AcidsLesson 3

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. 

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 

PO43- Base can gain H+, cannot lose H+

HPO42-

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 

CO32- Base

HCO3-

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 + 2KOH K2SO4 + 2HOH(l)

  2H+ + SO4

2-

In Chemistry 11  H2SO4 + 2KOH K2SO4 + 2HOH(l)

  2H+ + SO4

2- + 2K+ + 2OH-

In Chemistry 11  H2SO4 + 2KOH K2SO4 + 2HOH(l)

  2H+ + SO4

2- + 2K+ + 2OH- 2K+ + SO42- +

In Chemistry 11  H2SO4 + 2KOH K2SO4 + 2HOH(l)

  2H+ + SO4

2- + 2K+ + 2OH- 2K+ + SO42- + 2HOH(l)

  

In Chemistry 11  H2SO4 + 2KOH K2SO4 + 2HOH(l)

  2H+ + SO4

2- + 2K+ + 2OH- 2K+ + SO42- + 2HOH(l)

  H+ + OH- HOH(l)

Use an arrow if you have a strong acid or a strong base!

Strong acids, strong bases, and soluble salts are ionized!

In Chemistry 12

H2C2O4 + 2KOH

  

In Chemistry 12

H2C2O4 + 2KOH

  

In Chemistry 12

H2C2O4 + 2KOH K2C2O4+ 2HOH(l)

  

In Chemistry 12

H2C2O4 + 2KOH K2C2O4+ 2HOH(l)

  H2C2O4+ 2K+ + 2OH- 2K+ + C2O4

2- + 2HOH(l)

  

In Chemistry 12

H2C2O4 + 2KOH K2C2O4+ 2HOH(l)

  H2C2O4+ 2K+ + 2OH- 2K+ + C2O4

2- + 2HOH(l)

  H2C2O4+ 2OH- C2O4

2- + 2HOH(l)

The weak acid or base does not dissociate!

Break up strong acids, strong bases, and soluble salts!

Conductivity

Good Conductors Strong Acids Strong Bases Soluble Salts

HCl NaOH KCl

Weak Conductors Weak Acids Weak Bases Low Solubility Salts

HF Zn(OH)2 AgCl

Nonconductors Molecular covalent

C12H22O11

In Chemistry 12    HC2O4

- + HCO3-

H+

The higher one on the acid side of the chart will be the acid and donate a proton.

Weak acids and weak bases react but do not go to completion (⇋)

⇋ C2O42- + H2CO3

H+

Base Acid

Label all acids and bases- note H2C2O4 donates in the reverse reaction

The acid on the left HC2O4- is stronger than H2CO3 so the other side or

the products are favoured.

Acid Base

⇋

There are more products at equilibrium

The stronger acid H2SO3 more successfully donates its proton making more reactants.

Complete the reaction 

HSO4- + HSO3

-

⇋

Reactants are Favoured because H2SO3 is a stronger acid than HSO4-

Acid Base Base Acid

SO42- + H2SO3 ⇋

H+

H+