Acid/Base Chemistry
Part 2 (5.2-5.3)
Science 10
CT05D02
Resource:
Brown, Ford, Ryan, IB Chem
Topic 05 – Acids/Bases
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5.1
5.2
5.3
5.4
5.5
5.6
Solutions
Definitions of Acids and Bases
Properties of Acids and Bases
Calculating pH, pOH, H+, OHNeutralization equations
Titrations
5.2 - Definitions of Acids and
Bases
 5.2.1 Arrhenius: Acids donate H+, Bases donate OH-
ions in solution
 5.2.2 Lowry/Bronsted: Acids donate a proton, Bases
accept a proton (H+)
 You will need to know each of these definitions
5.2 - Old Dudes define A/B
Svante Arrhenius
(Sweden)
J.N. Brønsted (Denmark) Thomas
Lowry (England)
5.2 - Arrhenius Definition
 An acid is a material that can release a proton or
hydrogen (H+) ion. Just like a salt, hydrogen chloride
(HCl) in water solutions ionizes and becomes
hydrogen ions (H+) and chloride ions (Cl-).
HCl  H+(aq) + Cl-(aq)
 A base, or alkali, is a material that can donate a
hydroxide ion (OH-). Sodium hydroxide in water
solutions becomes sodium ions (Na+) and hydroxide
ions (OH-).
NaOH  Na+(aq) + OH(aq)
5.2 - Lowry-Brønsted Definition
 An acid is a material that donates a proton.
 A base is a material that can accept a proton.
5.3 - Properties of Acids and Bases
 5.3.1 Acids (donate H+, turn litmus red, corrode
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active metals, neutralize bases, taste sour)
5.3.2 Bases (donate OH-, turn litmus blue, denature
protein, neutralize acids, taste bitter
5.3.2 Nomenclature of simple Acids and Bases
5.3.4 Protonaety of Acids and Bases
There are five general properties of both acids and
bases. Common properties are known beyond this
but it is these five that you need to know.
5.3 - Properties of Acids
For the properties of Acids and Bases, the Arrhenius
definition will be used.
 A1: Acids release a hydrogen ion into water (aqueous)
solution.
 A2: Acids neutralize bases in a neutralization reaction.
An acid and a base combine to make a salt and water.
The hydrogen ion of the acid and the hydroxide ion of
the base unite to form water.
HCl + NaOH  HOH + NaCl
5.3 - Properties of Acids
 A3: Acids corrode active metals. When an acid
reacts with a metal, it produces a compound with
the cation of the metal and the anion of the acid
and hydrogen gas.
 A4: Acids turn blue litmus to red. Litmus is the
oldest known pH indicator. It is red in acid and blue
in base.
 A5: Acids taste sour. TASTING LAB ACIDS IS NOT
PERMITTED!! Stomach acid is hydrochloric acid.
Citrus fruits such as lemons, grapefruit, oranges,
and limes have citric acid in the juice.
5.3 - Properties of Bases
 B1: Bases release a hydroxide ion into water
solution.
 B2: Bases neutralize acids in a neutralization
reaction.
HCl + NaOH  HOH + NaCl
 B3: Bases denature protein. To denature a protein
means to render parts of it useless most likely by
unfolding it. Serious damage to flesh can be
avoided by careful used of strong bases.
5.3 - Properties of Bases
 B4: Bases turn red litmus to blue. This is not to say
that litmus is the only acid- base indicator, but that
it is likely the oldest one.
 B5: Bases taste bitter. There are very few food
materials that are alkaline, but those that are taste
bitter. It is even more important that care be taken
in tasting bases. Again, TASTING OF LAB
CHEMICALS IS STRICTLY PROHIBITED. Tasting of
bases is more dangerous than tasting acids due to
the property of stronger bases to denature essential
proteins in the body.
Nomenclature Review!!
 To determine the naming system of a compound, you
can simply look at the first element:
 A metal = MUST BE IONIC
 Does it have a polyatomic?
 Does it have a transition metal?
 A nonmetal = MUST BE COVALENT
 Hydrogen = MUST BE AN ACID
 Binary Acid?
 Oxoacid (Polyatomic)?
first element
Metal = Ionic
 NO prefixes
 The simplest whole number ratio is generally the ionic
formula. (empirical formula)
Binary
Polyatomic
Transition
NaCl
Na2CO3
FeCl3
MgBr2
Mg(NO3)2
Ni3(PO3)2
Li2S
Li3PO4
ZrSO4
First element
nonmetal = Covalent
 Greek Prefixes
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Mono (1), di (2), tri (3), tetra (4), penta (5), etc….
First nonmetal keeps element name
Change ending of second nonmetal to –ide
P 2 O5
CCl4
CO2
CO
SiO2
NO2
CF4
SF6
PF5
NO
First element
hydrogen = Acid
Binary
Oxoacid
H and another element
H and 2 or more
Use hydro- prefix
NO prefix
Use –ic suffix
If poly –ate  -ic
HCl
HF
H2S
HI
HBr
If poly –ite  -ous
HNO3
H3PO4
H3PO3
H2SO4
Polyatomic Ions
(they keep coming back!)
3PO4
NO2
2SO3
ClO3
3PO3
NO3
2SO4
ClO2
OH
+
NH4
2CO3
5.3 – Simple Base Nomenclature
 A common base is an ionic compound formed
between a metal (M+) and hydroxide (OH-) ion.
 (sodium hydroxide) NaOH  Na+ + OH (magnesium hydroxide) Mg(OH)2  Mg2+ + 2 OH Any compound with available room to accept an H+
is also considered a base
 (ammonia) NH3 + H+  NH4+
 Covalent compounds with a hydroxide functional
group, such as the alcohols (CH3OH, C2H5OH) are
not considered to be bases
5.3 – Acid/Base Nomenclature
Acid Formula
Acid Nomenclature
Base Formula Base Nomenclature
H2SO4
NaOH
H2SO3
LiOH
H2CO3
KOH
HNO3
RbOH
HNO2
Mg(OH)2
H3PO4
Ca(OH)2
H3PO3
Sr(OH)2
HClO3
NH3
HClO2
HCl
HBr
HI
H2S
HF
5.3 – Protonaety (is that a word?)
 Acids can be either monoprotic, diprotic, or
triprotic where they can donate one, two, or
three protons respectively
 Monoprotic (HCl, HNO3, HClO3)
 Diprotic (H2S, H2SO4, H2CO3)
 Triprotic (H3P, H3PO4, H3PO3)
 Bases can also be considered as such because of
their ability to accept protons (donate OH-)
 Monoprotic (NaOH, NH3)
 Diprotic (Mg(OH)2, NH2-)
5.3 - Protonaety
 Monoprotic Acid Formula:
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HCl  H+ + Cl-
 Monoprotic Base Formula:
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NH3 + H+  NH4+
 Diprotic Acid Formula:
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H2SO4  H+ + HSO4-  2 H+ + SO42-
 Diprotic Base Formula:
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Mg(OH)2 + 2H+  Mg(OH)+ + H+ + H2O  Mg2+ + 2H2O
 Triprotic Acid Formula:
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H3P  H+ + H2P-  2H+ + HP2-  3H+ + P3-