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Acids and Bases
http://www.unit5.org/chemistry/Acids.htm
http://www.chem1.com/acad/webtext/abcon/index.html7/29/2019 Acids and Bases (Muy Bueno)
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http://www.chalkbored.com/lessons/chemistry-11/acid-bronsted.ppt
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Guiding Questions
What is an acid?
What makes acids dangerous?
Is acid rain an issue for us?
What does pH balanced mean?
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pH scale
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
ACID BASE
NEUTRAL
Each step on pH scale represents a factor of 10.
pH 5 vs. pH 6 (10X more acidic)pH 3 vs. pH 5 (100X different)
pH 8 vs. pH 13 (100,000X different)
: measures acidity/basicity
10x10x10x100x
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pH scale
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
ACID BASE
NEUTRAL
Each step on pH scale represents a factor of 10.
pH 5 vs. pH 6 (10X more acidic)pH 3 vs. pH 5 (100X different)
pH 8 vs. pH 13 (100,000X different)
: measures acidity/basicity
10x10x10x100x
Sren Sorensen(1868 - 1939)
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Acid vs. Base
Acid
pH > 7
bitter taste
does not
react with
metals
pH < 7
sour taste
react with
metals
AlikeDifferent
Related to
H+ (proton)
concentration
pH + pOH = 14
Affects pH
and
litmus paper
Base
Different
Topic Topic
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Properties
electrolytes
turn litmus red
sour taste
react with metals toform H2 gas
slippery feel
turn litmus blue
bitter taste
ChemASAP
vinegar, milk, soda,
apples, citrus fruits
ammonia, lye, antacid,
baking soda
electrolytes
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Acid
Sour taste
Turns blue litmus red
Reacts with some metals to produce H2Dissolves carbonate salts, releasing CO2
Base
Bitter tasteTurns red litmus blue
Slippery to the touch
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Common Acids and Bases
Strong Acids (strong electrolytes)
HCl hydrochloric acid
HNO3 nitric acid
HClO4 perchloric acidH2SO4 sulfuric acid
Weak Acids (weak electrolytes)
CH3COOH acetic acid
H2CO3 carbonic
Strong Bases (strong electrolytes)
NaOH sodium hydroxide
KOH potassium hydroxide
Ca(OH)2 calcium hydroxide
Weak Base (weak electrolyte)
NH3 ammonia
Kotz, Purcell, Chemistry & Chemical Reactivity 1991, page 145
Weak Base (weak electrolyte)
NH4OH ammonia
NH3 + H2O NH4OH
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Acid + Base Salt + Water
Orange juice + milk bad taste
Evergreen shrub + concrete dead bush
Under a pine tree + fertilizer white powder
HCl + NaOH NaCl + HOHsalt water
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Acid-Base Neutralization
1+ 1-
+ +
Hydronium ion Hydroxide ion
H3O+ OH-
Water
H2O
Water
H2O
Water
H2O
Water
H2O
Dorin, Demmin, Gabel, Chemistry The Study of Matter 3rd Edition, page 584
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Acid-Base Neutralization
1+ 1-
+ +
Hydronium ion Hydroxide ion Water
H3O+ OH- H2O
Water
H2O
Dorin, Demmin, Gabel, Chemistry The Study of Matter 3rd Edition, page 584
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Acid Precipitation
http://nadp.sws.uiuc.edu/amaps2/
http://nadp.sws.uiuc.edu/amaps2/http://nadp.sws.uiuc.edu/amaps2/7/29/2019 Acids and Bases (Muy Bueno)
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Formation of Sulfuric Acid
Kelter, Carr, Scott, Chemistry A World of Choices 1999, page 302
SO2(g) + H2O(l) H2SO3(aq)
2SO2(g) + O2(g) 2SO3(g)
SO3(g) + H2O(l) H2SO4(aq)
SO2(g) + H2O2(l) H2SO4(aq)
Catalyzed by atmospheric dust
Sulfuric acid
+
+
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Figure courtesy of the National Atmospheric Deposition Program, Champaign, Ill.
The progressively darker red areas on the map indicate the lowest pH levels
and areas most prone to problems from acid rain.
Hydrogen ion concentration as pH from measurements
made at the field laboratories during 2003
National Atmospheric Deposition Program/National Trends Network
http://nadp.sws.uiuc.edu
made at the Central Analytical Laboratory, 1999
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Acid Rain
Smoke stacks pollute SO2into the atmosphere. This
combines with water to form
acid rain.
Estimated sulfate ion deposition, 1999
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CO2 (g) H2O (l) H2CO3 (aq)Carbondioxide CarbonicacidWater
Weakacid
Copyright 2007 Pearson Benjamin Cummings. All rights reserved.
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Common Acids
Sulfuric Acid H2SO4
Nitric Acid HNO3
Phosphoric Acid H3PO4
Hydrochloric Acid HCl
Acetic Acid CH3COOH
Carbonic Acid H2CO3
Battery acid
Used to make fertilizers
and explosives
Food flavoring
Stomach acid
Vinegar
Carbonated water
http://upload.wikimedia.org/wikipedia/commons/2/24/Sulfuric-acid-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/6/69/Nitric-acid-3D-balls-B.pnghttp://upload.wikimedia.org/wikipedia/commons/0/08/Phosphoric-acid-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/4/48/Hydrogen-chloride-3D-vdW-labelled.pnghttp://upload.wikimedia.org/wikipedia/commons/e/ef/Acetic-acid-3D-balls.pnghttp://upload.wikimedia.org/wikipedia/commons/8/81/Carbonic-acid-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/8/81/Carbonic-acid-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/4/48/Hydrogen-chloride-3D-vdW-labelled.pnghttp://upload.wikimedia.org/wikipedia/commons/6/69/Nitric-acid-3D-balls-B.pnghttp://upload.wikimedia.org/wikipedia/commons/e/ef/Acetic-acid-3D-balls.pnghttp://upload.wikimedia.org/wikipedia/commons/2/24/Sulfuric-acid-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/0/08/Phosphoric-acid-3D-vdW.png7/29/2019 Acids and Bases (Muy Bueno)
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Common Acids
Formula Name of Acid Name of NegativeIon of Salt
HF hydrofluoric fluoride
HBr hydrobromic bromide
HI hydroiodic iodide
HCl hydrochloric chloride
HClO hypochlorous hypochloriteHClO2 chlorous chlorite
HClO3 chloric chlorate
HClO4 perchloric perchlorate
H2S hydrosulfuric sulfide
H2SO3 sulfurous sulfite
H2SO4 sulfuric sulfate
HNO2 nitrous nitrite
HNO3 nitric nitrate
H2CO3 carbonic carbonate
H3PO3 phosphorous phosphite
H3PO
4phosphoric phosphate
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Sulfuric Acid, H2SO4Sulfuric acid is the most commonly produced industrial chemical in the world.
Uses: petroleum refining, metallurgy, manufacture of fertilizer,
many industrial processes: metals, paper, paint, dyes, detergents
Sulfuric acid is used in
automobile batteries.
H2SO4oil of vitriol
http://upload.wikimedia.org/wikipedia/commons/2/24/Sulfuric-acid-3D-vdW.png7/29/2019 Acids and Bases (Muy Bueno)
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Nitric Acid, HNO3
Nitric acid stains proteins yellow (like your skin).
Uses: make explosives, fertilizers, rubber, plastics, dyes, and pharmaceuticals.
HNO3
aqua fortis
O
OO
N
H
http://upload.wikimedia.org/wikipedia/commons/6/69/Nitric-acid-3D-balls-B.pnghttp://upload.wikimedia.org/wikipedia/commons/6/69/Nitric-acid-3D-balls-B.pnghttp://upload.wikimedia.org/wikipedia/commons/6/69/Nitric-acid-3D-balls-B.pnghttp://upload.wikimedia.org/wikipedia/commons/6/69/Nitric-acid-3D-balls-B.pnghttp://upload.wikimedia.org/wikipedia/commons/6/69/Nitric-acid-3D-balls-B.pnghttp://upload.wikimedia.org/wikipedia/commons/6/69/Nitric-acid-3D-balls-B.png7/29/2019 Acids and Bases (Muy Bueno)
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Hydrochloric Acid, HCl
The stomach produces HCl to aid in the digestion of food.
Uses: For pickling iron and steel.
Pickling is the immersion of metals in acid solution to remove
surface impurities.
A dilute solution of HCl is called muriatic acid (available in many hardware
stores). Muriatic acid is commonly used to adjust pH in swimming pools
and in the cleaning of masonry.
HCl(g) + H2O(l) HCl(aq)hydrogen chloride water hydrochloric acid
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Common Bases
Sodium hydroxide NaOH lye or caustic soda
Potassium hydroxide KOH lye or caustic potash
Magnesium hydroxide Mg(OH)2 milk of magnesia
Calcium hydroxide Ca(OH) 2 slaked lime
Ammonia water NH3 H2O household ammonia
Name Formula Common Name
.NH4OH
NH41+ + OH1-
ammonium hydroxide
hydroxideion
OH1-
http://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.png7/29/2019 Acids and Bases (Muy Bueno)
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Common Bases
Sodium hydroxide NaOH lye or caustic soda
Potassium hydroxide KOH lye or caustic potash
Magnesium hydroxide Mg(OH)2 milk of magnesia
Calcium hydroxide Ca(OH) 2 slaked lime
Ammonia water NH3 H2O household ammonia
Name Formula Common Name
.NH4OH
NH41+ + OH1-
ammonium hydroxide
hydroxideion
OH1-
http://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.pnghttp://upload.wikimedia.org/wikipedia/commons/5/5a/Hydroxide-3D-vdW.png7/29/2019 Acids and Bases (Muy Bueno)
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Binary Hydrogen Compoundsof Nonmetals When Dissolved in Water
(These compounds are commonly called acids.)
The prefix hydro- is used to represent hydrogen, followed by the nameof the nonmetal with its ending replaced by the suffixicand the word
acid added.
Examples:
*HCl
HBr
*The name of this compound would be hydrogen chloride if it was NOT dissolved in water.
Hydrochloricacid
Hydrobromicacid
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Naming Ternary Compounds
from Oxyacids
The following table lists the most common families of oxy acids.
one more
oxyg en atom
most
common
one less
oxygen
two less
oxygen
HClO4perchloric acid
HClO3chloric acid
HClO2
chlorous acid
HClO
hypochlorous acid
H2SO4sulfuric acid
H2SO3
sulfurous acid
H3PO4phosphoric acid
H3PO3
phosphorous acid
H3PO2hypophosphorous acid
HNO3nitric acid
HNO2
nitrous acid
(HNO)2hyponitrous acid
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An acid with a
name ending in
A salt with a
name ending in
-ic
-ous
-ate
-iteforms
forms
Hill, Petrucci, General ChemistryAn Integrated Approach1999, page 60
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Oxyacids Oxysalts
If you replace hydrogen with a metal, you have formed an oxysalt.A saltis a compound consisting of a metal and a non-metal. If the
salt consists of a metal, a nonmetal, and oxygen it is called an
oxysalt. NaClO4, sodium perchlorate, is an oxysalt.
HClO4perchloric acid
HClO3
chloric acid
HClO2chlorous acid
HClO
hypochlorous acid
NaClO4sodium perchlorate
NaClO3
sodium chlorate
NaClO2sodium chlorite
NaClO
sodium hypochlorite
OXYACID OXYSALT
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Acid Base Systems
Type Acid Base
Arrhenius H+
or H3O+
producer
OH-
producer
Brnsted-
Lowry
Proton (H +)
donor
Proton (H +)
acceptor
Lewis Electron-pair
acceptor
Electron-pair
donor
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Arrhenius Acid
1+
+ +
hydronium ion
H3O+
1-
chloride ion
Cl-
water
H2O
hydrogen chloride
HCl
(an Arrhenius acid)
Any substance that releases H+ ions as the
onlypositive ion in the aqueous solution.
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Definitions
Arrhenius - In aqueous solution
HCl+ H2O H3O+ + Cl
Acidsform hydronium ions (H3O+)
H
HH H H
H
ClClO O
+
acid Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Brnsted-Lowry Acids and Bases
1+
+
hydronium ion
H3O+
1-
chloride ion
Cl-
(base)
H2O
(acid)
HCl
d+ d-
Acid = any substance that donates a proton.
Base = any substance that accepts a proton.
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Brnsted-Lowry Acids and Bases
1+
+
hydronium ion
H3O+
1-
chloride ion
Cl-
(base)
H2O
(acid)
HCl
d+ d-
Acid = any substance that donates a proton.
Base = any substance that accepts a proton.
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Definitions
F -
H2PO4-
H2O
HF
H3PO4
H3O+
Give the conjugate base for each of the following:
Polyprotic - an acid with more than one H+
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Neutralization
Neutralization is a chemical reaction between an acid and a base
to produce a salt (an ionic compound) and water.
NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l)
base acid salt water
Some neutralization reactions:
H2SO4(aq) + NaOH(aq) Na2SO4 + HOH
sulfuric acid sodium hydroxide sodium sulfate water
HC2H3O2(aq) + Ca(OH)2(aq) Ca(C2H3O2)2 + HOH
acetic acid calcium hydroxide calcium acetate water
2 2
2 2
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ACID + BASE SALT + WATER
HCl + NaOH NaCl + H2O
HC2H3O2 + NaOH NaC2H3O2 + H2O
Salts can be neutral, acidic, or basic.
Neutralization does not mean pH = 7.
weak
strong strong
strong
neutral
basic
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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pH = - log [H+]
pH = 4.6
pH = - log [H+]
4.6 = - log [H+]
- 4.6 = log [H+]
- 4.6 = log [H+]
Given:
2nd log
10x
antilog
multiply both sides by -1
substitute pH value in equation
take antilog of both sides
determine the [hydronium ion]
choose proper equation
[H+] = 2.51x10-5M
You can check your answer by working backwards.
pH = - log [H+]
pH = - log [2.51x10-5M]
pH = 4.6
Recall, [H+] = [H3O+]
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Acid Dissociation
monoprotic
diprotic
polyprotic
HA(aq) H1+(aq) + A1-(aq)
0.03 M 0.03 M 0.03 M
pH = - log [H+]
pH = - log [0.03M]
pH = 1.52
e.g. HCl, HNO3
H2A(aq) 2 H1+(aq) + A2-(aq)
0.3 M 0.6 M 0.3 M
pH = - log [H+]
pH = - log [0.6M]
pH = 0.22
e.g. H2SO4
Given: pH = 2.1find [H3PO4]
assume 100%
dissociation
e.g. H3PO4H3PO4(aq) 3 H
1+
(aq) + PO43-
(aq)? M x M
pH = ?
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Given: pH = 2.1
find [H3PO4]
assume 100%dissociation
H3PO4(aq) 3 H1+(aq) + PO4
3-(aq)
XM 0.00794 M
Step 1) Write the dissociation of phosphoric acid
Step 2) Calculate the [H+] concentration pH = - log [H+]
2.1 = - log [H+]
- 2.1 = log [H+]
2nd log - 2.1 = log [H+]2nd log
[H+] = 10-pH
[H+] = 10-2.1
[H+] = 0.00794 M
[H+] = 7.94 x10-3M7.94 x10-3M
Step 3) Calculate [H3PO4] concentration
Note: coefficients (1:3) for (H3PO4 : H+)
7.94 x10-3M3
= 0.00265 MH3PO4
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pH Indicators
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pH Paper
pH 0 1 2 3 4 5 6
pH 7 8 9 10 11 12 13
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Indicator Colors in Titration
http://images.google.com/imgres?imgurl=http://www.funsci.com/fun3_en/acids/acids_01.jpg&imgrefurl=http://www.funsci.com/fun3_en/acids/acids.htm&h=294&w=304&sz=17&hl=en&start=1&tbnid=PW71Yfkt-yvLCM:&tbnh=112&tbnw=116&prev=/images?q=acids&gbv=2&hl%7/29/2019 Acids and Bases (Muy Bueno)
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Red Cabbage IndicatorCopyright 2007 Pearson Benjamin Cummings. All rights reserved.
http://images.google.com/imgres?imgurl=http://www.funsci.com/fun3_en/acids/acids_01.jpg&imgrefurl=http://www.funsci.com/fun3_en/acids/acids.htm&h=294&w=304&sz=17&hl=en&start=1&tbnid=PW71Yfkt-yvLCM:&tbnh=112&tbnw=116&prev=/images?q=acids&gbv=2&hl%7/29/2019 Acids and Bases (Muy Bueno)
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23
24
How to read a buret volume
23.45 mL
(not 24.55 mL)
24.55 mL?
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Titration
Titration
Analytical method in which
a standard solution is
used to determine theconcentration of an
unknown solution.
standard solution
unknown solutionCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Equivalence point (endpoint)
Point at which equal amounts of
H3O+ and OH- have been added.
Determined by
indicator color change
Titration
dramatic change in pH