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Section 2.4—Defining, Naming & Writing Acids & Bases

Section 2.4—Defining, Naming & Writing Acids & Bases. We need to know how acids and bases behave when talking about ant-acids!. Acids. H. +1. +1. H. water. O. O. H. H. H. H. Acids – Arrhenius Definition.

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Section 2.4—Defining, Naming & Writing Acids & Bases

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  1. Section 2.4—Defining, Naming & Writing Acids & Bases We need to know how acids and bases behave when talking about ant-acids!

  2. Acids

  3. H +1 +1 H water O O H H H H Acids – Arrhenius Definition • A compound that has a H+ cation that it can donate to water to produce the hydronium ion (H3O+1) hydronium ion By this definition, if an acid is to give a H+1 to water, then all acids will have hydrogen as the cation (first element written).

  4. - H O H H How do Acids produce Hydronium? water acid Hydrogen cation with some anion

  5. - H O H H How do Acids produce Hydronium? +1

  6. - H O H H How do Acids produce Hydronium? +1 Hydronium ion Anion

  7. Naming Acids

  8. Naming Non-oxygen Acids • These compounds : • Start with “H” (more than 1 “H” is OK, too). • Have only 2 elements in total (One of them is hydrogen the other is NOT oxygen.) • Examples: HCl H2S • To name these compounds: • Use “hydro____ic acid” • Fill in the blank with the anion’s name without the last syllable

  9. Example #1 HBr

  10. Example #1 It’s an acid Hydrogen cation HBr Hydrobromic acid Bromine No oxygen Use “hydro___ic”

  11. Naming Oxygen Acids • These compounds have: • Start with “H” (more than 1 “H” is OK, too). • Contain a polyatomic ion that has oxygen in it. • To name these compounds: • Use “___ic acid” for “-ate” anions; the blank is filled in with the polyatomic ions name without the suffix. • Use “___ous acid” for “-ite” anions; the blank is filled in with the polyatomic ions name without the suffix. Examples: HNO2 is . . . HNO3 is . . .

  12. Example #2 H2SO3

  13. Example #2 It’s an acid Hydrogen cation H2SO3 Sulfite ion “-ite” ion Use “___ous” acid Sulfurous acid

  14. Example #3 H2SO4

  15. Example #3 It’s an acid Hydrogen cation H2SO4 Sulfate ion “-ate” ion Use “___ic” Sulfuric acid

  16. Let’s Practice HI H2CO3 HC2H3O2 H3PO3 Example: Write the name for the following compounds

  17. Let’s Practice HI H2CO3 HC2H3O2 H3PO3 hydroiodic acid carbonic acid acetic acid phosphorous acid Example: Write the name for the following compounds

  18. Writing Acid Formulas

  19. “Hydro-” acids • To write these formulas: • The cation is H+1 • Write the anion and charge • Balance the charges by adding the appropriate subscript to the hydrogen cation

  20. Example #4 Hydrofluoric acid

  21. Example #4 H+1 Hydrogen cation Hydrofluoric acid Only one other element F-1

  22. Example #4 H+1 Hydrogen cation Hydrofluoric acid Does not contain oxygen H+1F-1 F-1 HF

  23. NON “Hydro-” acids • To write these formulas: • The cation is H+1 • If it is an “-ic” acid, the anion is the “-ate” polyatomic ion • If it is an “-ous” acid, the anion is the “-ite” polyatomic ion • Add subscript to the hydrogen cation to balance charges

  24. Example #5 Carbonic acid

  25. Example #5 H+1 Hydrogen cation Carbonic acid From the “___ate” anion CO3-2

  26. Example #5 H+1 Hydrogen cation Carbonic acid H+CO32- From the “___ate” anion CO3-2 H2CO3

  27. Example #6 Nitrous acid

  28. Example #6 H+1 Hydrogen cation Nitrous acid From the “___ite” anion NO2-1

  29. Example #6 H+1 Hydrogen cation Nitrous acid H+NO2- From the “___ite” anion HNO2 NO2-1

  30. Let’s Practice Phosphoric acid Hydroiodic acid Acetic acid Perchloric acid Example: Write the formula for the following acids

  31. Let’s Practice Phosphoric acid Hydroiodic acid Acetic acid Perchloric acid H3PO4 HI HC2H3O2 HClO4 Example: Write the formula for the following acids

  32. Bases • Objective: • Define and distinguish between acids & bases • Explain and use nomenclature rules for naming and writing formulas for bases

  33. -1 O H Bases – Arrhenius Definition • Bases produce the hydroxide ion in water • MOST bases will be ionic compounds with the OH-1 anion. (Ex. NaOH or Ca(OH)2) • MOST IMPORTANT EXCEPTION is NH3 (ammonia). • NH3 + H2O  NH4+1 + OH-1 Hydroxide Ion

  34. Naming & Writing Bases

  35. Naming Bases • Most bases are just ionic compounds with “hydroxide” as their anion • The most common exception to this is ammonia. NH3 is a base even though it doesn’t contain “-OH” as the anion.

  36. Example #7 NaOH

  37. Example #7 Sodium NaOH Sodium Hydroxide Hydroxide

  38. Example #8 Iron (III)hydroxide Fe+3 OH-1 criss –cross the number of the charges Fe(OH)3

  39. Let’s Practice Ca(OH)2 KOH Sr(OH)2 Copper (II) hydroxide Magnesium hydroxide Example: Write the formula or name for each

  40. Let’s Practice Ca(OH)2 KOH Sr(OH)2 Copper (II) hydroxide Magnesium hydroxide Calcium hydroxide Potassium hydroxide Strontium hydroxide Cu(OH)2 Mg(OH)2 Example: Write the formula or name for each

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