitricAcidAscorbicAcidTartaricAcid
Acetyl SalicylicAcid
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7/419 - 7CH110: Chpt 9
Naming Acids
Binary Acids:Hydrogen & non metal.
ex. HCl HBr H2S
hydro- ______________-ic Acid
HCl Hydrochloric acid
H2S Hydrosulfuric acid
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8/419 - 8CH110: Chpt 9
Naming Oxygen containing acids
Oxoacids:Hydrogen, oxygen, and a nonmetalex. HNO3 HNO2 H2SO4
The higher number of Os______________-ic AcidHNO3 = Nitric Acid
The lower number of Os______________ -ous ending.HNO2 = NitrousAcid
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9/419 - 9CH110: Chpt 9
THE COMMON -IC ACIDS
H2SO4 SULFURIC ACID
HNO3 NITRIC ACID
H2CO3 CARBONIC ACID
H3PO4 PHOSPHORIC ACID
HClO3 CHLORIC ACID
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10/419 - 13CH110: Chpt 9
H2SO4HCl
H3PO4
H2CO3HC2H3O2H
3C
6O
7H
8
HC6O6H7H2C4O6H4H2C9O4H8
CommonAcids
Battery AcidStomach Acid
Coca Cola
Carbonated WaterVinegar
Citrus fruitsVitamin C
Grapes
Aspirin
Strong100% ionizationStrong electrolyte
WeakPartial ionizationWeak electrolyte
Taste sour
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11/419 - 14CH110: Chpt 9
Acids
H-Cl + H-O-H
+ Cl
-
H O H
H
+
HO
H
H
+Cl-
H-Cl
H+
HC2H3O2
C2H3O21-
HC2H3O2
H-C2H3O2 + H-O-HH
OH
H
+ + C2H3O2-
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12/419 - 15CH110: Chpt 9
Acids
H+
H-Cl
H+Cl-
Cl-
Weak Strong
Lots of IonsOnly a few Ions
H+
HC2H3O2
C2H3O21-
HC2H3O2
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Base =gives hydroxideionsin water.(Arrhenius definition)
=takes hydrogen ionsin water.(Bronsted-Lowry definition)
Bases
NaOH
Na+ + OH-OH-
OH-
Na+
Na+
NaOH
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Common Bases
Lye, DranoPotash
Cleaners
Milk of Magnesia
Baking soda
Tums /RolaidsLimestone, shells
SoapsDetergents
NaOHKOH
NH3 or NH4OH
Mg(OH)2NaHCO3
CaCO3NaC16O2H31NaC12O4H25S
Sodium HydroxidePotassium Hydroxide
Ammonia
Magnesium Hydroxide
Sodium BicarbonateCalcium Carbonate
Sodium Palmitate
Sodium LaurylSulfate
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Common Bases
Lye, DranoPotash
Cleaners
Milk of Magnesia
Baking soda
Tums /RolaidsLimestone, shells
SoapsDetergents
NaOHKOH
NH3 or NH4OH
Mg(OH)2NaHCO3
CaCO3NaC16O2H31NaC12O4H25S
Strong100% ionizationStrong electrolyte
WeakPartial ionizationWeak electrolyte
Taste bitterFeel Slippery
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HClO4
H2SO4HIHBrHCl
HNO3
Perchloric Acid
Sulfuric AcidHydroIodic Acid
Hydrobromic Acid
Hydrochloric Acid
Nitric Acid
Strong Acids
LiOH
NaOHKOH
Ca(OH)2
Lithium Hydroxide
Sodium HydroxidePotassium Hydroxide
Calcium Hydroxide
Strong Bases
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17/419 - 20CH110: Chpt 9
HNO3 + H2O H3O+ + NO3
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Water is Amphoteric
Aciddonates
a proton
Basetakes
a proton
NH3 + H2O NH4+ + OH-
NH3
Aciddonatesa proton
Basetakes
a proton
HNO3
Aciddonatesa proton
Basetakes
a proton
Acid Base
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NH3 + H2O NH4+ + OH-
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H2CO3 + H2O H3O+ + HCO3
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Conjugate Acid - Base Pairs
conjugate pair
ACID BASE conj acid conj base
conjugate pair
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9 - 23CH110: Chpt 9
H2O
Conjugate Acid - Base Pairs
Acid - BaseH2CO3 HCO3
1-
CO32-
H3O+ HO1-
H3PO4 H2PO41- PO4
3-HPO42-
Acid - Base
Acid - Base
Acid - Base
Acid - BaseAcid - BaseAcid - Base
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9 - 24CH110: Chpt 9
H2O + H2O HO- + H3O
+
Ionization of Water
conjugate pair
ACID BASE conj acidconj base
conjugate pair
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9 - 25CH110: Chpt 9
H2O + H2O HO- + H3O
+
Ion product constant of Water
ACID BASE conj acidconj base
0.000,000,1M= 1 x 10-7M
0.000,000,1M= 1 x 10-7M
Neutral: if [H3
O+] = [OH-]
Acidic: if [H3O+] > [OH-]
Basic: if [H3O+] < [OH-]
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9 - 26CH110: Chpt 9
H2O + H2O HO- + H3O
+
Ion product constant of Water
ACID BASE conj acidconj base
0.000,000,1M= 1 x 10-7M
0.000,000,1M= 1 x 10-7M
Kw = [H3O+] [OH-] = 1 x 10-14
[H3O+
] [OH-
] = (1 x 10-7
)(1 x 10-7
) =1 x 10-14
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9 - 27CH110: Chpt 9
pH = 1 x 10 -pH pH = - log [H+]
HCl
HC2H3O2
H2O
NaOH
0.000,000,1 M= 1 x 10 -7 M
[H+]
0.000,1 M= 1 x 10 -4 M
0.000,000,000,001 M
= 1 x 10 -12 M
100 M= 1 x 10 2 M
7
4
12
-2
90.000,000,001 M= 1 x 10 -9 MNH3
Neutral
Acidic
Basic
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9 - 28CH110: Chpt 9
pH = 1 x 10 -pH pH = - log [H+]
HCl
HC2H3O2
H2O
NaOH
0.000,000,1 M= 1 x 10 -7 M
[H+]
0.000,1 M= 1 x 10 -4 M
0.000,000,000,001 M
= 1 x 10 -12 M
100 M= 1 x 10 2 M
7
4
12
-2
90.000,000,001 M= 1 x 10 -9 MNH3
Neutral
Acidic
Basic
Citric Acid0.000,76 M
= 7.6 x 10 -4 M
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9 - 29CH110: Chpt 9
pH = 1 x 10 -pH pH = - log [H+]
HC2H3O2
[H+]
0.000,1 M= 1 x 10 -4 M 4
3 - 4
Citric Acid
0.001 M= 1 x 10 -3 M
0.000,76 M= 7.6 x 10 -4 M
3
pH =- log (7.6 x 10 -4)
= 3.1
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9 - 30CH110: Chpt 9
pH [H+]= 1 x 10 -pH pH = - log [H+]
0.000,000,04 M= 4.0 x 10 -8 M
9.3
8.5BakingSoda
= 1 x 10 -8.5 M= 3.2 x 10 -9 M
pH =- log (4.0 x 10 -8)
= 7.4
Cleaner = 1 x 10-9.4 M
= 5.0 x 10 -10 M
Blood
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9 - 31CH110: Chpt 9
pH of somecommon materials
Substance pH
1 M HCl 0.0
Lemon juice 2.3
Coffee 5.0
Pure Water 7.0
Blood 7.35-7.45
Milk of Magnesia 10.5
1M NaOH 14.0
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9 - 35CH110: Chpt 9
pH paper:
Litmuspaper:
Anthocyanins:red cabbage, cranberries, roses
Phenolphthalein:Turmeric:
pH meter:
Pigments:
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9 - 36CH110: Chpt 9
Indicator examples
Acid-base indicators undergo a color changeat a known pH.
bromthymol blue
phenolphthalein methyl red
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9 - 37CH110: Chpt 9
Acid Reactions
HCl + Zn
Cl-
Zn
H+
ZnCl2 + H2Acid Metal Salt
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9 - 38CH110: Chpt 9
Activity series of metals
potassiumsodium
calcium
magnesiumaluminum
zincchromium
ironnickel
tinlead
coppersilver
platinumgold
incre
asing
rea
ctivity
Reacts violently with cold water
Reacts slowly with cold water
Reacts very slowly with steambut quite reactive in acid
Reacts moderately with high
levels of acid
Unreactive in acid
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9 - 39CH110: Chpt 9
Acid-Base Reactions
HCl + NaOH
OH-
Cl-
Na+
H+
NaCl + HOHAcid Base Salt Water
Neutralization:Strong Acid
+
Strong Base
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9 - 40CH110: Chpt 9
Acid-Base Reactions
H2SO4 + KOH
OH-
SO4-2
K+
H+
K2SO4 + HOHAcid Base Salt Water
22
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9 - 42CH110: Chpt 9
Acid-Base Reactions
Acid Rain on Marble
Cream of Tartar & Baking Soda
HC2H3O2 + NaHCO3 NaC2H3O2 + H2CO3
H2O + CO2(g)
Acid Base Salt
H2SO4 + CaCO3 CaSO4 + H2CO3
H2O + CO2(g)
Acid Base Salt
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9 - 43CH110: Chpt 9
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9 - 44CH110: Chpt 9
Acid-Base Reactions
Lemon on FishH3C6H8O7 + R-NH2 C6H8O7
1- + R-NH31+
Acid BaseSalt
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9 - 45CH110: Chpt 9
Buffers Weak acid + Weak base
Resists change in pH
NaC2H3O2HC2H
3O
2
NaC2H3O2 + H2O
HClNaOH
NaCl + HC2H3O2
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9 - 53CH110: Chpt 9
pOH examples
Determine the following:pOH = -log[OH-]or 14 - pH
1. pOH of 1.7x10-4 M NaOH
pOH = 3.8 pH = 10.22. pOH of 5.2x10-12 M H+
pH = 11.2 pOH = 2.8
3. [OH-] , if the pH is 4.5pOH = 9.5[OH-] = 3.2x10-10 M
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pH scale
A log based scale used to keep track of thelarge change important to acids and bases.
14 7 0
10-14 M 10-7 M 1 MVery Neutral VeryBasic Acidic
When you add an acid, the pH gets smaller.
When you add a base, the pH gets larger.