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Review of Acids, Bases, & Salts

Review of Acids, Bases, & Salts. Arrhenius Acid. Has H in the formula Produces H + as the only positive ion in solution. Formula of an Acid. Inorganic – formula starts with H Organic – formula ends with COOH. Properties of Acids. Sour Taste Electrolytes

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Review of Acids, Bases, & Salts

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  1. Review of Acids, Bases, & Salts

  2. Arrhenius Acid Has H in the formula Produces H+ as the only positive ion in solution

  3. Formula of an Acid Inorganic – formula starts with H Organic – formula ends with COOH

  4. Properties of Acids Sour Taste Electrolytes React with bases to form a salt + H2O Turn litmus RED React with most metals to produce H2(g)

  5. Ionization of an Acid or HCl + H2O  H3O+ + Cl- HCl  H+ + Cl-

  6. Arrhenius Base Has OH in the formula Produces OH- as the only negative ion in solution

  7. Formula of a Base Has format MOH M is a metal

  8. Properties of Bases Bitter Taste Slippery Feel Electrolytes React with acids to form a salt + H2O Turn litmus BLUE

  9. Ionization of a Base NaOH  Na+ + OH-

  10. Ionization of NH3 NH3 + H2O  NH4+ + OH-

  11. Formula of a Salt Metal + Nonmetal

  12. Write the formula of potasium sulfate K2SO4 K+ & (SO4)2-

  13. Electrolytes Solutions conduct – they contain ions Acids (HX), bases (MOH), & salts (MX) are electrolytes

  14. NONelectrolytes Solutions of covalent compounds (all nonmetals). They do NOT conduct.

  15. LiOH CH3COOH C6H12O6 NaNO3 H2SO4 CH3OH Ca(OH)2 HCl C8H18 Al(OH)3 HNO3 CH3CH2COOH K2SO4 CH3CHOHCH3 CH3OCH3 H3PO4 Mg(OH)2 CH3CH2OH Identify the electrolytes Yes - B Yes - B Yes - A Yes - A Yes - A No Yes - S Yes - S Yes - A No No No Yes - A Yes - B Yes - A Yes - B No No

  16. pH scale 0-14 Acidic: 0 to 7, Neutral: 7 Basic: 7-14

  17. Most acidic on pH scale pH = 0

  18. Most basic on pH scale pH = 14

  19. OH- Hydroxide ion

  20. H+ Hydrogen ion or Proton

  21. H3O+ Hydronium ion. Interchangeable with H+.

  22. Acidic Solution [H+]  [OH-]

  23. Basic Solution [OH-]  [H+]

  24. If the pH changes from 3 to 5, how does the [H+] change? The pH changes by 2, so the [H+] changes by 102or 100X. Since the pH went up, it became LESS acidic. The new solution has a [H+] 100 times less than the original solution.

  25. How can pH be safely tested? Instrumental – use pH meter Indicators – use a series of indicators to narrow down the pH range Test acids with metals (NOT Cu, Ag, or Au)

  26. Bronsted-Lowry Acid Proton Donor

  27. Bronsted-Lowry Base Proton Acceptor

  28. Bronsted-Lowry Acids & Bases HCl + H2O  H3O+ + Cl-

  29. Strong Acids & Bases Complete or almost complete ionization.

  30. Weak Acids & Bases Ionization occurs only to a slight extent, a few percent.

  31. Reactions of Acids with Metals Metal + Acid  H2(g) + salt

  32. Zn(s) + HCl  ? Zn(s) + 2HCl  H2(g) + ZnCl2

  33. Al(s) + HCl  ? 2Al(s) + 6HCl  3H2(g) + 2AlCl3

  34. Neutralization Reactions Acid + Base  Salt + H2O

  35. Net Ionic Equation for Neutralization Reactions H+ + OH-  H2O

  36. At neutralization Moles H+ = Moles OH-

  37. Molarity (M) Liters of soln Molarity = Moles solute

  38. Titration Equation This equation works when the number of H’s on the acid EQUALS the number of OH’s on the base! MaVa = MbVb

  39. Titration Equation This equation works when the number of H’s on the acid does NOT equal the number of OH’s on the base! na = number of acidic H’s in acid. nb = number of OH’s in base. naMaVa = nbMbVb

  40. pH -log[H+] or –log[H3O+]

  41. pOH -log[OH-]

  42. pOH + pH = 14

  43. [OH-] X [H+] = 1.0 X 10-14

  44. 3 If the [H+] = 1 X 10-3 11 1 X 10-11 The pH = The pOH = The [OH-] =

  45. Indicator Substance that changes color over a narrow pH range.

  46. Molarity H2SO4 Vs. Molarity H+ H2SO4  2H+ + SO42- [H+] = 2[H2SO4] 2M H2SO4  4M H+

  47. What is the concentration of a hydrochloric acid solution if 50.0 mL of a 0.250 M KOH solution are needed to neutralize 20.0 mL of the HCl solution of unknown concentration? MaVa = MbVb X(20.0 mls) = .250M(50.0mls)

  48. (1.50 M)(10.62 mls) = X(20.20 mls)

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