Acids Lesson 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+ + SO42-

In Chemistry 11   H2SO4 + 2KOH  K2SO4 + 2HOH(l) 2H+ + SO42- + 2K+ + 2OH- 

In Chemistry 11   H2SO4 + 2KOH  K2SO4 + 2HOH(l) 2H+ + SO42- + 2K+ + 2OH-  2K+ + SO42- +

In Chemistry 11   H2SO4 + 2KOH  K2SO4 + 2HOH(l) 2H+ + SO42- + 2K+ + 2OH-  2K+ + SO42- + 2HOH(l)

In Chemistry 11   H2SO4 + 2KOH  K2SO4 + 2HOH(l) 2H+ + SO42- + 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+ + C2O42- + 2HOH(l)

In Chemistry 12 H2C2O4 + 2KOH  K2C2O4 + 2HOH(l)   H2C2O4 + 2K+ + 2OH-  2K+ + C2O42- + 2HOH(l) H2C2O4 + 2OH-  C2O42- + 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+ H+ ⇋ C2O42- + H2CO3 Base Acid Acid Base Weak acids and weak bases react but do not go to completion (⇋) The higher one on the acid side of the chart will be the acid and donate a proton. Label all acids and bases- note H2C2O4 donates in the reverse reaction The acid on the left HC2O4- is stronger than H2CO3 so the opposite side or the products are favoured.

Opposite side Favoured Stronger acid Products ⇋ Reactants There are more products at equilibrium

Complete the reaction   HSO4- + HSO3- H+ H+ SO42- + H2SO3 ⇋ Acid Base Base Acid Reactants are Favoured because H2SO3 is a stronger acid than HSO4- The stronger acid H2SO3 more successfully donates its proton making more reactants. ⇋