Ch 14 Acids and Bases
14.1 Properties of Acids and Bases
Objectives
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List 5 general properties of acids and bases
Name common binary and oxyacids given their chemical formula
List 5 acids commonly used in the lab and industry and give 2 properties of each
Define acid and base according to Arrhenius’s theory of ionization
Explain the differences between strong and weak acids and bases
Name some foods and the acids they contain
Name some common items and the bases they contain
MOST acids begin with H
What does “aqueous solution” mean?
List 5 properties of acids
What is a binary acid?
How do you name a binary acid?
What is an oxyacid?
When naming an oxy acid, if the polyatomic ion ends in “ate”, the acid name ends in “ic”. HNO3 is an oxyacid made of
hydrogen and the polyatomic ion nitrate. The name of the acid is nitric acid
Name the following acids: HClO3, H3PO4
If the polyatomic ion ends in “ite”, the acid name ends in “ous”. HNO2 is an oxy acid made of hydrogen and the
polyatomic ion nitrite. The name of the acid is nitrous acid.
Name the following acids: H2SO3, HClO2
List 5 acids commonly used in the lab and industry and give 2 properties of each
Name 5 properties of bases
How did Arrhenius define acids and bases
What is an ionizable hydrogen?
How many ionizable hydrogens do each of the following acids have? Hydrobromic, carbonic and sulfurous
Write the ionization equation for iodic acid, perchloric acid, phosphoric acid and sulfuric acid
What ion is always formed when an acid ionizes?
How can you distinguish between a strong and weak acid
In strong acids, is the bond holding onto the ionizable hydrogen strong or weak?
Is the equation for the ionization of a strong acid a reversible reaction?
In a strong acid, how many ionizable hydrogens are removed?
In weak acids, is the bond holding onto the ionizable hydrogen strong or weak?
Is the equation for the ionization of weak acids a reversible equation?
Does the number of hydrogen atoms in the chemical formula of an acid indicate the strength of the acid?
Acetic acid is the only organic acid you have to know about. It has only one ionizable hydrogen.
MOST bases end in OH
Are most bases ionic compounds? Do all ionic compounds completely dissociate in water?
Name a common base that does not contain OH
How can you distinguish between a strong and weak base?
Are all strong acids and bases also strong electrolytes according to Arrhenius?
14.1 assignment
address objectives
p 450, 1 to 4 p466, 1 to 11 skip 4 WS pages
14.2
Objectives
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Define and recognize Bronsted acids and bases
Define a Lewis acid and Base
What is a Bronsted acid? Why was the Bronsted theory developed?
What is a proton?
Which definition of acids is broader, Bronsted or Arrhenius?
What is a Bronsted base?
What occurs in a Bronsted acid base reaction?
Label the Bronsted acid and base in the following equations:
a)
CN– + H2O -> HCN + OH–
b)
B(OH)3 + 2 H2O -> B(OH)4– + H3O+
c)
H2O + HCl -> H3O+ + Cl–
d)
4 LiH + AlCl3 -> LiAlH4 + 3 LiCl
How many ionizable hydrogens does a monoprotic acid have? A polyprotic acid?
In polyprotic acids, all hydrogens are not removed at once, but rather they are removed one at a time in separate
ionization reactions. The removal of the first hydrogen represents a strong acid, the reaction is not reversible. The
remaining equations are reversible. See p 455
How many ionization equations are need to completely ionize H3PO4
Write the 2 ionization equations for H2SO4
Define a Lewis acid and A Lewis base. All you have to know are the definitions. You will not be asked to identify Lewis
acids and bases.
What is occurring is a Lewis acid base reaction?
14.2 assignment
to 18. WS
address objectives
p 456, 1 and 3 (no Lewis) p 466 12 to 18 cp skip the net ionic part of 15
14.3
Objectives
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Describe a conjugate acid, a conjugate base and an amphoteric compound
Explain the process of neutralization
Define acid rain, give examples of compounds that cause acid rain and describe the effects of acid rain
We will be using the Bronsted theory to describe acid base reactions
Define conjugate acid and conjugate base
On p 457 your book refers to acid1 and base1. We will not be using this designation, but rather will be using “acid and its
conjugate base” and Base and its conjugate acid”
Label the acid base conjugate pairs in the following reactions: (The acid and base will always be in the reactants, the
conjugate acid and conjugate base will always be on the product side)
a)
CN– + H2O -> HCN + OH–
b)
B(OH)3 + 2 H2O -> B(OH)4– + H3O+
c)
H2O + HCl -> H3O+ + Cl–
d)
4 LiH + AlCl3 -> LiAlH4 + 3 LiCl
How can you determine the strength of a conjugate acid or base?
To predict which will be present in greater quantities, the reactants or products, in a reversible acid base reaction:
o
o
o
Label the acid base conjugate pairs
Look up the acid and the conjugate acid on the table p 459. Label them stronger and weaker
Nature always favors the formation of the more stable compound, which is the weaker acid (remember
the weaker acid has the stronger bond)
What is an amphoteric substance? What is the most common amphoteric substance?
What determines whether an amphoteric substance will act as an acid or will act as a base?
What does the neutralization reaction between and acid and a base produce?
Which industrial gasses produce acid rain?
List some of the damages caused by acid rain
How can we reduce acid rain?
14.3 assignment
address the objectives p463, 1 to 3, p 466 19 to 25
ws pages
Review assignment
P 467 26 to 37, all skip 30b, 31, 32
cp skip the net ionic part of any question
p 469 1 to 11
ws pages