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Acids
Lesson 4
Acid and Base
Reactions
Conductivity
The conductivity of an acid is determined by the number of ions
generated in a solution and is therefore a combination of both the
strength and concentration of the acid.
1.0 M HCl is a better conductor than 0.10 M HCl
1.0 M HI is a better conductor than 1.0 M HF.
1.0 M HF has the same conductivity as 0.02 M HCl.
The same is true for a base.
0.004 M NaOH has the same conductivity as 1.0 M NH3
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43-
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43HPO42-
Base
can gain H+, cannot lose H+
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43-
Base
can gain H+, cannot lose H+
HPO42-
Amphiprotic
can gain H+and lose H+
H2PO4-
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43-
Base
can gain H+, cannot lose H+
HPO42-
Amphiprotic
can gain H+and lose H+
H2PO4-
Amphiprotic
can gain H+and lose H+
H3PO4
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
PO43-
Base
can gain H+, cannot lose H+
HPO42-
Amphiprotic
can gain H+and lose H+
H2PO4-
Amphiprotic
can gain H+and lose H+
H3PO4
Acid
cannot gain H+, can lose H+
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
CO32-
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
CO32HCO3-
Base
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
CO32-
Base
HCO3-
Amphiprotic
H2CO3
Amphiprotic Chemical Species
Amphiprotic chemical species can act as acids and donate protons or
bases and accept protons. They are listed both on the left side of the
table as an acid and the right side as a base.
Acid, Base, or Amphiprotic
CO32-
Base
HCO3-
Amphiprotic
H2CO3
Acid
In Chemistry 11
H2SO4
+
2KOH

In Chemistry 11
H2SO4
+
2KOH

K2SO4 +
2HOH(l)
In Chemistry 11
H2SO4
+
2H+ + SO42-
2KOH

K2SO4 +
2HOH(l)
In Chemistry 11
H2SO4
+
2KOH

2H+ + SO42- + 2K+ + 2OH- 
K2SO4 +
2HOH(l)
In Chemistry 11
H2SO4
+
2KOH

K2SO4 +
2H+ + SO42- + 2K+ + 2OH-  2K+ +
2HOH(l)
SO42-
+
In Chemistry 11
H2SO4
+
2KOH

K2SO4 +
2H+ + SO42- + 2K+ + 2OH-  2K+ +
2HOH(l)
SO42-
+ 2HOH(l)
In Chemistry 11
H2SO4
+
2KOH

K2SO4 +
2H+ + SO42- + 2K+ + 2OH-  2K+ +
H+ + OH- 
2HOH(l)
SO42-
HOH(l)
Use an arrow if you have a strong acid or a strong base!
Strong acids, strong bases, and soluble salts are ionized!
+ 2HOH(l)
In Chemistry 12
H2C2O4
+
2KOH 
In Chemistry 12
H2C2O4
+
2KOH 
K2C2O4
+
2HOH(l)
In Chemistry 12
H2C2O4
+
2KOH 
H2C2O4
+ 2K+ + 2OH-  2K+ +
K2C2O4
+
2HOH(l)
C2O42- + 2HOH(l)
In Chemistry 12
H2C2O4
+
2KOH 
H2C2O4
+ 2K+ + 2OH-  2K+ +
H2C2O4
+ 2OH-

K2C2O4
+
2HOH(l)
C2O42- + 2HOH(l)
C2O42- + 2HOH(l)
The weak acid or base does not dissociate!
Break up strong acids, strong bases, and soluble salts!
Conductivity
Good Conductors
Weak Conductors
Nonconductors
Strong Acids Strong Bases Soluble Salts
HCl
NaOH
KCl
Weak Acids
Weak Bases
Low Solubility Salts
HF
Zn(OH)2
AgCl
Molecular covalent
C12H22O11
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
HC2O4-
+
HCO3-
⇋
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
HC2O4-
+
HCO3-
⇋
Look up the two amphiprotic ions on the left side of the acid chart. The
higher one is the stronger acid and will be the acid and donate a
proton to the base.
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
H+
HC2O4+ HCO3⇋
Acid
Base
Look up the two amphiprotic ions on the left side of the acid chart. The
higher one is the stronger acid and will be the acid and donate a
proton to the base.
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
HC2O4Acid
+
HCO3Base
⇋
C2O42-
+ H2CO3
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
HC2O4Acid
+
HCO3-
⇋
C2O42-
+ H2CO3
Base
Label the acid and base on the other side of the equation. You do this by
considering which species will donate the proton in the reverse
reaction.
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
HC2O4Acid
+
HCO3-
⇋
C2O42-
H+
+ H2CO3
Base
Label the acid and base on the other side of the equation. You do this by
considering which species will donate the proton in the reverse
reaction.
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
HC2O4Acid
+
HCO3Base
⇋
C2O42Base
H+
+ H2CO3
Acid
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
HC2O4Acid
+
HCO3Base
⇋
C2O42Base
+ H2CO3
Acid
Now compare the acid on the left HC2O4- to the acid on the right H2CO3.
HC2O4- is the stronger acid and more successfully donates its proton to
favour the formation of products.
This means there are more products than reactants at equilibrium.
When you find the stronger acid, the other side is always favoured.
In Chemistry 12
Weak acids and weak bases also react.
Use ⇋
Do not go to completion.
HC2O4Acid
+
HCO3-
⇋
C2O42-
Base
Base
Stronger acid
Products are favoured!
⇋
+ H2CO3
Acid
In Chemistry 12
HSO4-
+
HSO3-
⇋
In Chemistry 12
HSO4-
+
HSO3-
⇋
HSO4- is a stronger acid than HSO3- so it donates the proton.
In Chemistry 12
HSO4-
Acid
+
HSO3-
Base
⇋
SO42-
+
H2SO3
In Chemistry 12
HSO4-
Acid
+
HSO3-
⇋
SO42-
Base
Base
+
H2SO3
Acid
H+
Reactants are Favoured because H2SO3 is a stronger acid than HSO4-
The stronger acid H2SO3 more successfully donates its proton making
more reactants.
⇋