Acids, Bases, and
Salts
I. Properties of Acids
Sour taste
 Change colors of acid-base indicators warm
colors– turns litmus paper red
 Some react with active metals to release H2
 Acid + Base → Salt + water
 Conduct electric current
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III. Properties of Bases
Bitter taste
 Change colors of acid-base indicators cool
colors– turns litmus paper blue
 Feel slippery
 React with acids to produce salts and water
 Conduct electric current
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Write dissociation equation &
balance
HCl →
2. HNO3 →
3. NaOH →
4. Mg(OH)2 →
5. NaCl →
Note any similarities between the equations
1.
IV. ARRHENIUS THEORY
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Acids, bases, and salts conduct a current when
dissolved in water - electrolytes
An acid produces H+ in a water solution
HCl(g) --> H+(aq) + Cl-(aq)
A base produces OH- in a water solution
NaOH(cr) --> Na+(aq) + OH-(aq)
II. Naming Acids - Binary
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Binary acid – contains 2 elements; hydrogen and
one of the more electronegative elements.
Ex. HF
1. Begins with prefix hydro
2. Followed by root of name of second element
3. Ends with suffix -ic
hydro – fluor – ic acid
H2S
II. Naming Acids - oxyacids
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Compound of hydrogen, oxygen, and a 3rd element
that is usually a nonmetal
Formula is usually one or more H atoms followed
by polyatomic anion
Pg. 250
HNO2 – nitrous acid
NO2- nitrite
HNO3 – nitric acid
NO3- nitrate
Common industrial – sulfuric, nitric, phosphoric,
hydrochloric, acetic
Practice problems
Pg.250 #’s 18-22
 Pg. 596 1a,1b
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Strong vs. weak
Strong acids and bases fully dissociate
 Weak acids and bases partially dissociate
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V. BRONSTED-LOWRY
THEORY
Acid – proton (H+) donor Base – proton acceptor
 The conjugate base of an acid is the particle that remains
after a proton is released by the acid.
 The conjugate acid of a base is formed when the base
receives a proton from an acid.
 In the reaction NH3(g) + water(l)->NH4 +
(aq) + OH-: NH3 is the base, water is the acid,
NH4+ is the conjugate acid, and OH- is the conjugate
base.
H H
N
N
H
O H
O
H
H
H
H
H
H
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PRACTICE PROBLEMS
Which is the conjugate base / conjugate acid in:
H3PO4 + H2O --> H3O+ + H2PO4H3O is the conjugate acid and H2PO4 is the conjugate base.
One more, which is the conjugate base / conjugate acid in:
H4P2O7 + H2O --> H3O+ + H3P2O7Again H3O is the conjugate acid and H3P2O7- is the
conjugate base.
BRONSTED-LOWRY Acid Base
Reactions
HF + H2O → F- + H3O+
 Subscripts designate 2 conjugate acid base pairs
 HF + H2O → F- + H3O+
acid1 base2
base1 acid2
 Strength of conjugate acid and base – strong acid
– weak conj. Base. Reactions favors direction that
produces weaker acids and bases
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Amphoteric
Can act as acid or base (H2O)
 H2SO4 + H2O →
base
 NH3 + H2O →
acid
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BRONSTED-LOWRY THEORY
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Monoprotic acid – donates only one proton
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Polyprotic acid – donates more than one proton
Diprotic – donates 2 protons
Triprotic – donates 3 protons
All polyprotic ionize in steps
H3PO4(aq) pg. 601 #3a,3b
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LEWIS THEORY
Lewis focused on an electron transfer rather
than a proton transfer.
 Lewis described an acid as an electron-pair
acceptor and a base as an electron-pair
donor.
 An acid or base in Arrhenius theory is the
same under the Lewis and Bronsted-Lowry
theories.
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MORE PRACTICE PROBLEMS
CLASSIFY THE FOLLOWING
SUBSTANCES AS LEWIS ACIDS OR
BASES.
a. Cl- b. Al+ c. Br- d. I+
a and c = Lewis Base
b and d = Lewis Acid
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