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Naming Acids

Naming Acids. Chemistry 11 Mrs. Kay. 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

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Naming Acids

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  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.

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

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