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Chapter 20 Notes, part I

Chapter 20 Notes, part I. Acids and Bases. What are some common acids?. Vinegar (acetic acid) Carbonated drinks (carbonic and phosphoric acid) Citrus fruits (citric acid) Car battery (sulfuric acid). What are some common bases?. Milk of magnesia (an antacid containing magnesium hydroxide)

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Chapter 20 Notes, part I

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  1. Chapter 20 Notes, part I Acids and Bases

  2. What are some common acids? • Vinegar (acetic acid) • Carbonated drinks (carbonic and phosphoric acid) • Citrus fruits (citric acid) • Car battery (sulfuric acid)

  3. What are some common bases? • Milk of magnesia (an antacid containing magnesium hydroxide) • Many cleaning products (ammonia, etc)

  4. What properties do acids have? • Acids tend to be: • Tart or sour tasting • In solution, they are an electrolyte • They can cause chemical dyes (called indicators) to change colors

  5. What properties do bases have? • Bases tend to be: • Bitter tasting • Slippery feeling when touched • Able to neutralize an acid

  6. Salts are ionic compounds formed from a cation (other than H+) and an anion (other than OH-). • any ionic compound that is not classified as an acid or base. • taste salty! • Electrolytes are substances that can conduct electricity when dissolved in water. • electricity is the flow of electrons (e-). • cations (+) allow (-) e- to flow through water. • There are three classes of electrolytes… • acids, bases and salts! • Good electrolytes ionize (dissociate) completely (100%) in water. • HNO3, HCl, NaOH and KOH all ionize completely

  7. So what IS an acid? • An acid is a compound that produces hydrogen ions (H+) when dissolved in water. • The formula would be HaX, where X is any monatomic or polyatomic anion and a is the anion’s charge.

  8. Obj. 5-6…Acid Nomenclature • Two types of acids…binary and ternary • Binary acids (two capital letters)… • ‘hydro______ic acid’ hydrofluoric acid • HF = • H2S = hydrosulfuric acid • Ternary acids (three or more capital letters)… • NO HYDRO!!! • ‘ate – ic / ite – ous’ • anions ending in ‘ate’ change to ‘ic’…anions ending in ‘ite’ change to ‘ous’! sulfuric acid • H2SO4 = nitrous acid • HNO2 = sulfate nitrite

  9. Obj. 5-6 cont… • To write formulas for acids… • formula starts with H • prefix ‘hydro’ = only 2 capital letters • no ‘hydro’ = H + polyatomic ion (ate – ic / ite – ous) • look at oxidation #s to see if subscripts are needed • Ex… H2C2O4 • oxalic acid = H+1 and C2O4-2 = • hydroiodic acid = H+1 and I -1 = HI • sulfurous acid = H+1 and SO3 -2 = H2SO3

  10. Naming an acid • When the name of the anion (X) ends in –ide, the name begins with hydro-, then the stem of the anion, then the name ends with –ic acid instead of -ide. • When the name of the ion ends in –ite, then the name would be the stem of the anion and the suffix –ous acid instead of –ite. • When the name of the ion ends in –ate, then the name would be the stem of the anion and the suffix –ic acid instead of-ate.

  11. Then what is a base? • A base is a compound that produces hydroxide (OH-) ions when in solution. • Bases are named the same way that an ionic compound would be named.

  12. Name the following acids and bases:

  13. HClO3 ChloricAcid

  14. H3PO4 Phosphoric Acid

  15. HF Hydrofluoric Acid

  16. HNO3 Nitric Acid

  17. KOH Potassium Hydroxide

  18. H2SO4 Sulfuric Acid

  19. Ba(OH)2 Barium Hydroxide

  20. HCN Hydrocyanic Acid

  21. H3PO3 Phosphorous Acid

  22. HClO4 Perchloric Acid

  23. HBr Hydrobromic Acid

  24. H2CO3 Carbonic Acid

  25. Al(OH)3 Aluminum Hydroxide

  26. Write the formula for the following acids and bases:

  27. Hydrochloric Acid HCl

  28. Barium Hydroxide Ba(OH)2

  29. Sulfuric Acid H2SO4

  30. Phosphorous Acid H3PO3

  31. Sodium Hydroxide NaOH

  32. Hydroiodic Acid HI

  33. Nitrous Acid HNO2

  34. Ammonium Hydroxide NH4OH

  35. Chromic Acid H2CrO4

  36. Permanganic Acid HMnO4

  37. Hydrobromic Acid HBr

  38. Lithium Hydroxide LiOH

  39. Nitric Acid HNO3

  40. Thiocyanic Acid HSCN

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