O – Acids and Bases
I. Properties of Acids
A. _______________ substances which _____________ when added to water to form
_____________________ (H3O+1) ions  all acids are ___________________
B. React with active metals to form H2(g)
1. ____ Mg(s) + ____ HCl(aq) 
2. _____ Zn(s) +_____ HCl(aq) 
3. _____ Cu(s) + ______ HCl(aq) 
C. Acids affect the colors of __________________________
Universal Indicator 
Phenolphthalein 
D. Acids ______________________ bases
E. Dilute acids taste _________________ 
**SAFETY TIP: Acids release tremendous amounts of heat when you dilute them
(esp. H2SO4)  ALWAYS ADD ACID TO WATER
II. Naming Acids
* treated as an ionic compound with H+1 (hydrogen ion) as cation
* negative ion can be nonmetal (binary acid) or polyatomic anion (ternary acid)
A) Binary acids – acids that contain a negative ion ending in “-ide”
1) Formula  Name
* use prefix: hydro* use root of anion’s name
* use suffix: -ic
a) HCl
b) HBr
2) Name  Formula
* follow above rules in reverse
* be sure to balance charges
a) hydroiodic acid
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b) hydrosulfuric acid
c) HF
O – Acids and Bases
B) Ternary acids
* DO
NOT BEGIN WITH “hydro-“!!!!!!!
* use name of polyatomic ion and switch its ending:
Ion Ending
Acid Name
-ide
hydro-____-ic acid
-ate
_______-ic acid
* NOTE: sulfur stays “sulfur-” + ending, phosphorus stays “phosphor-” + ending
1) Formula  Name
a) H2CO3
b) H2SO4
2) Name  Formula
a) acetic acid
b) phosphoric acid
c) nitric acid
** Some acids are ___________________ than others; see below:
Acid
HI 
HBr 
HCl 
HNO3
H2SO4
H2SO3 
HSO4-1 
H3PO4 
HF 
HNO2 
HC2H3O2 
Conjugate Base
H+1
H+1
H+1
H+1
H+1
H+1
H+1
H+1
H+1
H+1
H+1
+
+
+
+
+
+
+
+
+
+
+
I-1
Br-1
Cl-1
NO3-1
HSO4-1
HSO3-1
SO4-2
H2PO4-2
F-1
NO-1
C2H3O2-1
Ka
very large
very large
very large
very large
large
1.5 x 10-2
1.2 x 10-2
7.5 x 10-3
6.3 x 10-4
5.6 x 10-4
1.8 x 10-5
Acid
H2CO3 
HSO3-1
H2S 
H2PO4-1 
NH4+1 
HCO3-1 
HPO4-2 
HS-1 
H2O
OH-1 
Conjugate
Base
H+1 + HCO3-1
H+1 + SO3-2
H+1 + HS-1
H+1 + HPO4-2
H+1 + NH3
H+1 + CO3-2
H+1 + PO4-3
H+1 + S-2
H+1 + OH-1
H+1 + O-2
Ka
4.3 x 10-7
1.1 x 10-7
9.5 x 10-8
6.2 x 10-8
5.7 x 10-10
5.6 x 10-11
2.2 x 10-13
1.3 x 10-14
1.0 x 10-14
< 10-36
** Rank the following acids from weakest to strongest: sulfuric acid, carbonic acid,
hydrochloric acid, hydrofluoric acid, acetic acid
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O – Acids and Bases
III. Bases - _____________ substance which dissociates to form ________________ (OH-1)
ions in water
* examples: ________ (NaOH) ,
(Ca(OH)2) ,
(Mg(OH)2)
Naming Review. Name (or give the formula for) the following bases:
1. NaOH
2. Mg(OH)2
3. aluminum hydroxide
4. ammonium hydroxide
IV. Properties of Bases - often referred to as caustic or alkaline substances
-
A. Bases are _______________________________ - dissociate in water to form OH .
B. Bases affect the colors of ___________________________.
Universal Indicator 
Phenolphthalein 
C. Bases _____________________ acids.
D. Water solutions are ___________________ and ________________________.
E. Emulsify ________________ and ____________________ 
Fox Trot Comic? Baseball
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O – Acids and Bases
V. Salt – any __________________ compound that does not contain ________________ (OH-1)
* all are good _________________________________
* formed by a ________________________________ reaction.
Acid + Base  Salt + Water
1) _____ HCl(aq) + _____ NaOH(aq) 
2) _____ H2SO4(aq) + ______ KOH(aq) 
3) _____ HBr(aq) + _____ Ca(OH)2(aq) 
4) _____ HC2H3O2(aq) + _____ NaOH(aq) 
Acid, Base, Salt, or Neither:
1. NaCl
2. KCl
3. KOH
4. SO2
5. NH4C2H3O2
1. KBr
2. H2SO4
3. HgCl2
4. Al(OH)3
5. HCl
6. KOH
7. CaO
8. K3PO4
9. CO2
10. NH4OH
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O – Acids and Bases
VI. pH – a mathematical way of measuring how ____________ a ________________ is
* It’s a ___________________ scale; that means each step is worth 10
- lemon juice is 10 times more acidic than vinegar
- battery acid is 10 times more acidic than lemon juice
- How many times more acidic is battery acid than vinegar?
pH = -log[H+1]
H+
1
2
3
4
5
7
9
8
sea
water
milk
vinegar
battery
6
Acidity
neutral
acidic
basic
10-10M
10-7M
10-4M
10-1M
acid
pH
7
less than 7
greater than 7
10 11 12 13
milk
of
magnesia
lemon
juice
Color scale for Universal Indicator:
pH:
Red
Orange
Green
3
5
7
Blue
Purple
9
11
1) Which of the solutions above is the most acidic?
2) Which of the solutions above is the most basic?
3) Look at the solutions that your teacher is testing with universal indicator.
 Label each as acidic, basic, or neutral
 Estimate the pH based on the color
 Rank the substances from most acidic to least acidic
Substance
1
2
3
4
Rank:
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acidic, basic, neutral
pH
10-13M
lye
O – Acids and Bases
VII. Buffer - a solution which is able to resist major changes in pH
weak acid
* example: HC2H3O2(aq)
H+1(aq) + C2H3O2-1(aq)
- common-ion effect - by adding a salt with the negative ion (NaC2H3O2,
KC2H3O2), we increase the concentration of that ion, therefore:
* add H+1:
* add OH-1:
* biological example: carbonic acid/bicarbonate in blood
VIII. Acid-Base Indicators - chemicals specifically designed to show specific colors in acids and
different colors in bases
* most are weak acids:
HIn
acid color
H+1 + In-1
base color
Indicator
pH Range below pH color above pH color
methyl violet
0.0 – 1.6
yellow
blue
methyl yellow
2.9 – 4.0
red
yellow
bromophenol blue 3.0 – 4.6
yellow
blue
methyl orange
3.2 – 4.4
red
yellow
methyl red
4.8 – 6.0
red
yellow
litmus
5.5 – 8.0
red
blue
bromothymol blue 6.0 – 7.6
yellow
blue
phenol red
6.6 – 8.0
yellow
red
phenolphthalein
8.2 – 10.6
colorless
red
thymolphthalein
9.4 – 10.6
colorless
blue
alizarin yellow
10.0 – 12.0
yellow
red
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O – Acids and Bases
IX. Acid-Base Neutralization
H+1 + OH-1
*
H2O
if you have 35 molecules of acid, 35 molecules of base will neutralize it
* equivalence point - when an equivalent amount of OH-1 ions has been added to H+1
ions  it’s “neutralized”
X. Acid-Base Titration - lab procedure used to determine the concentration of an unknown acid
or base solution.
* standard solution – solution whose concentration is known
* unknown solution – solution whose concentration you are trying to determine
MaVa = MbVb
T.
1) If you begin a titration with 20.0 mL of unknown HCl and titrate it to the equivalence point
using 35.6 mL of 0.600 M standard NaOH, what is the concentration of HCl?
2) If you titrate 65.0 mL of an unknown NH3 solution to the equivalence point with 31.2 mL of a
1.50 M HCl solution, what is the concentration of the ammonia?
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O – Acids and Bases
S.
1) Ma = ???
Va = 50.0 mL
Mb = 1.50 M
Vb = 71.3 mL
2) What is the concentration of an unknown NaOH solution if you titrate 100.0 mL of it to the
equivalence point with 43.5 mL of 6.0 M HCl?
3) What is the concentration of a vinegar (HC2H3O2) solution if you titrate exactly 20 drops of it
to the equivalence point with 26 drops of 0.600M NaOH?
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