1. Acids and Bases For now, acids ionize in aqueous solutions to form a hydrogen ion (H + ). -- “proton donors” -- monoprotic acids e.g., -- diprotic acids e.g., (only first ionization is complete) HCl, HNO 3, CH 3 COOH H 2 SO 4 H 2 SO 4 (aq) H + (aq) + HSO 4 – (aq) HSO 4 – (aq) H + (aq) + SO 4 2– (aq) In soln… With weak acids, the first ionization isn’t even close to complete.

2. For now, bases are substances that accept hydrogen ions (i.e., protons). -- OH – is very basic -- equation: The most common weak base is ammonia, NH 3 ; it ionizes only about 1%. -- equation: H + (aq) + OH – (aq)  H 2 O(l) H + + OH –  H 2 O NH 3 (aq) + H 2 O(l) NH 4 + (aq) + OH – (aq)

3. LiOH Classify as a… strong electrolyte, weak electrolyte, or nonelectrolyte. HClO 3 C 6 H 12 O 6 HClO strong strong non- weak If 0.40 mol of each of the following are dissolved in 2.5 L of water, rank them from least to greatest electrical conductivity. HBrO 2 CH 3 OH Ca(CH 3 COO) 2 KNO 3 CH 3 OH<HBrO 2 <KNO 3 <Ca(CH 3 COO) 2

4. A neutralization reaction has the form: -- recall that “salt” means an ionic compound ACID + BASE  SALT + WATER Write the balanced molecular equation when nitric acid reacts w /barium hydroxide. Write the net ionic equation for the above reaction. HNO 3 Ba(OH) 2 +  Ba(NO 3 ) 2 H2OH2O 22+ (aq)(l)(aq) H + + OH –  H 2 O NO 3 – H+H+ Ba 2+ OH – NO 3 – H2OH2OBa 2+

5. Write the balanced molecular eq. when perchloric acid reacts w /potassium hydroxide. Write the net ionic equation for the above reaction. HClO 4 KOH+  KClO 4 H2OH2O + (aq)(l)(aq) H + + OH –  H 2 O ClO 4 – H+H+ K+K+ OH – ClO 4 – H2OH2OK+K+ For EVERY strong acid/strong base rxn, the net ionic equation is… H + + OH –  H 2 O.

6. 2 Three other anions that act as bases (i.e., as p + acceptors) are the sulfide ion (S 2– ), the carbonate ion (CO 3 2– ), and the bicarbonate ion (HCO 3 – ). All react w /acids to form gases. -- sulfide ion: reacts w /acids to form H 2 S(g) HCl(aq) + K 2 S(aq) e.g., H 2 S(g) + KCl(aq) 2 Hydrogen sulfide is produced by anaerobic bacteria associated with water collection and treatment processes. It is corrosive, odorous, toxic, and contributes to the formation of acid rain. Net ionic eq…2 H + (aq) + S 2– (aq)  H 2 S(g)

7. -- carbonate and bicarbonate ions: react w /acids to form CO 2 (g) 2 HNO 3 (aq) + CaCO 3 (s) CO 2(g) + H 2 O (l) + Ca(NO 3 ) 2 (aq) HCl (aq) + NaHCO 3 (s or aq) CO 2(g) + H 2 O (l) + NaCl (aq) The acidification of baking soda (i.e., sodium hydrogen carbonate or sodium bicarbonate) with vinegar (i.e., acetic acid) is a well-known reaction that has carbon dioxide as one of the products.