AcidsLesson 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 

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 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  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.  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.

H+

In Chemistry 12  Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC2O4

- + HCO3- ⇋ C2O4

2- + H2CO3

Acid Base

In Chemistry 12  Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC2O4

- + HCO3- ⇋ C2O4

2- + H2CO3

Acid 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. HC2O4

- + HCO3- ⇋ C2O4

2- + H2CO3

Acid 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.

H+

In Chemistry 12  Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC2O4

- + HCO3- ⇋ C2O4

2- + H2CO3

Acid Base Base Acid

H+

In Chemistry 12  Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC2O4

- + HCO3- ⇋ C2O4

2- + H2CO3

Acid Base Base 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. HC2O4

- + HCO3- ⇋ C2O4

2- + H2CO3

Acid Base Base Acid

Stronger acidProducts are favoured!

⇋

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- + HSO3

- ⇋ SO42- + H2SO3

Acid Base

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

In Chemistry 12  

HSO4- + HSO3

- ⇋ SO42- + H2SO3

Acid Base Base Acid

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

H+

⇋