1. Naming Acids Chemistry 11 Mrs. Kay

2. Acids • When these compounds dissolve in water they produce hydrogen ions. • The concentration of hydrogen ions produced is related to its molarity (simple ratios) • HCl  H+ + Cl- 2M 2M 2M • pH of acids is directly related to the amount of dissociation of the hydrogen.

3. Binary Acids (made of 2 elements only) • Prefix is always hydro • Name the second element with the suffix? ic Example: HCl hydrochloric acid

4. Practice HBr Hydrofluoric acid HI

5. Strong Acids • These acids dissociate 100% in water, which makes them different from other weaker acids (has to do with pH, not concentration) • You need to memorize them: • Sulfuric acid, H2SO4 • Nitric acid, HNO3 • Hydrochloric acid, HCl • Hydroiodic acid, HI • Hydrobromic acid, HBr • Perchloric acid, HClO4 • dissociation: HNO3 H+ + NO3-

6. Tertiary acids (made up of 3 elements) • H +-atepolyatomic ion: If the acid has an -ate polyatomic ion after the H, that makes it an -ic acid. H2SO4 is sulfuric acid. • H +-itepolyatomic ion: When the acid has an -ite polyatomic ion after the H, that makes it an -ous acid. H2SO3 is sulfurous acid.

8. Practice: Nitrous acid H2CO3 Phosphoric acid CH3COOH Sulfurous acid