UNIT IV Acid Rain.

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UNIT IV Acid Rain

Metal Oxides Metal Oxides (or Basic Anhydrides) act as BASES in solution. Group 1 and Group 2 Oxides are ionic. They dissociate to form the oxide ion (O2-). Ex. Na2O (s)  2 Na+(aq) + O2-(aq) O2-(aq) + H2O (l)  2 OH- (aq) ___________________________________________

Metal Oxides Ex. BaO (s)  Ba2+(aq) + O2-(aq) O2-(aq) + H2O (l)  2 OH- (aq) ___________________________________________ Ex. Write a balanced formula equation for the overall reactions of the following oxides with water: CaO: Li2O:

Non-Metal Oxides Non-Metal Oxides (or Acidic Anhydrides) act as ACIDS in solution. Some common examples of non-metal oxides: NO2 , N2O5 , SO2 , SO3 , CO2 , Cl2O Ex. SO2(g) + H2O(l)  H2SO3 (aq) H2SO3 (aq) + H2O(l) H3O+(aq) + HSO3- (aq)

Non-Metal Oxides Ex. 2NO2(g) + H2O(l)  HNO3 (aq) + HNO2 (aq) HNO3 (aq) + H2O(l)  H3O+(aq) + NO3-(aq) Metalloid Oxides usually have LOW solubility so not many ions are freed to undergo hydrolysis. So very little hydrolysis occurs and they do not act AS acids or bases. Hebden Textbook Page 185 Questions #144-145

CO2(g) + 2H2O(l) H3O+(aq) + HCO3-(aq) Acid Rain Since our atmosphere naturally contains CO2 (an acidic anhydride), some of this reacts with water (rain) to make the rain slightly acidic: CO2(g) + 2H2O(l) H3O+(aq) + HCO3-(aq) So natural rainwater (unaffected by human activities) can have a pH as low as 5.6 (due to the CO2 in air). If rain has a pH < 5.6 it is called ACID RAIN.

Acid Rain The main human sources of acid rain are: 1. Burning fuels containing sulphur. (SOx) 2. Car exhaust. (NOx)

Acid Rain Read pages 186-189 of your textbook. Review: Sources of Acidity in Acid Rain Natural Protection Against Acid Rain Problems Associated with Acid Rain Possible Solutions Hebden Textbook Page 188 Questions #146-147