Year 12 Chemistry

He classified all chemicals into three categories – acids, bases and salts He classified all chemicals into three categories – acids, bases and salts He believed that all acids contained oxygen and it was this that gave them their sour taste He believed that all acids contained oxygen and it was this that gave them their sour taste Flaw: not all acids contain oxygen and metal oxides form bases Flaw: not all acids contain oxygen and metal oxides form bases

Showed that all acids do not contain oxygen Showed that all acids do not contain oxygen Proposed that acids are hydrogen containing materials following the discovery of HCl Proposed that acids are hydrogen containing materials following the discovery of HCl Flaw: not all substances that contain hydrogen are acids Flaw: not all substances that contain hydrogen are acids

Acids dissociate in water forming H + as one product Acids dissociate in water forming H + as one product Bases dissociate in water forming OH - as one product Bases dissociate in water forming OH - as one product Neutralisation involves the reaction of H + and OH - forming a salt in water Neutralisation involves the reaction of H + and OH - forming a salt in water Flaws: Flaws: theories only apply to aqueous solutions theories only apply to aqueous solutions Some substances such as NH3 are bases and do not contain OH- Some substances such as NH3 are bases and do not contain OH- Relative strengths not addressed Relative strengths not addressed Amphoteric substances not addressed Amphoteric substances not addressed

An acid is a proton (H + ) donor An acid is a proton (H + ) donor A base is a proton acceptor A base is a proton acceptor Examples: Examples: HCl + H 2 O H 3 O + + Cl¯ HCl + H 2 O H 3 O + + Cl¯ NH 3 + H 2 O NH OH¯ NH 3 + H 2 O NH OH¯ Identify the acids/bases Any other acids/bases here?

HCl + H2O  H3O + + Cl - NH3 + H2SO4  NH4 + + HSO4 - HBr + NH2 +  NH3 + + Br - Identify the B-L acids and bases in each of these reactions.

Amphiprotic substances are those that can act as bases and acids. They can donate or accept protons. Water is an obvious example Notice in the previous slide that water reacts with both acids and bases.

Bisulfate is another amphiprotic substance. Construct chemical equations to show this property.

Lewis Theory An acid is an electron pair receptor A base is an electron pair donor Note that BF3 would not be an acid under the B-L Theory as there is no H+ to donate.

A cobalt metal complex has 6 dative bonds formed by the donation of e- pairs from the ammonia molecules (Lewis bases) Which of these substances are Lewis bases? Lewis acids?

Water reacts with carbon dioxide to form carbonic acid. Write out the structures and show how the electrons are transferred, thereby identifying the Lewis acid and Lewis base.

Acid 1 + Base 2  Base 1 + Acid 2 Acid 1 + Base 2  Base 1 + Acid 2 What does this mean? What does this mean? An acid reacts and forms a conjugate base which can also accept a proton An acid reacts and forms a conjugate base which can also accept a proton A base reacts and forms a conjugate acid which can donate a proton A base reacts and forms a conjugate acid which can donate a proton Conjugate pairs differ only by one H + Conjugate pairs differ only by one H + Conjugate pair 1 Conjugate pair 2

Example: Example: HNO 3 + H 2 O H 3 O + + NO 3 ¯ HNO 3 + H 2 O H 3 O + + NO 3 ¯ Identify the conjugate pairs in this reaction Here, nitric acid and the nitrate ion are conjugates and water and the hydronium ion are also conjugates

Strong acids completely dissociate in water HA + H2O  H3O + + A - In general, these reactions are reversible, but for a strong acid the equilibrium is far right. So, HA + H2O  H3O + + A - Examples: HCl, HNO3, H2SO4 Weak acids Partially dissociate in water HA + H2O  H3O + + A - There is an equilibrium established with weak acids, which means that there is less H3O + ions in solution. CH3COOH + H2O  H3O + + CH3COO - Examples: CH3COOH, H2CO3 What do you think is the difference in electrical conductivity?

Strong bases completely dissociate in water NaOH  Na + + OH - Again, as with acids, the equilibrium is far right. So, 1 mol NaOH  1 mol OH - Examples: group I hydroxides, Ba(OH)2 Weak bases Partially dissociate in water NH3 + H2O  NH4 + + OH - Only about 1% of ammonia dissociates into hydroxide ions. 1 mol NH3  << 1mol OH - Examples: NH3, other amines Again, the electrical conductivity is greater for strong bases

Predicting Equilibrium Predicting Equilibrium The direction of acid-base equilibria is away from the stronger acid base side and towards the weaker acid base side The direction of acid-base equilibria is away from the stronger acid base side and towards the weaker acid base side The stronger the acid, the weaker its conjugate base The stronger the acid, the weaker its conjugate base The stronger the base, the weaker its conjugate acid The stronger the base, the weaker its conjugate acid

Reactions that proceed to a large extent: Reactions that proceed to a large extent: A strong acid will force the equilibrium in the opposite direction (in this case, forward or right) A strong acid will force the equilibrium in the opposite direction (in this case, forward or right) HCl + H 2 O H 3 O + + Cl¯ HCl + H 2 O H 3 O + + Cl¯ Reactions that proceed to a small extent: Reactions that proceed to a small extent: If the weaker of the two acids and the weaker of the two bases are reactants (appear on the left side of the equation), the reaction is said to proceed to only a small extent: If the weaker of the two acids and the weaker of the two bases are reactants (appear on the left side of the equation), the reaction is said to proceed to only a small extent: NH 3 + H 2 O NH OH¯ NH 3 + H 2 O NH OH¯ Identify the conjugate acid base pairs in each reaction. Identify the conjugate acid base pairs in each reaction.