1 Chapter 10 Acids and Bases 10.1 Acids and Bases 10.2 Conjugate Acid-Base Pairs

2 Arrhenius acids  Produce H + ions in water. H 2 O HCl H + (aq) + Cl - (aq)  Are electrolytes.  Have a sour taste.  Corrode metals.  React with bases to form salts and water. Acids

3 Arrhenius bases  Produce OH - ions in water.  Taste bitter or chalky.  Are electrolytes.  Feel soapy and slippery.  React with acids to form salts and water. Bases

4 Comparing Acids and Bases

5 Names of Acids Acids with H and one nonmetal are named with the prefix hydro- and end with -ic acid. HClhydrochloric acid Acids with H and a polyatomic ion are named by changing the end of an –ate ion to -ic acid and an –ite ion to -ous acid. HClO 3 chloric acid HClO 2 chlorous acid

6  Bases with OH - ions are named as the hydroxide of the metal in the formula. NaOHsodium hydroxide KOH potassium hydroxide Ba(OH) 2 barium hydroxide Al(OH) 3 aluminum hydroxide Fe(OH) 3 iron (III) hydroxide Some Common Bases

7 According to the Br Ø nsted-Lowry theory, Acids are hydrogen ion (H + ) donors. Bases are hydrogen ion (H + ) acceptors. donor acceptor hydronium ion HCl + H 2 O H 3 O + + Cl Br Ø nsted-Lowry Acids and Bases

8 When NH 3 dissolves in water, a few NH 3 molecules react with water to form ammonium ion NH 4 + and a hydroxide ion. NH 3 + H 2 O NH 4 + (aq) + OH - (aq) acceptor donor NH 3, A Bronsted-Lowry Base

9 Conjugate Acids and Bases An acid that donates H + forms a conjugate base. A base that accepts a H + forms a conjugate acid. In an acid-base reaction, there are two conjugate acid-base pairs. acid 1 conjugate base base 2 conjugate acid 2 HF H2OH2O H3O+H3O+ F -

10 Conjugate Acid-Base Pairs A conjugate acid-base pair is two substances related by a loss or gain of H acid 1– conjugate base 1 base 2– conjugate acid 2 HF H2OH2O H3O+H3O+ F - HF, F - H 2 O, H 3 O +