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 - 2M2M 2M pH of acids is directly related to the amount of dissociation of the hydrogen.

3. Binary Acids (made of 2 elements only) 1.Prefix is always hydro 2.Name the second element with the suffix? ic Example: HCl hydrochloric acid

4. Practice NameFormula Hydrobromic acid HF Hydroiodic acid 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, H 2 SO 4 –Nitric acid, HNO 3 –Hydrochloric acid, HCl –Hydroiodic acid, HI –Hydrobromic acid, HBr –Perchloric acid, HClO 4 dissociation: HNO 3  H + + NO 3 -

6. Tertiary acids (made up of 3 elements) H + -ate polyatomic ion: If the acid has an -ate polyatomic ion after the H, that makes it an -ic acid. H 2 SO 4 is sulfuric acid. H + -ite polyatomic ion: When the acid has an -ite polyatomic ion after the H, that makes it an -ous acid. H 2 SO 3 is sulfurous acid.

7. Anion Acid Name Hypo ______ite Hypo _____ous acid _______ite _______ous acid _______ate ________ic acid per_______ate per_______ic acid

8. Practice: NameFormula HNO 2 Carbonic acid H 3 PO 4 Acetic acid H 2 SO 3 Nitrous acid H 2 CO 3 Phosphoric acid CH 3 COOH Sulfurous acid